Chemistry:

Chemistry:Atomic

Structureby Tim F. Rowbotham - modified in 2008 , 2011

Pre-Assessment Questions

• Ready your remote

Which of the following is the most accurate model of the structure of an atom?

0% 1. Tiny solid sphere2. Tiny solar system3. Spherical Cloud4. Chocolate chip cookie

Which of the following is not a particle found in an atom?

0% 1. Neutron2. Electron3. Proton4. Cathode

The Mass Number of an atom is the total number of what?

0% 1. Protons & Electron2. Protons & Neutrons3. Neutrons & Electrons4. Protons, Neutrons & Electrons

The Atomic Number of an atom is the total number of what in an atom?

0% 1. Protons2. Protons & Electrons3. Protons, Neutrons & Electrons4. Chemical Bonds

Which of the following has a negative charge?

0% 1. Proton2. Neutron3. Electron4. Positron

Atomic Structure Notes•PAGE 1

Chemistry:Atomic

StructureCreated in 2008 by Tim F. Rowbotham

Atomic History• Ancient Greeks thought there were only 4 elements: earth, air, fire, & water.

• All matter, they thought, included one or more of these elements.

Atomic History• Democritus (440 BC) was the first to challenge this idea.

• He thought that matter could eventually be divided up into its smallest piece. This piece he theorized, he called atomos, which means “indivisible.”

Atomic Theory• In 1802, John Dalton (a British school teacher) proposed an atomic theory, which included several ideas.

• Dalton’s Atomic Theory VIDEO CLIP

Dalton’s Atomic Theory

• Atoms are tiny, invisible spheres impossible to break.

• Atoms of different elements are different and have specific masses.

• Atoms can combine in exact ratios to form compounds.

Thompson’s Model

• In the late 1800s, JJ Thompson discovered that there were negatively charged particles which he called electrons. He pictured the atom as a ball of positive charge with negatively charged electrons floating in it.

• VIDEO CLIPS:• THOMSON ,

THOMSON feat Eminem

Rutherford’s Model

• In 1911, Ernest Rutherford determined that the center of the atom had a positive charge.

• This positively charged center was called the nucleus.

• RUTHERFORD• Rutherford Gold Foil Experiment - Backstage Science

Chadwick’s Discovery

• James Chadwick discovered that the nucleus also held particles with no charge, which he called neutrons.

• The positively charged particles in the nucleus were called protons.

The Bohr Model• Neils Bohr hypothesized that the atom was like a tiny solar system, with electrons circling the nucleus in well defined orbits like planets

• The speculated paths of the electrons were called orbitals, shells, or energy levels.

Modern Atomic Theory• It was later discovered that

electrons do not have well defined orbits, but rather move much more haphazardly.

• In fact, Heisenberg determined that we can not simultaneously know the location and velocity of an electron!!!

• Uncertainty principle 1• Uncertainty Principle 2• Schrodinger’s Cat – Big Bang Theory

Electron Cloud Model• However, each electron has certain regions where it is more likely to be found.

• The electron cloud describes the “blur” created from the more frequent movement of electrons through these regions.

Electron Cloud Model

• The electron cloud is a spherical cloud around the nucleus that shows were an electron is most likely to be.

• It is the most accurate model of an atom, but not the most useful.

Electron Cloud Model

The denser areas are where the electrons are MOST likely to be.Atomic Model Video Clip

Learning Checks• Ready your remote

0% 1. Spherical Cloud2. Tiny solid sphere3. Tiny solar system4. Chocolate chip cookie

Which scientist is considered the Father of Chemistry because of his atomic theory?

0% 1. J.J. Thomson2. Neils Bohr3. John Dalton4. James Chadwick

Learning Checks•Return your remote

• Read & Complete p.10 – 11 “Particles of Matter”

Review Questions•Ready your remote

Which part of Dalton’s Atomic theory was later found out to be incorrect?

0% 1. Atoms of different elements are different2. Atoms are tiny unbreakable spheres3. Atoms combine in specific ratios4. Different atoms have different masses

0% 1. Tiny solid sphere2. Tiny solar system3. Spherical Cloud4. Chocolate chip cookie

Subatomic Particles

• An atom consists of a positive core called a nucleus, which contains positive protons and neutral neutrons.

• This nucleus is surrounded by a cloud of negatively charged electrons.

The Charge of Atoms

• Alone, atoms are electrically neutral.

• This means that they have no OVERALL electric charge.

