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AP Chem Chapter 2. Elements Compounds & Mixtures. Elements On the Periodic Table Compounds Ionic (metal bonded to nonmetal) Molecular (2 nonmetals bonded together) Mixtures Homogeneous = Solution = 1 phase Heterogeneous = more than 1 phase. What is….?. Salt Silver Sand Salt Water. - PowerPoint PPT Presentation
Citation preview
AP ChemChapter 2
Elements Compounds amp Mixtures Elements
On the Periodic Table Compounds
Ionic (metal bonded to nonmetal) Molecular (2 nonmetals bonded together)
Mixtures Homogeneous = Solution = 1 phase Heterogeneous = more than 1 phase
What ishellip Salt
Silver
Sand
Salt Water
Section 2 Law of Conservation of Mass
Law of Definite Proportions
Law of Multiple Proportions
Daltonrsquos Atomic Theory Very Important The foundation upon
which chemistry is built
Know the 4 postulates
Understand how they relate to the Laws
Section 4mdashChemical History JJ Thompson
Discovered the masscharge ratio for a particle that was over 11000th times smaller than a Hydrogen atomhellipknow to be the least massive atom
He concluded that this particles helped make up the atom
Plum Pudding Model
Oil Drop Experiment Used X-rays to knock electrons off of gas
molecules Oil droplets fell through this area and the
electrons would stick to the drop He could measure the mass of the drop by
its rate of falling By turning on an electric field that the drop
was falling through he could make the drop slow down stop or even move back up
Oil Drop Experiment In other words the charged drop was
repelled by the electrical charge
Millikan was able to calculate the charge and found that the charge was always a whole number multiple of -1602 x 10-19C
In relative terms that charge is -1
MassCharge ratio Since we now know the charge we can
multiple the charge times the masscharge ratio to find the mass of the electron
The mass of the electron is 9109 x 10-28 g
In relative terms it has a mass of 0 because protons and neutrons are 1840 times as massive and they have a relative mass of 1
Mass of a Proton A proton has a mass of 166 x 10-24 g
A neutrons mass is slightly more
1 amu = approximately the mass of a proton
1 amu = 112 of a C-12 atom
Mass of Carbon 1 atom of C-12 has a mass of 12 amu
1 mole of C-12 has a mass of 12 g
Mass of 1 C atom in gramshellip 12 amu (166 X 10-24 g amu) = 1992 X 10-23 g
To find the mass of a mole of C atom multiply x Avogadrorsquos number 1992 X 10-23 g x 602 X 1023 = 120 g
Gold Foil Experiment Rutherford discovered the nucleus
Rutherford was investigating the behavior of alpha particles
However his discovery changed our notions of the structure of the atom
Gold Foil Experiment Rutherford is also credited by some with
discovering the proton as well
James Chadwich discovered the neutron in 1932
Actually the gold foil experiments were carried out by Geiger who worked in Rutherfordrsquos lab
Section 5 Mass number Atomic Number Average Atomic Mass Isotopes Calculating Average Atomic Mass
Isotope notation
A fresh look at atomic theory in light of about 100 years of new discoveries
The Periodic Table Big Fat Review at the table in the back
Section 7 review of bonding Ionic compounds (metal
cationnonmetal anion or polyatomic ion)
Criss Cross Simplify if necessary Name by naming ions
Metal = same as element Nonmetal = root of word + -ide suffix Polyatomic = name of polyatomic ion
Coulombrsquos Law Energy = k q1 x q2 distance
k is a constant q are charges of the two ions Distance is the distance between the two nuclei
Increase in charges means more energy in the bond So MgO has more than NaCl
Decrease in distance means more energy So NaCl has more than RbI because the ions are
smaller and therefore can get closer to one another
Know Common Charges Monatomic ions (consult the periodic table)
Polyatomic ions pretty much have to memorize (pg 68)
Remember that ammonia (NH4+1) is the only
polyatomic cation
Remember ldquoateiterdquo rule
Know Common Charges Transition metals have multiple charges (also called
oxidation numbers or oxidation states)
Cr is +2 +3 or +6 Cr+2 is chromous or chromium (II) Cr+3 is chromic or chromium (III) Cr+6 is chromium (VI)
Remember that a polyatomic ion is a group of ions (bonded covalently to each other) and the overall group has an ionic charge
Hydrates Means that water is ldquotied uprdquo as a part
of the crystal structure
CuSO4 5 H2O is copper (II) sulfate pentahydrate That is the correct name If you heat it and drive off the water
(which ought to be there) we then say that we have anhydrous copper(II) sulfate
Covalent compounds Two nonmetals bonded together Use prefixes in the name (Table 26 on pg
69) NO2 is nitrogen dioxide (no mono prefix is
needed if itrsquos the first element) You name both elements but add ndashide to the root of the second element
N2O is dinitrogen monoxide (if mono is for the second element you must use it)
Acids Look at the anion the H is bonded to Remember H in front of the formula = acid HCl (bonded to chloride a monatomic ion)
Name is hydrochloric acid Hydro prefix -ic suffix and add acid
HNO2 (bonded to nitrite so ndashite) Name is nitrous acid Use the root of the anion add ndashous suffix and acid
HNO3 (bonded to nitrate so ndashate) Name is nitric acid Use the root of the anion add ndashic suffix and acid
Simple Organic Compounds New from Last Year
Prefixes Meth = 1 carbon Eth = 2 carbons Prop = 3 But = 4 Pent = 5 Hex = 6 Hept = 7 Oct = 8 Non = 9 Dec = 10 Undec = 11 Dodec = 12
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Elements Compounds amp Mixtures Elements
On the Periodic Table Compounds
Ionic (metal bonded to nonmetal) Molecular (2 nonmetals bonded together)
Mixtures Homogeneous = Solution = 1 phase Heterogeneous = more than 1 phase
What ishellip Salt
Silver
Sand
Salt Water
Section 2 Law of Conservation of Mass
Law of Definite Proportions
Law of Multiple Proportions
Daltonrsquos Atomic Theory Very Important The foundation upon
which chemistry is built
Know the 4 postulates
Understand how they relate to the Laws
Section 4mdashChemical History JJ Thompson
Discovered the masscharge ratio for a particle that was over 11000th times smaller than a Hydrogen atomhellipknow to be the least massive atom
He concluded that this particles helped make up the atom
Plum Pudding Model
Oil Drop Experiment Used X-rays to knock electrons off of gas
molecules Oil droplets fell through this area and the
electrons would stick to the drop He could measure the mass of the drop by
its rate of falling By turning on an electric field that the drop
was falling through he could make the drop slow down stop or even move back up
Oil Drop Experiment In other words the charged drop was
repelled by the electrical charge
Millikan was able to calculate the charge and found that the charge was always a whole number multiple of -1602 x 10-19C
In relative terms that charge is -1
MassCharge ratio Since we now know the charge we can
multiple the charge times the masscharge ratio to find the mass of the electron
The mass of the electron is 9109 x 10-28 g
In relative terms it has a mass of 0 because protons and neutrons are 1840 times as massive and they have a relative mass of 1
Mass of a Proton A proton has a mass of 166 x 10-24 g
A neutrons mass is slightly more
1 amu = approximately the mass of a proton
1 amu = 112 of a C-12 atom
Mass of Carbon 1 atom of C-12 has a mass of 12 amu
1 mole of C-12 has a mass of 12 g
Mass of 1 C atom in gramshellip 12 amu (166 X 10-24 g amu) = 1992 X 10-23 g
To find the mass of a mole of C atom multiply x Avogadrorsquos number 1992 X 10-23 g x 602 X 1023 = 120 g
Gold Foil Experiment Rutherford discovered the nucleus
Rutherford was investigating the behavior of alpha particles
However his discovery changed our notions of the structure of the atom
Gold Foil Experiment Rutherford is also credited by some with
discovering the proton as well
James Chadwich discovered the neutron in 1932
Actually the gold foil experiments were carried out by Geiger who worked in Rutherfordrsquos lab
Section 5 Mass number Atomic Number Average Atomic Mass Isotopes Calculating Average Atomic Mass
Isotope notation
A fresh look at atomic theory in light of about 100 years of new discoveries
The Periodic Table Big Fat Review at the table in the back
Section 7 review of bonding Ionic compounds (metal
cationnonmetal anion or polyatomic ion)
Criss Cross Simplify if necessary Name by naming ions
Metal = same as element Nonmetal = root of word + -ide suffix Polyatomic = name of polyatomic ion
Coulombrsquos Law Energy = k q1 x q2 distance
k is a constant q are charges of the two ions Distance is the distance between the two nuclei
Increase in charges means more energy in the bond So MgO has more than NaCl
Decrease in distance means more energy So NaCl has more than RbI because the ions are
smaller and therefore can get closer to one another
Know Common Charges Monatomic ions (consult the periodic table)
Polyatomic ions pretty much have to memorize (pg 68)
Remember that ammonia (NH4+1) is the only
polyatomic cation
Remember ldquoateiterdquo rule
Know Common Charges Transition metals have multiple charges (also called
oxidation numbers or oxidation states)
Cr is +2 +3 or +6 Cr+2 is chromous or chromium (II) Cr+3 is chromic or chromium (III) Cr+6 is chromium (VI)
