Level 3 Review for Periodic Table Test
Directions: Answer the questions using a separate sheet of paper. Questions in bold
are required. Other questions are optional, but recommended. Remember that even if
you are not required to answer a question, you are still held responsible for knowing
how to answer it on the test.
1. Write the noble gas configurations for the following elements
a.
b.
c.
d.
e.
f.
g.
h.
i.
j.
k.
Si: [Ne] 3s23p2
Sb: [Kr] 5s24d105p3
Re: [Xe] 6s24f145d5
Cu: [Ar] 4s13d10
Cd: [Kr] 5s24d10
Br: [Ar] 4s23d104p5
Kr: [Ar] 4s23d104p6
K: [Ar] 4s1
Y: [Kr] 5s24d1
S: [Ne] 3s23p4
Mo: [Kr] 5s14d5
2. Identify the following elements based in their electron configurations
a.
b.
c.
d.
e.
f.
g.
h.
i.
j.
k.
l.
m.
Se
Br
Kr
Fr
Ds
Po
Mn
Sn
Sb
Xe
K
Rh
Al
3. How many periods are on the periodic table? How are they numbered?
7, numbered 1-7
4. How many groups are on the periodic table? How are they numbered?
18, numbered 1-18
5. Of Cesium (Cs), Hafnium (Hf), and Gold (Au), which element has the smallest
atomic radius? Explain your answer in terms of atomic structure.
Gold has the smallest radius because it has the greatest effective nuclear charge
(most protons in the nucleus).
6. Arrange the following elements in order of decreasing electronegativities: C, O,
Li, Na, Rb, and F.
F, O, C, Li, Na, Rb
7. Arrange the following atoms in order of decreasing first ionization energies: Li,
O, C, K, Ne, and F.
Ne, F, O, C, Li K
8. Which element is most electronegative among C, N, O, Br, and S? Which group
does it belong to?
O, group 16
9. The two ions K+ and Ca2+ each have 18 electrons surrounding the nucleus.
Which would you expect to have the smaller radius? Why?
Ca2+ because it has a greater effective nuclear charge (more protons)
10. Describe the state of matter (solid, liquid, or gas), reactivity, conductivity, and
ionization energy of each of the following elements:
a. Fluorine (F)
Gas, very reactive, not a conductor, high ionization energy
b. Xenon (Xe)
Gas, very unreactive, not a conductor, high ionization energy
c. Sodium (Na)
Solid, very reactive, conductor, low ionization energy
From the textbook:
Page 151 #27- see notes, 31 (c) , 32 see notes, 48 see notes, 50 see notes
Page 122 #6 same number of occupied energy levels, 7 same number of valence
electrons
Page 131 #1 noble gases- full valence shells, 3 see notes, 7 see notes
Page 141 #3 see notes, 8 more electron shells, 10 decreases down a group,
increases across a period, 13 gets smaller because electron repulsion decreases,
and in come cases atom loses an electron shell
Page 155 #3 a, 5 a, 7 c, 8 c, 9 a, 10 b, 11 d