1. What is the maximum number of electrons that can occupy each of the following subshells?
a) 4p
b) 5f
c) 2s
d) 3d
2. Write the condensed electron configurations for the following atoms:
a) Sulfer
b) Iron
c) Silver
d) Antimony
e) Chromium
f) Platinum
3. Determine if the following sets of quantum numbers are permissible for an electron in a hydrogen atom. (If it is permissible give the orbital type, if it is not permissible, explain why):
a) n=3, l=3, m=1
b) n=2, l=1, m=0
c) n=5, l=2, m=-3
d) n=4, l=3, m=2
4. What is the maximum number of electrons in an atom that can have the following quantum numbers?
a) n=3, l=2
b) n=1, s= 1/2
c) n=2, m=0
d) n=4, l=3
5. Determine what is wrong with the following electron configurations for atoms in their ground states and correct it:
a) 1s^2 2s^2 2p^6 3s^2 2d^1
b) [Ar] 4s^2 4d^10 4p^2
c) [Kr] 3d^2 4s^2
6. List the possible values for l and m when:
a) n=2
b) n=4
c) n=1
d) n=6
7. Draw the orbital diagrams for the valence electrons of each of the following elements and indicate how many unpaired electrons each has:
a) Aluminum
b) Vanadium
c) Rubidium
d) Molybdenum
e) Arsenic
f) Chlorine
g) Copper