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Science 10 – Chemistry Notes Name: _________________

What is Chemistry? Chemistry is the science in which substances are examined to find out:

- What things are made of

- How they act under different conditions

- How they are combined or separated to form other substances.

Essentially, chemistry is the study of ___matter____.

Matter:

- anything that has ____mass______ and takes up ____space____.

- Is the make up of the entire universe.

- Is made up of atoms and elements.

Periodic Table of the Elements

Metals: Found to the __left__ of the “ladder”. Generally

shiny ___solids__ at room temperature and

___good____ conductors of heat and electricity.

Non-Metals: Found to the ___right__ of the “ladder”.

Exist in all three states of matter, __dull__, and

___poor__ conductors.

Metalloids: Found along ___both sides____ of the

ladder. Have properties of ___both___ metals and non-

metals.

Horizontal rows are called ____periods____.

Vertical columns are called ___groups____ or ____families_____.

Periodic Table Analogy Lab

How to Read the Periodic Table:

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Anatomy of an Atom Element: A __pure___ substance that ___cannot___ be broken down into a simpler

substance (made up of ___the same__ kind of atom).

Atom: the basic unit of an __element (of matter)___.

Let’s determine which element this is:

How many electrons? ______6__

How many valence electrons? ___4______

How many protons? ______6______________

How many neutrons? _____6______________

Atomic number = number of protons = ___6_____

Atomic mass = # protons + # neutrons = ___12_

Element Symbol Atomic

#

Atomic

Mass

Protons

p+

Neutrons

n0

Electrons

e-

Cesium

Cs 55 133 55

133-55

=78 55

Selenium

Se 34 79 34

79-34

= 45 34

Bromine

Br 35 80 35

80-35

= 45 35

Assignment: How to Count Protons, Neutrons and Electrons

Bohr Diagrams of Atoms Neils Bohr developed a theory to identify where ___electrons__ are found around the

nucleus (Hotel Analogy)

e- surround the nucleus in __orbits__/ __rings__/__energy levels_

1st Ring can hold max _2_ e- 2nd Ring can hold max _8_e- 3rd Ring can hold max _8_e-

Ex) Na atom (__11__ e-) ex) Sulfur atom (__16__ e-)

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Assignment: Bohr Diagram Periodic Table Worksheet

How Atoms Become Stable (p+≠ e-)

Electrons in the outermost ring are called ___valence electrons____

When outermost shell is full, element is __stable__

Atoms may gain or lose __ELECTRONS__ in order to get a full valence shell, thus becoming

____IONS__ (charged particles).

Ex) Sodium atom Outer shell has __1_ electron Sodium ION

Na1+

P+ = 11 e- = 11 p+ = 11 e- = 10

Ex) Fluoride atom Outer shell has __9_ electron Fluoride ION

F1-

P+ = 9 e- = 9 P+ = 9 e- = 10

Group Valence e- Lose or Gain

1 1 lose 1 gain 7

2 2 lose 2 gain 6

3/13 3 lose 3 gain 5

4/14 4 lose 4 gain 4

5/15 5 lose 5 gain 3

6/16 6 lose 6 gain 2

7/17 7 lose 7 gain 1

8/18 8 lose 8 gain 0

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Fill in the chart for the following:

Atom Bohr diagram for

atom

Bohr diagram for

stable ion

Gained/lost

electrons

Formula of

ION that is

formed

Same number of

electrons as what

Noble Gas?

a) Lithium

lose __1 e-___

gain _____

Li 1+

He

b) Nitrogen

lose ______

gain _3 e-_

N3-

Ne

Assignment: Atom/Ion Worksheet

- Only ____ELECTRONS__ can be gained or lost from an atom.

o The atomic number is different for every element on the periodic table of the

elements. It is characteristic for that element. You ___CANNOT____ change the

number of protons! If you change the number of protons, you change the atomic

number, and you have a different element!!

