Deck 7: Quantum Theory and the Electronic Structure of Atoms

Question 1

Calculate the wavelength, in nanometers, of the light emitted by a hydrogen atom when its electron falls from the n = 7 to the n = 4 principal energy level. Recall that the energy levels of the H atom are given by E_n = -2.18 * 10^-18 J(1/n²)

A) 9.18 * 10^-20 nm
B) 4.45 * 10^-20 nm
C) 2.16 * 10^-6 nm
D) 2.16 * 10³ nm
E) 1.38 * 10¹⁴ nm

Answer 1

2.16 * 10³ nm

Question 2

Using the figure below, categorize electromagnetic radiation with an energy of 6.6 x 10^-16 J/photon.

A) Gamma rays
B) X rays
C) Ultraviolet
D) Infrared
E) Microwave

Answer 2

X rays

Question 3

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) 6.46 * 10^-16 J
C) 2.46 * 10^-4 J
D) 12.4 kJ
E) 246 kJ

Answer 3

246 kJ

Question 4

Using the figure below, categorize electromagnetic radiation with a wavelength of 1.0 x 10^-3 m.

A) Gamma rays
B) X rays
C) Ultraviolet
D) Infrared
E) Microwave

Question 5

Which of the following wavelengths of electromagnetic radiation has the highest energy

A) 450. nm
B) 225 nm
C) 3.50 x 10^-9 m
D) 8.40 x 10^-7 m
E) 2.50 x 10^-5 m

Question 6

Calculate the energy, in joules, required to excite a hydrogen atom by causing an electronic transition from the n = 1 to the n = 4 principal energy level. Recall that the energy levels of the H atom are given by E_n = -2.18 * 10^-18 J(1/n²)

A) 2.07 * 10^-29 J
B) 2.25 * 10^-18 J
C) 2.04 * 10^-18 J
D) 3.27 * 10^-17 J
E) 2.19 * 10⁵ J

Question 7

In the following diagram of a wave

A) (a) is amplitude and (b) is wavelength
B) (a) is frequency and (b) is amplitude
C) (a) is wavelength and (b) is frequency
D) (a) is amplitude and (b) is frequency
E) (a) is wavelength and (b) is amplitude

Question 8

Calculate the frequency of visible light having a wavelength of 686 nm.

A) 4.37 * 10¹⁴ /s
B) 4.37 * 10⁵ /s
C) 6.17 * 10¹⁴ /s
D) 2.29 * 10^-15 /s
E) 2.29 * 10^-6 /s

Question 9

Which of the following frequencies of light has the highest energy

A) 2.5 x 10¹⁰ s^-1
B) 7.0 x 10¹³ s^-1
C) 2.3 x 10¹⁴ s^-1
D) 5.0 x 10¹⁴ s^-1
E) 1.4 x 10¹⁵ s^-1

Question 10

What is the wavelength of radiation that has a frequency of 5.39 * 10¹⁴ s^-1? (c = 2.9979 * 10⁸ m/s)

A) 1.80 * 10^-3 nm
B) 556 nm
C) 618 nm
D) 6180 nm
E) 1.61 * 10²³ nm

Question 11

Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 6 to the n = 3 principal energy level. Recall that for hydrogen E_n = -2.18 * 10^-18 J(1/n²).

A) 1.82 * 10^-19 /s
B) 9.13 * 10¹³ /s
C) 2.74 * 10¹⁴/s
D) 3.65 * 10¹⁴ /s
E) 1.64 * 10¹⁵ /s

Question 12

What is the wavelength of radiation that has a frequency of 3.4 x 10¹¹ s ^-1

A) 8.8 x 10^-4 nm
B) 8.8 x 10⁵ nm
C) 8.8 x 10^-13 nm
D) 1.0 x 10¹¹ nm
E) 1.0 x 10^-9 nm

Question 13

Using the figure below, categorize electromagnetic radiation with a wavelength of 1.0 x 10^-1 m.

A) Gamma rays
B) X rays
C) Ultraviolet
D) Infrared
E) Microwave

Question 14

Calculate the frequency of visible light having a wavelength of 486 nm.

