AP Chem
Atomic Structure Homework
1. Tell how each affect the energy of an electron in an atom:
A. Spin
B. Electrostatic attraction/repulsion
2. Define each term and tell how each affects the energy of an electron in an atom:
A. Shielding
B. Penetration
3. Rank each type of orbital from highest to lowest in:
A. Shielding ability
B. Penetration
C. Relative energy for the same n
4. Give the term that fits the prompt
A. Electrons fill orbitals so as to maximize spin
B. No two electrons can have the same four quantum numbers
C. It is impossible to know the position and momentum of a particle simultaneously
D. Positive and negative charges attract
E. The energy cost of putting two electrons in the same orbital
F. Energy can only exist in discrete multiples of one minimum amount of energy
G. Electrons fill the lowest energy orbitals first
H. Charge of the nucleus
I. Charge an electron “feels”
5. Which configurations are possible and which are impossible? Which are possible but not the ground state? Tell what is wrong with each impossible and modify the impossibles to make them possible. Modify the high energy possibles to put them in the ground state
A. 1s12s1
B. 1s22s12p1
C. 1s22s12p3
D. 1s22s23s2
E. 1s21p1
F. 1s32s1
G. 1s22s22p62d2
H. 1s22s22p63p1
I. 1s22s22p7
J. 2s12p2
K. 1s22s22p53s1
6. Which orbital diagrams are possible and which are impossible? Modify the impossibles to make them possible. Since I don’t have a drawing program that can do orbital diagrams take the configuration, draw the corresponding orbital diagram, and then do the problem.
A. 1s12s1
B. 1s22s12p1
C. 1s22s12p3
D. 1s22s23s2
E. 1s21p1
F. 1s32s1
G. 1s22s22p62d2
H. 1s22s22p63p1
I. 1s22s22p7
J. 2s12p2
K. 1s22s22p53s1
L. [He] 2s2 2p5
M. [Xe] 6s2 4f14 5d10 6p5
N. [Ar] 4s1
7. For each pair circle the right answer:
A. More reactive
I. F vs Cl
II. Na vs K
III. Na vs Mg
IV. O vs F
B. Larger
I. F vs Ne
II. H vs He
III. Li vs He
C. More electronegative
I. Br vs C
II. Mg vs Ca
D. More favorable electron affinity
I. F vs Cl
II. B vs C
III. Be vs B
IV. S vs P
V. Cl vs Ar
E. Higher first ionization energy
I. Li vs Be
II. Be vs B
III. B vs C
IV. C vs N
V. N vs O
VI. O vs F
VII. F vs Ne
VIII. H vs He
IX. Cu vs Zn
F. Higher second ionization energy
I. Na vs Mg
II. Mg vs Al
III. F vs Cl
8. Explain these exceptions to trends:
A. Boron has a lower first ionization energy than beryllium
B. Oxygen has a lower first ionization energy than nitrogen
C. Chlorine’s electron affinity is more favorable than fluorine’s
D. Chromium has 6 unpaired electrons, not 4
9. Explain
A. 3d orbitals are between 4s and 4p in energy.
B. n= 8 is about the same as n = ∞
C. The lanthanide contraction
D. We can’t use the Rydberg equation for non-hydrogenic systems
E. We store sodium under kerosene but magnesium ribbon is stored in the cabinet
F. Chlorine is 3 times as effective as iodine in disinfecting water with E. Coli. Also, the chlorine tablets last only 3 days after being opened while the iodine tablets last for 30 days.