- If an atom loses an electron, it becomes a positive ion (__caTion__)

- If an atom gains an electron, it becomes a negative ion (__aNion__)

Determining p+, n0, e- of Ions

Ions ≠ Neutral # ____ p+___ ≠ # __e-___

Ex) Li1+ atomic # = p+= no = e- =

Ca2+ O2- S2- Cl1-

p+ 20 8 16 17

no 20 8 16 18

e- 18 10 18 18

Assignment: Determining Protons, Neutrons, and Electrons for Ions

Gold Penny Lab

In-Class Assignment: p+, n0, e- for atoms/ions; Bohr diagrams for atoms/ions,

gained/lost electrons, ion that’s formed, same Bohr diagram as what atom?

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How Elements Form Compounds In order for atoms to have a stable valence shell, they will link up with other atoms by ___gaining__, giving up or

____sharing__ electrons. This is how elements combine to form compounds.

There are two major types of compounds that can form between atoms:

1. Ionic Compounds: where ____metals___________ bond with ___non-metals_____.

2. Covalent Compounds: where ____non-metals____ bond with other __non-metals__.

1. Ionic Compounds Ex) Sodium + Chlorine Here we see that sodium (___metal__) will give its valence

electron to chlorine (__non-metal___) so that they both have

stable shells.

Once this happens, the ionic charge of sodium will be _Na1+_

and the ionic charge of chlorine will be _Cl1-_.

These two opposing charges will attract each other and a

chemical bond will be formed creating the compound __sodium

chloride (NaCl)___.

Sometimes, more than one electron can be transferred.

Ex) Calcium + Oxygen

This compound’s name is ____calcium oxide_____.

Sometimes more than one atom of each element will have to be involved.

Ex) Calcium + Chlorine

This compound’s name is ___calcium chloride___.

Assignment: Making Simple Ionic Compounds

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2. Simple Ionic Compounds (M + NM)

a) Writing Formulas (Ions→ formula)

Writing Formulas for Ionic Compounds

Look up the Symbol and Charge

left-hand side right hand side

metal and non-metal (or polyatomic)

Figure out how many of each element you need to make sure your charges cancel out

THE CHARGES GO AWAY BECAUSE YOUR PLUSES CANCEL YOUR MINUSES!!!!

ionic formula ionic formula

left-hand side right hand side left-hand side right hand side

sodium phosphide magnesium sulfide

Na1+ P3- I need 3 Na1+ Mg2+ S2- I need 1 Mg2+

Na1+ to cancel out P3- to cancel out 1

Na1+ Na3P S2-

MgS

Given the name, write the formula

Potassium bromide____KBr____

Aluminum chloride____AlCl3______

Calcium phosphide ___Ca3P2_____

Lithium nitride____Li3N_______

Potassium selenide ___K2Se____

b) Naming Simple Ionic Compounds ( M + NM) Formula → Name

ionic naming ionic naming

Na3P CaI2

left-hand side right hand side left-hand side right hand side

sodium phosphide calcium iodide

Ex) NaCl K2O CaF2

BaS2 Na3N Li3As

Assignment:

Naming Ionic

Compounds and

Writing Ionic

Formulas

Worksheet

sodium chloride potassium oxide

chloride

calcium fluoride

chloride

barium sulfide sodium nitride

chloride

lithium astetide

chloride

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3. Transition Metal Ionic Compounds (M + NM)

a) Writing Formulas (Name Formula)

Copper (II) sulfide _____CuS_______

Copper (I) sulfide ____Cu2S__________

iron (III) oxide _____Fe2O3_________

mercury (II) phosphide ______Hg3P2______

b) Naming (Formula Name)

MnCl2 Cu3N2

left-hand side right hand side left-hand side right hand side

manganese (II)? chloride copper (I)? nitride

OR manganese (III)? chloride OR copper (II)? nitride

Mn? Cl1- 2 minuses Cu? N3-

Cl1- Cu? N3-

Cu?

therefore must be Mn+2 so 1 Mn cancels therefore must be Cu+2 so 3 Cu cancels

with 2 Cl1- with 2 N3-

manganese (II) chloride copper (II) nitride

PbO ______lead (II) oxide__________ PbO2 ________lead (IV) oxide___________

CoS _____cobalt (II) sulfide_______ Co2S3 _____cobalt (III) sulfide_______

Assignment: Ionic Compounds: Metals with More than one Charge

4. Polyatomic Compounds

a) Writing Formulas (Name Formula)

ionic formula ionic formula

left-hand side right hand side left-hand side right hand side

sodium iodate gold (III) nitrate

Na1+ IO3- I need 1 Na1+ Au3+ NO3

1- I need 1 Au3+

to cancel out 1 IO3- NO3

1- to cancel out 3

NaIO3 NO3 1- NO3

3-

Au(NO3)

