Deck 6: Quantum Theory and the Electronic Structure of Atoms

Question 1

In the ________, electrons are ejected from the surface of a metal exposed to light of a certain minimum frequency.

A) aura effect
B) photon effect
C) ritzwald effect
D) photoelectric effect
E) None of the answers is correct.

Answer 1

photoelectric effect

Question 2

What is the energy in joules of a mole of photons associated with red light of wavelength 7.00 × 10² nm? (c = 3.00 × 10⁸ m/s; h = 6.63 × 10^-34 J • s; N_A = 6.022 × 10²³ /mole)

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

Answer 2

1.71 × 10⁵ J

Question 3

Select the arrangement of electromagnetic radiation which starts with the shortest wavelength and increases to longest wavelength.

A) radio, infrared, ultraviolet, gamma rays
B) radio, ultraviolet, infrared, gamma rays
C) gamma rays, radio, ultraviolet, infrared
D) gamma rays, infrared, radio, ultraviolet
E) gamma rays, ultraviolet, infrared, radio

Answer 3

gamma rays, ultraviolet, infrared, radio

Question 4

When a solid is heated, it emits electromagnetic radiation known as ________. An example of such radiation is the element of a stove stop burning bright red.

A) isoelectric radiation
B) visible and ultraviolet radiation
C) blackbody radiation
D) paramagnetic radiation
E) whitebody radiation

Question 5

What is defined as the vertical distance from the midline of a wave to the top of the peak or the bottom of the trough?

A) light
B) amplitude
C) magnitude
D) wavelength
E) frequency

Question 6

What is the frequency of electromagnetic radiation with wavelength 532 nm? (c = 3.00 × 10⁸ m/s)

A) 5.64 × 10¹⁴ s^-1
B) 6.48 × 10¹² s^-1
C) 4.18 × 10¹⁸ s^-1
D) 6.23 × 10¹⁴ s^-1
E) 3.75 × 10¹⁵ s^-1

Question 7

What is defined as the number of waves that pass through a particular point in one second?

A) light
B) amplitude
C) magnitude
D) wavelength
E) frequency

Question 8

Calculate the frequency of visible light having a wavelength of 686 nm. (c = 3.00 × 10⁸ m/s)

A) 4.37 × 10¹⁴ s^-1
B) 4.34 × 10⁵ s^-1
C) 6.17 × 10¹⁴ s^-1
D) 2.29 × 10^-15 s^-1
E) 2.29 × 10^-6 s^-1

Question 9

The FM station KDUL broadcasts music at 99.1 MHz. Find the wavelength of these waves. (c = 3.00 × 10⁸ m/s)

A) 1.88 × 10^-2 m
B) 0.330 m
C) 3.03 m
D) 5.33 × 10² m
E) > 10³ m

Question 10

What is the frequency of light having a wavelength of 360 nm? (c = 3.00 x 108 m/s)

A) 8.3 × 10¹⁴ s^-1
B) 1.2 × 10^-6 s^-1
C) 8.3 × 10⁵ s^-1
D) 108 s^-1
E) 1.2 × 10^-15 s^-1

Question 11

What is the wavelength of light having a frequency of 4.8 × 10¹⁴ s^-1? (c = 3.00 x 10⁸ m/s)

A) 0.0016 nm
B) 1600 m
C) 630 nm
D) 1600 nm
E) 6.3 × 10^-7 nm

Question 12

Select the arrangement of electromagnetic radiation which starts with the lowest energy and increases to the greatest energy.

A) radio, infrared, ultraviolet, gamma rays
B) radio, ultraviolet, infrared, gamma rays
C) gamma rays, infrared, radio, ultraviolet
D) gamma rays, ultraviolet, infrared, radio
E) infrared, ultraviolet, radio, gamma rays

Question 13

A(n) ________ is a point at which a standing wave has zero amplitude.

A) crevice
B) node
C) pit
D) burrow
E) orbital

Question 14

What is the wavelength of radiation that has a frequency of 6.912 × 10¹⁴ s^-1? (c = 3.00 × 10⁸ m/s)

A) 1.447 × 10^-15 nm
B) 4.337 × 10² nm
C) 2.304 × 10⁶ nm
D) 2.074 × 10²³ nm
E) 4.337 × 10^-7 nm

Question 15

What is defined as the distance between identical points on successive waves?

A) frequency
B) amplitude
C) magnitude
D) wavelength
E) light

Question 16

Visible light, radio waves, microwave radiation, infrared, ultraviolet radiation, X-rays, and gamma rays all constitute the electromagnetic spectrum. Which of the following characteristics do all of these kinds of radiation share?