• The positive charge of an atom is exactly equal to its negative charge.

The Negative of Atoms

• The extremely rapid movement of electrons forms the cloud of negative charge outside an atom’s nucleus.

• Each electron has a charge of -1.

The Positive of Atoms

• The nucleus of an atom holds a positive charge due to the presence of protons.

• Each proton has a charge exactly opposite to that of an electron equaling +1.

The Nucleus of an Atom

• The nucleus of an atom contains the bulk of the mass of the atom.

• In it are positively charged protons and neutrons, which have NO charge.

Atomic Mass Unit• Because atoms are so small, we use a special unit of measurement called an atomic mass unit.

• An atomic mass unit is really equal to about 1.66 x 10-27 kg.

Masses of Subatomic Particles

• A Proton’s mass = 1 a.m.u.• A Neutron’s mass = 1 a.m.u.• A Electron’s mass = 0 a.m.u.*

*An electron has a mass of 1/1836th of a proton (which is relatively insignificant)

Charges of Subatomic Particles•A Proton’s charge = +1

•A Neutron’s charge = 0

•A Electron’s charge = -1

COMPLETE THIS TABLE

Sub-atomic Particle

Proton Neutron Electron

Charge

Location

COMPLETE THIS TABLESub-

atomic Particle

Proton Neutron Electron

Mass 1 amu 1 amu 0 amu

Charge +1 0 -1

Location nucleus nucleus electron cloud

Exit QuestionsReady your remote

0% 1. Tiny solid sphere2. Tiny solar system3. Spherical electron cloud4. Chocolate chip cookie

Which of the following has a positive charge?

0% 1. Proton2. Neutron3. Electron4. Beta particle

Which of the following has a mass of 1 amu?

0% 1. Proton2. Neutron3. Electron4. Proton & Neutron

Modern Atomic TheoryReturn your remoteAtom – Bill Nye VIDEO

Read & complete PACKET pages 12-13“What is Matter?”

Entrance Review Questions•Ready your remote

Which of the following has no considerable mass (effectively making it 0 amu?

Which subatomic particle has a negative charge?

0% 1. Proton2. Neutron3. Electron4. Positron

Which subatomic particle has a positive charge?

Which subatomic particle has no overall charge?

0% 1. Proton2. Neutron3. Electron4. Quark

Atomic Number• The atomic number is the number of protons in an atom.

• It is a unique property that identifies the element.

• (If it has a different number of protons it is a different element!!!)

Atomic Number• For example, an atom with 6 protons would be carbon.

• But if a proton could be knocked free, then it would become boron, because boron has 5 protons!!!

What is the atomic number of oxygen?(USE THE PERIODIC TABLE)

0% 1. 22. 83. 164. 24

How many protons does an oxygen atom have?

0% 1. 22. 83. 164. 24

What is the atomic number of calcium?

0% 1. 62. 173. 204. 40

How many protons are there in a calcium atom?

0% 1. 62. 173. 204. 40

How many protons are there in an argon atom?

0% 1. 182. 403. 484. 58

Mass Number• Since electrons have virtually no mass (1/1836th of a proton), the mass of an atom is determined by adding only the number of protons & neutrons and is called its mass number.

Mass Number• Mass Number is also referred to as Atomic Mass or Atomic Weight

• Mass # = # protons + # neutrons

• Model of the Atom video clip• Atomic Number & Mass Number

video clip

What is the mass # of an atom with 2 protons, 2 neutrons, & 2 electrons?

0% 1. 2 2. 4 3. 6 4. 8

0% 1. 3 2. 6 3. 7 4. 10

What is the atomic # of an atom with 3 protons, 4 neutrons, & 3 electrons?

0% 1. 3 2. 6 3. 7 4. 10

What type of atom would have 3 protons, 4 neutrons, & 3 electrons?

0% 1. Lithium2. Beryllium3. Nitrogen4. Neon

0% 1. 9 2. 10 3. 19 4. 28

What is the atomic # of an atom with 5 protons, 6 neutrons, & 5 electrons?

0% 1. 52. 63. 104. 11

Review Questions•Return your

remote• Complete PACKET p.15

– 16 “The Amazing Atom”

JOURNAL # 1: Half Sheet

Create a table showing the mass, charge, &

location of each subatomic particle.

Entrance QuestionsReturn your remoteGet in groups of 2 – 4

Get 1 Atom Poster & 1 bag of subatomic particles & 1 Atom Building worksheet per group

Atom Building4

MASS #

ATOMIC #

This is a short- hand way

chemists use to write down a

lot of info about an atom!!