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sodium chlorite

barium nitrate

magnesium carbonate

calcium hydroxide

b) Naming (Formula Name)

Na3PO4 Ca(OH)2

left-hand side right hand side left-hand side right hand side

sodium phosphate calcium hydroxide

Name the following compounds:

Na2SO4 Al(ClO3)3 NH4NO3 Rb2HSO3

Assignment: Making Polyatomic Ionic Compounds Using Models Activity

Assignment: Polyatomic Compounds Names and Formulas Worksheet

5. Acids Are covalent compounds (electrons are SHARED) that give off hydrogen ions when dissolved in

water.

They ALWAYS start with H+ bonded to some negative ion (either a non-metal or a polyatomic ion).

There are three kinds of acids:

o Hydrogen bonding with an –ate ions

o Hydrogen bonding with an –ite ions

o Hydrogen bonding with an –ide ions

a) Writing Names (formula name) Naming Acids

If the anion ends in –ate, it is called ________ic acid

Ex) Hydrogen Nitrate, HNO3 ____nitric_____ acid

If the anion ends in –ite, it is called ________ous acid

Ex) Hydrogen Nitrite, HNO2 ____nitrous____ acid

If the anion ends in –ide, it is called hydro______ic acid

Ex) Hydrogen Chloride, HCl __hydrochloric_ acid

H+ and a polyatomic

H+ and a non-metal

(most of the

time…exceptions are

OH-, CN-)

sodium sulfate Aluminum chlorate

chloride

Ammonium nitrate

nitrate

astetide

chloride

rubidium hydrogen sulfite OR

rubidium bisulfite

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Practice: name the following acids.

1. HI _________________________ 4. H3P

2.

3.

Acid

Starts with H Ends with

-ide -ate -ite

(one symbol after the H)

hydro________ic acid __________ic acid __________ous acid

H2S H3BO3 H2CrO3

hydrogen selenide hydrogen borate hydrogen chromite

hydroselenic acid boric acid chromous acid

-IDE acids If there is only one symbol after the H, write “hydro”, then take the element’s name

and change the ending to “ic”. Ex) H2Se = hydroselenic acid

-ATE acids change the “ate” to say “ic” and say “acid”. Ex) H3BO3… BO3 is called borate. So call

this boric acid.

–ITE change the “ite” to say “ous” and say “acid”. Ex) H2CrO3… CrO3 is called chromite. So call

this chromous acid

b) Writing Formulas (name formula)

Use the same criss-cross method as with ionic compounds. H1+ will ALWAYS be at the

start of your criss-cross.

Writing Formulas for Acids hydro________ic acid ___________ic acid _______________ous acid

hydronitric acid nitric acid nitrous acid

hydrogen nitride hydrogen nitrate hydrogen nitrite

H1+ N3- I need 3 H1+ H1+ NO31- I need 1 H+1 H1+ NO2

1- I need 1H+

H1+ to cancel out to cancel out to cancel

H1+ N3- NO31- NO2

1-

H3N HNO3 HNO2

Examples:

Hydrosulfuric acid (H1+ and ) _________________

Carbonic acid (H1+ and ) _______________

Nitrous acid (H1+ and ) _______________

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Practice: write the formula for the following acids

1. chromic acid ____H2CrO4__

2. sulfurous acid____H2SO3_____

3. carbonous acid ____H2CO2____

4. hydrocyanic acid___HCN___

5. hydrochloric acid __HCl__

6. oxalic acid _____H2C2O4______

7. sulfuric acid ____H2SO4__________

8. chlorous acid _____HClO2_______

9. hydrosulfuric acid __H2S_____

10. boric acid ____H3BO3________

Assignment: Acids – Names and Formulas

Understanding Concepts

In your own words, explain what is meant by the term “polyatomic ion”. Give 2

examples.

many atoms with a charge – anything from the right hand side of the ion chart

11. Covalent (Molecular) Compounds (Non Metal/Non Metal)

Are formed when 2 NON-METALS bond

Here, electrons are SHARED, not transferred as they are in ionic compounds.