Remember that a polyatomic ion is a group of ions (bonded covalently to each other) and the overall group has an ionic charge
Hydrates Means that water is ldquotied uprdquo as a part
of the crystal structure
CuSO4 5 H2O is copper (II) sulfate pentahydrate That is the correct name If you heat it and drive off the water
(which ought to be there) we then say that we have anhydrous copper(II) sulfate
Covalent compounds Two nonmetals bonded together Use prefixes in the name (Table 26 on pg
69) NO2 is nitrogen dioxide (no mono prefix is
needed if itrsquos the first element) You name both elements but add ndashide to the root of the second element
N2O is dinitrogen monoxide (if mono is for the second element you must use it)
Acids Look at the anion the H is bonded to Remember H in front of the formula = acid HCl (bonded to chloride a monatomic ion)
Name is hydrochloric acid Hydro prefix -ic suffix and add acid
HNO2 (bonded to nitrite so ndashite) Name is nitrous acid Use the root of the anion add ndashous suffix and acid
HNO3 (bonded to nitrate so ndashate) Name is nitric acid Use the root of the anion add ndashic suffix and acid
Simple Organic Compounds New from Last Year
Prefixes Meth = 1 carbon Eth = 2 carbons Prop = 3 But = 4 Pent = 5 Hex = 6 Hept = 7 Oct = 8 Non = 9 Dec = 10 Undec = 11 Dodec = 12
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
What ishellip Salt
Silver
Sand
Salt Water
Section 2 Law of Conservation of Mass
Law of Definite Proportions
Law of Multiple Proportions
Daltonrsquos Atomic Theory Very Important The foundation upon
which chemistry is built
Know the 4 postulates
Understand how they relate to the Laws
Section 4mdashChemical History JJ Thompson
Discovered the masscharge ratio for a particle that was over 11000th times smaller than a Hydrogen atomhellipknow to be the least massive atom
He concluded that this particles helped make up the atom
Plum Pudding Model
Oil Drop Experiment Used X-rays to knock electrons off of gas
molecules Oil droplets fell through this area and the
electrons would stick to the drop He could measure the mass of the drop by
its rate of falling By turning on an electric field that the drop
was falling through he could make the drop slow down stop or even move back up
Oil Drop Experiment In other words the charged drop was
repelled by the electrical charge
Millikan was able to calculate the charge and found that the charge was always a whole number multiple of -1602 x 10-19C
In relative terms that charge is -1
MassCharge ratio Since we now know the charge we can
multiple the charge times the masscharge ratio to find the mass of the electron
The mass of the electron is 9109 x 10-28 g
In relative terms it has a mass of 0 because protons and neutrons are 1840 times as massive and they have a relative mass of 1
Mass of a Proton A proton has a mass of 166 x 10-24 g
A neutrons mass is slightly more
1 amu = approximately the mass of a proton
1 amu = 112 of a C-12 atom
Mass of Carbon 1 atom of C-12 has a mass of 12 amu
1 mole of C-12 has a mass of 12 g
Mass of 1 C atom in gramshellip 12 amu (166 X 10-24 g amu) = 1992 X 10-23 g
To find the mass of a mole of C atom multiply x Avogadrorsquos number 1992 X 10-23 g x 602 X 1023 = 120 g
Gold Foil Experiment Rutherford discovered the nucleus
Rutherford was investigating the behavior of alpha particles
However his discovery changed our notions of the structure of the atom
Gold Foil Experiment Rutherford is also credited by some with
discovering the proton as well
James Chadwich discovered the neutron in 1932
Actually the gold foil experiments were carried out by Geiger who worked in Rutherfordrsquos lab
Section 5 Mass number Atomic Number Average Atomic Mass Isotopes Calculating Average Atomic Mass
Isotope notation
A fresh look at atomic theory in light of about 100 years of new discoveries
The Periodic Table Big Fat Review at the table in the back
Section 7 review of bonding Ionic compounds (metal
cationnonmetal anion or polyatomic ion)
Criss Cross Simplify if necessary Name by naming ions
Metal = same as element Nonmetal = root of word + -ide suffix Polyatomic = name of polyatomic ion
Coulombrsquos Law Energy = k q1 x q2 distance
k is a constant q are charges of the two ions Distance is the distance between the two nuclei
Increase in charges means more energy in the bond So MgO has more than NaCl
Decrease in distance means more energy So NaCl has more than RbI because the ions are
smaller and therefore can get closer to one another
Know Common Charges Monatomic ions (consult the periodic table)
Polyatomic ions pretty much have to memorize (pg 68)
Remember that ammonia (NH4+1) is the only
polyatomic cation
Remember ldquoateiterdquo rule
Know Common Charges Transition metals have multiple charges (also called
oxidation numbers or oxidation states)
Cr is +2 +3 or +6 Cr+2 is chromous or chromium (II) Cr+3 is chromic or chromium (III) Cr+6 is chromium (VI)
Remember that a polyatomic ion is a group of ions (bonded covalently to each other) and the overall group has an ionic charge
Hydrates Means that water is ldquotied uprdquo as a part
of the crystal structure
CuSO4 5 H2O is copper (II) sulfate pentahydrate That is the correct name If you heat it and drive off the water
(which ought to be there) we then say that we have anhydrous copper(II) sulfate
Covalent compounds Two nonmetals bonded together Use prefixes in the name (Table 26 on pg
69) NO2 is nitrogen dioxide (no mono prefix is
needed if itrsquos the first element) You name both elements but add ndashide to the root of the second element
N2O is dinitrogen monoxide (if mono is for the second element you must use it)
Acids Look at the anion the H is bonded to Remember H in front of the formula = acid HCl (bonded to chloride a monatomic ion)
Name is hydrochloric acid Hydro prefix -ic suffix and add acid
HNO2 (bonded to nitrite so ndashite) Name is nitrous acid Use the root of the anion add ndashous suffix and acid
HNO3 (bonded to nitrate so ndashate) Name is nitric acid Use the root of the anion add ndashic suffix and acid
Simple Organic Compounds New from Last Year
Prefixes Meth = 1 carbon Eth = 2 carbons Prop = 3 But = 4 Pent = 5 Hex = 6 Hept = 7 Oct = 8 Non = 9 Dec = 10 Undec = 11 Dodec = 12
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Section 2 Law of Conservation of Mass
Law of Definite Proportions
Law of Multiple Proportions
Daltonrsquos Atomic Theory Very Important The foundation upon
which chemistry is built
Know the 4 postulates
Understand how they relate to the Laws
Section 4mdashChemical History JJ Thompson
Discovered the masscharge ratio for a particle that was over 11000th times smaller than a Hydrogen atomhellipknow to be the least massive atom
He concluded that this particles helped make up the atom
Plum Pudding Model
Oil Drop Experiment Used X-rays to knock electrons off of gas
molecules Oil droplets fell through this area and the
electrons would stick to the drop He could measure the mass of the drop by
its rate of falling By turning on an electric field that the drop
was falling through he could make the drop slow down stop or even move back up
Oil Drop Experiment In other words the charged drop was
repelled by the electrical charge
Millikan was able to calculate the charge and found that the charge was always a whole number multiple of -1602 x 10-19C
In relative terms that charge is -1
MassCharge ratio Since we now know the charge we can
multiple the charge times the masscharge ratio to find the mass of the electron
The mass of the electron is 9109 x 10-28 g
In relative terms it has a mass of 0 because protons and neutrons are 1840 times as massive and they have a relative mass of 1
Mass of a Proton A proton has a mass of 166 x 10-24 g
A neutrons mass is slightly more
1 amu = approximately the mass of a proton
1 amu = 112 of a C-12 atom
Mass of Carbon 1 atom of C-12 has a mass of 12 amu
1 mole of C-12 has a mass of 12 g
Mass of 1 C atom in gramshellip 12 amu (166 X 10-24 g amu) = 1992 X 10-23 g
To find the mass of a mole of C atom multiply x Avogadrorsquos number 1992 X 10-23 g x 602 X 1023 = 120 g
Gold Foil Experiment Rutherford discovered the nucleus
Rutherford was investigating the behavior of alpha particles
However his discovery changed our notions of the structure of the atom
Gold Foil Experiment Rutherford is also credited by some with
discovering the proton as well
James Chadwich discovered the neutron in 1932
Actually the gold foil experiments were carried out by Geiger who worked in Rutherfordrsquos lab
Section 5 Mass number Atomic Number Average Atomic Mass Isotopes Calculating Average Atomic Mass
Isotope notation
A fresh look at atomic theory in light of about 100 years of new discoveries
The Periodic Table Big Fat Review at the table in the back
Section 7 review of bonding Ionic compounds (metal
cationnonmetal anion or polyatomic ion)
Criss Cross Simplify if necessary Name by naming ions
Metal = same as element Nonmetal = root of word + -ide suffix Polyatomic = name of polyatomic ion
Coulombrsquos Law Energy = k q1 x q2 distance
k is a constant q are charges of the two ions Distance is the distance between the two nuclei
Increase in charges means more energy in the bond So MgO has more than NaCl
Decrease in distance means more energy So NaCl has more than RbI because the ions are
smaller and therefore can get closer to one another
Know Common Charges Monatomic ions (consult the periodic table)
