Deck 7: Electronic Structure

Question 1

What is the wavelength of light with a frequency of 5.2×10¹⁴ Hz?

A) 1.7×10⁶ m
B) 1.9×10 ^{- 7} m
C) 5.8×10 ^{- 7} m
D) 3.8×10 ^{- 5} m
E) none of these

Answer 1

5.8×10 ^{- 7} m

Question 2

The threshold frequency for the photoelectric effect of a particular metal is 3.0×10¹⁴ sec ^{- 1}. When this metal is illuminated by light with a frequency of 2.0×10¹⁴ sec ^{- 1}, which of the following is true?

A) The kinetic energy of the emitted electrons is greater than those emitted by light at the threshold frequency.
B) The number of electrons emitted is greater than that emitted by light at the threshold frequency.
C) The light energy absorbed by the metal decreases the distance between atoms.
D) No electrons will be emitted due to the photoelectric effect.
E) None of these are true.

Answer 2

No electrons will be emitted due to the photoelectric effect.

Question 3

The energy of a photon of electromagnetic radiation with a wavelength of 1.0 nm is

A) 9.2×10 ^{- 13} J
B) 5.0×10 ^{- 16} J
C) 2.0×10 ^{- 16} J
D) 1.1×10 ^{- 14} J
E) none of these

Answer 3

2.0×10 ^{- 16} J

Question 4

Calculate the wavelength of light emitted when an electron in a hydrogen atom falls from the n = 4 orbit to the n = 1 orbit (R_h = 1.1×10⁷ m ^{- 1}).

A) 9.7×10 ^{- 8} m
B) 6.5×10 ^{- 7} m
C) 3.6×10 ^{- 7} m
D) 6.4×10 ^{- 6} m
E) none of these

Question 5

An argon ion laser emits light at 489 nm. What is the frequency of this radiation?

A) 147 sec ^{- 1}
B) 6.13×10⁵ sec ^{- 1}
C) 1.47×10¹¹ sec ^{- 1}
D) 6.13×10¹⁴ sec ^{- 1}
E) None of these

Question 6

One type of sunburn occurs on exposure to UV light of wavelength equal to 325 nm. What is the frequency given in sec ^{- 1} for this wavelength?

A) 1.08×10 ^{- 15} sec ^{- 1}
B) 9.23×10 ^{- 4} sec ^{- 1}
C) 9.75×10¹ sec ^{- 1}
D) 9.23×10⁵ sec ^{- 1}
E) 9.23×10¹⁴ sec ^{- 1}

Question 7

What is the energy of a photon of light that has a frequency of 2.3×10¹⁴ s ^{- 1} (h = 6.6×10 ^{- 34} J × s)?

A) 2.8×10 ^{- 18} J
B) 1.5×10 ^{- 19} J
C) 2.9×10 ^{- 48} J
D) 6.4×10 ^{- 22} J
E) none of these

Question 8

Calculate the frequency of light whose wavelength is 4.2×10 ^{- 7} meters.

A) 6.2×10¹³ s ^{- 1}
B) 7.1×10¹⁴ s ^{- 1}
C) 8.3×10¹³ s ^{- 1}
D) 1.8×10¹⁴ s ^{- 1}
E) none of these

Question 9

Calculate the frequency of light whose wavelength is 711 nm.

A) 2.80×10 ^{- 19} s ^{- 1}
B) 4.22×10¹⁴ s ^{- 1}
C) 4.22×10⁵ s ^{- 1}
D) 2.10×10⁸ s ^{- 1}
E) none of these

Question 10

The energy of a photon of electromagnetic radiation with a frequency of 1.5×10¹⁴ Hz is

A) 6.6×10 ^{- 34} J
B) 9.9×10 ^{- 20} J
C) 9.9×10 ^{- 17} J
D) 1.1×10 ^{- 14} J
E) none of these

Question 11

The distance between two adjacent peaks of a wave is known as the ____ of the wave.

A) frequency
B) wave amplitude
C) wavelength
D) velocity
E) none of these

Question 12

A certain blue light has a wavelength oF₄53 nm ( l = 453 nm). What is the energy (in Joules) of one photon of this blue light with this wavelength?

A) 9.97×10 ^{- 49} J
B) 2.99×10 ^{- 40} J
C) 1.46×10 ^{- 27} J
D) 4.37×10 ^{- 19} J
E) 6.86×10²⁶ J

Question 13

Calculate the frequency of light whose wavelength is 5.0×10 ^{- 6} meters.