ChemicalSymbol

Atom Building4

MASS # = neutrons + protons

ATOMIC # = protons= electrons, if neutral

We can also figure out the

number of protons

neutrons & electrons from

this info

Neutrons = MASS# – ATOMIC #

Atom Building4

M # = n + p =

A# = p = = e

Using the protons, neutrons, & electrons

provided, create a model of this helium atom.

(It has 2 protons, 2 neutrons, & 2

electrons.)RECORD THIS INFO ON YOUR

ATOM BUILDING WORKSHEET

n= M# – A# = 2

Atom Building1

Continue Atom Building with this

atom and record all the information on the Atom Building

work sheet

Atom Building9

Build this atom and record all the

information on the Atom Building work

Atom Building12

Atom Building19

Atom Building20

QuizNo Talking or Sharing

AnswersWhen you finish turn your

quiz face down on the desk wait quietly for further directions

You have 15 minutes

Atom BuildingPass in your QuizGet in groups from yesterday

Get 1 Atom Poster & 1 bag of subatomic particles & 1 Atom Building worksheet per group

Atom Building14

Atom Building24

Atom Building23

Atom Building• Don’t forget to clean up

your Atom Building Particles before you leave.• Complete pages 17 – 18

“Observing Atoms”

Entrance Questions

Ready your remote

0% 1. Tiny solid sphere2. Tiny solar system3. Spherical electron cloud4. Chocolate chip cookie

Which of the following has a positive charge?

How do you find the mass # of an atom?

0% 1. Protons2. Neutrons3. Protons + Neutrons4. Protons + Neutrons + Electrons

How do you find the atomic # of an atom?

0% 1. Protons2. Neutrons3. Protons + Neutrons4. Protons + Neutrons + Electrons

0% 1. 62. 12 3. 14 4. 20

Atoms Review• Half a sheet of paper with your

neighbor!• Draw and identify each of the

following atoms of elements, labeling properly the protons, neutrons, and electrons in their correct locations.

• Pay attention and copy the example that we do together as a class!

Atoms & Chemical Bonding Flip Chart

Atomic #ProtonsElectronsBohr ModelsValence ElectronsElectron Dot DiagramIonic Bond

Mass #NeutronsEnergy LevelChargeValence ShellOxidation #Covalent Bond

Entrance Questions

Ready your remote

Notes - Isotopes• Turn to page 5 of your Atomic Structure Packet

Isotopes• All atoms of a certain element will have EXACTLY the same amount of protons, however, some atoms of the same element may have DIFFERING numbers of neutrons.

• These are called isotopes of that element.

Isotopes• Isotopes have the SAME number of protons, but a DIFFERENT number of neutrons.

• Since isotopes have DIFFERENT amounts of neutrons, they will have DIFFERENT mass numbers!!!

Isotopes• Isotopes are referred to as the element followed by the mass number.

• Carbon-12 has a mass of 12. Carbon-13 has a mass of 13. Carbon-14 has a mass of 14.

Average Mass Number

• SPECIAL NOTE: The mass numbers listed on the periodic table are AVERAGE MASS NUMBERS of those elements, because each element may a have a number of different isotopes!!!

Examples of Isotopes

Carbon-12 Carbon-14

___ protons ___ protons

___ neutrons ___ neutrons

___ electrons ___ electrons

Examples of IsotopesCarbon-12 Carbon-14

6 protons 6 protons

6 neutrons 8 neutrons

6 electrons 6 electrons

Neon-20 Neon-22

____ protons ____ protons

____ neutrons ____ neutrons

____ electrons ____ electrons

Neon-20 Neon-22

10 protons 10 protons

Sodium-23 Sodium-24

Examples of IsotopesSodium-23 Sodium-24

Phosphorus-31 Phosphorus-32

Iron-56 Iron-58

Examples of IsotopesChlorine-35 Chlorine-37

Review QuestionsReady your remote

What do you call atoms that have the same number of protons, but different masses?

0% 1. Heavy atoms2. Radioactive atoms3. Isotopes4. Ions

0% 1. 9 2. 10 3. 19 4. 28

0% 1. 29 2. 20 3. 18 4. 9

0% 1. 92. 123. 214. 30

IsotopesReturn your remoteVIDEO CLIP REVIEW:Protons, Neutrons, Electrons - IsotopesComplete PACKET pages

Entrance QuestionsReady your remote

What do you call atoms that have the same atomic number, but different mass numbers?