Polyatomic ions pretty much have to memorize (pg 68)
Remember that ammonia (NH4+1) is the only
polyatomic cation
Remember ldquoateiterdquo rule
Know Common Charges Transition metals have multiple charges (also called
oxidation numbers or oxidation states)
Cr is +2 +3 or +6 Cr+2 is chromous or chromium (II) Cr+3 is chromic or chromium (III) Cr+6 is chromium (VI)
Remember that a polyatomic ion is a group of ions (bonded covalently to each other) and the overall group has an ionic charge
Hydrates Means that water is ldquotied uprdquo as a part
of the crystal structure
CuSO4 5 H2O is copper (II) sulfate pentahydrate That is the correct name If you heat it and drive off the water
(which ought to be there) we then say that we have anhydrous copper(II) sulfate
Covalent compounds Two nonmetals bonded together Use prefixes in the name (Table 26 on pg
69) NO2 is nitrogen dioxide (no mono prefix is
needed if itrsquos the first element) You name both elements but add ndashide to the root of the second element
N2O is dinitrogen monoxide (if mono is for the second element you must use it)
Acids Look at the anion the H is bonded to Remember H in front of the formula = acid HCl (bonded to chloride a monatomic ion)
Name is hydrochloric acid Hydro prefix -ic suffix and add acid
HNO2 (bonded to nitrite so ndashite) Name is nitrous acid Use the root of the anion add ndashous suffix and acid
HNO3 (bonded to nitrate so ndashate) Name is nitric acid Use the root of the anion add ndashic suffix and acid
Simple Organic Compounds New from Last Year
Prefixes Meth = 1 carbon Eth = 2 carbons Prop = 3 But = 4 Pent = 5 Hex = 6 Hept = 7 Oct = 8 Non = 9 Dec = 10 Undec = 11 Dodec = 12
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Daltonrsquos Atomic Theory Very Important The foundation upon
which chemistry is built
Know the 4 postulates
Understand how they relate to the Laws
Section 4mdashChemical History JJ Thompson
Discovered the masscharge ratio for a particle that was over 11000th times smaller than a Hydrogen atomhellipknow to be the least massive atom
He concluded that this particles helped make up the atom
Plum Pudding Model
Oil Drop Experiment Used X-rays to knock electrons off of gas
molecules Oil droplets fell through this area and the
electrons would stick to the drop He could measure the mass of the drop by
its rate of falling By turning on an electric field that the drop
was falling through he could make the drop slow down stop or even move back up
Oil Drop Experiment In other words the charged drop was
repelled by the electrical charge
Millikan was able to calculate the charge and found that the charge was always a whole number multiple of -1602 x 10-19C
In relative terms that charge is -1
MassCharge ratio Since we now know the charge we can
multiple the charge times the masscharge ratio to find the mass of the electron
The mass of the electron is 9109 x 10-28 g
In relative terms it has a mass of 0 because protons and neutrons are 1840 times as massive and they have a relative mass of 1
Mass of a Proton A proton has a mass of 166 x 10-24 g
A neutrons mass is slightly more
1 amu = approximately the mass of a proton
1 amu = 112 of a C-12 atom
Mass of Carbon 1 atom of C-12 has a mass of 12 amu
1 mole of C-12 has a mass of 12 g
Mass of 1 C atom in gramshellip 12 amu (166 X 10-24 g amu) = 1992 X 10-23 g
To find the mass of a mole of C atom multiply x Avogadrorsquos number 1992 X 10-23 g x 602 X 1023 = 120 g
Gold Foil Experiment Rutherford discovered the nucleus
Rutherford was investigating the behavior of alpha particles
However his discovery changed our notions of the structure of the atom
Gold Foil Experiment Rutherford is also credited by some with
discovering the proton as well
James Chadwich discovered the neutron in 1932
Actually the gold foil experiments were carried out by Geiger who worked in Rutherfordrsquos lab
Section 5 Mass number Atomic Number Average Atomic Mass Isotopes Calculating Average Atomic Mass
Isotope notation
A fresh look at atomic theory in light of about 100 years of new discoveries
The Periodic Table Big Fat Review at the table in the back
Section 7 review of bonding Ionic compounds (metal
cationnonmetal anion or polyatomic ion)
Criss Cross Simplify if necessary Name by naming ions
Metal = same as element Nonmetal = root of word + -ide suffix Polyatomic = name of polyatomic ion
Coulombrsquos Law Energy = k q1 x q2 distance
k is a constant q are charges of the two ions Distance is the distance between the two nuclei
Increase in charges means more energy in the bond So MgO has more than NaCl
Decrease in distance means more energy So NaCl has more than RbI because the ions are
smaller and therefore can get closer to one another
Know Common Charges Monatomic ions (consult the periodic table)
Polyatomic ions pretty much have to memorize (pg 68)
Remember that ammonia (NH4+1) is the only
polyatomic cation
Remember ldquoateiterdquo rule
Know Common Charges Transition metals have multiple charges (also called
oxidation numbers or oxidation states)
Cr is +2 +3 or +6 Cr+2 is chromous or chromium (II) Cr+3 is chromic or chromium (III) Cr+6 is chromium (VI)
Remember that a polyatomic ion is a group of ions (bonded covalently to each other) and the overall group has an ionic charge
Hydrates Means that water is ldquotied uprdquo as a part
of the crystal structure
CuSO4 5 H2O is copper (II) sulfate pentahydrate That is the correct name If you heat it and drive off the water
(which ought to be there) we then say that we have anhydrous copper(II) sulfate
Covalent compounds Two nonmetals bonded together Use prefixes in the name (Table 26 on pg
69) NO2 is nitrogen dioxide (no mono prefix is
needed if itrsquos the first element) You name both elements but add ndashide to the root of the second element
N2O is dinitrogen monoxide (if mono is for the second element you must use it)
Acids Look at the anion the H is bonded to Remember H in front of the formula = acid HCl (bonded to chloride a monatomic ion)
Name is hydrochloric acid Hydro prefix -ic suffix and add acid
HNO2 (bonded to nitrite so ndashite) Name is nitrous acid Use the root of the anion add ndashous suffix and acid
HNO3 (bonded to nitrate so ndashate) Name is nitric acid Use the root of the anion add ndashic suffix and acid
Simple Organic Compounds New from Last Year
Prefixes Meth = 1 carbon Eth = 2 carbons Prop = 3 But = 4 Pent = 5 Hex = 6 Hept = 7 Oct = 8 Non = 9 Dec = 10 Undec = 11 Dodec = 12
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Section 4mdashChemical History JJ Thompson
Discovered the masscharge ratio for a particle that was over 11000th times smaller than a Hydrogen atomhellipknow to be the least massive atom
He concluded that this particles helped make up the atom
Plum Pudding Model
Oil Drop Experiment Used X-rays to knock electrons off of gas
molecules Oil droplets fell through this area and the
electrons would stick to the drop He could measure the mass of the drop by
its rate of falling By turning on an electric field that the drop
was falling through he could make the drop slow down stop or even move back up
Oil Drop Experiment In other words the charged drop was
repelled by the electrical charge
Millikan was able to calculate the charge and found that the charge was always a whole number multiple of -1602 x 10-19C
In relative terms that charge is -1
MassCharge ratio Since we now know the charge we can
multiple the charge times the masscharge ratio to find the mass of the electron
The mass of the electron is 9109 x 10-28 g
In relative terms it has a mass of 0 because protons and neutrons are 1840 times as massive and they have a relative mass of 1
Mass of a Proton A proton has a mass of 166 x 10-24 g
A neutrons mass is slightly more
1 amu = approximately the mass of a proton
1 amu = 112 of a C-12 atom
Mass of Carbon 1 atom of C-12 has a mass of 12 amu
1 mole of C-12 has a mass of 12 g
Mass of 1 C atom in gramshellip 12 amu (166 X 10-24 g amu) = 1992 X 10-23 g
To find the mass of a mole of C atom multiply x Avogadrorsquos number 1992 X 10-23 g x 602 X 1023 = 120 g
Gold Foil Experiment Rutherford discovered the nucleus
Rutherford was investigating the behavior of alpha particles
However his discovery changed our notions of the structure of the atom
Gold Foil Experiment Rutherford is also credited by some with
discovering the proton as well
James Chadwich discovered the neutron in 1932
Actually the gold foil experiments were carried out by Geiger who worked in Rutherfordrsquos lab
Section 5 Mass number Atomic Number Average Atomic Mass Isotopes Calculating Average Atomic Mass
Isotope notation
A fresh look at atomic theory in light of about 100 years of new discoveries
The Periodic Table Big Fat Review at the table in the back
Section 7 review of bonding Ionic compounds (metal
cationnonmetal anion or polyatomic ion)
Criss Cross Simplify if necessary Name by naming ions
Metal = same as element Nonmetal = root of word + -ide suffix Polyatomic = name of polyatomic ion
Coulombrsquos Law Energy = k q1 x q2 distance
k is a constant q are charges of the two ions Distance is the distance between the two nuclei
Increase in charges means more energy in the bond So MgO has more than NaCl
Decrease in distance means more energy So NaCl has more than RbI because the ions are
smaller and therefore can get closer to one another