A) 6.0×10¹³ s ^{- 1}
B) 2.0×10⁵ s ^{- 1}
C) 3.0×10⁸ s ^{- 1}
D) 4.0×10 ^{- 20} s ^{- 1}
E) none of these

Question 14

What is the wavelength of light with a frequency of 8.2×10¹³ s ^{- 1}?

A) 2.8×10 ^{- 5} m
B) 7.2×10 ^{- 7} m
C) 4.8×10 ^{- 7} m
D) 3.7×10 ^{- 6} m
E) none of these

Question 15

If waves are hitting the beach every 2.0 seconds and are 12 m apart, what is the velocity of the waves?

A) 6.0 m/s
B) 24 m/s
C) 18 m/s
D) 2.0 m/s
E) none of these

Question 16

How much energy does a single photon of an argon ion laser emit if the wavelength of this photon is 489 nm?

A) 4.06×10 ^{- 19} J
B) 9.74×10 ^{- 23} J
C) 4.06×10 ^{- 28} J
D) 9.74×10 ^{- 32} J
E) None of these

Question 17

Which equation below properly relates energy (E) to wavelength ( l ) given h = Plank's constant, c = speed of light, and n = frequency?

A) E = h l
B)
C)
D)
E) none of these

Question 18

The number of wave crests that pass a fixed point each second is known as the ____ of the wave.

A) frequency
B) wave amplitude
C) wavelength
D) velocity
E) none of these

Question 19

What is the energy of one photon of radiation with a wavelength of 325 nm?

A) 7.13×10 ^{- 49} J
B) 6.09×10 ^{- 37} J
C) 6.43×10 ^{- 32} J
D) 2.15×10 ^{- 31} J
E) 6.09×10 ^{- 19} J

Question 20

The frequency of a photon of electromagnetic radiation with an energy of 7.3×10 ^{- 18} J is

A) 2.7×10 ^{- 8} s ^{- 1}
B) 9.9×10¹⁹ s ^{- 1}
C) 2.0×10¹⁶ s ^{- 1}
D) 1.1×10¹⁶ s ^{- 1}
E) none of these

Question 21

What quantum number(s) provide(s) information with respect to the shape of an atomic orbital?

A) Principal quantum number, "n"
B) Angular Momentum quantum number, "l"
C) Magnetic quantum number, "m_l"
D) Electron spin quantum number, "m_s"
E) Principle and Angular Momentum quantum numbers

Question 22

What is the wavelength of an electron (mass = 9.11×10 ^{- 31} kg) moving with a velocity of 60 m/s (h = 6.6×10 ^{- 34} J × s)?

A) 2.8×10 ^{- 5} m
B) 3.6×10 ^{- 7} m
C) 1.2×10 ^{- 5} m
D) 4.2×10 ^{- 7} m
E) none of these

Question 23

Calculate the wavelength of light emitted when an electron in a He⁺ ion goes from the n = 5 shell to the n = 2 shell.

A) 2.30×10⁶ m
B) 4.34×10 ^{- 7} m
C) 1.08×10 ^{- 7} m
D) 1.52×10 ^{- 7} m
E) none of these

Question 24

Three sets of quantum numbers are given below. Choose the best answer.
I. n = 3, = 3, = 0, m s = 1 / 2
II. n = 2, = 1, = 1, m s = 1 / 2
III. n = 4, = 2, = 3, m s = - 1 / 2

A) I and II are allowed sets, III is not
B) I and III are allowed sets, II is not
C) only I is allowed
D) only II is allowed
E) none of these are allowed

Question 25

From the modern day Quantum theory of the atom, which theory postulates that the mass of the electron and its exact position cannot be deduced simultaneously and that we must be satisfied with the probability of finding the electron?

A) Pauli Exclusion Principle
B) Heisenberg uncertainty principle
C) Einstein's theory of relativity
D) Light as a particle and a wave
E) Bohr's model of the Hydrogen atom

Question 26

According to the Bohr model for a hydrogen atom, the lines on the hydrogen emission spectrum are related to what type of energy change?

A) Electronic transitions from a higher energy state to a lower energy state.
B) Electronic transitions from a lower to a higher energy state.
C) The amount of energy released during high speed collisions of hydrogen molecules.
D) The amount of energy released when hydrogen molecules are split into hydrogen atoms during an electrical discharge in a vacuum tube.
E) None of these.

Question 27

What quantum number(s) provide(s) information with respect to the spatial orientation of an atomic orbital?

