CHEM 131 Extra Practice Questions for Chapter 3 and Nomenclature
1. What is the wavelength of electromagnetic radiation which has a frequency of 6.282 × 1014
s-1?
a.
b.
c.
d.
e.
2.
Calculate the frequency of visible light having a wavelength of 464.1 nm.
a.
b.
c.
d.
e.
3.
314.7 nm
314.7 m
3.147 cm
314.7 cm
31.78 m
Calculate the frequency of visible light having a wavelength of 568.8 nm.
a.
b.
c.
d.
e.
5.
139.1 s-1
1.548 × 10-6 s-1
1.548 × 10-15 s-1
6.460 × 1014 s-1
6.460 × 105 s-1
A police radar unit is operating on a frequency of 9.527 gigahertz. What is the wavelength
of the radiation being employed?
a.
b.
c.
d.
e.
4.
1.883 × 1023 m
2.095 × 106 m
4.772 × 10-7 m
4.772 × 10-7 nm
530.9 nm
170.5 s-1
1.897 x 106 s-1
1.897 x 1015 s-1
5.271 x 10-9 s-1
5.271 x 1014 s-1
Which one of the following types of radiation has the lowest frequency?
a.
b.
c.
d.
e.
radio waves
infrared radiation
microwave radiation
X--rays
ultraviolet rays
6.
What is the energy of one photon of microwave radiation with a wavelength of 0.158 m?
a.
b.
c.
d.
e.
7.
1.26 × 10-24 J
3.14 × 10-26 J
3.19 × 1025 J
3.49 × 10-43 J
7.15 × 1040 J
What is the energy of one photon of visible radiation with a wavelength of 464.1 nm?
a.
b.
c.
d.
e.
1.026 × 10-48 J
2.100 × 1035 J
2.341 × 1011 J
4.280 × 10-19 J
4.280 × 10-12 J
8.
Calculate the wavelength of the spectral line in the spectrum of hydrogen for which n1 = 1
and n2 = 3.
a. 277 nm
b. 103 nm
c. 345 nm
d. 397 nm
e. 489 nm
9.
A hydrogen atom starts in the n = 1 energy level. What energy level would the atom end up
in if it were to absorb 2.092 × 10-18 J of energy?
a.
b.
c.
d.
e.
n=2
n=3
n=4
n=5
n=6
10. Calculate the wavelength, in nanometers, of light emitted by a hydrogen atom when the
electron falls from an n = 7 energy level to an n = 4 energy level. Recall that the quantized
energies of the levels in the hydrogen atom are given by:
a.
b.
c.
d.
e.
4.451 × 10-20 nm
8.509 × 102 nm
2.166 × 103 nm
1.381 × 1014 nm
2.157 × 103 nm
11. Calculate the wavelength of a helium atom (mass = 6.65 x 10-27 kg) travelling at 1.25 km/s.
a.
b.
c.
d.
e.
79.7 nm
79.7 pm
8.31 x 10-27 m
1.25 x 1010 m
831 pm
12. The letter designation for the electron subshell in an atom is based on
a.
b.
c.
d.
e.
the value of the secondary quantum number, l.
the value of the principal quantum number, n.
the value of the magnetic quantum number, ml.
the value of the spin quantum number, ms.
the transverse polarization of the optical emission from the H atom.
13. The three quantum numbers which characterize the solutions to Schrodinger’s equation
describing the behavior of the electron in the H atom are usually designated as
a.
b.
c.
d.
e.
1s
n
ml
n
l
2s
l
ms
l
ml
2p
ms
mp
ml
ms
14. The notation for the subshell with n = 4 and l = 2 is
a.
b.
c.
d.
e.
4d subshell.
4p subshell.
4f subshell.
4s subshell.
There is no subshell fitting this description.
15. The notation for the subshell with n = 3 and l = 3 is
a.
b.
c.
d.
e.
3d subshell.
3f subshell.
3p subshell.
3s subshell.
There is no subshell fitting this description.
16. The maximum number of electrons required to fill all the energy levels for a shell having
principal quantum number n is
a.
b.
c.
d.
e.
n
n+1
2n
n2
2n2
17. Which of the following gives a possible quantum number assignment for the last electron
added to the sodium atom when developing the electron configuration using the aufbau
principle?
a.
b.
c.
d.
e.
n
2
3
3
3
4
l ml
1 -1
1 -1
0 0
2 +1
1 -1
ms
-½
½
½
-½
0
18. Which of the following gives a possible quantum number assignment for the last electron
added to the oxygen atom when developing the electron configuration using the aufbau
principle?
a.
b.
c.
d.
e.
n
2
3
3
3
4
l ml
1 +1
1 0
0 0
2 +1
1 -1
ms
-½
½
½
-½
0
19. Given the following sets of quantum numbers for n, l, ml, and ms, which one of these sets is
not possible for an electron in an atom?
n
a.
b.
c.
d.
e.
l
3
3
4
4
5
ml
2
1
3
4
2
ms
2 -½
-1 ½
2 ½
-3 -½
-2 ½
20. Given the following sets of quantum numbers for n, l, ml, and ms, which one of these sets is
not possible for an electron in an atom?
n
a.
b.
c.
d.
e.
l
3
3
4
4
5
ml
1
2
3
3
3
ms
-1 0
2 -½
2 ½
-2 -½
2 ½
21. Based on its expected electron configuration, element Z = 120
a.
b.
c.
d.
e.
should be an inert gas element.
should have two unpaired electrons.
should be an alkali metal.
should be an alkaline earth element.
should have four unpaired electrons.