Know Common Charges Monatomic ions (consult the periodic table)
Polyatomic ions pretty much have to memorize (pg 68)
Remember that ammonia (NH4+1) is the only
polyatomic cation
Remember ldquoateiterdquo rule
Know Common Charges Transition metals have multiple charges (also called
oxidation numbers or oxidation states)
Cr is +2 +3 or +6 Cr+2 is chromous or chromium (II) Cr+3 is chromic or chromium (III) Cr+6 is chromium (VI)
Remember that a polyatomic ion is a group of ions (bonded covalently to each other) and the overall group has an ionic charge
Hydrates Means that water is ldquotied uprdquo as a part
of the crystal structure
CuSO4 5 H2O is copper (II) sulfate pentahydrate That is the correct name If you heat it and drive off the water
(which ought to be there) we then say that we have anhydrous copper(II) sulfate
Covalent compounds Two nonmetals bonded together Use prefixes in the name (Table 26 on pg
69) NO2 is nitrogen dioxide (no mono prefix is
needed if itrsquos the first element) You name both elements but add ndashide to the root of the second element
N2O is dinitrogen monoxide (if mono is for the second element you must use it)
Acids Look at the anion the H is bonded to Remember H in front of the formula = acid HCl (bonded to chloride a monatomic ion)
Name is hydrochloric acid Hydro prefix -ic suffix and add acid
HNO2 (bonded to nitrite so ndashite) Name is nitrous acid Use the root of the anion add ndashous suffix and acid
HNO3 (bonded to nitrate so ndashate) Name is nitric acid Use the root of the anion add ndashic suffix and acid
Simple Organic Compounds New from Last Year
Prefixes Meth = 1 carbon Eth = 2 carbons Prop = 3 But = 4 Pent = 5 Hex = 6 Hept = 7 Oct = 8 Non = 9 Dec = 10 Undec = 11 Dodec = 12
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Oil Drop Experiment Used X-rays to knock electrons off of gas
molecules Oil droplets fell through this area and the
electrons would stick to the drop He could measure the mass of the drop by
its rate of falling By turning on an electric field that the drop
was falling through he could make the drop slow down stop or even move back up
Oil Drop Experiment In other words the charged drop was
repelled by the electrical charge
Millikan was able to calculate the charge and found that the charge was always a whole number multiple of -1602 x 10-19C
In relative terms that charge is -1
MassCharge ratio Since we now know the charge we can
multiple the charge times the masscharge ratio to find the mass of the electron
The mass of the electron is 9109 x 10-28 g
In relative terms it has a mass of 0 because protons and neutrons are 1840 times as massive and they have a relative mass of 1
Mass of a Proton A proton has a mass of 166 x 10-24 g
A neutrons mass is slightly more
1 amu = approximately the mass of a proton
1 amu = 112 of a C-12 atom
Mass of Carbon 1 atom of C-12 has a mass of 12 amu
1 mole of C-12 has a mass of 12 g
Mass of 1 C atom in gramshellip 12 amu (166 X 10-24 g amu) = 1992 X 10-23 g
To find the mass of a mole of C atom multiply x Avogadrorsquos number 1992 X 10-23 g x 602 X 1023 = 120 g
Gold Foil Experiment Rutherford discovered the nucleus
Rutherford was investigating the behavior of alpha particles
However his discovery changed our notions of the structure of the atom
Gold Foil Experiment Rutherford is also credited by some with
discovering the proton as well
James Chadwich discovered the neutron in 1932
Actually the gold foil experiments were carried out by Geiger who worked in Rutherfordrsquos lab
Section 5 Mass number Atomic Number Average Atomic Mass Isotopes Calculating Average Atomic Mass
Isotope notation
A fresh look at atomic theory in light of about 100 years of new discoveries
The Periodic Table Big Fat Review at the table in the back
Section 7 review of bonding Ionic compounds (metal
cationnonmetal anion or polyatomic ion)
Criss Cross Simplify if necessary Name by naming ions
Metal = same as element Nonmetal = root of word + -ide suffix Polyatomic = name of polyatomic ion
Coulombrsquos Law Energy = k q1 x q2 distance
k is a constant q are charges of the two ions Distance is the distance between the two nuclei
Increase in charges means more energy in the bond So MgO has more than NaCl
Decrease in distance means more energy So NaCl has more than RbI because the ions are
smaller and therefore can get closer to one another
Know Common Charges Monatomic ions (consult the periodic table)
Polyatomic ions pretty much have to memorize (pg 68)
Remember that ammonia (NH4+1) is the only
polyatomic cation
Remember ldquoateiterdquo rule
Know Common Charges Transition metals have multiple charges (also called
oxidation numbers or oxidation states)
Cr is +2 +3 or +6 Cr+2 is chromous or chromium (II) Cr+3 is chromic or chromium (III) Cr+6 is chromium (VI)
Remember that a polyatomic ion is a group of ions (bonded covalently to each other) and the overall group has an ionic charge
Hydrates Means that water is ldquotied uprdquo as a part
of the crystal structure
CuSO4 5 H2O is copper (II) sulfate pentahydrate That is the correct name If you heat it and drive off the water
(which ought to be there) we then say that we have anhydrous copper(II) sulfate
Covalent compounds Two nonmetals bonded together Use prefixes in the name (Table 26 on pg
69) NO2 is nitrogen dioxide (no mono prefix is
needed if itrsquos the first element) You name both elements but add ndashide to the root of the second element
N2O is dinitrogen monoxide (if mono is for the second element you must use it)
Acids Look at the anion the H is bonded to Remember H in front of the formula = acid HCl (bonded to chloride a monatomic ion)
Name is hydrochloric acid Hydro prefix -ic suffix and add acid
HNO2 (bonded to nitrite so ndashite) Name is nitrous acid Use the root of the anion add ndashous suffix and acid
HNO3 (bonded to nitrate so ndashate) Name is nitric acid Use the root of the anion add ndashic suffix and acid
Simple Organic Compounds New from Last Year
Prefixes Meth = 1 carbon Eth = 2 carbons Prop = 3 But = 4 Pent = 5 Hex = 6 Hept = 7 Oct = 8 Non = 9 Dec = 10 Undec = 11 Dodec = 12
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Oil Drop Experiment In other words the charged drop was
repelled by the electrical charge
Millikan was able to calculate the charge and found that the charge was always a whole number multiple of -1602 x 10-19C
In relative terms that charge is -1
MassCharge ratio Since we now know the charge we can
multiple the charge times the masscharge ratio to find the mass of the electron
The mass of the electron is 9109 x 10-28 g
In relative terms it has a mass of 0 because protons and neutrons are 1840 times as massive and they have a relative mass of 1
Mass of a Proton A proton has a mass of 166 x 10-24 g
A neutrons mass is slightly more
1 amu = approximately the mass of a proton
1 amu = 112 of a C-12 atom
Mass of Carbon 1 atom of C-12 has a mass of 12 amu
1 mole of C-12 has a mass of 12 g
Mass of 1 C atom in gramshellip 12 amu (166 X 10-24 g amu) = 1992 X 10-23 g
To find the mass of a mole of C atom multiply x Avogadrorsquos number 1992 X 10-23 g x 602 X 1023 = 120 g
Gold Foil Experiment Rutherford discovered the nucleus
Rutherford was investigating the behavior of alpha particles
However his discovery changed our notions of the structure of the atom
Gold Foil Experiment Rutherford is also credited by some with
discovering the proton as well
James Chadwich discovered the neutron in 1932
Actually the gold foil experiments were carried out by Geiger who worked in Rutherfordrsquos lab
Section 5 Mass number Atomic Number Average Atomic Mass Isotopes Calculating Average Atomic Mass
Isotope notation
A fresh look at atomic theory in light of about 100 years of new discoveries
The Periodic Table Big Fat Review at the table in the back
Section 7 review of bonding Ionic compounds (metal
cationnonmetal anion or polyatomic ion)
Criss Cross Simplify if necessary Name by naming ions
Metal = same as element Nonmetal = root of word + -ide suffix Polyatomic = name of polyatomic ion
Coulombrsquos Law Energy = k q1 x q2 distance
k is a constant q are charges of the two ions Distance is the distance between the two nuclei
Increase in charges means more energy in the bond So MgO has more than NaCl
Decrease in distance means more energy So NaCl has more than RbI because the ions are
smaller and therefore can get closer to one another
Know Common Charges Monatomic ions (consult the periodic table)
Polyatomic ions pretty much have to memorize (pg 68)
Remember that ammonia (NH4+1) is the only
polyatomic cation
Remember ldquoateiterdquo rule
Know Common Charges Transition metals have multiple charges (also called
oxidation numbers or oxidation states)
Cr is +2 +3 or +6 Cr+2 is chromous or chromium (II) Cr+3 is chromic or chromium (III) Cr+6 is chromium (VI)
Remember that a polyatomic ion is a group of ions (bonded covalently to each other) and the overall group has an ionic charge
Hydrates Means that water is ldquotied uprdquo as a part
of the crystal structure
CuSO4 5 H2O is copper (II) sulfate pentahydrate That is the correct name If you heat it and drive off the water
(which ought to be there) we then say that we have anhydrous copper(II) sulfate
Covalent compounds Two nonmetals bonded together Use prefixes in the name (Table 26 on pg
69) NO2 is nitrogen dioxide (no mono prefix is