A) They all have the ability to generate heat in objects.
B) They all have the same frequencies.
C) They are all the transmission of energy in the form of waves.
D) They have equal energies.
E) They have the same electron spin state.

Question 17

What is the energy in joules of a mole of photons associated with visible light of wavelength 486 nm? (c = 3.00 × 10⁸ m/s; h = 6.63 × 10^-34 J • s; N_A = 6.022 × 10²³ moles^-1)

A) 6.46 × 10^-16 J
B) 6.46 × 10^-25 J
C) 2.46 × 10^-4 J
D) 12.4 kJ
E) 246 kJ

Question 18

According to scientist James Clerk Maxwell in the year 1873, a(n) ________ consists of an electric field component and a magnetic field component.

A) electrostatic wave
B) isoelectric wave
C) atom
D) paramagnetic wave
E) electromagnetic wave

Question 19

The solar radiation spectrum peaks at a wavelength of approximately 500 nm. Calculate the energy of one photon of that radiation (c = 3.00 × 10⁸ m/s; h = 6.63 × 10^-34 J • s).

A) 4 × 10^-10 J
B) 6 × 10¹⁴ J
C) 1 × 10^-27 J
D) 2 × 10^-25 J
E) 4 × 10^-19 J

Question 20

A radio wave has a frequency of 8.6 × 10⁸ Hz. What is the energy of one photon of this radiation? (h = 6.63 × 10^-34 J • s)

A) 7.7 × 10^-43 J
B) 2.3 × 10^-34 J
C) 5.7 × 10^-25 J
D) 1.7 × 10^-16 J
E) > 10^-15 J

Question 21

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 ). (h = 6.63 × 10^-34 J • s)

A) 3.08 × 10¹⁵ s^-1
B) 1.03 × 10⁸ s^-1
C) 2.06 × 10¹⁴ s^-1
D) 1.35 × 10^-51 s^-1
E) 8.22 × 10¹⁴ s^-1

Question 22

The de Broglie equation predicts that the wavelength (in m) of a proton moving at 1000. m/s is ________. (h = 6.63 × 10^-34 J • s; mass of a proton = 1.673 × 10^-24 g)

A) 3.96 × 10^-10 m
B) 3.96 × 10^-7 m
C) 2.52 × 10⁶ m
D) 2.52 × 10⁹ m
E) > 10¹⁰ m

Question 23

Calculate the de Broglie wavelength associated with a ²⁰Ne⁺ ion moving at a velocity of 2.0 × 10⁵ m/s. The atomic mass of Ne-20 is 19.992 amu. (1 amu = 1.66 × 10^-24 g and h = 6.63 × 10^-34 J • s)

A) 1.0 × 10^-13 m
B) 1.0 × 10^-16 m
C) 1.0 × 10^-18 m
D) 9.7 × 10¹² m
E) 2.0 × 10^-13 cm

Question 24

Which scientist proposed that energy of radiation is composed of extremely small indivisible packages called quanta? ("Quanta" is the plural of "quantum.")

A) Max Planck
B) Louis de Broglie
C) Clinton Davisson
D) Sir Isaac Newton
E) Lothan Meyer

Question 25

What is the emission of light at only specific wavelengths?

A) Emission spectra
B) Hydrogen spectrum
C) Wave spectra
D) Limited spectra
E) Line spectra

Question 26

A photon has an energy of 5.53 × 10^-17 J. What is its frequency in s^-1 (h = 6.63 × 10^-34 J • s)?

A) 3.66 × 10^-50 s^-1
B) 1.20 × 10^-17 s^-1
C) 3.59 × 10^-9 s^-1
D) 2.78 × 10⁸ s^-1
E) 8.34 × 10¹⁶ s^-1

Question 27

The orientation in space of an atomic orbital is associated with

A) the principal quantum number (n).
B) the angular momentum quantum number (l).
C) the magnetic quantum number (m_l).
D) the spin quantum number (m_s).
E) none of these choices is correct.

Question 28

Use the Rydberg equation to calculate the frequency of a photon absorbed when the hydrogen atom undergoes a transition from n₁ = 2 to n₂ = 4. (R = 1.096776 × 10⁷ m^-1; c = 3.00 × 10⁸ m/s)

A) 2.06 × 10⁶ s^-1
B) 2.74 × 10⁶ s^-1
C) 6.17 × 10¹⁴ s^-1
D) 8.23 × 10¹⁴ s^-1
E) > 10¹⁵ s^-1

Question 29

The word ________ is used as an acronym for the amplification of light which is stimulated by the emission of radiation.

