1. ATOMIC THEORY REVIEW

2. Where did the elements come from?
Hydrogen, a little helium and an even smaller amount of lithium were created in the big bang. The universe is about 95% hydrogen. Clouds of hydrogen gas and dust are compressed by gravity into stars. When a star's core runs out of hydrogen, the nuclear reaction pauses, and gravity compresses the star, heating it up enough to fuse helium.

3. Where did the elements come from?
If the star is big enough it can eventually create all the elements in the periodic table up to iron (through nuclear reactions and gravity). If a giant star explodes (supernova), it will release enough energy to make all the elements heavier than iron. So stars created the first elements!

4. The most common Elements in the Earth’s CRUST
Amount
Oxygen
46.1 %
Silicon
28.2 %
Aluminum
8.23 %
Iron
5.63 %
Calcium
4.15 %

5. The most common Elements in the Earth’s OCEANS
Amount
Oxygen
85.84 %
Hydrogen
10.82 %
Chlorine
1.94 %
Sodium
1.08 %
Magnesium %

6. The most common Elements in the Earth’s ATMOSPHERE
Amount
Nitrogen
78.1 %
Oxygen
20.9 %
Argon
0.96 %

7. What is ALL matter made of?
ATOMS !!!
What are the 3 subatomic particles?
Protons
Neutrons
Electrons

8. What are the charges of the subatomic particles?
protons (+)
positive
neutrons (0)
neutral
electrons (-)
negative
We know that there are the same number of p+ and e- in atoms on the Periodic Table… So What is the overall charge of any atom?
The overall charge of any atom is
NEUTRAL… the positive charge cancels out the negative charge = 0!!!

9. What are the masses (amu) of the subatomic particles?
Atomic mass unit (AMU)
p+ = 1amu n = 1amu e- = 0 amu
What is this AMU stuff?????
2.2 lbs= 1 kg
1.66 x kg = 1 amu

10. What are the two areas of an atom?
Nucleus
Electron Cloud e-
P+ & No

11. Where are the p+, n, and e- located in an atom?
p+ in the nucleus no in the nucleus e- in the electron cloud

12. Where is ALL the mass in an atom located?
Where is most of the volume of an atom located?
Electron Cloud
Where is ALL the mass in an atom located?
Nucleus

13. What does a Bohr model of the atom look like?
The nucleus contains the p+ and n… while the electrons “orbit” the nucleus in the energy rings of the e- cloud.

14. So what are the charges of the different areas?
1. So what is the overall charge of the nucleus?
Positive
2. So what is the overall charge of the electron cloud?
Negative
(opposite charges attract)

15. QUICK REVIEW- ATOMS Protons + 1 nucleus p+ neutrons nucleus no 1 _
Sub-atomic particles:.
protons, neutrons, and electrons
Parts of the atom:
nucleus and electron cloud
particles
charge
amu
location
abbrev.
Protons + 1
nucleus p+
Neutral (0)
neutrons
nucleus no 1
Electron
cloud _
Electrons e-

16. Energy Levels of the Atom
Atoms can have several energy levels. Sometimes they are also called energy rings, shells or orbits.
The Nucleus
2e-
8 e-
8 e-
18 e-
18 e-
32e-
32e-
P+ N0
1st
shell
2nd
shell
3rd
shell
4th
shell
5th
shell
6th
shell
7th
shell

17. Beginning with Bohr Models
Let’s try a few easy bohr models: Li Be

18. Bohr Model Practice 1. Ca 2. O 3. Ne 4. K 5. Rb 6. P 7. F 8. Cl 9. Br
10. Au

19. Ca O Ne K Rb P F Cl Br Au

20. More Bohr Model Practice
11. Fr 12. Te 13. Sn 14. Cs 15. Kr
16. At
17. Ga
18. Rn
19. Ag
20. W

21. Fr Te Sn Cs Kr
At Ga Rn Ag W

22. Complete the Bohr Models for the following elements. Ne, Ar, Kr and Xe
What 4 patterns or trends did you notice they have in common?
“Predict” what you think Radon’s (Rn) bohr model would look like.
Six rings
Full shell
More massive
All of the rings or shells are full.
They are all in the same group (18)
They gain an energy ring as you go down a period.
They gain more subatomic particles as you go down.

23. Lets take a look at the Periodic Table!
The periods equal the number of energy shells or rings in an atom.
The rows equal the energy shells of bohr models.

24. Patterns from the Bohr Models
Ne Ar Kr Xe
Radon Bohr Model

25. Even More Bohr Model Practice!
21. Os 22. Hf 23. Cm 24. Sr 25. Ho
26. Tc
27. Ac
28. Zr
29. Po
30. Np
(Stop Whining)

26. Bohr Model
Draw the bohr models for the following atoms.
Explain why we use helium filled balloons instead hydrogen filled balloons at Parties.
H vs. He
Energy rings are not filled
Energy rings are filled
Hydrogen is unstable and flammable and helium is stable!

