Common Exam 2 Chapter 7 Learning Objectives and Review Questions
Chapter 7: Atomic Structure and Periodicity
1. Nature of light
a. The electromagnetic spectrum
b. Photoelectric effect
c. Constructive and destructive interference
2. Bohr Model
a. Line spectra
b. Wavelike behavior of electrons, de Broglie equation, uncertainty
principle
c. State v. Path functions
d. Intensive v. extensive variables
3. Schrodinger model for the Hydrogen atom
a. Quantum numbers and their relevance
Common Exam 2 is up to Quantum numbers (Where we reached in class)
Chapter 7: Questions
1. What is the frequency of light having a wavelength of 681 nm?
Solution
C= λ ν
C is speed of light
λ is wavelength
ν is frequency
C = 2.998 x108 ms-1
Wavelength (λ) = 681 nm = 681 nm x1m/109 nm= 6.81 x10-7 m
ν=
𝐶
𝜆
=
2.998 𝑥108 𝑚/𝑠
681 𝑥 10−9 𝑚
= (2.998 x108 ms-1)/ (6.81x10-7 m)
ν = 4.402 x 1014 s-1 = 4.402 x 1014 Hz
2. What is the frequency (ν, in Hz) of the photons emitted by a He–Ne laser
with a wavelength (λ) of 632.8 nm?
A) 4.741 x 105 Hz
B) 1.897 x 102 Hz
C) 1.897 x 1011 Hz
D) 4.741 x 1014 Hz
E) 1.897 x 1014 Hz
3. Which transition in a hydrogen atom requires the largest change in energy?
A) n1 = 2 to n2 = 3
B) n1 = 2 to n2 = 4
C) n1 = 1 to n2 = 3
D) n1 = 1 to n2 = 2
E) n1 = 9 to n2 = 10
4. Which of the following is a possible set of quantum numbers for a 3d
orbital?
A) n = 3, l = 1, ml = 2
B) n = 3, l = 2, ml = 3
C) n = 3, l = 2, m l = 0
D) n = 3, l = 0, ml = 0
E) n = 3, l = 1, ml = –1
5. What is the maximum number of electrons in an atom that can have the
following quantum numbers: n=4, l=3?
A. 2
B. 6
C. 10
D. 14
E. 1
6. What is the energy in joules of a mole of photons associated with visible
light of wavelength 486 nm?
A. 6.46 × 10–25 J
B. 1.24 × 105 J
C. 6.46 × 10–16 J
D. 2.46 × 10–4 J
E. 2.46 × 105 J
E=
ℎ𝑐
λ
7. Which of the following involves the emission of a photon with longest
wavelength? Use the following energy-level information for hydrogen:
n=4
–0.1361 × 10–18 J
n=3
–0.2420 × 10–18 J
n=2
–0.5445 × 10–18 J
n=1
–2.178 × 10–18 J
A. n=4  n=3
B. n=3  n=1
C. n=2  n=1
D. n=3  n=4
E. n=4  n=1
8. Which orbital can be described by the following quantum numbers?
n= 3, l = 1, ml =0
A. 3p
B. 3s
C. 3d
D. 3f
E. 1s
9. Which of the set of four quantum numbers does not specify an orbital in the
Hydrogen atom?
A. n = 5, l = 2, ml = -2, ms = +½
B. n = 4, l = 1, ml = 0, ms = 1
Remember ms = +½ or -½
C. n = 4, l = 0, ml = 0, ms = +½
D. n = 5, l = 0, ml = 0, ms = +½
E. n = 3, l = 2, ml = -1, ms = -½
10.The emission spectra of hydrogen best supports the idea that:
A. Electrons have wave-like properties
B. Electrons exist in quantized energy levels
C. Electrons are negatively charged
D. Electrons have particle like behaviour
E. Electrons exist in the space around the nucleus
11.Which wavelength of light has the highest energy?
A. 10 mm
B. 100 μm
C. 100 mm
D. 1 m
E. 10 nm
𝒉𝒄
Remember E =
Hence the smallest wavelength (λ) will yield the
𝛌
highest energy. Nanometer scale is the smallest I nm =10-9 m
12.How many orbitals are there in the set of quantum where n = 4 and l = 1?
A. 6
B. 5
C. 3
D. 7
E. 9
13.What is the wavelength of light emitted when the electron in a hydrogen
atom undergoes a transition from level n = 9 to level n = 4?
A. 5.49 x 105 m
B. 1.09 x 10-19 m
C. 1.65 x 1014 m
D. 3.64 x 10-28 m
E. 1.82 x 10-6 m
14.Which of the following is NOT an allowed set of quantum numbers?
A. n = 4 l = 3 ml = 3
B. n = 1 l = 0 ml = 0
C. n = 5 l = 4 ml = -2
D. n = 2 l = 1 ml = 0
E. n = 3 l = 3 ml = -2
15.What is the energy (E, in J) of the photons emitted by an Ar+ laser with a
wavelength of λ = 488 nm?
A) 2.46 x 1018 J
B) 9.69 x 10–23 J
C) 1.36 x 10–36 J
D) 4.07 x 10–19 J
E) 2.46 x 10–18 J