Naming: A prefix is used to indicate the number of each element in the compound. (The exception is we don’t use

mono- for the first element).

Charges are not of concern in covalent compounds.

Drop the ending of the second element and add –ide.

Examples: CCl4 carbon tetrachloride

N2O3 dinitrogen trioxide

Prefix Number

Mono- 1

Di- 2

Tri- 3

Tetra- 4

Penta- 5

Hexa- 6

Hepta- 7

Octa- 8

Nona- 9

Deca- 10

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Practice: Name the following covalent compounds. 1. PBr3 ________phosphorus tribromide_______

2. P2O3 ________diphosphorus trioxide_________

3. CF4 __________carbon tetrafluoride________

4. SO2 _______silicon dioxide________

5. N2O _______dinitrogen monoxide_______

Writing Formulas Completely ignore the charges of the non-metals!!!

The prefixes will tell you how many atoms of each element you need.

DO NOT reduce compounds to lowest form! Leave them as the name states.

Examples: Nitrogen trihydride NH3

Dinitrogen tetraoxide N2O4

Practice: Write the formulas for the following covalent compounds.

1. tetraphosphorus triselenide ____P4Se3_____

2. disilicon hexabromide ____Si2Br6_____

3. diarsenic trioxide ____As2O3_____

4. selenium monosulfide ____SeO____

5. carbon tetrabromide ____CBr4______

6. boron trifluoride ____BF3________

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Understanding Concepts

1. How can you tell the difference between an ionic compound and a molecular

compound?

ionic – something from the right hand side and the left hand side

covalent – two things from the right hand side

2. What kinds of atoms form molecular compounds?

two non-metals

3. How do the atoms in molecular compounds form stable electron arrangements?

In other words, what happens to the electrons?

Molecular compounds SHARE electrons

Assignment: Covalent (Molecular) Compounds: Names and Formula Worksheet

BONUS: Mixed Ionic and Covalent Compounds

IN-CLASS ASSIGNMENT #2: Naming and Writing Formulas for ionic, metals with more than one

charge, polyatomic ions, acids, covalent, and mixed naming

12. Hydrocarbons: Alkanes and Alkenes

a) Alkanes An alkane is a saturated hydrocarbon. In other words, an alkane is a long chain of carbon linked

together by single bonds.

The general formula for alkanes is CnH2n+2.

Formula Structure

The simplest alkane is methane

Formula Structure

o The next simplest is ethane

o The series continues indefinitely

**Each C must have 4 bonds **

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Naming Alkanes Naming alkanes is quite simple: just use prefixes counting the number of carbon atoms in the

formula and add the suffix –ane.

The prefixes are as follows:

Examples:

NAME: butane hexane

Alkanes can be symbolized in a few different ways:

Molecular Formula Expanded structural Formula Condensed structural Formula

Ex) propane

b) Alkenes Alkenes are unsaturated hydrocarbons which means their carbon structure contains double bonds.

The general formula for alkenes is CnH2n

The simplest alkene is ethene (C2H4)

Naming Alkenes Naming alkenes is generally the same as naming alkanes, but with the suffix -ene and a

number indicating which carbon the double-bonded is attached to in the chain.

You can number the carbons either left to right or right to left. You must pick whichever

way gives the carbon with the double bond the LOWEST possible number.

Ethene and propene do not require numbers, since there is no question as to where the

double-bonded carbon is in the structures.

Example: propene C3H6

Example: butene C4H8 can have the double bonded

carbon in two different places. NAME:

NAME:

**Give the double bond the lowest

number **

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Assignment: Simple Alkanes and Alkenes

Naming Alcohols

Alcohols are organic carbons similar to alkanes but one of the hydrogen’s is substituted with a

hydroxide group, OH.

Alcohols are named by replacing the final –e of the alkane with the suffix “–ol”.

The location of the hydroxyl group is indicated with a number. The chain is numbered to give the

alcohol functional group the lowest possible number.

Example)

NAME: methanol ethanol 3-propanol 1-propanol 2-propanol

Draw 2-pentanol and 3-pentanol

2-pentanol 3-pentanol

Assignment: Naming Alcohols

Practice Exam/Review

EXAM