needed if itrsquos the first element) You name both elements but add ndashide to the root of the second element
N2O is dinitrogen monoxide (if mono is for the second element you must use it)
Acids Look at the anion the H is bonded to Remember H in front of the formula = acid HCl (bonded to chloride a monatomic ion)
Name is hydrochloric acid Hydro prefix -ic suffix and add acid
HNO2 (bonded to nitrite so ndashite) Name is nitrous acid Use the root of the anion add ndashous suffix and acid
HNO3 (bonded to nitrate so ndashate) Name is nitric acid Use the root of the anion add ndashic suffix and acid
Simple Organic Compounds New from Last Year
Prefixes Meth = 1 carbon Eth = 2 carbons Prop = 3 But = 4 Pent = 5 Hex = 6 Hept = 7 Oct = 8 Non = 9 Dec = 10 Undec = 11 Dodec = 12
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
MassCharge ratio Since we now know the charge we can
multiple the charge times the masscharge ratio to find the mass of the electron
The mass of the electron is 9109 x 10-28 g
In relative terms it has a mass of 0 because protons and neutrons are 1840 times as massive and they have a relative mass of 1
Mass of a Proton A proton has a mass of 166 x 10-24 g
A neutrons mass is slightly more
1 amu = approximately the mass of a proton
1 amu = 112 of a C-12 atom
Mass of Carbon 1 atom of C-12 has a mass of 12 amu
1 mole of C-12 has a mass of 12 g
Mass of 1 C atom in gramshellip 12 amu (166 X 10-24 g amu) = 1992 X 10-23 g
To find the mass of a mole of C atom multiply x Avogadrorsquos number 1992 X 10-23 g x 602 X 1023 = 120 g
Gold Foil Experiment Rutherford discovered the nucleus
Rutherford was investigating the behavior of alpha particles
However his discovery changed our notions of the structure of the atom
Gold Foil Experiment Rutherford is also credited by some with
discovering the proton as well
James Chadwich discovered the neutron in 1932
Actually the gold foil experiments were carried out by Geiger who worked in Rutherfordrsquos lab
Section 5 Mass number Atomic Number Average Atomic Mass Isotopes Calculating Average Atomic Mass
Isotope notation
A fresh look at atomic theory in light of about 100 years of new discoveries
The Periodic Table Big Fat Review at the table in the back
Section 7 review of bonding Ionic compounds (metal
cationnonmetal anion or polyatomic ion)
Criss Cross Simplify if necessary Name by naming ions
Metal = same as element Nonmetal = root of word + -ide suffix Polyatomic = name of polyatomic ion
Coulombrsquos Law Energy = k q1 x q2 distance
k is a constant q are charges of the two ions Distance is the distance between the two nuclei
Increase in charges means more energy in the bond So MgO has more than NaCl
Decrease in distance means more energy So NaCl has more than RbI because the ions are
smaller and therefore can get closer to one another
Know Common Charges Monatomic ions (consult the periodic table)
Polyatomic ions pretty much have to memorize (pg 68)
Remember that ammonia (NH4+1) is the only
polyatomic cation
Remember ldquoateiterdquo rule
Know Common Charges Transition metals have multiple charges (also called
oxidation numbers or oxidation states)
Cr is +2 +3 or +6 Cr+2 is chromous or chromium (II) Cr+3 is chromic or chromium (III) Cr+6 is chromium (VI)
Remember that a polyatomic ion is a group of ions (bonded covalently to each other) and the overall group has an ionic charge
Hydrates Means that water is ldquotied uprdquo as a part
of the crystal structure
CuSO4 5 H2O is copper (II) sulfate pentahydrate That is the correct name If you heat it and drive off the water
(which ought to be there) we then say that we have anhydrous copper(II) sulfate
Covalent compounds Two nonmetals bonded together Use prefixes in the name (Table 26 on pg
69) NO2 is nitrogen dioxide (no mono prefix is
needed if itrsquos the first element) You name both elements but add ndashide to the root of the second element
N2O is dinitrogen monoxide (if mono is for the second element you must use it)
Acids Look at the anion the H is bonded to Remember H in front of the formula = acid HCl (bonded to chloride a monatomic ion)
Name is hydrochloric acid Hydro prefix -ic suffix and add acid
HNO2 (bonded to nitrite so ndashite) Name is nitrous acid Use the root of the anion add ndashous suffix and acid
HNO3 (bonded to nitrate so ndashate) Name is nitric acid Use the root of the anion add ndashic suffix and acid
Simple Organic Compounds New from Last Year
Prefixes Meth = 1 carbon Eth = 2 carbons Prop = 3 But = 4 Pent = 5 Hex = 6 Hept = 7 Oct = 8 Non = 9 Dec = 10 Undec = 11 Dodec = 12
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Mass of a Proton A proton has a mass of 166 x 10-24 g
A neutrons mass is slightly more
1 amu = approximately the mass of a proton
1 amu = 112 of a C-12 atom
Mass of Carbon 1 atom of C-12 has a mass of 12 amu
1 mole of C-12 has a mass of 12 g
Mass of 1 C atom in gramshellip 12 amu (166 X 10-24 g amu) = 1992 X 10-23 g
To find the mass of a mole of C atom multiply x Avogadrorsquos number 1992 X 10-23 g x 602 X 1023 = 120 g
Gold Foil Experiment Rutherford discovered the nucleus
Rutherford was investigating the behavior of alpha particles
However his discovery changed our notions of the structure of the atom
Gold Foil Experiment Rutherford is also credited by some with
discovering the proton as well
James Chadwich discovered the neutron in 1932
Actually the gold foil experiments were carried out by Geiger who worked in Rutherfordrsquos lab
Section 5 Mass number Atomic Number Average Atomic Mass Isotopes Calculating Average Atomic Mass
Isotope notation
A fresh look at atomic theory in light of about 100 years of new discoveries
The Periodic Table Big Fat Review at the table in the back
Section 7 review of bonding Ionic compounds (metal
cationnonmetal anion or polyatomic ion)
Criss Cross Simplify if necessary Name by naming ions
Metal = same as element Nonmetal = root of word + -ide suffix Polyatomic = name of polyatomic ion
Coulombrsquos Law Energy = k q1 x q2 distance
k is a constant q are charges of the two ions Distance is the distance between the two nuclei
Increase in charges means more energy in the bond So MgO has more than NaCl
Decrease in distance means more energy So NaCl has more than RbI because the ions are
smaller and therefore can get closer to one another
Know Common Charges Monatomic ions (consult the periodic table)
Polyatomic ions pretty much have to memorize (pg 68)
Remember that ammonia (NH4+1) is the only
polyatomic cation
Remember ldquoateiterdquo rule
Know Common Charges Transition metals have multiple charges (also called
oxidation numbers or oxidation states)
Cr is +2 +3 or +6 Cr+2 is chromous or chromium (II) Cr+3 is chromic or chromium (III) Cr+6 is chromium (VI)
Remember that a polyatomic ion is a group of ions (bonded covalently to each other) and the overall group has an ionic charge
Hydrates Means that water is ldquotied uprdquo as a part
of the crystal structure
CuSO4 5 H2O is copper (II) sulfate pentahydrate That is the correct name If you heat it and drive off the water
(which ought to be there) we then say that we have anhydrous copper(II) sulfate
Covalent compounds Two nonmetals bonded together Use prefixes in the name (Table 26 on pg
69) NO2 is nitrogen dioxide (no mono prefix is
needed if itrsquos the first element) You name both elements but add ndashide to the root of the second element
N2O is dinitrogen monoxide (if mono is for the second element you must use it)
Acids Look at the anion the H is bonded to Remember H in front of the formula = acid HCl (bonded to chloride a monatomic ion)
Name is hydrochloric acid Hydro prefix -ic suffix and add acid
HNO2 (bonded to nitrite so ndashite) Name is nitrous acid Use the root of the anion add ndashous suffix and acid
HNO3 (bonded to nitrate so ndashate) Name is nitric acid Use the root of the anion add ndashic suffix and acid
Simple Organic Compounds New from Last Year
Prefixes Meth = 1 carbon Eth = 2 carbons Prop = 3 But = 4 Pent = 5 Hex = 6 Hept = 7 Oct = 8 Non = 9 Dec = 10 Undec = 11 Dodec = 12
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Mass of Carbon 1 atom of C-12 has a mass of 12 amu
1 mole of C-12 has a mass of 12 g
Mass of 1 C atom in gramshellip 12 amu (166 X 10-24 g amu) = 1992 X 10-23 g
To find the mass of a mole of C atom multiply x Avogadrorsquos number 1992 X 10-23 g x 602 X 1023 = 120 g
Gold Foil Experiment Rutherford discovered the nucleus
Rutherford was investigating the behavior of alpha particles
However his discovery changed our notions of the structure of the atom
Gold Foil Experiment Rutherford is also credited by some with
discovering the proton as well
James Chadwich discovered the neutron in 1932
Actually the gold foil experiments were carried out by Geiger who worked in Rutherfordrsquos lab
Section 5 Mass number Atomic Number Average Atomic Mass Isotopes Calculating Average Atomic Mass
Isotope notation
A fresh look at atomic theory in light of about 100 years of new discoveries
The Periodic Table Big Fat Review at the table in the back
Section 7 review of bonding Ionic compounds (metal
cationnonmetal anion or polyatomic ion)
Criss Cross Simplify if necessary Name by naming ions
Metal = same as element Nonmetal = root of word + -ide suffix Polyatomic = name of polyatomic ion
Coulombrsquos Law Energy = k q1 x q2 distance