A) 2.06 * 10¹⁴ /s
B) 2.06 * 10⁶ /s
C) 6.17 * 10¹⁴ /s
D) 1.20 * 10^-15 /s
E) 4.86 * 10^-7 /s

Question 15

Using the figure below, categorize electromagnetic radiation with an energy of 6.7 x 10^-18 J/photon.

A) Gamma rays
B) X rays
C) Ultraviolet
D) Infrared
E) Microwave

Question 16

What is the energy in joules of one photon of x-ray radiation with a wavelength of 0.120 nm

A) 2.50 x 10⁹ J
B) 1.66 x 10^-24 J
C) 1.66 x 10^-33 J
D) 2.50 x 10¹⁸J
E) 1.66 x 10^-15J

Question 17

What is the energy in joules of a mole of photons associated with red light of wavelength 7.00 * 10² nm

A) 4.72 * 10^-43 J
B) 1.71 * 10⁵ J
C) 12.4 kJ
D) 256 kJ
E) 2.12 * 10⁴² J

Question 18

What is the energy in joules of one photon of microwave radiation with a wavelength 0.122 m (c = 2.9979 * 10⁸ m/s; h = 6.626 * 10^-34 J.s)

A) 2.70 * 10^-43 J
B) 5.43 * 10^-33 J
C) 1.63 * 10^-24 J
D) 4.07 * 10^-10 J
E) 2.46 * 10⁹ J

Question 19

Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level. Recall that for hydrogen E_n = -2.18 * 10 ^-18 J(1/n²).

A) 1.35 * 10^-51 /s
B) 1.03 * 10⁸ /s
C) 2.06 * 10¹⁴ /s
D) 8.22 * 10¹⁴ /s
E) 3.08 * 10¹⁵ /s

Question 20

What is the binding energy (in J/mol or kJ/mol) of an electron in a metal whose threshold frequency for photoelectrons is 2.50 * 10¹⁴ /s

A) 2.75 * 10^-43 J/mol
B) 1.66 * 10^-19 J/mol
C) 1.20 * 10^-6 J/mol
D) 99.7 kJ/mol
E) 7.22 * 10¹⁷ kJ/mol

Question 21

Calculate the wavelength of a neutron that has a velocity of 250 cm/s. (The mass of a neutron = 1.675 * 10^-24 g)

A) 1.6 pm
B) 0.016 nm
C) 0.16 nm
D) 160 nm
E) 1.6 * 10^-4 m

Question 22

Calculate the wavelength associated with a ²⁰Ne⁺ ion moving at a velocity of 2.0 * 10⁵ m/s. The atomic mass of ²⁰Ne is 19.992 amu.

A) 1.7 * 10^-40 m
B) 1.0 * 10^-18 m
C) 1.0 * 10^-16 m
D) 1.0 * 10^-13 m
E) 9.7 * 10¹² m

Question 23

Which one of the following sets of quantum numbers represents an electron with the highest energy

A) n = 3, l = 2, m_l = -2, m_s = +1/2
B) n = 4, l = 1, m_l = 0, m_s = -1/2
C) n = 4, l = 0, m_l = 0, m_s = +1/2
D) n = 5, l = 0, m_l = 0, m_s = +1/2
E) n = 4, l = 2, m_l = -1, m_s = -1/2

Question 24

List the following sets of quantum numbers in order of increasing energy:
I. n = 4, l = 0, m_l = 0, m_s = -1/2
II. n = 4, l = 2, m_l = -1, m_s = -1/2
III. n = 5, l = 0, m_l = 0, m_s = +1/2

A) I < II < III
B) II < III < I
C) III < II < I
D) I < III < II
E) III < I < II

Question 25

A single pulse of a laser yields an average of 5.00 * 10¹⁸ photons with l= 633 nm. If melting ice to water at 0 ^$\circ$ C requires 6.01 kJ/mol, what is the fewest number of laser pulses needed to melt 10.0 g of ice

