Section 7.2
The Periodic Table and Atomic Structure
Practice Test
1.
The number of valence electrons in a sulfur atom is __________.
a.
two
b.
four
c.
six
d.
eight
Hint
2.
An electron in an atom emits energy in the form of light when it ________________.
a.
falls back to a lower energy level
b.
rises to a new energy level
c.
leaves the atom
d.
leaves the nucleus
Hint
3.
Energy sublevels are designated _____________.
a.
s, p, d, and f
b.
a, b, c, and d
c.
x, y, and z
d.
1, 2, 3, and 4
Hint
4.
The third energy level may have ____________ sublevels.
a.
two
b.
three
c.
four
d.
eight
Hint
5.
How many electrons may be contained in a p sublevel?
a.
three
b.
six
c.
eight
d.
ten
Hint
6.
The space in which there is a 95% probability of finding an electron is called __________.
a.
an energy level
b.
an energy sublevel
c.
an electron sphere
d.
an orbital
Hint
7.
These orbitals are aligned along the x, y, and z axes.
a.
s orbitals
b.
p orbitals
c.
d orbitals
d.
f orbitals
Hint
8.
The Heisenberg uncertainty principle states that it is fundamentally impossible to know both the ____________________ of the electron at the same time.
a.
position and energy
b.
mass and size
c.
mass and position
d.
energy and orientation
Hint
9.
The fourth energy level can hold _______ more electrons than the third energy level.
a.
2
b.
6
c.
10
d.
14
Hint
10.
The most stable arrangement of electrons in an atom's sublevels and orbitals is called its ________________.
a.
electron configuration
b.
electronic arrangement
c.
shape
d.
electron orientation
Hint
11.
The underlying reason that some periods have eighteen elements is that the combined _______ sublevels may contain 18 electrons.
a.
s, p, and d
b.
d and f
c.
p and d
d.
s, p, d, and f
Hint
12.
1s
2
2s
2
2p
1
is the electron configuration for _________.
a.
boron
b.
lithium
c.
hydrogen
d.
fluorine
Hint
13.
What element has the electron configuration [Ar]4s
2
3d
3
?
a.
arsenic
b.
nitrogen
c.
scandium
d.
vanadium
Hint
14.
What is the electron configuration of radon?
a.
[Xe]6s
2
6p
6
b.
[Rn]6s
2
6p
6
c.
[Xe]5s
2
5p
6
d.
[Xe]5d
8
Hint
15.
Except for helium, noble gas atoms have _________.
a.
duets
b.
octets
c.
quartets
d.
trios
Hint
16.
When an iron atom loses all its 4s electrons and one 3d electron, its oxidation number is ______.
a.
3+
b.
11+
c.
5+
d.
1+
Hint
17.
What electron configuration describes the outermost energy level of a molybdenum atom?
a.
5s
2
b.
4d
4
c.
6p
6
d.
5d
4
Hint
18.
What electron configuration describes the outermost energy level of a selenium atom?
a.
4s
2
4p
4
b.
4s
2
3d
10
c.
4s
2
4d
4
d.
4s
2
4d
10
4p
4
Hint
19.
If an s sublevel could contain up to three electrons, which element would be the first noble gas?
a.
carbon
b.
helium
c.
lithium
d.
neon
Hint
20.
Which of these is the electron configuration of an atom most likely to lose an electron?
a.
1s2 2s2 2p6
b.
[He]2s2 2p5
c.
1s2 2s2 2p6 3s2 3p5
d.
1s2 2s2 2p6 3s2 3p6 4s1
Hint
21.
Which of these is the electron configuration of an atom most likely to gain an electron?
a.
1s2 2s2 2p6
b.
1s2 2s2 2p6 3s1
c.
1s2 2s2 2p6 3s2 3p5
d.
1s2 2s2 2p6 3s2 3p6 4s1
Hint
