Deck 7: The Structure of Atoms

Question 1

What is the wavelength of a photon that has an energy of $7.863 \times 10 ^ { 4 }$ J

A) ? $7.86 \times 10 ^ { 13 }$ nm
B) ? $1.19 \times 10 ^ { 38 }$ nm
C) ? $2.53 \times 10 ^ { - 21 }$ nm
D) $2.36 \times 10 ^ { 22 }$ nm
E) $1.56 \times 10 ^ { - 11 }$ nm

Answer 1

? $2.53 \times 10 ^ { - 21 }$ nm

Question 2

For which of the following electron transitions would a hydrogen atom emit a photon of the longest wavelength?

A)
B)
C)
D)

Answer 2

Question 3

According to the Bohr model of the hydrogen atom, the energy necessary to excite an electron from energy level n = 4 to n = 5 is _____ the energy necessary to excite an electron from energy level n = 6 to n = 7.

A) less than
B) greater than
C) equal to
D) either equal to or greater than
E) either less than or equal to

Answer 3

less than

Question 4

If the energy of 1.00 mole of photons is 245 kJ, what is the wavelength of the light?

A) 122 nm
B) 488 nm
C) 1220 nm
D) 787 nm
E) 811 nm

Question 5

A device operates at a frequency of $7.7 \times 10 ^ { 14 }$ Hz. What is the wavelength of this radiation?

A) ?390 nm
B) $2.57 \times 10 ^ { 31 }$ nm
C) $2.58 \times 10 ^ { - 31 }$ nm
D) 0.153 nm
E) $5.11 \times 10 ^ { - 10 }$ nm

Question 6

Which of the following regions of the electromagnetic spectrum has the lowest frequency?

A) x-ray
B) gamma ray
C) ultraviolet
D) infrared
E) visible

Question 7

Which of the following ranks the regions of the electromagnetic spectrum from shortest to longest wavelength.

A) microwaves > x-rays> gamma rays > visible > infrared
B) gamma rays > x-rays > visible > infrared> microwaves
C) infrared > gamma rays > x-rays > visible > microwaves
D) x-rays > gamma rays > infrared > visible > microwaves
E) visible > infrared > microwaves > x-rays > gamma rays

Question 8

What is the energy per mole of photons of light with a frequency of 9.01 × 10¹⁴ Hz?

A) 2.21 × 10^-31 kJ/mol
B) 3.6 × 10² kJ/mol
C) 2 × 10²³ kJ/mol
D) 1.33 × 10^-10 kJ/mol
E) 3.33 × 10² kJ/mol

Question 9

​A device emits light at 219.4 nm. What is the frequency of this radiation?

A) ​1.37 × 10^-3 Hz
B) 3.31 × 10²⁶ Hz
C) 1.37 × 10¹⁵ Hz
D) 9.07 × 10^-37 Hz
E) 9.07 × 10^-19 Hz

Question 10

What is the energy per mole of photons of light with a wavelength of 690.8 nm?

A) 2.88 × 10^-19 kJ/mol
B) 4.16 × 10¹⁴ kJ/mol
C) 2.61 × 10³⁵ kJ/mol
D) 4.34 × 10¹⁴ kJ/mol
E) 1.73 × 10² kJ/mol

Question 11

What is the frequency of gamma ray radiation that has a wavelength of 11.4 pm?

A) 3.80 × 10^-20 s^-1
B) 1.74 × 10^-14 s^-1
C) 2.63 × 10⁷ s^-1
D) 3.42 × 10⁹ s^-1
E) 2.63 × 10¹⁹ s^-1

Question 12

The energy required to break one mole of fluorine-fluorine bonds in F₂ is 155 kJ/mol. What is the longest wavelength of light capable of breaking a single F-F bond?

A) 0.972 nm
B) 617 nm
C) 630 nm
D) 772 nm
E) 972 nm

Question 13

If a cordless phone operates at a frequency of 9.00 × 10⁸ s^-1, what is the wavelength of this radiation?

A) 0.333 m
B) 1.99 m
C) 3.33 × 10^-9 m
D) 3.71 × 10^-18 m
E) 2.70 × 10¹⁷ m

Question 14

Which of the following colors of visible light has the longest wavelength?