A) 38300
B) 3830
C) 3340
D) 2120
E) 212

Question 26

List the following sets of quantum numbers in order of increasing energy:
I. n = 4, l = 1, m_l = 1, m_s = +1/2
II. n = 3, l = 2, m_l = -1, m_s = +1/2
III. n = 4, l = 0, m_l = 0, m_s = +1/2

A) I < II < III
B) II < III < I
C) III < II < I
D) I < III < II
E) III < I < II

Question 27

The longest wavelength of light that causes electrons to be ejected from the surface of a copper plate is 243 nm. What is the maximum velocity of the electrons ejected when light of wavelength 200. nm shines on a copper plate

A) 1.97 * 10⁴ m/s
B) 4.67 * 10⁴ m/s
C) 6.22 * 10⁵ m/s
D) 1.34 * 10⁶ m/s
E) 1.48 * 10⁶ m/s

Question 28

Calculate the wavelength of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level. Recall that for hydrogen E_n = -2.18 * 10^-18 J(1/n²).

A) 6.8 * 10^-18 nm
B) 0.612 nm
C) 82.6 nm
D) 97.2 nm
E) 365 nm

Question 29

A proton is roughly 1800 times more massive than an electron. If a proton and an electron are traveling at the same speed,

A) the wavelength of the proton will be about 1800 times longer than the wavelength of the electron.
B)the wavelength of the proton will be about $\sqrt{1800}$ times longer than the wavelength of the electron.
C) the wavelength of the proton will be roughly equal to the wavelength of the electron.
D)the wavelength of the electron will be about $\sqrt{1800}$ times longer than the wavelength of the proton.
E) the wavelength of the electron will be about 1800 times longer than the wavelength of the proton.

Question 30

Which one of the following sets of quantum numbers represents an electron with the highest energy

A) n = 2, l = 1, m_l = 0, m_s = +1/2
B) n = 3, l = 0, m_l = 0, m_s = -1/2
C) n = 2, l = 0, m_l = 0, m_s = +1/2
D) n = 3, l = 2, m_l = 1, m_s = -1/2
E) n = 3, l = 1, m_l = 1, m_s = +1/2

Question 31

A proton is roughly 1800 times more massive than an electron. If a proton and an electron have the same kinetic energy,

A) the wavelength of the proton will be about 1800 times longer than the wavelength of the electron.
B)the wavelength of the proton will be about $\sqrt{1800}$ times longer than the wavelength of the electron.
C) the wavelength of the proton will be roughly equal to the wavelength of the electron.
D)the wavelength of the electron will be about $\sqrt{1800}$ times longer than the wavelength of the proton.
E) the wavelength of the electron will be about 1800 times longer than the wavelength of the proton.

Question 32

If a hydrogen atom and a helium atom are traveling at the same speed,

A) the wavelength of the hydrogen atom will be about 4 times longer than the wavelength of the helium atom.
B) the wavelength of the hydrogen atom will be about 2 times longer than the wavelength of the helium.
C) the wavelength of the hydrogen atom will be roughly equal to the wavelength of the helium atom.
D) the wavelength of the helium atom will be about 2 times longer than the wavelength of the hydrogen atom.
E) the wavelength of the helium atom will be about 4 times longer than the wavelength of the hydrogen atom.

Question 33

Which one of the following sets of quantum numbers is not possible $\begin{array}{lccc}~~~~~\text { n } & l & \mathrm{~m}_{l} & \mathrm{~m}_{5} \\\text { A. } 4 & 3 & -2 & +1 / 2 \\\text { B. } 3 & 2 & -3 & -1 / 2 \\\text { C. } 3 & 0 & 0 & +1 / 2 \\\text { D. } 4 & 1 & 1 & -1 / 2 \\\text { E. } 2 & 0 & 0 & +1 / 2\end{array}$

Question 34

In an electron microscope, electrons are accelerated to great velocities. Calculate the wavelength of an electron traveling with a velocity of 7.0 * 10³ kilometers per second. The mass of an electron is 9.1 * 10^-28 g.

