Chapter 5:
Electrons in Atoms
Practice Test
1.
The Heisenberg uncertainty principle states that ____________.
a.
electrons of atoms in their ground states enter energetically equivalent sets of orbitals singly before they pair up in any orbital of the set
b.
no two electrons in the same atom can have the same set of four quantum numbers
c.
two atoms of the same element must have the same number of protons
d.
it is impossible to simultaneously know the precise position and velocity of a particle
Hint
2.
How many electrons are in the highest energy p orbitals of a group 4A atom?
a.
4
b.
3
c.
1
d.
2
Hint
3.
What is the lowest energy state of an atom called?
a.
the chaotic state
b.
the solid state
c.
the excited state
d.
the ground state
Hint
4.
How many valence electrons does a group 1A metal atom have?
a.
3
b.
4
c.
1
d.
2
Hint
5.
What is the symbol of the element that has the following electron configuration?1s
2
2s
2
2p
x
2
2p
y
2
2p
z
2
3s
2
3p
x
2
3p
y
2
3p
z
1
a.
Si
b.
Cl
c.
P
d.
S
Hint
6.
When an atom loses energy by electron transition, a(n) _____________ is produced.
a.
adsorption
b.
absorption
c.
emission
d.
ion
Hint
7.
The concept that all moving particles have wave characteristics is attributed to ___________.
a.
Thomson
b.
Bohr
c.
de Broglie
d.
Heisenberg
Hint
8.
How many types of orbitals are present in atoms of elements in the third period of the periodic table?
a.
2
b.
3
c.
1
d.
4
Hint
9.
The principle that states each electron occupies the lowest energy orbital available is the ______________.
a.
aufbau principle
b.
exclusion principle
c.
uncertainty principle
d.
photoelectric principle
Hint
10.
How many electrons can an orbital contain?
a.
4
b.
2
c.
1
d.
3
Hint
11.
A wavelength of 500 nm is associated with the _______ portion of the electromagnetic spectrum.
a.
visible
b.
microwave
c.
infrared
d.
ultraviolet
Hint
12.
Which one of the following electron configurations is incorrect?
a.
Ca-----1s
2
2s
2
2p
6
3s
2
3p
6
4s
2
b.
Xe-----[Kr]4d
10
5s
2
5p
6
c.
Cu-----[Ar]3d
10
4s
1
d.
Mn-----[Ar]4s
2
4d
5
Hint
13.
In the periodic table, the principal quantum number corresponds to the ________.
a.
lanthanides
b.
group number
c.
transition metals
d.
period number
Hint
14.
An element whose atoms have four valence electrons is _______.
a.
Cr
b.
Ti
c.
Nb
d.
Sn
Hint
15.
An element with the outermost electron configuration,
n
s
2
n
p
4
, could be _______.
a.
Zr
b.
Pb
c.
Se
d.
Mo
Hint
16.
What is an electron dot structure?
a.
An element symbol surrounded by its innermost electrons.
b.
An element symbol with a positive charge.
c.
An element symbol surrounded by dots representing its valence electrons.
d.
A filled noble gas in brackets plus the remaining electron configuration expressed by filled orbitals.
Hint
17.
Which of the following power sources makes use of the photoelectric effect?
a.
alkaline batteries
b.
diesel engines
c.
solar power cells
d.
nuclear power plants
Hint
18.
The total number of electrons in s orbitals in a germanium atom is ________.
a.
6
b.
18
c.
15
d.
8
Hint
19.
One of mercury’s spectral lines has a wavelength of 6.234 × 10
-7
m. What is the line’s frequency?
a.
4.81 × 10
14
s
-1
b.
4.81 × 10
6
s
-1
c.
1.87 × 10
6
s
-1
d.
1.87 × 10
14
s
-1
Hint
20.
The minimum amount of energy that can be gained or lost by an electron is a _________.
a.
planck
b.
queue
c.
quantum
d.
quart
Hint