A) Principal quantum number, "n"
B) Angular Momentum quantum number, "l"
C) Magnetic quantum number, "m_l"
D) Electron spin quantum number, "m_s"
E) Principle and Angular Momentum quantum numbers

Question 28

What quantum number(s) provide(s) information with respect to the size of an atomic orbital?

A) Principal quantum number, "n"
B) Angular Momentum quantum number, "l"
C) Magnetic quantum number, "m_l"
D) Electron spin quantum number, "m_s"
E) Principle and Angular Momentum quantum numbers

Question 29

What quantum number(s) is(are) required to completely describe an orbital , the region in space in which an electron has a high probability of being found?
I. Principal quantum number
II. Angular Momentum quantum number
III. Magnetic quantum number

A) I only
B) I and II
C) I and III
D) II and III
E) I, II and III

Question 30

The energy of the electron in the hydrogen atom depends on the quantum number(s)

A) n only
B) n and
C) and
D) only
E) n, and

Question 31

Three sets of quantum numbers are listed below. Pick the best answer.
I. n = 2, = 2, = 2, m s = 1 / 2
II. n = 4, = 0, = 0, m s = 1 / 2
III. n = 3, = 2, = 3, m s = 1 / 2

A) I and II are allowed sets, III is not
B) II and III are allowed sets, I is not
C) all 3 are allowed sets
D) only II is an allowed set
E) all 3 are not allowed sets

Question 32

What quantum number(s) is(are) required to completely describe a subshell , a set of orbitals with the same energy and shape?
I. Principal quantum number
II. Angular Momentum quantum number
III. Magnetic quantum number

A) I only
B) I and II
C) I and III
D) II and III
E) I, II and III

Question 33

The quantum number l for an electron in an atom is 2. This electron is definitely located in:

A) the first principal shell
B) the second principal shell
C) an s subshell
D) a p subshell
E) a d subshell

Question 34

Calculate the wavelength of light emitted when an electron in the hydrogen atom goes from the n = 4 shell to the n = 2 shell.

A) 2.06×10⁶ m
B) 4.86×10 ^{- 7} m
C) 3.65×10 ^{- 7} m
D) 4.09×10 ^{- 19} m
E) none of these

Question 35

From the restrictions on the three quantum numbers that define an orbital, which set of three quantum numbers listed below is forbidden ?

A) n = 3, = 3, = 3
B) n = 3, = 2, = - 2
C) n = 3, = 2, = +2
D) n = 3, = 1, = +1
E) n = 3, = 0, = 0

Question 36

Given the three statements below, pick the best answer.
I. c = ln
II. E = h n
III. heating gaseous Li atoms yields white light

A) II and III are true, I is false
B) I and II are true, III is false
C) I and III are true, II is false
D) all three are true
E) only I is true

Question 37

Only one set of quantum numbers listed below is a correct set. Which one?
(n, l , m _l , m_s)

A) 3, 2, 0, 1/2
B) 2, 2, - 2, 1/2
C) 3, 3, - 3, 1/2
D) 4, 4, - 3, 1/2
E) none of these

Question 38

Calculate the frequency of light emitted when an electron in a hydrogen atom goes from the n = 5 shell to the n = 2 shell.

A) 6.9×10¹⁴ s ^{- 1}
B) 8.2×10¹³ s ^{- 1}
C) 7.8×10¹⁴ s ^{- 1}
D) 1.2×10¹⁴ s ^{- 1}
E) none of these

Question 39

Given the three statements below, which answer is best?
I. Although the wavelength of light and the frequency of light can change, the energy remains constant.
II. An important consequence of quantum theory is that the energy of various electronic states for atoms are at fixed discrete levels.
III. The energy of an electronic state for a hydrogen atom is dependent only on the principal quantum number n.

A) I and II are true, III is false
B) II and III are true, I is false
C) I and III are true, II is false
D) all are true
E) all are false

Question 40

Scientists of the 19th Century found that the equation, 1/ l = R_H(1/n²₁ - 1/n²₂) (where R_H = 1.097×10⁷ m ^{- 1}, and n₁ and n₂ are whole numbers) predicts the wavelength of the lines in the emission spectrum of the H atom. This equation is properly referred to as:

A) a theory
B) a postulate
C) a law
D) a hypothesis
E) none of these

Question 41

Three sets of quantum numbers are listed below. Pick the best answer.
I. n = 3, = 3, = 2
II. n = 4, = 2, = 0
III. n = 1, = 0, = 0

A) I and II are allowed sets, III is not
B) only III is an allowed set
C) II and III are allowed sets, I is not
D) all three sets are allowed
E) only II is an allowed set

Question 42

Which set(s) of three quantum numbers is(are) permissible?
I. n = 2, = 1, and = 1
II. n = 4, = 2, and = - 2
III. n = 3, = 3, and = 0

A) I only
B) II only
C) III only
D) I and II
E) All of these.

