1.
How many electrons can be accommodated in
a. a d subshell 10
b. a set of f orbitals 14
c. the n = 4 shell 32
d. the 7s orbital 2
e. a px orbital? 2
2. Is anything wrong with the following ground state electron configurations? If so, what?
a.
b.
c.
d.
e.
3.
OK as drawn
4s is not completely filled before 4p
4s violates Pauli exclusion principle
OK as drawn ** note that this is one of the exceptions we talked about in class**
4p violates Hunds rule
How many unpaired electrons are there in
a. a nitrogen atom 3 1s22s22p3
b. an iodine atom 1 [Kr] 5s24d105d5
c. a nickel (II) cation 2 [Ar] 4s23d10
d. an oxide ion? 0 [Ne]
4. Which orbital is filled following these orbitals?
a. 3d 4p
b. 4s 3d
c. 5p 6s
d. 5f 6d
5. Which elements fit the following descriptions:
a. has a valence shell configuration 4f14 5d10 6s1 Au
b. has 13 more electrons than argon Ga
c. its 3+ ion has the electron configuration [Kr] 4d10 In3+
6. How many orbitals make up the 4d subshell?
a) 0
b) 1
c) 3
d) 5
e) 7
7. The correct electron configuration for nitrogen is
a) 1s2 2s2 2p6 3s2 3p2
b)
c)
d)
e)
1s2 2s2 2p6 2d4
1s2 2s2 2p3
1s2 2s2 3s2 4s1
1s2 1p5
8. The electron configuration of the indicated atom in the ground state is correctly written for
which atom?
a) Ga
[Ar] 3d12 4s2
b) Ni
[Ar] 3d10
c) Ni
[Ar] 3s2 3p8
d) Cu
[Ar] 3d10 4s1
9. In what section of the periodic table is the 4f subshell being filled?
a) period 4
b) transition elements Y to Cd
c) noble gases
d) group IA
e) lanthanides
10. Which one of the following elements has 3 electrons in a p subshell?
a) Sb
b) Na
c) Sc
d) V
e) Nd
11. Which of the following distributions of electrons is correct for three electrons in p-subshell?
a)



b)


c)



d)


e)


12. Write the electron configuration for silver:
Long form: 1s22s22p63s23p64s23d104p65s14d10
Short form: [Kr]5s14d10