A) green
B) orange
C) red
D) yellow
E) blue

Question 15

What is the wavelength of a photon having a frequency of 54.1 THz? (1 THz = 1015 Hz)

A) ​0.180 nm
B) 3.59 × 10^-23 nm
C) 1.08 × 10^-14 nm
D) 5.55 nm
E) 5.55 × 10¹⁵ nm

Question 16

What is the binding energy of an electron in a photosensitive metal (in kJ/mol) if the longest wavelength of light that can eject electrons from the metal is 299.0 nm?

A) 279 kJ/mol
B) 400 kJ/mol
C) 792 kJ/mol
D) 2.50 × 10¹⁹ kJ/mol
E) 4.00 × 10^-20 kJ/mol

Question 17

What is the energy of a photon of electromagnetic radiation with a frequency of $8.44 \times 10 ^ { 14 }$ Hz?

A) ? $2.53 \times 10 ^ { 23 }$ J
B) ? $1.68 \times 10 ^ { - 10 }$ J
C) ? $2.36 \times 10^{ - 40}$ J
D) $3.55 \times 10 ^ { - 7 }$ J
E) $5.6 \times 10 ^ { - 19 }$ J

Question 18

The ____ of a photon of light is ____ proportional to its frequency and ____ proportional to its wavelength.

A) energy, directly, inversely
B) energy, inversely, directly
C) velocity, directly, inversely
D) intensity, inversely, directly
E) amplitude, directly, inversely

Question 19

A light emitting diode (L.E.D.) emits photons with an energy of
$5.315 \times 10 ^ { - 19 }$
J. What is the energy per mole of photons emitted? ?

A) $3.201 \times 10 ^ { 5 }$ J/mol
B) $8.826 \times 10 ^ { 0 }$ J/mol
C) $3.201 \times 10 ^ { 8 }$ J/mol
D) $5.315 \times 10 ^ { - 19 }$ J/mol
E) $8.826 \times 10 ^ { 6 }$ J/mol

Question 20

A red laser pointer emits light at a wavelength of 488 nm. If the laser emits 7.5 × 10^-4 J of energy per second in the form of visible radiation, how many photons per second are emitted from the laser?

A) 4.1 × 10^-19 photons/sec
B) 5.4 × 10^-16 photons/sec
C) 8.9 × 10¹⁴ photons/sec
D) 1.8 × 10¹⁵ photons/sec
E) 2.5 × 10¹⁸ photons/sec

Question 21

For which of the following transitions would a hydrogen atom absorb a photon with the longest wavelength?

A) n = 1 to n = 2
B) n = 4 to n = 6
C) n = 5 to n = 4
D) n = 7 to n = 6
E) n = 6 to n = 7

Question 22

If the de Broglie wavelength of an electron is 44 nm, what is its velocity? (The mass of an electron is 9.11 × 10^-31 kg.)

A) 6.0 × 10^-5 m/s
B) 1.2 × 10³ m/s
C) 1.7 × 10⁴ m/s
D) 3.1 × 10¹⁰ m/s
E) 4.8 × 10²² m/s

Question 23

The contribution for which de Broglie is best remembered in modern science is

A) his statement that no electron can have identical values for all four quantum numbers.
B) his proposal that particles of matter should be associated with wavelike behavior.
C) his statement that an electron can exist in an atom only in discrete energy levels.
D) his statement that elements show periodic repetition of properties.
E) his statement that electrons occupy all the orbitals of a given sublevel singly before pairing begins.

Question 24

For which of the following transitions would a hydrogen atom emit the lowest energy photon?

A) n = 4 to n = 5
B) n = 5 to n = 2
C) n = 4 to n = 3
D) n = 3 to n = 1
E) n = 3 to n = 2

Question 25

If a hydrogen atom in the excited n = 3 state relaxes to the ground state, what is the maximum number of possible emission lines?

A) 1
B) 3
C) 6
D) 8
E) infinite

Question 26

What is the value of the orbital angular momentum quantum number ( $\ell$ ) for an electron in a 4f orbital?

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

Question 27

Which type of experiment demonstrates that an electron has the properties of a wave?