A) 1.0 * 10^-13 m
B) 1.0 * 10^-10 m
C) 1.0 * 10^-7 m
D) 1.0 m

Question 35

A common way of initiating certain chemical reactions with light involves the generation of free halogen atoms in solution. If DH for the reaction Cl₂(g) $\rarr$ 2Cl(g) is 242.8 kJ/mol, what is the longest wavelength of light that will produce free chlorine atoms in solution

A) 246.3 nm
B) 349.3 nm
C) 465.2 nm
D) 492.6 nm
E) 698.6 nm

Question 36

Which one of the following sets of quantum numbers is not possible $\begin{array}{lrrr}~~~~~\text { n } & \text { l } & \mathrm{m}_{l} & \mathrm{~m}_{\mathrm{s}} \\\text { A. } 4 & 3 & -2 & +1 / 2 \\\text { B. } 3 & 0 & 1 & -1 / 2 \\\text { C. } 3 & 0 & 0 & +1 / 2 \\\text { D. } 2 & 1 & 1 & -1 / 2 \\\text { E. } 2 & 0 & 0 & +1 / 2\end{array}$

Question 37

Electrons can be used to probe the arrangement of atoms on a solid surface if the wavelength of the electrons is comparable with the spacing between the atoms. Which of the following electron velocities would be appropriate for use in this application if the atoms are separated by 0.320 nm

A) 1.24 * 10³ m/s
B) 8.06 * 10³ m/s
C) 2.27 * 10⁶ m/s
D) 4.41 * 10⁶ m/s
E) 3.00 * 10⁸ m/s

Question 38

When photons with a wavelength of 310. nm strike a magnesium plate, the maximum velocity of the ejected electrons is 3.45 * 10⁵ m/s. Calculate the binding energy of electrons to the magnesium surface.

A) 32.7 kJ/mol
B) 321 kJ/mol
C) 353 kJ/mol
D) 386 kJ/mol
E) 419 kJ/mol

Question 39

The second line of the Balmer series occurs at a wavelength of 486.1 nm. What is the energy difference between the initial and final levels of the hydrogen atom in this emission process

A) 2.44 * 10¹⁸ J
B) 4.09 * 10^-19 J
C) 4.09 * 10^-22 J
D) 4.09 * 10^-28 J
E) 1.07 * 10^-48 J

Question 40

If a hydrogen atom and a helium atom have the same kinetic energy,

A) the wavelength of the hydrogen atom will be about 4 times longer than the wavelength of the helium atom.
B) the wavelength of the hydrogen atom will be about 2 times longer than the wavelength of the helium.
C) the wavelength of the hydrogen atom will be roughly equal to the wavelength of the helium atom.
D) the wavelength of the helium atom will be about 2 times longer than the wavelength of the hydrogen atom.
E) the wavelength of the helium atom will be about 4 times longer than the wavelength of the hydrogen atom.

Question 41

A possible set of quantum numbers to describe an electron in a 4s subshell is

A) n = 4, l = 0, m_l = 1 , m_s = +1/2
B) n = 4, l = 0, m_l = 0, m_s = - 1/2
C) n = 4, l = 1, m_l = 1, m_s = +1/2
D) n = 3, l = 1, m_l = 1, m_s = - 1/2
E) n = 3, l = 0, m_l = 0, m_s = +1/2

Question 42

"No two electrons in an atom can have the same four quantum numbers" is a statement of

A) the Pauli exclusion principle.
B) Bohr's equation.
C) Hund's rule.
D) de Broglie's relation.
E) Dalton's atomic theory.

Question 43

The orbital diagram for a ground-state oxygen atom is

Question 44

What is the maximum number of electrons in an atom that can have the following set of quantum numbers
N = 3 $~~$ l = 2 $~~$ m_l = -2

A) 18
B) 10
C) 5
D) 2
E) 1

Question 45

A possible set of quantum numbers to describe an electron in a 5p subshell is

A) n = 5, l = 2, m_l = 2 , m_s = +1/2
B) n = 4, l = 0, m_l = 0, m_s = - 1/2
C) n = 5, l = 0, m_l = 0, m_s = +1/2
D) n = 3, l = 1, m_l = 1, m_s = - 1/2
E) n = 5, l = 1, m_l = 0, m_s = +1/2

Question 46

Electrons in an orbital with l = 3 are in a/an

A) d orbital.
B) f orbital.
C) g orbital.
D) p orbital.
E) s orbital.

