Deck 6: Quantum Theory and the Electronic Structure of Atoms

Question 1

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

Answer 1

5.7 × 10^-25 J

Question 2

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

Answer 2

electromagnetic wave

Question 3

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

Answer 3

amplitude

Question 4

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 5

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 6

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; NA = 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 7

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 8

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

Question 9

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 10

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

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

Question 11

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.

Question 12

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

Question 13

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 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

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 16

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 17

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 18

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

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

Question 19

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 20

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 21

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 22

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 23

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 (ml).
D)the spin quantum number (ms).
E)the angular momentum and magnetic quantum numbers,together.

Question 24

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 25

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 En = -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 26

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 En = -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 × 10^{14 s-1}
D)1.35 × 10^{-51 s-1}
E)8.22 × 10^{14 s-1}

Question 27

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 28

Calculate the 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 29

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 30

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 31

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 32

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 En = -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 33

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 & ml).
E)the principal,angular momentum,and magnetic quantum numbers.

Question 34

A sprinter must average 24.0 mi/h to win a 100-m dash in 9.30 s.What is his 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 35

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 36

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 (ml).
D)the spin quantum number (ms).
E)the magnetic and spin quantum numbers,together.

Question 37

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 38

Calculate the 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 39

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 (ml).
D)the spin quantum number (ms).
E)none of these choices is correct.

Question 40

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 41

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 42

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

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

Question 43

How many electrons are there in the 3^rd principal energy level (n = 3)of a phosphorus atom?

A)3
B)5
C)6
D)8
E)10

Question 44

How many electrons are there in the 2^nd principal energy level (n = 2)of a phosphorus atom?

A)3
B)5
C)6
D)8
E)10

Question 45

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 46

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 47

"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 48

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 49

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 50

___________________ 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 51

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

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

Question 52

How many electrons are in the 4p orbitals of selenium?

A)0
B)2
C)4
D)5
E)6

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

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

Question 55

Atomic orbitals that have the same amount of energy are ______________.
A.regenerative
B.negatively charged
C.degenerate
D.positively charged
E.zwitterionic

Question 56

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 57

How many electrons are in the 4p orbitals of vanadium?

A)0
B)2
C)4
D)5
E)6

Question 58

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 59

How many electrons are in the 4d orbitals of Tc?

A)1
B)2
C)3
D)4
E)5

Question 60

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 61

What wavelength,in nm,can strike a metal surface and eject an electron at 1.89 × 10^-19 J if the binding energy of the metal is 289 kJ/mol?

A)1.89 × 10^-19 nm
B)2.75 nm
C)189 nm
D)290 nm
E)297 nm

Question 62

De Broglie explained electron movements by relating them to
A.waves only.
B.particles only.
C.waves and particles.
D.none of the.

Question 63

What element is represented by the electron configuration 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s¹4d¹⁰?

A)Ag
B)Rb
C)Cd
D)Sr
E)Cu

Question 64

The principal quantum number designates the size of the orbital.

Question 65

What is the electron configuration for tungsten?

A)1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s²4f¹⁴5d⁶
B)1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s¹4f¹⁴5d⁵
C)1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s²4f¹⁴5d⁴
D)1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s²4f¹⁴5d⁷
E)1s²2s²2p⁶3s²3p⁵4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s²4f¹⁴5d⁷

Question 66

Which of the following elements has the largest number of unpaired electrons in the ground state?

A)K
B)V
C)S
D)Si
E)Cl

Question 67

Which is the correct electron configuration for gold?

A)[Xe]4f¹⁴5d⁹6s²
B)"[Xe]4f¹⁴5d¹⁰6s¹"
C)[Xe]4f¹³5d¹⁰6s²
D)[Xe]4f¹⁴5d¹⁰6s¹
E)None of the electron configurations is correct.

Question 68

The frequency of a photon is inversely proportional to the wavelength of the radiation.

Question 69

What element is represented by the electron configuration 1s²2s²2p⁶3s²3p⁶4s¹3d⁵?

A)Mn
B)Ca
C)K
D)Cr
E)V

Question 70

A neutral atom in its ground state contains 28 electrons.This element is considered a __________ element,and has _______ electrons in orbitals with l = 2.

A)main group,8
B)actinide,10
C)main group,10
D)transition,10
E)transition,8

Question 71

What is the electron configuration for bromine?

A)1s²2s²2p⁶3s²3p⁶4s¹4d¹⁰4p⁶
B)1s²2s²2p⁶3s²3p⁶4s²4d¹⁰4p⁵
C)1s²2s²2p⁶3s²3p⁶4s¹3d¹⁰4p⁶
D)1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁴
E)1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁵

Question 72

List the following types of radiation from lowest frequency to highest frequency: microwave,X ray,ultraviolet,visible,and infrared

A)microwave < infrared < visible < ultraviolet < X ray
B)X ray < ultraviolet < visible < infrared < microwave
C)visible < ultraviolet < microwave < X ray < infrared
D)infrared < X ray < microwave < ultraviolet < visible
E)infrared < visible < microwave < ultraviolet < X ray

Question 73

What is the electron configuration for silicon?

A)1s²2s²2p⁶3s¹3p³
B)1s²2s²2p⁶3s²3p²
C)1s²2s²2p⁶3s⁴
D)1s²2s²2p⁶3p⁴
E)1s²2s²2p⁶3s²3p³

Question 74

An atom in its ground state contains 33 electrons.How many of these electrons are in p orbitals?

A)15
B)12
C)3
D)33
E)None of the

Question 75

Which of the following subshells has the highest energy in the element tantalum?

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

Question 76

The unusual electron configuration of Mo indicates the

A)unusual stability of half-filled d-orbitals.
B)unpredictability of the electron filling patterns of the non-representative elements.
C)unusually large size of Mo atoms.
D)greater than expected electronegativity of Mo.

Question 77

If one s orbital were combined with one p orbital (dumbbell shaped),which would best describe the resulting shape?

A)spherical
B)mostly spherical,slightly dumbbell
C)an equal ratio of spherical and dumbbell
D)slightly spherical,mostly dumbbell
E)mostly dumbbell

Question 78

The energy of a photon is directly proportional to the wavelength of the radiation.

Question 79

Emission spectra

A)cannot be used to identify an unknown atom.
B)can be used to identify unknown atoms.
C)can be explained by the movement of protons colliding with electrons.
D)none of the.

Question 80

A 6.0-gram champagne cork is shot out of an opened champagne bottle and traveled at a speed of 65 km/hour.Calculate the de Broglie wavelength (in meters)of the cork.

A)6.1 × 10^-33 m
B)1.7 × 10^-36 m
C)6.1 × 10^-36 m
D)1.7 × 10^-33 m
E)5.5 × 10^-20 m