A) nuclear fission
B) electron diffraction
C) light emission from atomic gases
D) mass spectroscopy
E) photoelectric effect

Question 28

In Bohr's atomic theory, when an electron moves from one energy level to another energy level more distant from the nucleus,

A) energy is absorbed.
B) light is emitted.
C) energy is emitted.
D) no change in energy occurs.
E) none of these

Question 29

What is the de Broglie wavelength of a 146-g baseball traveling at 99 mph? (1 mi = 1.609 km and h = 6.63 × 10^-34 J·s)

A) 3.51 × 10³⁷ m
B) 1.03 × 10^-34 m
C) 1.03 × 10^-37 m
D) 9.74 × 10³³ m
E) 2.85 × 10^-38 m

Question 30

What is the wavelength of light emitted when an electron in a hydrogen atom undergoes a transition from energy level
n = 6 to level n = 1? (c = 3.00 × 10⁸ m/s, h = 6.63 × 10^-34 J·s, R_H = 2.179 × 10^-18 J)

A) 9.39 × 10^-8 kJ/mol
B) 7.06 × 10^-27 kJ/mol
C) 1.07 × 10⁷ kJ/mol
D) 2.12 × 10^-18 kJ/mol
E) 3.2 × 10¹⁵ kJ/mol

Question 31

Which of the following statements is INCORRECT?

A) It is not possible to know the exact location of an electron and its exact energy simultaneously.
B) The energies of an atom's electrons are quantized.
C) Quantum numbers define the energy states and the orbitals available to an electron.
D) The behavior of an atom's electrons can be described by circular orbits around a nucleus.
E) Electrons have both wave and particle properties.

Question 32

What is the de Broglie wavelength of an electron traveling at 5.18% of the speed of light?
(c = 3.00 × 10⁸ m/s, h = 6.63 × 10^-34 J·s, m_e = 9.109 × 10^-31 J)

A) 2.14 × 10¹⁰ m
B) 2.43 × 10^-12 m
C) 4.68 × 10^-11 m
D) 2.14 × 10¹² m
E) 4.68 × 10^-13 m

Question 33

The electron in a hydrogen atom, originally in level n = 10, undergoes a transition to a lower level by emitting a photon of wavelength 1739 nm. What is the final level of the electron?
(c = 3.00 × 10⁸ m/s, h = 6.626 × 10^-34 J·s, R_H = 2.179 × 10^-18 J)

A) ?4
B) ?5
C) ?10
D) ?20
E) 1

Question 34

How many orbitals have the following set of quantum numbers: n = 5, $\ell$ = 3, $m _ { \ell }$ = -1?

A) 0
B) 1
C) 3
D) 6
E) 7

Question 35

For a proton (mass = 1.673 × 10^-27 kg) moving with a velocity of 2.83 × 10⁴ m/s, what is the de Broglie wavelength of the proton (in pm)?

A) 0.356 pm
B) 3.56 pm
C) 14.0 pm
D) 7.15 pm
E) 28.5 pm

Question 36

Which type of experiment demonstrates that light has the properties of a particle?

A) nuclear fission
B) electron diffraction
C) light emission from atomic gases
D) mass spectroscopy
E) photoelectric effect

Question 37

Which of the following is/are correct postulates of Bohr's theory of the hydrogen atom ?

Question 38

According to Heisenberg's _____ principle, it is impossible to simultaneously measure the exact location and energy of an electron.

Question 39

A 4d orbital has ?

A) 3 planar nodes and 3 spherical nodes.
B) 1 planar node and 1 spherical node.
C) 2 planar nodes and 1 spherical node.
D) 2 planar nodes and 4 spherical nodes.
E) 4 planar nodes and 2 spherical nodes.

Question 40

Which of the following orbital boundary surfaces represent d-orbitals?

A) 1 only
B) 3 only
C) 2 only
D) 1 and 2
E) 1 and 4

Question 41

What is the value of the spin quantum number for an electron in a 3d orbital?

A) 3
B) 2
C) either $+ \frac { 1 } { 2 }$ or $- \frac { 1 } { 2 }$
D) $- \frac { 1 } { 2 }$
E) $+ \frac { 1 } { 2 }$

Question 42

What type of orbital is designated n = 4, $\ell$ = 2, $m _ { \ell }$ = 2?

A) 4f
B) 4d
C) 4p
D) 4g
E) 4s

Question 43

What is the total number of subshells found in the n = 7 shell?