A) beam
B) laser
C) emit
D) brighten
E) light

Question 30

If the energy of a photon is 1.32 × 10^-18 J, what is its wavelength in nm (c = 3.00 × 10⁸ m/s; h = 6.63 × 10^-34 J • s)?

A) 1.51 × 10^-7 nm
B) 151 nm
C) 1.99 × 10¹⁵ nm
D) 1.99 × 10²⁴ nm
E) None of these choices is correct.

Question 31

Atomic orbitals developed using quantum mechanics

A) describe regions of space in which one is most likely to find an electron.
B) describe exact paths for electron motion.
C) give a description of the atomic structure which is essentially the same as the Bohr model.
D) allow scientists to calculate an exact volume for the hydrogen atom.
E) are in conflict with the Heisenberg uncertainty principle.

Question 32

The shape of an atomic orbital is associated with

A) the principal quantum number (n).
B) the angular momentum quantum number (l).
C) the magnetic quantum number (m_l).
D) the spin quantum number (m_s).
E) the magnetic and spin quantum numbers, together.

Question 33

Calculate the de Broglie wavelength of a neutron that has a velocity of 200. cm/s. (mass of a neutron = 1.675 × 10^-27 kg and h = 6.63 × 10^-34 J • s)

A) 1.98 × 10^-9 m
B) 216 nm
C) 1.8 × 10⁵⁰ m
D) 198 nm
E) 5.05 mm

Question 34

The size of an atomic orbital is associated with

A) the principal quantum number (n).
B) the angular momentum quantum number (l).
C) the magnetic quantum number (m_l).
D) the spin quantum number (m_s).
E) the angular momentum and magnetic quantum numbers, together.

Question 35

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) 2.19 × 10⁵ J
C) 2.04 × 10^-18 J
D) 3.27 × 10^-17 J
E) 2.25 × 10^-18 J

Question 36

According to the Heisenberg uncertainty principle, if the uncertainty in the speed of an electron is 3.5 × 10³ m/s, the uncertainty in its position (in m) is at least ________. (mass of an electron = 9.11 × 10^-28 g)

A) 1.7 × 10^-8 m
B) 6.6 × 10^-8 m
C) 17 m
D) 66 m
E) None of these choices is correct.

Question 37

The energy of an electron in the hydrogen atom is determined by

A) the principal quantum number (n) only.
B) the angular momentum quantum number (l) only.
C) the principal and angular momentum quantum numbers (n & l).
D) the principal and magnetic quantum numbers (n & m_l).
E) the principal, angular momentum, and magnetic quantum numbers.

Question 38

Line spectra from all regions of the electromagnetic spectrum, including the Paschen series of infrared lines for hydrogen, are used by astronomers to identify elements present in the atmospheres of stars. Calculate the wavelength of the photon emitted when the hydrogen atom undergoes a transition from n = 5 to n = 3. (R = 1.096776 × 10⁷ m^-1)

A) 205.1 nm
B) 384.6 nm
C) 683.8 nm
D) 1282 nm
E) > 1500 nm

Question 39

A sprinter must average 24.0 mi/h to win a 100-m dash in 9.30 s. What is his de Broglie wavelength at this speed if his mass is 84.5 kg ? (h = 6.63 × 10^-34 J • s)

A) 7.31 × 10^-37 m
B) 3.26 × 10^-37 m
C) 5.08 × 10^-30 m
D) 1.34 × 10^-30 m
E) None of these choices is correct.

Question 40

Calculate the wavelength, in nanometers, of the light emitted by a hydrogen atom when its electron drops 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). (c = 3.00 × 10⁸ m/s; h = 6.63 × 10^-34 J • s)

A) 4.45 × 10^-20 nm
B) 2.16 × 10^-6 nm
C) 9.18 × 10^-20 nm
D) 1.38 × 10¹⁴ nm
E) 2.17 × 10³ nm

Question 41

Which of the following is a correct set of quantum numbers for an electron in a 5f orbital?

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

Question 42

What type of configuration specifies the arrangement of electrons in the orbitals of an atom?

A) Heisenberg configuration
B) Nuclear configuration
C) Atomic configuration
D) Proton configuration
E) Electron configuration

Question 43

The maximum number of electrons that can occupy an energy level described by the principal quantum number, n, is

A) n.
B) n + 1.
C) 2n.
D) 2n²_.
E) n²_.

Question 44

A possible set of quantum numbers for the last electron added to complete an atom of gallium (Ga) in its ground state is

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

Question 45

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 46

The Pauli exclusion principle states that no ________ electrons within an atom can have the same ________ quantum numbers.