k is a constant q are charges of the two ions Distance is the distance between the two nuclei
Increase in charges means more energy in the bond So MgO has more than NaCl
Decrease in distance means more energy So NaCl has more than RbI because the ions are
smaller and therefore can get closer to one another
Know Common Charges Monatomic ions (consult the periodic table)
Polyatomic ions pretty much have to memorize (pg 68)
Remember that ammonia (NH4+1) is the only
polyatomic cation
Remember ldquoateiterdquo rule
Know Common Charges Transition metals have multiple charges (also called
oxidation numbers or oxidation states)
Cr is +2 +3 or +6 Cr+2 is chromous or chromium (II) Cr+3 is chromic or chromium (III) Cr+6 is chromium (VI)
Remember that a polyatomic ion is a group of ions (bonded covalently to each other) and the overall group has an ionic charge
Hydrates Means that water is ldquotied uprdquo as a part
of the crystal structure
CuSO4 5 H2O is copper (II) sulfate pentahydrate That is the correct name If you heat it and drive off the water
(which ought to be there) we then say that we have anhydrous copper(II) sulfate
Covalent compounds Two nonmetals bonded together Use prefixes in the name (Table 26 on pg
69) NO2 is nitrogen dioxide (no mono prefix is
needed if itrsquos the first element) You name both elements but add ndashide to the root of the second element
N2O is dinitrogen monoxide (if mono is for the second element you must use it)
Acids Look at the anion the H is bonded to Remember H in front of the formula = acid HCl (bonded to chloride a monatomic ion)
Name is hydrochloric acid Hydro prefix -ic suffix and add acid
HNO2 (bonded to nitrite so ndashite) Name is nitrous acid Use the root of the anion add ndashous suffix and acid
HNO3 (bonded to nitrate so ndashate) Name is nitric acid Use the root of the anion add ndashic suffix and acid
Simple Organic Compounds New from Last Year
Prefixes Meth = 1 carbon Eth = 2 carbons Prop = 3 But = 4 Pent = 5 Hex = 6 Hept = 7 Oct = 8 Non = 9 Dec = 10 Undec = 11 Dodec = 12
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Gold Foil Experiment Rutherford discovered the nucleus
Rutherford was investigating the behavior of alpha particles
However his discovery changed our notions of the structure of the atom
Gold Foil Experiment Rutherford is also credited by some with
discovering the proton as well
James Chadwich discovered the neutron in 1932
Actually the gold foil experiments were carried out by Geiger who worked in Rutherfordrsquos lab
Section 5 Mass number Atomic Number Average Atomic Mass Isotopes Calculating Average Atomic Mass
Isotope notation
A fresh look at atomic theory in light of about 100 years of new discoveries
The Periodic Table Big Fat Review at the table in the back
Section 7 review of bonding Ionic compounds (metal
cationnonmetal anion or polyatomic ion)
Criss Cross Simplify if necessary Name by naming ions
Metal = same as element Nonmetal = root of word + -ide suffix Polyatomic = name of polyatomic ion
Coulombrsquos Law Energy = k q1 x q2 distance
k is a constant q are charges of the two ions Distance is the distance between the two nuclei
Increase in charges means more energy in the bond So MgO has more than NaCl
Decrease in distance means more energy So NaCl has more than RbI because the ions are
smaller and therefore can get closer to one another
Know Common Charges Monatomic ions (consult the periodic table)
Polyatomic ions pretty much have to memorize (pg 68)
Remember that ammonia (NH4+1) is the only
polyatomic cation
Remember ldquoateiterdquo rule
Know Common Charges Transition metals have multiple charges (also called
oxidation numbers or oxidation states)
Cr is +2 +3 or +6 Cr+2 is chromous or chromium (II) Cr+3 is chromic or chromium (III) Cr+6 is chromium (VI)
Remember that a polyatomic ion is a group of ions (bonded covalently to each other) and the overall group has an ionic charge
Hydrates Means that water is ldquotied uprdquo as a part
of the crystal structure
CuSO4 5 H2O is copper (II) sulfate pentahydrate That is the correct name If you heat it and drive off the water
(which ought to be there) we then say that we have anhydrous copper(II) sulfate
Covalent compounds Two nonmetals bonded together Use prefixes in the name (Table 26 on pg
69) NO2 is nitrogen dioxide (no mono prefix is
needed if itrsquos the first element) You name both elements but add ndashide to the root of the second element
N2O is dinitrogen monoxide (if mono is for the second element you must use it)
Acids Look at the anion the H is bonded to Remember H in front of the formula = acid HCl (bonded to chloride a monatomic ion)
Name is hydrochloric acid Hydro prefix -ic suffix and add acid
HNO2 (bonded to nitrite so ndashite) Name is nitrous acid Use the root of the anion add ndashous suffix and acid
HNO3 (bonded to nitrate so ndashate) Name is nitric acid Use the root of the anion add ndashic suffix and acid
Simple Organic Compounds New from Last Year
Prefixes Meth = 1 carbon Eth = 2 carbons Prop = 3 But = 4 Pent = 5 Hex = 6 Hept = 7 Oct = 8 Non = 9 Dec = 10 Undec = 11 Dodec = 12
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Gold Foil Experiment Rutherford is also credited by some with
discovering the proton as well
James Chadwich discovered the neutron in 1932
Actually the gold foil experiments were carried out by Geiger who worked in Rutherfordrsquos lab
Section 5 Mass number Atomic Number Average Atomic Mass Isotopes Calculating Average Atomic Mass
Isotope notation
A fresh look at atomic theory in light of about 100 years of new discoveries
The Periodic Table Big Fat Review at the table in the back
Section 7 review of bonding Ionic compounds (metal
cationnonmetal anion or polyatomic ion)
Criss Cross Simplify if necessary Name by naming ions
Metal = same as element Nonmetal = root of word + -ide suffix Polyatomic = name of polyatomic ion
Coulombrsquos Law Energy = k q1 x q2 distance
k is a constant q are charges of the two ions Distance is the distance between the two nuclei
Increase in charges means more energy in the bond So MgO has more than NaCl
Decrease in distance means more energy So NaCl has more than RbI because the ions are
smaller and therefore can get closer to one another
Know Common Charges Monatomic ions (consult the periodic table)
Polyatomic ions pretty much have to memorize (pg 68)
Remember that ammonia (NH4+1) is the only
polyatomic cation
Remember ldquoateiterdquo rule
Know Common Charges Transition metals have multiple charges (also called
oxidation numbers or oxidation states)
Cr is +2 +3 or +6 Cr+2 is chromous or chromium (II) Cr+3 is chromic or chromium (III) Cr+6 is chromium (VI)
Remember that a polyatomic ion is a group of ions (bonded covalently to each other) and the overall group has an ionic charge
Hydrates Means that water is ldquotied uprdquo as a part
of the crystal structure
CuSO4 5 H2O is copper (II) sulfate pentahydrate That is the correct name If you heat it and drive off the water
(which ought to be there) we then say that we have anhydrous copper(II) sulfate
Covalent compounds Two nonmetals bonded together Use prefixes in the name (Table 26 on pg
69) NO2 is nitrogen dioxide (no mono prefix is
needed if itrsquos the first element) You name both elements but add ndashide to the root of the second element
N2O is dinitrogen monoxide (if mono is for the second element you must use it)
Acids Look at the anion the H is bonded to Remember H in front of the formula = acid HCl (bonded to chloride a monatomic ion)
Name is hydrochloric acid Hydro prefix -ic suffix and add acid
HNO2 (bonded to nitrite so ndashite) Name is nitrous acid Use the root of the anion add ndashous suffix and acid
HNO3 (bonded to nitrate so ndashate) Name is nitric acid Use the root of the anion add ndashic suffix and acid
Simple Organic Compounds New from Last Year
Prefixes Meth = 1 carbon Eth = 2 carbons Prop = 3 But = 4 Pent = 5 Hex = 6 Hept = 7 Oct = 8 Non = 9 Dec = 10 Undec = 11 Dodec = 12
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Section 5 Mass number Atomic Number Average Atomic Mass Isotopes Calculating Average Atomic Mass
Isotope notation
A fresh look at atomic theory in light of about 100 years of new discoveries
The Periodic Table Big Fat Review at the table in the back
Section 7 review of bonding Ionic compounds (metal
cationnonmetal anion or polyatomic ion)
Criss Cross Simplify if necessary Name by naming ions
Metal = same as element Nonmetal = root of word + -ide suffix Polyatomic = name of polyatomic ion
Coulombrsquos Law Energy = k q1 x q2 distance
k is a constant q are charges of the two ions Distance is the distance between the two nuclei
Increase in charges means more energy in the bond So MgO has more than NaCl
Decrease in distance means more energy So NaCl has more than RbI because the ions are
smaller and therefore can get closer to one another
Know Common Charges Monatomic ions (consult the periodic table)
Polyatomic ions pretty much have to memorize (pg 68)
Remember that ammonia (NH4+1) is the only
polyatomic cation
Remember ldquoateiterdquo rule
Know Common Charges Transition metals have multiple charges (also called
oxidation numbers or oxidation states)
Cr is +2 +3 or +6 Cr+2 is chromous or chromium (II) Cr+3 is chromic or chromium (III) Cr+6 is chromium (VI)
Remember that a polyatomic ion is a group of ions (bonded covalently to each other) and the overall group has an ionic charge
