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elements and
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The Periodic Table
and Stuff
Name: ______________
Block: ___
1. How many protons are in each of the following?
a. Be
4
b. U
92
c. Mn
25
36
e. O2-
2. How many electrons are in each of the following?
a. Na+ 10
b. V3+
20
c. Fe2+
d. As3-
24
10
3. Predict the electron configuration of the following:
a. P 1s22s22p63s23p3
b. Ti 1s22s22p63s23p64s23d2
c. Br 1s22s22p63s23p64s23d104p5
d. Sr 1s22s22p63s23p64s23d104p65s2
e. Ar 1s22s22p63s23p6
f. K 1s22s22p63s23p64s1
g. Cd 1s22s22p63s23p64s23d104p65s24d10h. Ca 1s22s22p63s23p64s2
i.
Xe 1s22s22p63s23p64s23d104p65s24d105p6j. Cs 1s22s22p63s23p64s23d104p65s24d105p66s1
4. Re-write the electron configurations in question 3 using core notation.
a. [Ne] 3s23p3
b. [Ar] 4s23d2
d. [Ar] 4s23d104p5
d. [Kr] 5s2
f. [Ne] 3s23p6
f. [Ar] 4s1
g. [Kr] 5s24d10
h. [Ar] 4s2
i.
[Kr] 5s24d105p6
j. [Xe] 6s1
5. Predict the electron configuration of the following ions, using core notation.
a.
c.
e.
g.
i.
H- 1s2
Br- [Ar] 4s23d10 4p6
Ti2+ [Ar] 3d2
Mn2+ [Ar] 3d5
Fe3+ [Ar] 3d5
b.
d.
f.
h.
j.
[Ar] 4s23d104p6
Sr2+ [Kr]
N3+ [He] 2s2
N2- [He] 2s22p5
Ge4+ [Ar] 3d10
Ge2+ [Ar] 4s23d10
6. How many valence electrons do the following contain?
a. O
6
b. P
c. V
5
d. Ca
0
l-
e. Xe
g. I
i.
5+
-
O
5
f. C
2
5
2+
0
4+
3
h. Zn
7
2
j. Tc
7. Which elements have the following electron configuration?
a. 1s2 2s2 2p3
2
2
6
N
2
b. 1s 2s 2p 3s 3p3
P
c. 1s2 2s2 2p6 3s2 3p6 4s2 3d1 Sc
d. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10
2
2
6
2
6
2
10
6
2
10
Cd
e. 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p6 6s2 4f14 5d6
Os
4. When an electron in a 2p orbital of a Lithium atom makes a transition to the 2s
orbital, a photon of wavelength 670.8 nm is emitted. The energy difference between
these 2p and 2s orbitals is?
5. How many f orbitals have the value n = 3?
6. How many electrons in an atom can have the quantum numbers n = 3, l = 2?
7. How many electrons can be described by the quantum numbers n = 3, l = 3, ml = 1?
8. The electron configuration for the Barium atom is?
9. Give the quantum numbers for the last electron in:
a. Gold
b. Magnesium
c. Iodine
-1/2
d. Cadmium
10. How many electrons in an atom can have the following quantum numbers:
a. n = 3
b. n = 2, l = 0
c. n = 2, l = 2, me = 0
d. n = 2, l = 0, me = 0, ms = ½
11. Consider the following sets of quantum numbers. Which set(s) represent(s)
impossible combinations?
SET
n
l
ml
ms
A
1
0
1
+1/2
B
3
3
0
+1/2
C
2
1
1
-1/2
D
3
2
-2
-1/2
E
3
1
-2
-1/2
F
2
0
0
-1/2
Use the following to answer questions 12 – 16.
Given the following electronic configuration of neutral atoms, identify the element and
state the number of unpaired electrons in the ground state:
12. [Ar]4s23d4
13. [Ne]3s23p5
14. [Kr]5s24d105p4
15. [Ar]4s13d10
16. [He]2s22p3
Use the following to answer questions 17 – 22.
Write the electron configuration for the following:
17. P
18. Ag
19. S220. I
21. Fe3+
22. K+
23. If n = 2, how many orbitals are possible?
a.
b.
c.
d.
e.
3
4
2
8
6
24. The electron configuration of Indium is:
a.
b.
c.
d.
e.
1s22s22p63s23p63d104s24p64d105s25p15d10
1s22s22p63s23p63d104s24p64d104p1
1s22s22p63s23p64s24p64d105s25p105d1
1s22s22p63s23p63d104s24p64d105s25p1
None of the above.