Question 47

How many orbitals are allowed in a subshell if l = 2

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

Question 48

What is the maximum number of electrons in an atom that can have the following quantum numbers
N = 3 $~~$ l = 1

A) 18
B) 6
C) 3
D) 2
E) 1

Question 49

Which ground-state atom has an electron configuration described by the following orbital diagram

A) phosphorus
B) germanium
C) selenium
D) tellurium
E) none of these

Question 50

A possible set of quantum numbers for the last electron added to complete an atom of gallium (Ga) in its ground state is $\begin{array}{llll}~~~~~\text { n } & l & \mathrm{~m}_{l} & \mathrm{~m}_{5} \\\text { A. } 4 & 0 & 0 & -1 / 2 \\\text { B. } 3 & 1 & 0 & -1 / 2 \\\text { C. } 4 & 1 & 0 & +1 / 2 \\\text { D. } 3 & 1 & 1 & +1 / 2 \\\text { E. } 4 & 2 & 1 & +1 / 2\end{array}$

Question 51

How many orbitals are allowed in a subshell if l = 3

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

Question 52

Which of the following electronic transitions is consistent with an increase in energy

A) From a 4s subshell to a 3d subshell
B) From a 5p subshell to a 4d subshell
C) From a 4d subshell to a 5s subshell
D) From a 4f subshell to a 6s subshell
E) From a 5d subshell to a 6s subshell

Question 53

What is the maximum number of electrons in an atom that can have the following quantum numbers
N = 3 $~~$ l = 2

A) 18
B) 10
C) 5
D) 2
E) 1

Question 54

What is the maximum number of electrons in an atom that can have the following set of quantum numbers
N = 4 $~~$ l = 3 $~~$ m_l = -2 $~~$ m_s = +1/2

A) 0
B) 1
C) 2
D) 6
E) 10

Question 55

A possible set of quantum numbers to describe an electron in a 3d subshell is

A) n = 3, l = 0, m_l = 0 , m_s = +1/2
B) n = 3, l = 1, m_l = 0, m_s = - 1/2
C) n = 3, l = 2, m_l = 1, m_s = +1/2
D) n = 3, l = 3, m_l = 1, m_s = - 1/2
E) n = 2, l = 0, m_l = 0, m_s = +1/2

Question 56

Which of the following electronic transitions is consistent with a decrease in energy

A) From a 5s subshell to a 4d subshell
B) From a 4f subshell to a 5p subshell
C) From a 6s subshell to a 5d subshell
D) From a 5s subshell to a 5p subshell
E) From a 4f subshell to a 6p subshell

Question 57

The orbital diagram for a ground-state nitrogen atom is

Question 58

A possible set of quantum numbers for the last electron added to complete an atom of germanium (Ge) in its ground state is $\begin{array}{cccc}~~~~~\text { n } & l & \mathrm{~m}_{l} & \mathrm{~m}_{\mathrm{s}} \\\text { A. } 4 & 0 & 0 & +1 / 2 \\\text { B. } 3 & 0 & +1 & -1 / 2 \\\text { C. } 4 & 1 & -1 & +1 / 2 \\\text { D. } 3 & 1 & +1 & -1 / 2 \\\text { E. } 4 & 2 & +2 & -1 / 2\end{array}$

A) A
B) B
C) C
D) D
E) E

Question 59

The orbital diagram for a ground state carbon atom is

Question 60

What is the maximum number of electrons in an atom that can have the following set of quantum numbers
N = 3 $~~$ l = 1 $~~$ m_l = -1

A) 18
B) 6
C) 3
D) 2
E) 1

Question 61

Which ground-state atom has an electron configuration described by the following orbital diagram

A) antimony
B) germanium
C) indium
D) lead
E) tin

Question 62

Which element has the following ground-state electron configuration
1s²2s²2p⁶3s²

A) Na
B) Mg
C) Al
D) Si
E) Ne

Question 63

Which of the following is the ground-state electron configuration of Pb

A) [Xe]6s²5d¹⁰6p²
B) [Xe]6s²6d¹⁰6p²
C) [Xe]6s²4f¹⁴6p²
D) [Xe]6s²5f¹⁴6d¹⁰6p²
E) [Xe]6s²4f¹⁴5d¹⁰6p²

Question 64

A ground-state atom of manganese has ___ unpaired electrons and is _____.