Hydrates Means that water is ldquotied uprdquo as a part
of the crystal structure
CuSO4 5 H2O is copper (II) sulfate pentahydrate That is the correct name If you heat it and drive off the water
(which ought to be there) we then say that we have anhydrous copper(II) sulfate
Covalent compounds Two nonmetals bonded together Use prefixes in the name (Table 26 on pg
69) NO2 is nitrogen dioxide (no mono prefix is
needed if itrsquos the first element) You name both elements but add ndashide to the root of the second element
N2O is dinitrogen monoxide (if mono is for the second element you must use it)
Acids Look at the anion the H is bonded to Remember H in front of the formula = acid HCl (bonded to chloride a monatomic ion)
Name is hydrochloric acid Hydro prefix -ic suffix and add acid
HNO2 (bonded to nitrite so ndashite) Name is nitrous acid Use the root of the anion add ndashous suffix and acid
HNO3 (bonded to nitrate so ndashate) Name is nitric acid Use the root of the anion add ndashic suffix and acid
Simple Organic Compounds New from Last Year
Prefixes Meth = 1 carbon Eth = 2 carbons Prop = 3 But = 4 Pent = 5 Hex = 6 Hept = 7 Oct = 8 Non = 9 Dec = 10 Undec = 11 Dodec = 12
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
The Periodic Table Big Fat Review at the table in the back
Section 7 review of bonding Ionic compounds (metal
cationnonmetal anion or polyatomic ion)
Criss Cross Simplify if necessary Name by naming ions
Metal = same as element Nonmetal = root of word + -ide suffix Polyatomic = name of polyatomic ion
Coulombrsquos Law Energy = k q1 x q2 distance
k is a constant q are charges of the two ions Distance is the distance between the two nuclei
Increase in charges means more energy in the bond So MgO has more than NaCl
Decrease in distance means more energy So NaCl has more than RbI because the ions are
smaller and therefore can get closer to one another
Know Common Charges Monatomic ions (consult the periodic table)
Polyatomic ions pretty much have to memorize (pg 68)
Remember that ammonia (NH4+1) is the only
polyatomic cation
Remember ldquoateiterdquo rule
Know Common Charges Transition metals have multiple charges (also called
oxidation numbers or oxidation states)
Cr is +2 +3 or +6 Cr+2 is chromous or chromium (II) Cr+3 is chromic or chromium (III) Cr+6 is chromium (VI)
Remember that a polyatomic ion is a group of ions (bonded covalently to each other) and the overall group has an ionic charge
Hydrates Means that water is ldquotied uprdquo as a part
of the crystal structure
CuSO4 5 H2O is copper (II) sulfate pentahydrate That is the correct name If you heat it and drive off the water
(which ought to be there) we then say that we have anhydrous copper(II) sulfate
Covalent compounds Two nonmetals bonded together Use prefixes in the name (Table 26 on pg
69) NO2 is nitrogen dioxide (no mono prefix is
needed if itrsquos the first element) You name both elements but add ndashide to the root of the second element
N2O is dinitrogen monoxide (if mono is for the second element you must use it)
Acids Look at the anion the H is bonded to Remember H in front of the formula = acid HCl (bonded to chloride a monatomic ion)
Name is hydrochloric acid Hydro prefix -ic suffix and add acid
HNO2 (bonded to nitrite so ndashite) Name is nitrous acid Use the root of the anion add ndashous suffix and acid
HNO3 (bonded to nitrate so ndashate) Name is nitric acid Use the root of the anion add ndashic suffix and acid
Simple Organic Compounds New from Last Year
Prefixes Meth = 1 carbon Eth = 2 carbons Prop = 3 But = 4 Pent = 5 Hex = 6 Hept = 7 Oct = 8 Non = 9 Dec = 10 Undec = 11 Dodec = 12
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Section 7 review of bonding Ionic compounds (metal
cationnonmetal anion or polyatomic ion)
Criss Cross Simplify if necessary Name by naming ions
Metal = same as element Nonmetal = root of word + -ide suffix Polyatomic = name of polyatomic ion
Coulombrsquos Law Energy = k q1 x q2 distance
k is a constant q are charges of the two ions Distance is the distance between the two nuclei
Increase in charges means more energy in the bond So MgO has more than NaCl
Decrease in distance means more energy So NaCl has more than RbI because the ions are
smaller and therefore can get closer to one another
Know Common Charges Monatomic ions (consult the periodic table)
Polyatomic ions pretty much have to memorize (pg 68)
Remember that ammonia (NH4+1) is the only
polyatomic cation
Remember ldquoateiterdquo rule
Know Common Charges Transition metals have multiple charges (also called
oxidation numbers or oxidation states)
Cr is +2 +3 or +6 Cr+2 is chromous or chromium (II) Cr+3 is chromic or chromium (III) Cr+6 is chromium (VI)
Remember that a polyatomic ion is a group of ions (bonded covalently to each other) and the overall group has an ionic charge
Hydrates Means that water is ldquotied uprdquo as a part
of the crystal structure
CuSO4 5 H2O is copper (II) sulfate pentahydrate That is the correct name If you heat it and drive off the water
(which ought to be there) we then say that we have anhydrous copper(II) sulfate
Covalent compounds Two nonmetals bonded together Use prefixes in the name (Table 26 on pg
69) NO2 is nitrogen dioxide (no mono prefix is
needed if itrsquos the first element) You name both elements but add ndashide to the root of the second element
N2O is dinitrogen monoxide (if mono is for the second element you must use it)
Acids Look at the anion the H is bonded to Remember H in front of the formula = acid HCl (bonded to chloride a monatomic ion)
Name is hydrochloric acid Hydro prefix -ic suffix and add acid
HNO2 (bonded to nitrite so ndashite) Name is nitrous acid Use the root of the anion add ndashous suffix and acid
HNO3 (bonded to nitrate so ndashate) Name is nitric acid Use the root of the anion add ndashic suffix and acid
Simple Organic Compounds New from Last Year
Prefixes Meth = 1 carbon Eth = 2 carbons Prop = 3 But = 4 Pent = 5 Hex = 6 Hept = 7 Oct = 8 Non = 9 Dec = 10 Undec = 11 Dodec = 12
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Coulombrsquos Law Energy = k q1 x q2 distance
k is a constant q are charges of the two ions Distance is the distance between the two nuclei
Increase in charges means more energy in the bond So MgO has more than NaCl
Decrease in distance means more energy So NaCl has more than RbI because the ions are
smaller and therefore can get closer to one another
Know Common Charges Monatomic ions (consult the periodic table)
Polyatomic ions pretty much have to memorize (pg 68)
Remember that ammonia (NH4+1) is the only
polyatomic cation
Remember ldquoateiterdquo rule
Know Common Charges Transition metals have multiple charges (also called
oxidation numbers or oxidation states)
Cr is +2 +3 or +6 Cr+2 is chromous or chromium (II) Cr+3 is chromic or chromium (III) Cr+6 is chromium (VI)
Remember that a polyatomic ion is a group of ions (bonded covalently to each other) and the overall group has an ionic charge
Hydrates Means that water is ldquotied uprdquo as a part
of the crystal structure
CuSO4 5 H2O is copper (II) sulfate pentahydrate That is the correct name If you heat it and drive off the water
(which ought to be there) we then say that we have anhydrous copper(II) sulfate
Covalent compounds Two nonmetals bonded together Use prefixes in the name (Table 26 on pg
69) NO2 is nitrogen dioxide (no mono prefix is
needed if itrsquos the first element) You name both elements but add ndashide to the root of the second element
N2O is dinitrogen monoxide (if mono is for the second element you must use it)
Acids Look at the anion the H is bonded to Remember H in front of the formula = acid HCl (bonded to chloride a monatomic ion)
Name is hydrochloric acid Hydro prefix -ic suffix and add acid
HNO2 (bonded to nitrite so ndashite) Name is nitrous acid Use the root of the anion add ndashous suffix and acid
HNO3 (bonded to nitrate so ndashate) Name is nitric acid Use the root of the anion add ndashic suffix and acid
Simple Organic Compounds New from Last Year
Prefixes Meth = 1 carbon Eth = 2 carbons Prop = 3 But = 4 Pent = 5 Hex = 6 Hept = 7 Oct = 8 Non = 9 Dec = 10 Undec = 11 Dodec = 12
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Know Common Charges Monatomic ions (consult the periodic table)
Polyatomic ions pretty much have to memorize (pg 68)
Remember that ammonia (NH4+1) is the only
polyatomic cation
Remember ldquoateiterdquo rule
Know Common Charges Transition metals have multiple charges (also called
oxidation numbers or oxidation states)
Cr is +2 +3 or +6 Cr+2 is chromous or chromium (II) Cr+3 is chromic or chromium (III) Cr+6 is chromium (VI)
Remember that a polyatomic ion is a group of ions (bonded covalently to each other) and the overall group has an ionic charge
Hydrates Means that water is ldquotied uprdquo as a part
of the crystal structure
CuSO4 5 H2O is copper (II) sulfate pentahydrate That is the correct name If you heat it and drive off the water
(which ought to be there) we then say that we have anhydrous copper(II) sulfate
Covalent compounds Two nonmetals bonded together Use prefixes in the name (Table 26 on pg
69) NO2 is nitrogen dioxide (no mono prefix is
needed if itrsquos the first element) You name both elements but add ndashide to the root of the second element