Question 43

How many possible orientations are allowed when = 0?
(s-type sublevel; How many possible values are possible?)

A) 1
B) 2
C) 3
D) 5
E) 7

Question 44

Exhibit 7-1 Consider the shapes listed below to answer the following question(s):
I.
II.
III.
IV.
V.
Refer to Exhibit 7-1. Which of the shapes would represent one of seven possible 4f atomic orbitals?

A) I
B) II
C) III
D) IV
E) V

Question 45

From the restrictions on the three quantum numbers that define an orbital, which set of three quantum numbers listed below is forbidden?

A) n = 4, = 3, = - 2
B) n = 4, = 2, = - 2
C) n = 4, = 3, = 3
D) n = 4, = 4, = - 2
E) n = 4, = 1, = 1

Question 46

How many possible orientations are allowed when = 2?
(d-type sublevel; How many possible values are possible?)

A) 1
B) 2
C) 3
D) 5
E) 7

Question 47

The quantum number for a 3d electron is:

A) 1
B) 2
C) 3
D) 4
E) none of these

Question 48

How many possible orientations are allowed when = 1?
(p-type sublevel; How many possible values are possible?)

A) 1
B) 2
C) 3
D) 5
E) 7

Question 49

How many electrons can be placed in the subshell described by the quantum numbers n = 3, = 1?

A) 1
B) 2
C) 10
D) 6
E) none of these

Question 50

What are the possible values for 3p electrons?

A) 0, 1, 2
B) 1, 2, 3
C) - 1, 0, +1
D) - 2, 0, +1, +2
E) none of these

Question 51

Exhibit 7-1 Consider the shapes listed below to answer the following question(s):
I.
II.
III.
IV.
V.
Refer to Exhibit 7-1. Which of the shapes would represent one of three possible 2p atomic orbitals?

A) I
B) II
C) III
D) IV
E) V

Question 52

How many possible orientations are allowed when = 3?
(f-type sublevel; How many possible values are possible?)

A) 1
B) 2
C) 3
D) 5
E) 7

Question 53

How many electrons can be placed in the subshell described by the quantum numbers n = 2, = 0?

A) none
B) 2
C) 6
D) 10
E) none of these

Question 54

Which full set of four quantum numbers would be expected for the highest energy electron for a potassium atom?

A) n = 4, = 0, = 0, m s = +1/2
B) n = 4, = 1, = 1, m s = +1/2
C) n = 4, = 2, = 2, m s = +1/2
D) n = 3, = 1, = 1, m s = +1/2
E) n = 3, = 2, = 2, m s = +1/2

Question 55

The possible values of the magnetic quantum number, , of a 3d electron are:

A) 1, 2, 3
B) 0, 1, 2
C) - 2, - 1, 0, 1, 2
D) - 1, 0, 1
E) none of these

Question 56

A subshell is described by assigning values to the quantum numbers

A) n only
B) n, , and
C) n and
D) n and
E) only

Question 57

What is the order for filling the following subshells with electrons?
4d, 4f, 5s, 5p, 6s

A) 4d, 4f, 5s, 5p, 6s
B) 5s, 6s, 5p, 4d, 4f
C) 5s, 4d, 5p, 6s, 4f
D) 4d, 4f, 5p, 5s, 6s
E) 6s, 5p, 5s, 4f, 4d

Question 58

What is the order for filling the following atomic subshells?
(Lowest energy to highest energy) 4f, 5p, 5d, 6s

A) 4f < 5p < 5d < 6s
B) 6s < 5p < 5d < 4f
C) 6s < 5d < 5p < 4f
D) 4f < 5d < 5p < 6s
E) 5p < 6s < 4f < 5d

Question 59

The possible values of the magnetic quantum number, , of a 2p electron are:

A) - 1, 0, 1
B) - 2, - 1, 0, 1, 2
C) 0, 1, 2
D) 1, 2, 3
E) none of these

Question 60

What is the maximum number of electrons that can occupy a 5d sublevel?