0% 1. Isotopes2. Ions3. Heavy atoms4. Radioactive atoms

What is the atomic number of calcium?

0% 1. 62. 173. 204. 40

0% 1. 9 2. 10 3. 19 4. 28

End of Entrance QuestionsReturn your remoteGet in groups of 2 – 4

Get 1 Atom Poster & 1 bag of subatomic particles & 1 “Atom Building – Isotopes” worksheet per group

Atom Building - Isotopes4

MASS #

ATOMIC #

Remember the short- hand

way chemists use to write

down a lot of info about an

ChemicalSymbol

MASS # = neutrons + protons

ATOMIC # = protons= electrons, if neutral

We can figure out the

number of protons

neutrons & electrons from

this info

Neutrons = MASS# – ATOMIC #

M # = n + p =

A# = p = = e

Using the protons, neutrons, & electrons

provided, create a model of this helium atom.

(It has 2 protons, 2 neutrons, & 2

electrons.)n= M# – A# = 2

Continue Atom Building with this isotope of helium and record all the information on the

Atom Building work sheet

information on the Atom Building –

Isotopes work sheet

Atom Building - Isotopes

• Don’t forget to turn in your “Atom Building – Isotopes”

work sheet into your class bin before you leave.

• Complete PACKET page 21“Atoms R Us”

0% 1. 102. 163. 54. 11

What would be the charge of an atom with 7 protons, 7 neutrons, & 8 electrons?

0% 1. -1 2. 03. +14. +2

0% 1. -3 2. -13. +14. +3

End of Entrance QuestionsReturn your remoteGet in groups of 2 – 4

Get 1 Atom Poster & 1 bag of subatomic particles & 1 “Atom Building – Isotopes & Ions” worksheet per group

Atom Building – Isotopes & Ions

MASS #

ATOMIC #

Remember the short- hand way chemists use to write down a lot of info about an

Build this atom on your poster & record

it on your “Atom Building – Isotopes &

Ions” work sheet

ChemicalSymbol

MASS #

ATOMIC #

Chemists also add charge to the upper

right of the chemical symbol

ChemicalSymbol

CHARGE

M# = n+p

A# = p

By definition, The atomic

number is the number of

protons, so it WILL NOT CHANGE. Charge

comes from a change in the number of electrons

ChemicalSymbol

CHARGE = p – e

M# = n+p

A# = p

Charged atoms are

called ions.ChemicalSymbol

CHARGE = p – e

# electrons = # protons – CHARGE

M# = n+p =

A# = p =

ChemicalSymbol

CHARGE = p – e

# electrons = 11 – (+1) = 10

# neutrons = M# – A# = 23 – 11 = 12

Change your atom

to build this ion on your

poster & record it on your “Atom Building – Isotopes & Ions” work

Atom Building – Isotopes & Ions7

Continue Atom Building with this lithium atom and

record all the information on the “Atom Building – Isotopes & Ions”

work sheet

Atom Building – Isotopes & Ions7 +1

Build this ion and record all the

information on the “Atom Building – Isotopes & Ions”

work sheet

Atom Building – Isotopes & Ions20 -1

work sheet

Atom Building – Isotopes & Ions• Don’t forget to turn in your “Atom Building – Isotopes & Ions” work sheet into your class bin before you leave.

• Complete PACKET page 22 “Parts of An Atom”

JOURNAL ENTRY• Turn to Journal # 2

JOURNAL #2

Draw Models of the following atoms:

20 20 -1 25 25 +2

F F Mg Mg 9 9 12 12

Energy Level Smarts!!!

• YOU MAY EAT THE SMARTIES AT THE END OF CLASS!!!!

• UNTIL FURTHER NOTICE, THEY ARE ELECTRONS

0% 1. 82. 103. 184. 20

0% 1. -2 2. 03. +14. +2

0% 1. 9 2. 10 3. 19 4. 28

Atomic Structure Notes

• Turn to page 7 of your Atomic Structure Packet

The Electron Cloud

• Even though electrons move haphazardly outside the nucleus, there are certain regions where an electron is more likely to be.

• We call these regions energy levels. (They are also referred to as orbitals or shells).

Energy Levels• Electrons have more energy as they get further away from the nucleus.

• The higher the energy, the further away from the nucleus.

• (The first energy level is closest to the nucleus)

Energy Levels• Electrons will usually be found in the lowest energy level possible.