A) 7
B) 49
C) 6
D) 8
E) 9

Question 44

What is the total number of orbitals having n = 3 and $\ell$ = 2?

A) 1
B) 3
C) 5
D) 7
E) 10

Question 45

Which of the following sets of quantum numbers (n, l, ml_, m_s) is not permissible?

A) 2 2 1 + $\frac { 1 } { 2 }$
B) 3 1 0 - $\frac { 1 } { 2 }$
C) 1 0 0 + $\frac { 1 } { 2 }$
D) 2 1 0 + $\frac { 1 } { 2 }$
E) 4 0 0 - $\frac { 1 } { 2 }$

Question 46

Which of the following properties is associated with the value of the $\ell$ quantum number?

A) the shape of an orbital
B) the size of an orbital
C) the number of electrons in an orbital
D) the energy of an orbital
E) the orientation in space of an orbital

Question 47

Which of the following properties of orbital is associated with the value of the principal quantum number?

A) Number of electrons in an orbital
B) Size of an orbital
C) Orientation in space of an orbital
D) Energy of an orbital
E) Shape of an orbital

Question 48

How many f orbitals are in the n = 4 shell?

A) 5
B) 8
C) 3
D) 1
E) 7

Question 49

Which of the following orbital can be represented by n = 4, $\ell$ = 3, and $m _ { \ell }$ = -2?

A) 4s
B) 4p
C) 4d
D) 4f
E) None of these

Question 50

Which of the following sets of quantum numbers refers to a 4d orbital?

A) n = 2, $\ell$ = 1, $m _ { \ell }$ = -1
B) n = 2, $\ell$ = 4, $m _ { \ell }$ = -1
C) n = 4, $\ell$ = 2, $m _ { \ell }$ = -1
D) n = 4, $\ell$ = 3, $m _ { \ell }$ = 0
E) n = 4, $\ell$ = 3, $m _ { \ell }$ = +2

Question 51

A point in a standing wave that has zero amplitude is called a(n) ________.

Question 52

Which of the following orbital boundary surfaces is a representation of a $3 d _ { z ^ { 2 } }$ orbital?

A)
B)
C)
D)
E)

Question 53

Which of the following sets of quantum numbers is not allowed?

A) n = 4, $\ell$ = 2, and $m _ { \ell }$ = -2
B) n = 6, $\ell$ = 1, and $m _ { \ell }$ = 1
C) n = 5, $\ell$ = 4, and $m _ { \ell }$ = -4
D) n = 2, $\ell$ = 1, and $m _ { \ell }$ = -3
E) n = 6, $\ell$ = 3, and $m _ { \ell }$ = -2

Question 54

How many values are there for the magnetic quantum number ( $m _ { \ell }$ ) when the value of the angular momentum quantum number ( $\ell$ ) is 4?

A) 11
B) 9
C) 2
D) 4
E) 15

Question 55

Which type of orbital is designated n = 2 and $\ell$ = 1?

A) 2p
B) 3s
C) 4d
D) 1f
E) 2d

Question 56

The (principal quantum number) n = ____ shell is the lowest that may contain s-orbitals.

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

Question 57

Which of the following is a representation of a 3d_xy orbital?

A)
B)
C)
D)
E)

Question 58

The ________ quantum number is given the symbol . This quantum number is related to the orientation in space of an orbital.

Question 59

Which of the following is the correct series of lines that have energies in visible region of the hydrogen spectrum?

A) Balmer series
B) Lyman series
C) Brackett series
D) Pfund series
E) Humphreys series

Question 60

The Bohr model predicts that the energy of an atom's electron is _____. It means that the electron can only occupy orbitals of specific energies.

Question 61

The difference in energy between adjacent energy levels in an atom _____ as n increases.

Question 62

What evidence does the photoelectric effect provide that photons are not only waves?

Question 63

Occupied states or energy levels in the hydrogen atom with n > 1 are called _____ states.

Question 64

A ________, designated by the Greek symbol ψ, describes the wave behavior of an electron in an atom.

Question 65

The size of an electron orbital is often chosen to be the distance within which 90% of the electron density is found. Why is the orbital radius not chosen to be the distance within which 100% of the electron density is found?