1. Warmup
Review the standards below by considering what you have learned on each topic.
Identify areas of concern for further review.
Atomic Theory
Students can describe how key experiments advanced the Atomic Model.
They understand the difference between physical, chemical and nuclear changes, know the meaning of atomic number, atomic mass, quarks, and isotope, and can describe what occurs during alpha, beta, and gamma decay. They can solve radioactive decay problems involving half-life, and know that some elements only exist in laboratory settings.
Students know Avagadro’s number and can use it with molar mass to convert between mols and kilograms.
Electron Orbits
Students can synthesize information including orbital types, Pauli’s exclusion principle, quantum electron states, and hybridization to describe and diagram the general characteristics of an element’s electron cloud.
Students understand that electron orbits quantized, and that falling electrons emit unique light spectra.
Students can determine the ionized charge of an element on the basis of full, empty, hybrid, or half full orbitals.
Students can label the regions, groups, and periods of the periodic table and can describe element’s properties in these categories.

2. OCTOBER 6TH, 2010
Review

3. How many neutrons does Potassium usually have?15
30.974 19
39.098 20
None of the above

4. What is the atomic mass for an element which has 10 protons and either 10 (60%) or 11 (40%) neutrons?
10.4 20
20.4 21 31

5. What is a possible set of isotopes for an element with an atomic mass of 120.42?
119 (80%) and 125 (20%)
(100%)
120 (58%) and 121 (42%)
120 (40%), 121 (37%) and 122 (23%)
None of the above

6. Notetaking Preview Orbitals Shapes Relationship to Periodic Table
Relationship to # of e- and p+
Rules
Pauli’s Exclusion Principle
Aufbau Principle
Hund’s Rule

7. Periodic Table Structure2
10 wide 6 14

8. Orbital Shapes There are 4 types of orbitals:
S – comes in sets of 1 – holds 2 electrons
P – comes in sets of 3 – holds 6 electrons
D – comes in sets of 5 – holds 10 electrons
F – comes in sets of 7 – holds 14 electrons
Notice that they come in increasingly large odd sets, and this leads to increasingly even numbers of electrons stored there.

9. Pauli’s Exclusion Principle
Each orbital can only hold two electrons.
One spins one way, the other spins the opposite direction.
A Helium atom has one full orbital. How many electrons does it have?
A Scandium atom has 10 full orbitals and one half-full orbital. How many electrons does it have?
A mystery atom has one full and three half-full orbitals in its outside layer. How many electrons is that?

10. Aufbau Principle (Filling Order)
Electron orbitals are filled in order of the potential energy contained, from least to greatest.
Analogy:
Football players pile up near the grass. The stack gets higher as more jump on top. To undo the pile, you have to get the top ones off first.
You can’t have the football players make a tackle in the air and then add more beneath that! You also can’t get the guy off the bottom before the other people have moved first.

11. Electron Mapping Strategies
Count up and follow the shape of the periodic table to get your s’s, p’s, d’s, and f’s in the right order.
1,2 3, , , etc
s s p s p s d p
Then use the Aufbau diagram to assign numbers.
If the number is the same for two in a row, it doesn’t need to be rewritten
1s 2s p 3s p 4s 3d 4p
Then use superscripts (looks like exponents) to indicate how many electrons are in each set of orbitals.
1s2 2s2 p6 3s2 p6 4s2 3d10 4p1

12. Periods and Groups
Columns are called groups, and groups have similar chemical features. Each group is named.
Rows are called periods. Each period represents a new shell which is a set of electron orbitals.
Upper periods are inner shells, while the bottom period is the outer shell called the valence shell.

13. Hund’s Rule
Nature seeks ‘stable’ arrangements which have the lowest energy. These are:
Whole valence, empty or full
Whole valence, half full
Subset full, rest empty

14. Pauli’s Exclusion Principle Aufbau Principle Hund’s Rule
Inner orbitals are filled before outer ones, and simple orbitals are filled before complicated ones. Which idea is this?
Pauli’s Exclusion Principle
Aufbau Principle
Hund’s Rule
Bohr’s Quantization
None of the above

15. A shell with four orbitals (an s and three p’s) can hold eight electrons. This is an example of:
Pauli’s Exclusion Principle
Aufbau Principle
Hund’s Rule
Bohr’s Quantization
None of the above

16. According to Hund’s Rule, what number of electrons might Fluorine give or take in order to become the most stable?
Give 2
Take 1
Take 2
Give 7
Give 5

17. According to Hund’s Rule, what number of electrons might Magnesium give or take in order to become the most stable?
Take 3
None, already stable
Take 5
Give 2
Give 1

18. According to Hund’s Rule, if there are five electrons in the outer valence, they will be arranged:
2 in s, 2 in p1, 1 in p2, 0 in p3
0 in s, 2 in p1, 2 in p2, 1 in p3
1 in s, 2 in p1, 0 in p2, 2 in p3
2 in s, 1 in p1, 1 in p2, 1 in p3
None of the above

19. The correct electron mapping for Aluminum is:
1s2 2s2 p6 3s2 p6
1s2 2s2 3p6 4s2 p1
1s p 2s p 3s2
1s2 2s2 p6 3s2 p1
None of the above

20. The correct electron mapping for Titanium is:
1s2 2s2 p6 3s p6 4s2 3d2
1s2 2s2 p6 3s2 p6 4s2 d2
1s2 2s2 p6 3s p6 4s2 3d10
1s2 2s2 3p6 4s2 p6 s
None of the above

21. The correct electron mapping for Sodium is:
1s2 2s2 3p6 4s1
1s2 p6 2s2 p6 3s1
1s2 p6 2s2 3p6 4s1
1s2 2s2 p6 3s1
None of the above

22. The atom represented by the diagram is which element?
Berylium (Be)
Carbon (C)
Nitrogen (N)
Helium (He)
Phosphorous (P)

23. The atom represented by the diagram is which element?
Berylium (Be)
Aluminum (Al)
Carbon (C)
Oxygen (O)
Phosphorous (P)

24. The atom represented by the diagram is which element?
Berylium (Be)
Lithium (Li)
Oxygen (O)
Aluminum (Al)
None of the above

25. Half-Life and Decay α (Alpha) – 2 n0 and 2 p+ leave
β (Beta) – 1 n0 turns into a p+ and e-
γ (Gamma) – electromagnetic radiation
Now = Then * ½ ^ (t / λ)

26. 1M years 2M years 3M years 4M years 5M years 6M years 7M years
An element has a half-life of 1 million years. How long will it take for g of this element to decay down to grams?
1M years
2M years
3M years
4M years
5M years
6M years
7M years
8M years

27. An alien ring portal thingy was put on Earth 2700 years ago, and was made of 500. kg of radioactive metal. Scientists measure the half-life of a sample and find it to be 900 years. How much metal is left now?
250 kg
125 kg
62.5 kg
31.3 kg
15.6 kg
7.8 kg