• Each energy level has a maximum number of electrons it will contain at a time.

Energy Level Capacity

Energy Level Name Max # Electrons

1st K 22nd L 83rd M 184th N 325th O 32?6th P 32?7th Q 32?

Electrons in Energy Levels• Electrons will first be located

in the lowest energy levels• When lower energy levels are full, additional electrons will be in the next lowest energy level

**It does get more complicated than just filling the lowest levels first.**

Lots of Energy Levels!?!• In energy levels that can

contain more than 8 electrons...• Once the lowest energy level contains 8 electrons, the next 2 electrons will be found in the next highest energy level, before filling that lower level

Hydrogen’s ? Electron

Energy Level # Electrons

Hydrogen’s 1 Electron

Carbon’s ? Electrons

Carbon’s 6 Electrons

Neon’s ? ElectronsEnergy Level # Electrons

Neon’s 10 Electrons

Aluminum’s ? Electrons

Aluminum’s 13 Electrons

Calcium’s ? Electrons

Calcium’s 20 Electrons

Iron’s ? ElectronsEnergy Level # Electrons

Iron’s 26 ElectronsEnergy Level # Electrons

3rd 14

Review Questions

Ready your remote

You may now eat your electrons… or

Smarties

How many electrons are in the 3rd energy level of a magnesium atom?

0% 1. 22. 63. 124. 24

How many electrons are in the 2nd energy level of a nitrogen atom?

0% 1. 22. 53. 74. 8

How many electrons are in the 3rd energy level of a chlorine atom?

0% 1. 22. 73. 94. 17

Energy LevelsReturn your remote

0% 1. 10 2. 21 3. 204. 31

What is the charge of an atom with 15 protons, 16 neutrons, & 18 electrons?

0% 1. -3 2. -13. +14. +3

JOURNAL # 3

Create a table showing the maximum number of electrons

in each energy level.Share the “special rule” for

electrons in the 3rd through 7th energy levels.

Energy Level Capacity

Energy Level Name Max # Electrons

1st K 22nd L 83rd M 184th N 325th O 32?6th P 32?7th Q 32?

Bohr Models• Because these different

energy levels exist, a Bohr model or (electron shell diagram) is a good visual of the location of electrons.

• Remember this is NOT what an atom really looks like, but is much more organized than reality.

Drawing Bohr Models• It is a simple drawing of a

number of concentric circles.• The innermost circle contains

information about the nucleus (The number of protons & neutrons)

• The next circle out would be the 1st energy level, the next circle out the 2nd energy level, then the 3rd, and so on.

Electron Shell Diagram of Carbon

Electron Shell Diagram of Aluminum

Electron Shell Diagram of

Calcium

Electron Shell Diagram of Iron

How many electrons are in the 3rd energy level of a chlorine atom?

0% 1. 22. 73. 94. 17

How many electrons are in the 2nd energy level of an oxygen atom?

0% 1. 22. 43. 64. 8

What is the maximum number of electrons in the 3rd energy level?

0% 1. 22. 63. 84. 18

Assignments1.) Place your remote inside the

correct pocket!! 2. )Complete p.23-24 Bohr

Models

JOURNAL #4

Draw BOHR MODELS of the following atoms:

17 20 -1 28 27 +3

O F Al Al 8 9 13 13

How many protons are in oxygen-18?

0% 1. 8 2. 9 3. 104. 18

How many neutrons are in oxygen-18?

0% 1. 8 2. 9 3. 104. 18

How many protons are in phosphorus-32?

0% 1. 152. 163. 174. 32

How many neutrons are in phosphorus-32?

0% 1. 152. 163. 174. 32

How many electrons would be in an atom with a neutral charge ( equal to 0)?

0% 1. One less than a neutral atom2. One more than a neutral atom3. Two more than a neutral atom4. Same as the protons

How many electrons would be in an atom with a charge of -1?

How many electrons would be in an atom with a charge of +1?

Assignments1.) Return your remote2.) Complete PACKET p.25 Atomic

AlphabetLIST ONLY IMPORTANT TERMS (NOT NAMES OF ELEMENTS)

SOME LETTERS MAY BE BLANK 3.) Your Packet should be complete

now 4.) Atomic Structure Test FRI Jan 6

Atoms & Chemical Bonding Flip Chart

Atomic #ProtonsElectronsBohr ModelsValence ElectronsElectron Dot DiagramIonic Bond

Mass #NeutronsEnergy LevelChargeValence ShellOxidation #Covalent Bond

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