27. Burning Hindenburg

28. “Life on the Edge” with Valence Electrons
Valence electrons are electrons in the outermost shell of an atom.
They determine whether the atom will bond with another atom.
How many valence
electrons does
lithium have here?
1 valence electron
Circle the valence electron
and label it in your notes

29. Arrangement of the Periodic Table
1. What atom is this?
Oxygen
2. Which subatomic “particle” helped you to determine that this Bohr model was of oxygen?
Protons

30. Arrangement of the Periodic Table
1. The periodic table is arranged according to what?
A. Atomic Symbol
B. Atomic mass
C. Atomic number
D. Number of Energy Shells
Do the elements on the periodic table all increase according to their masses?
No!! Can you find where they are not? There are a few of them. Look carefully!

31. Periodic Table Card Sort Poster
Breaking the Code
Purpose: This lesson will help you identify many of the patterns that are contained in the periodic table of elements.
Use the card sort poster to answer the following questions on your paper.

32. Do you notice any patterns here as you move down a column on the Periodic Table?Li Na K Rb
Gaining more p+, no, and e-.
Gaining more mass
Gaining more energy rings
Can you “predict” how many energy rings a bohr model of Francium (Fr) would have?

33. Francium (Fr) Bohr Model
                                                         
1 valence electron
Seven energy rings

34. What Bohr model patterns are you starting to see develop?
Periodic Table Patterns
The atomic number is the same number as the number of protons and electrons.
Atoms get larger as you move down and to the right on the periodic table.
As you move from left to right on the periodic table, you gain protons and electrons and neutrons.
As you go down from the periodic table, the atom gains another energy shell or orbit.

35. Metals vs. Non-Metals Stair steps Non-metals Metals
Man made elements and Rare Earth metals

36. Metalloids on the Periodic Table
Periods/ Rows
Metalloids
FAMILIES/ GROUPS

37. Properties of Metals
Most elements are metals. 88 elements to the left of the stairstep line are metals or metal-like elements.
Tend to have Luster
High density
Ductile
Malleable
(shininess)
(heavy for their size)
(most metals can be made into thin wires)
(most metals can be hammered into thin sheets)

38. Properties of Non-metals
Nonmetals are found to the right of the stair step line.
No luster
Brittle
Not ductile
Not malleable
(dull)
(breaks easily)

39. Properties of Metalloids
Metalloids are elements on both sides of the stair step line. They have properties of both metals and nonmetals.
Solids
Can be shiny or dull
Ductile
Malleable

40. Families on the Periodic Table

41. So where do the names come from?
These abbreviations are for the LATIN names of the elements.
Iron (Fe)………….……Ferrum
Sodium (Na)….. …….Natrium
Gold (Au)……………Aurum
Silver (Ag)………….Argentum
Potassium (K)………… Kalium
Copper (Cu) ………….Cuprum
Mercury (Hg) ……Hydragyrum
Antimony (Sb)………… Stibium
Tin(Sn)….………… Stannum
Lead(Pb) ……………..Plumbum
Tungsten(W)………….Wolfran

42. Steps for creating a Bohr model
1. Complete the particle inventory for the atom (protons, electrons and neutrons).
2. Draw your nucleus.
3. Put the number of protons and neutrons in the nucleus.
4. Circle how many electrons you need to use in the shells.
5. Know how many electrons and shells you will need.
6. Put 2 electrons in the first shell. If there are more than 2, begin to fill the next shell (maximum of 8). 7. You cannot begin to fill the next shell until the previous shell is filled. 8. Remember` how many electrons each shell can hold a maximum of. (2, 8, 8, 18, 18, 32, 32,)

43. Zn Xe Au Hg I Element Atomic Number Atomic Mass # of Protons
# of Electrons
# of Neutrons Zn 30 65 Xe 54 77 Au 79
118 Hg 80
121 I
127 53 30 30 35 54 54
131 79
197 79 80
201 80 53 53 30

44. Yttrium Manganese Yttrium Manganese
P39
N50
P25
N30
Yttrium
First Energy Level: 2 Second Energy Level: 8 Third Energy Level: 8 Fourth Energy Level: 18
Fifth Energy Level: 3
Manganese
First Energy Level: 2 Second Energy Level: 8 Third Energy Level: 8 Fourth Energy Level: 7

45. Germanium Krypton Germanium Krypton
First Energy Level: 2 Second Energy Level: 8 Third Energy Level: 8 Fourth Energy Level: 14
Krypton
First Energy Level: 2 Second Energy Level: 8 Third Energy Level: 8 Fourth Energy Level: 18