A) 2
B) 5
C) 6
D) 10
E) 14

Question 61

Which orbital diagram for the ground state electronic configuration of a Nitrogen atom is correct?

A)
B)
C)
D)
E)

Question 62

What is the correct electronic configuration for Zirconium (Z = 40)?

A) 1s²2s²2p⁶3s²3p⁶3d¹⁰4s²4p⁶4d²5s²
B) 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d²
C) 1s²1p⁶1d¹⁰ 2s²2p⁶2d¹⁰3s²3p⁴
D) 1s²2s²3s²4s²5s²2p⁶3p⁶4p⁶3d¹⁰4d²
E) 1d²1f⁶1p¹⁰1s¹⁴2d²2f⁶

Question 63

What is the ground state electron configuration of fluorine?

A) 1s²2s²2p⁷
B) 1s²2s²2p⁵
C) 1s²2s²2p³
D) 1s²2s²3s⁵
E) none of these

Question 64

How many orbitals are present in a 3d subshell?

A) 1 orbital
B) 3 orbitals
C) 5 orbitals
D) 7 orbitals
E) 9 orbitals

Question 65

The element with a ground state electron configuration of 1s²2s²2p⁶ is

A) B
B) C
C) O
D) F
E) Ne

Question 66

Which of the following orbital diagrams for the ground state electronic configuration for a phosphorus atom is correct?

A)
B)
C)
D)
E)

Question 67

Which orbital diagram for the ground state electronic configuration of an oxygen atom is correct?

A)
B)
C)
D)
E)

Question 68

The Pauli exclusion principle:

A) allows only two electrons to occupy a given orbital.
B) requires that the spins of unpaired electrons be parallel.
C) limits the knowledge we can have concerning the simultaneous position and momentum of an electron.
D) gives the allowed energies of an electron in a hydrogen atom.
E) choices a-d are all incorrect.

Question 69

What is the correct electronic configuration for the element Manganese (Z = 25)?

A) [Ar]3d⁷
B) 1s²2s²2p⁶3s²3p⁶3d⁵4s²
C) 1s²2s²2p⁶3s²3p⁶3d⁷
D) 1s²2s²2p⁶3s²3p⁶4s²3d⁵
E) [Kr]3d⁷

Question 70

What is the ground state electron configuration of boron?

A) 1s²2s²2p³
B) 1s²2s²2p²
C) 1s²2s²2p¹
D) 1s²2s²3s¹
E) none of these

Question 71

What is the ground state electron configuration of oxygen?

A) 1s²2s²2p⁴
B) 1s²2s²2p²
C) 1s²2s²2p³
D) 1s²2s²3s⁴
E) none of these

Question 72

Which atomic subshell can hold up to 14 electrons?

A) 3d
B) 4s
C) 2p
D) 5f
E) 3p

Question 73

What is the correct electronic configuration for Nickel (Z = 28)?

A) [Ar]3d¹⁰
B) 1s²2s²2p⁶3s²3p⁶3d⁸4s²
C) 1s²2s²2p⁶3s²3p⁶3d¹⁰
D) 1s²2s²2p⁶3s²3p⁶4s²3d⁸
E) None of these

Question 74

What is the maximum number of electrons that can occupy a 5f subshell?

A) 2
B) 5
C) 6
D) 10
E) 14

Question 75

Which subshell can hold up to a total of ten electrons?

A) s-subshell
B) p-subshell
C) d-subshell
D) f-subshell
E) a and b

Question 76

What is the correct ground state electronic configuration of Lead (Z = 82)?

A) 1s²2s²2p⁶3s²3p⁶3d¹⁰4s²4p⁶4d¹⁰4f¹⁴5s²5p⁶5d¹⁰6s²6p²
B) [Xe]6s²6d¹⁰6p²
C) [Xe]6s²6f¹⁴6d¹⁰6p²
D) [Xe]6s²4f¹⁴5d¹⁰6p²
E) [Xe]6s²6p²

Question 77

Which orbital diagram for the ground state electronic configuration of a carbon atom is correct?
(Remember Hund's Rule)

A)
B)
C)
D)
E)

Question 78

The element with a ground state electron configuration of 1s²2s²2p¹ is

A) B
B) C
C) O
D) F
E) Ne

Question 79

How many electrons can occupy a single 3p_x atomic orbital ?

A) zero
B) one
C) two
D) three
E) six

Question 80

The element with a ground state electron configuration of 1s²2s²2p⁴ is

A) B
B) C
C) O
D) F
E) Ne