N2O is dinitrogen monoxide (if mono is for the second element you must use it)
Acids Look at the anion the H is bonded to Remember H in front of the formula = acid HCl (bonded to chloride a monatomic ion)
Name is hydrochloric acid Hydro prefix -ic suffix and add acid
HNO2 (bonded to nitrite so ndashite) Name is nitrous acid Use the root of the anion add ndashous suffix and acid
HNO3 (bonded to nitrate so ndashate) Name is nitric acid Use the root of the anion add ndashic suffix and acid
Simple Organic Compounds New from Last Year
Prefixes Meth = 1 carbon Eth = 2 carbons Prop = 3 But = 4 Pent = 5 Hex = 6 Hept = 7 Oct = 8 Non = 9 Dec = 10 Undec = 11 Dodec = 12
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Know Common Charges Transition metals have multiple charges (also called
oxidation numbers or oxidation states)
Cr is +2 +3 or +6 Cr+2 is chromous or chromium (II) Cr+3 is chromic or chromium (III) Cr+6 is chromium (VI)
Remember that a polyatomic ion is a group of ions (bonded covalently to each other) and the overall group has an ionic charge
Hydrates Means that water is ldquotied uprdquo as a part
of the crystal structure
CuSO4 5 H2O is copper (II) sulfate pentahydrate That is the correct name If you heat it and drive off the water
(which ought to be there) we then say that we have anhydrous copper(II) sulfate
Covalent compounds Two nonmetals bonded together Use prefixes in the name (Table 26 on pg
69) NO2 is nitrogen dioxide (no mono prefix is
needed if itrsquos the first element) You name both elements but add ndashide to the root of the second element
N2O is dinitrogen monoxide (if mono is for the second element you must use it)
Acids Look at the anion the H is bonded to Remember H in front of the formula = acid HCl (bonded to chloride a monatomic ion)
Name is hydrochloric acid Hydro prefix -ic suffix and add acid
HNO2 (bonded to nitrite so ndashite) Name is nitrous acid Use the root of the anion add ndashous suffix and acid
HNO3 (bonded to nitrate so ndashate) Name is nitric acid Use the root of the anion add ndashic suffix and acid
Simple Organic Compounds New from Last Year
Prefixes Meth = 1 carbon Eth = 2 carbons Prop = 3 But = 4 Pent = 5 Hex = 6 Hept = 7 Oct = 8 Non = 9 Dec = 10 Undec = 11 Dodec = 12
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Hydrates Means that water is ldquotied uprdquo as a part
of the crystal structure
CuSO4 5 H2O is copper (II) sulfate pentahydrate That is the correct name If you heat it and drive off the water
(which ought to be there) we then say that we have anhydrous copper(II) sulfate
Covalent compounds Two nonmetals bonded together Use prefixes in the name (Table 26 on pg
69) NO2 is nitrogen dioxide (no mono prefix is
needed if itrsquos the first element) You name both elements but add ndashide to the root of the second element
N2O is dinitrogen monoxide (if mono is for the second element you must use it)
Acids Look at the anion the H is bonded to Remember H in front of the formula = acid HCl (bonded to chloride a monatomic ion)
Name is hydrochloric acid Hydro prefix -ic suffix and add acid
HNO2 (bonded to nitrite so ndashite) Name is nitrous acid Use the root of the anion add ndashous suffix and acid
HNO3 (bonded to nitrate so ndashate) Name is nitric acid Use the root of the anion add ndashic suffix and acid
Simple Organic Compounds New from Last Year
Prefixes Meth = 1 carbon Eth = 2 carbons Prop = 3 But = 4 Pent = 5 Hex = 6 Hept = 7 Oct = 8 Non = 9 Dec = 10 Undec = 11 Dodec = 12
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Covalent compounds Two nonmetals bonded together Use prefixes in the name (Table 26 on pg
69) NO2 is nitrogen dioxide (no mono prefix is
needed if itrsquos the first element) You name both elements but add ndashide to the root of the second element
N2O is dinitrogen monoxide (if mono is for the second element you must use it)
Acids Look at the anion the H is bonded to Remember H in front of the formula = acid HCl (bonded to chloride a monatomic ion)
Name is hydrochloric acid Hydro prefix -ic suffix and add acid
HNO2 (bonded to nitrite so ndashite) Name is nitrous acid Use the root of the anion add ndashous suffix and acid
HNO3 (bonded to nitrate so ndashate) Name is nitric acid Use the root of the anion add ndashic suffix and acid
Simple Organic Compounds New from Last Year
Prefixes Meth = 1 carbon Eth = 2 carbons Prop = 3 But = 4 Pent = 5 Hex = 6 Hept = 7 Oct = 8 Non = 9 Dec = 10 Undec = 11 Dodec = 12
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Acids Look at the anion the H is bonded to Remember H in front of the formula = acid HCl (bonded to chloride a monatomic ion)
Name is hydrochloric acid Hydro prefix -ic suffix and add acid
HNO2 (bonded to nitrite so ndashite) Name is nitrous acid Use the root of the anion add ndashous suffix and acid
HNO3 (bonded to nitrate so ndashate) Name is nitric acid Use the root of the anion add ndashic suffix and acid
Simple Organic Compounds New from Last Year
Prefixes Meth = 1 carbon Eth = 2 carbons Prop = 3 But = 4 Pent = 5 Hex = 6 Hept = 7 Oct = 8 Non = 9 Dec = 10 Undec = 11 Dodec = 12
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Simple Organic Compounds New from Last Year
Prefixes Meth = 1 carbon Eth = 2 carbons Prop = 3 But = 4 Pent = 5 Hex = 6 Hept = 7 Oct = 8 Non = 9 Dec = 10 Undec = 11 Dodec = 12
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Types of Hydrocarbons Alkanesmdashall C-C single bonds
Ends in -ane Alkenesmdashcontains at least 1 C-C double bond
Ends in -ene Alkynesmdashcontains at least 1 C-C triple bond
Ends in -yne
1 lt 2 lt 3 and a lt e lt y
Aromaticmdashcontains at least 1 benzene ring
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
To Namehellip Find the longest continuous carbon chain Determine what type of hydrocarbon it is for
the suffix Number the chain so that any substituents
(things attached to the chain) have the lowest possible numbers
Keep adding prefixes to the front of the name until everything has been named Use numbers to specify WHICH carbon the substituent is attached to
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Sound complicatedhellip Itrsquos not Organic naming is very fun but it can get
pretty hairy There are millions of different organic compounds
so we had to come up with some way to classify everything
We do this by a concept called ldquofunctional grouprdquo A functional group always reacts the same no
matter WHAT ELSE is attached to it We use R- to represent some ldquorandom organic
fragmentrdquo which is attached to the functional group but which we really donrsquot care about right now
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Draw the structure 2 2-dichlorobutane
2 3-dimethyl propane
2-pentene (2 specifies the position of the double bond)
Cyclohexane
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Mixtures Heterogeneous Homogeneous = solutions
Solutions are very important this year ALL over the AP exam
Review physical separation techniques especially distillation and chromatography TLC = thin layer chromatography GC = gas chromatography HPLC = high pressure liquid chromatography
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Mass Spectrometry = Mass Spec
Used to determine masses of elements or compound very accurately Used a lot in organic chemistry
Compounds sometimes break into fragments especially larger organic molecules Analyzing the possible fragments gives you
insight into the overall structure of the molecule Itrsquos like putting together a puzzle
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Mass Spectrometry = Mass Spec
Basically the sample is ionized by bombarding it with high energy electrons
An electron is pried off and we now have a cation Same mass but it now has charge (remember an electron has no mass) But the fact that it is charged now is very useful
The charged particles are passed through an electric field (which accelerates them) and a series of slits (which focuses the beam of ions) Although they have the same energy since they have
different masses they are moving at slightly different speeds This causes them to begin to separate themselves by mass
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Mass Spectrometry = Mass Spec
The charged particles are then passed through a magnetic field which attracts the particles Lighter particles move closer to the source heavier particles
not so much They continue to separate by mass They literally separate
into separate streams of ions each one with a different mass They then hit a detector which records where they hit and
the relative amount that hit each spot The relative amounts are an indication of abundance Where they hit is then compared to known substances with
known mass that hits those same spots Using this information you can determine the mass of your
sample and the relative abundances very accurately
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
Molar Mass Simply add up the masses of each element in the
formula multiplying by any subscripts if necessary
For example Al2(SO4)3 has 2 Aluminum atoms 3 Sulfur atoms 12 Oxygen atoms MM = 34218 amu or g
Amu if we are talking about 1 atom or molecule Grams if we are talking about 1 mole of atoms or
molecules
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
The End See you in Chapter 3 on Weds
Quiz on Weds over Naming and Writing Formulas