A) 0, diamagnetic
B) 2, diamagnetic
C) 3, paramagnetic
D) 5, paramagnetic
E) 7, paramagnetic

Question 65

A ground-state atom of iron has ___ unpaired electrons and is _____.

A) 0, diamagnetic
B) 6, diamagnetic
C) 3, paramagnetic
D) 5, paramagnetic
E) 4, paramagnetic

Question 66

Transition metal elements have atoms or ions with partially filled

A) s subshells.
B) p subshells.
C) d subshells.
D) f subshells.
E) g subshells.

Question 67

Which element has the following ground-state electron configuration
[Kr]5s¹4d⁵

A) Mn
B) Mo
C) Nb
D) Re
E) Tc

Question 68

The electron configuration of a ground-state copper atom is

A) [Ar]4s²4d⁴.
B) [Ar]4s²4p⁶3d³.
C) [Ar]4s²3d⁹.
D) [Ar]3d⁹.
E) [Ar]4s¹3d¹⁰.

Question 69

Which element has the following ground-state electron configuration
[Xe]6s²4f¹⁴5d⁴

A) W
B) Pm
C) Mo
D) Np
E) Re

Question 70

The electron configuration of a ground-state vanadium atom is

A) [Ar]4s²4d³.
B) [Ar]4s²4p³.
C) [Ar]4s²3d³.
D) [Ar]3d⁵.

Question 71

The electron configuration of a ground-state Co atom is

A) [Ar]4s²3d⁷.
B) 1s²2s²2p⁶3s²3d⁹.
C) [Ne]3s²3d⁷.
D) [Ar]4s¹3d⁵.
E) [Ar]4s²4d⁷.

Question 72

Which ground-state atom has an electron configuration described by the following orbital diagram

A) phosphorus
B) nitrogen
C) arsenic
D) vanadium
E) none of these

Question 73

How many unpaired electrons does an atom of carbon have in its ground state

A) 0
B) 1
C) 2
D) 3
E) 4

Question 74

Which element has the following ground-state electron configuration
[Ar]4s²3d¹⁰4p⁵

A) arsenic
B) bromine
C) iodine
D) selenium
E) tellurium

Question 75

A ground-state atom of vanadium has ___ unpaired electrons and is _____.

A) 0, diamagnetic
B) 2, diamagnetic
C) 3, paramagnetic
D) 5, paramagnetic
E) 4, diamagnetic

Question 76

Which element has the following ground-state electron configuration
[Kr]5s²4d¹⁰5p³

A) Sn
B) Sb
C) Pb
D) Bi
E) Te

Question 77

Which of the following is the ground-state electron configuration of Ir

A) [Xe]6s²5d⁷
B) [Xe]6s²6d⁷
C) [Xe]6s²4f¹⁴5d⁷
D) [Xe]6s²5f¹⁴6d⁷
E) [Xe]4s²5f¹⁴6d⁷

Question 78

The ground-state electron configuration for an atom of indium is

A) [Kr]5s²4p⁶4d⁵.
B) [Ar]4s²3d¹⁰4p¹.
C) [Ar]4s²4p⁶3d⁵.
D) [Kr]5s²5p⁶4d⁵.
E) [Kr]5s²4d¹⁰5p¹.

Question 79

Which element has the following ground-state electron configuration
[Xe]6s²4f¹⁴5d¹⁰

A) Lu
B) Cd
C) Hg
D) Lr
E) Au

Question 80

How many unpaired electrons does an atom of sulfur have in its ground state

A) 0
B) 1
C) 2
D) 3
E) 4