22. The values of n for the valence shells of Sb, Ca, I, and Po are
a.
b.
c.
d.
e.
3, 4, 5, 6
5, 5, 6, 6
3, 4, 3, 6
5, 6, 5, 4
5, 4, 5, 6
23. Which of the following choices is the correct electron configuration for a sulfur atom?
3s
a.
b.
c.
d.
e.
[Ne]
[Ne]
[Ne]
[Ne]
[Ne]
↑↓
↑↓
↑
↑↓
____3p____
↑
↑↓
↑↓
↑↓
↑↓
↑ ↑
↑ ↑
↑ ↑↓
↑↓
↑↓ ↑↓
24. Which of the following choices is the correct electron configuration for a vanadium atom?
4s
a.
b.
c.
d.
[Ar]
[Ar]
[Ar]
[Ar]
↑↓
↑↓
↑
_______3d________
↑↓
↑
↑
↑
↑
↑
↑
↑
↑
↑
↑
↑
↑
↑
e. [Ar]
↑↓ ↑↓ ↑
25. Based on the aufbau principle and other applicable guiding principles, what electron
configuration would one reasonably expect to find for technetium (Z = 43)?
a.
b.
c.
d.
e.
[Kr] 4s2 3d5
[Kr] 4s2 4d5
[Kr] 4d7
[Kr] 5s2 4d5
[Kr] 5s2 5d5
26. Which configuration represents a halogen element?
a.
b.
c.
d.
e.
[Ar] 4s1 3d5
[Ar] 4s2 3d4
[Kr] 5s2 5p5 4d10
[Xe] 6s2 4f7
[Xe] 6s2 4f14 5d106p4
27. A sulfur atom has how many valence electrons?
a.
b.
c.
d.
e.
16
14
8
6
4
28. A nitrogen atom has how many valence electrons?
a.
b.
c.
d.
e.
16
12
5
6
4
29. Which statement is false?
a. The probability of finding an electron at a given point in space is equal to the
square of the amplitude of the electron wave.
b. The electron density in an orbital ends abruptly at some imaginary circumference
enclosing 90% of the electron density.
c. The p orbitals have the electron density equally distributed in two regions on
opposite sides of the nucleus.
d. All s orbitals are spherical in shape.
e. With the 2s orbital, there are certain places where the electron density drops to
zero.
30. Which atom would have the largest effective nuclear charge for its valence electrons?
a.
b.
c.
d.
e.
Li
Be
B
C
N
31. Which atom has the smallest radius?
a.
b.
c.
d.
e.
Ca
Ba
K
Mg
C
32. Which atom has the largest radius?
a.
b.
c.
d.
e.
Ca
Ba
Al
Mg
C
33. Which atom has the largest first ionization energy?
a.
b.
c.
d.
e.
Al
Sr
Ga
Cr
Fr
34. Which atom has the smallest first ionization energy?
a. Rb
b. Na
c. Al
d. Ne
e. O
35. Which atom has the most exothermic electron affinity?
a.
b.
c.
d.
e.
36.
Which atom has the most exothermic electron affinity?
a.
b.
c.
d.
e.
37.
O
He
Ga
Cr
F
Al
Sr
Ga
Cl
F
The decrease in atomic radius as one progresses from element Z = 11 to Z = 18 in the
periodic table can be attributed to
a. the increase in the principal quantum number of the outermost occupied orbital in
the atom.
b. the decrease in the principal quantum number of the outermost occupied orbital in
the atom.
c. the increase in the effective nuclear charge experienced by the electron(s) in the
outermost occupied orbital in the atom.
d. the decrease in the effective nuclear charge experienced by the electron(s) in the
outermost occupied orbital in the atom.
e. the increase in the secondary quantum number of the outermost occupied orbital
in the atom.
38. The increase in atomic radius as one progresses within the alkali metal family from element
Z = 3 to Z = 87 in the periodic table can be attributed to
a. the increase in the principal quantum number of the outermost occupied orbital in
the atom.
b. the decrease in the principal quantum number of the outermost occupied orbital in
the atom.
c. the increase in the effective nuclear charge being experienced by the electron(s) in
the outermost occupied orbital in the atom.
d. the decrease in the effective nuclear charge being experienced by the electron(s)
in the outermost occupied orbital in the atom.
e. the increase in the secondary quantum number of the outermost occupied orbital
in the atom.