A) 4; 6
B) 2; 4
C) 3; 6
D) 6; 10
E) 3; 8

Question 47

In the quantum mechanical treatment of the hydrogen atom, which one of the following combinations of quantum numbers is not allowed?

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

Question 48

Atomic orbitals that have the same amount of energy are ________.

A) regenerative
B) negatively charged
C) degenerate
D) positively charged
E) zwitterionic

Question 49

The number of orbitals in a d subshell is

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

Question 50

Which of the following is a correct set of quantum numbers for an electron in a 3d orbital?

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

Question 51

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 52

________ is the wavelength associated with a moving particle.

A) The de Broglie wavelength
B) The Heisenburg wavelength
C) The Hund wavelength
D) The Aufbau wavelength
E) None of the answers is correct.

Question 53

Hund's rule states that the most stable arrangement of electrons in orbitals of equal energy is the one in which the number of electrons with parallel spin is ________.

A) minimized
B) nullified
C) neutral
D) maximized
E) not relevant

Question 54

Which one of the following sets of quantum numbers is not possible?

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

Question 55

How many orbitals are allowed in a subshell if the angular momentum quantum number for electrons in that subshell is 3?

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

Question 56

Which one of the following sets of quantum numbers is not possible?

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

Question 57

A possible set of quantum numbers for the last electron added to complete an atom of germanium in its ground state is

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

Question 58

Which one of the following sets of quantum numbers can correctly represent a 3p orbital?

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

Question 59

The most stable arrangement of electrons in orbitals of equal energy is the one in which the number of electrons with the same spin is maximized is

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

Question 60

"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 61

The electronic structure 1s²2s²2p⁶3s²3p⁶4s²3d⁸ refers to the ground state of

A) Kr.
B) Ni.
C) Fe.
D) Pd.
E) None of these choices is correct.

Question 62

Select the correct electron configuration for Cu (Z = 29).

A) [Ar]4s²3d⁹
B) [Ar]4s¹3d¹⁰
C) [Ar]4s²4p⁶3d³
D) [Ar]4s²4d⁹
E) [Ar]5s²4d⁹

Question 63

How many unpaired electrons does a ground-state atom of sulfur have?

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

Question 64

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

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

Question 65

Select the correct electron configuration for sulfur (Z = 16).

A) 1s²1p⁶2s²2p⁶
B) 1s²2s²2p⁸3s²3p⁴
C) 1s²2s²2p⁸3s²3p²
D) 1s²2s²2p⁶3s²3p⁴
E) 1s²2s²2p⁶3s²3d⁴

Question 66

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

A) phosphorus
B) nitrogen
C) arsenic
D) vanadium
E) sulfur

Question 67

Which element has the following ground-state electron configuration? [Kr]5s²4d¹⁰5p²

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

Question 68

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

A) phosphorus
B) germanium
C) selenium
D) tellurium
E) potassium

Question 69

How many orbitals are there in the n = 4 level of the H-atom?

A) 4
B) 6
C) 8
D) 16
E) 18

Question 70

Which element has the following ground-state electron configuration? 1s² 2s² 2p⁶ 3s²

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

Question 71

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 72

The orbital diagram for a ground-state carbon atom is

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

Question 73

The ground-state electron configuration of a calcium atom is

A) [Ne]3s²_.
B) [Ne]3s²3p⁶_.
C) [Ar]4s¹3d¹_.
D) [Ar]4s²_.
E) [Ar]3d²_.

Question 74

The electron configuration of a ground-state vanadium atom is

A) [Ar]4s²4d³_.
B) [Ar]4s²4p³_.
C) [Ar]4s²3d³_.
D) [Ar]3d⁵_.
E) [Ar]4s²3d⁷_.

Question 75

The orbital diagram for a ground-state nitrogen atom is

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

Question 76

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 77

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 78

Select the correct electron configuration for Te (Z = 52).

A) [Kr]5s²5p⁶4d⁸
B) [Kr]5s²5d¹⁰5p⁴
C) [Kr]5s²4d¹⁰5p⁶
D) [Kr]5s²4f¹⁴
E) [Kr]5s²4d¹⁰5p⁴

Question 79

What is the correct electron configuration for a germanium (Ge) atom?

A) 1s²2s²2p⁶3s²3p⁶4s²4p²
B) 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p²
C) 1s²2s²2p⁶3s²3p²
D) 1s²2s²3s²3p⁵
E) None of the answers is correct.

Question 80

The orbital diagram for a ground-state oxygen atom is

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