# Quiz 29: Atomic Theory

Physics & Astronomy

Q 1Q 1

An alpha particle is:
A) any positively charged nucleus.
B) an X-ray.
C) a neutral helium atom.
D) None of these choices.

Free

Multiple Choice

D

Q 2Q 2

According to the Rutherford model of the atom, most of the volume of an atom:
A) is empty space.
B) was occupied by the nucleus.
C) excluded electrons.
D) contained positive charges.

Free

Multiple Choice

A

Q 3Q 3

In contrast to the plum-pudding model of the atom, Rutherford's model:
A) was first to explain atoms emitting discrete frequencies.
B) had the positive charge concentrated in a small region.
C) eliminated radiation from accelerating charges.
D) had the positive charge spread uniformly through the atom.

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Multiple Choice

B

Q 4Q 4

When a wire carries high current causing it to glow, it will emit which type of spectrum?
A) line absorption
B) monochromatic
C) continuous
D) line emission

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Multiple Choice

Q 5Q 5

When a high voltage is applied to a low-pressure gas causing it to glow, it will emit which type of spectrum?
A) line emission
B) line absorption
C) continuous
D) monochromatic

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Multiple Choice

Q 6Q 6

When a cool gas is placed between a glowing wire filament source and a diffraction grating, the resultant spectrum from the grating is which one of the following?
A) line emission
B) continuous
C) line absorption
D) monochromatic

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Multiple Choice

Q 7Q 7

If a hydrogen atom, originally in its ground state of energy -13.6 eV, absorbs a photon of energy 22.0 eV, what is the resulting kinetic energy of the electron if the proton has negligible kinetic energy?
A) Such a photon cannot be absorbed in this case.
B) .4 eV
C) 2.4 eV
D) 16.0 eV

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Multiple Choice

Q 8Q 8

The Lyman series of hydrogen is made up of those transitions made from higher levels to n = 1. If the first line (n = 2 to n = 1) in this series has a wavelength of 122 nm, what is the wavelength of the third line (n = 4 to n = 1)?
A) 364 nm
B) 97.6 nm
C) 103 nm
D) 486 nm

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Multiple Choice

Q 9Q 9

The ionization energy for the hydrogen atom is 13.6 eV. What is the energy of a photon that is emitted as a hydrogen atom makes a transition between the n = 4 and n = 3 states?
A) 3.40 eV
B) 0.66 eV
C) 6.80 eV
D) 2.55 eV

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Multiple Choice

Q 10Q 10

Of the wavelengths emitted from a hydrogen gas discharge tube, those that are associated with transitions from higher levels down to the n = 1 level produce which of the following?
A) infrared
B) visible
C) ultraviolet
D) mixture of infrared and visible

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Multiple Choice

Q 11Q 11

Of the various wavelengths emitted from a hydrogen gas discharge tube, those associated with transitions from higher levels down to the n = 2 level produce which of the following?
A) visible
B) infrared
C) ultraviolet
D) a mixture of visible and ultraviolet

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Multiple Choice

Q 12Q 12

What is the wavelength of the line in the hydrogen spectrum that is comprised of transitions from the n = 5 to the n = 3 levels?
A) 1880 nm
B) 1290 nm
C) 2250 nm
D) 1920 nm

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Multiple Choice

Q 13Q 13

The ionization energy of the hydrogen atom is 13.6 eV. What is the energy of the n = 5 state?
A) -0.544 eV
B) 0.378 eV
C) 0.544 eV
D) -0.378 eV

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Multiple Choice

Q 14Q 14

The ionization energy of the hydrogen atom is 13.6 eV. What is the energy of a photon emitted corresponding to a transition from the n = 6 to n = 2 state?
A) 7.9 eV
B) 2.9 eV
C) 3.0 eV
D) 4.0 eV

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Multiple Choice

Q 15Q 15

If the radius of the electron orbit in the n = 1 level of the hydrogen atoms is 0.0529 nm, what is its radius for the n = 4 level? (Assume the Bohr model is valid).
A) 1.32 nm
B) 0.265 nm
C) 0.106 nm
D) 0.846 nm

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Multiple Choice

Q 16Q 16

The Paschen series of hydrogen corresponds to electron transitions from higher levels to n = 3. What is the longest wavelength in that series? (h = 6.63 10

^{}^{34 }Js. The ground state of hydrogen is at -13.6 eV.) A) 822 nm B) 365 nm C) 1880 nm D) 1094 nmFree

Multiple Choice

Q 17Q 17

The Lyman series of hydrogen corresponds to electron transitions from higher levels to n = 1. What is the longest wavelength in that series? (h = 6.63 10

^{}^{34 }Js. The ground state of hydrogen is at -13.6 eV.) A) 91.4 nm B) 273 nm C) 456 nm D) 122 nmFree

Multiple Choice

Q 18Q 18

The ionization energy of the hydrogen atom is 13.6 eV. What is the wavelength of a photon having this much energy? (h = 6.63 10

^{}^{34 }Js, c = 3.00 10^{8}m/s, 1 eV = 1.6 10^{}^{19}J, and 1 nm = 10^{}^{9}m) A) 91.4 nm B) 360 nm C) 136 nm D) 273 nmFree

Multiple Choice

Q 19Q 19

The four visible colors emitted by hydrogen atoms are produced by electrons:
A) that start in the ground state.
B) that end up in the ground state.
C) that end up in the level with n = 2.
D) that start in the level with n = 2.

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Multiple Choice

Q 20Q 20

In the Bohr model of the atom, the orbits where electrons move slowest:
A) have the least radius.
B) have the highest energy.
C) have the least angular momentum.
D) have the lowest energy.

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Multiple Choice

Q 21Q 21

In the hydrogen atom the potential energy is negative, but the absolute value of the potential energy:
A) is half the kinetic energy of the electron.
B) is equal to n

^{2}times the kinetic energy of the electron. C) is equal to the kinetic energy of the electron. D) is twice the kinetic energy of the electron.Free

Multiple Choice

Q 22Q 22

When an electron moves from the n = 1 to the n = 3 orbit:
A) the radius doubles and the angular momentum increases by a factor of 9.
B) the radius increases by a factor of 9, and the angular momentum triples.
C) both the radius and the angular momentum increase by a factor of 9.
D) both the radius and the angular momentum triple.

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Multiple Choice

Q 23Q 23

A muon behaves like an electron except that it has 207 times the mass of the electron. If a muon were bound to a proton, how would the energy levels in the Bohr model compare to those for a bound electron?
A) They would be 207 times as much as those for the electron.
B) They would be (207)

^{2}times as much as those for the electron. C) They would be the same. D) They would be (1/207) times as much as those for the electron.Free

Multiple Choice

Q 24Q 24

A hydrogen atom in the ground state absorbs a 12.75-eV photon. To what level is the electron promoted? (The ionization energy of hydrogen is 13.6 eV).
A) n = 2
B) n = 3
C) n = 5
D) n = 4

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Multiple Choice

Q 25Q 25

A photon is emitted from a hydrogen atom that undergoes a transition from n = 3 to n = 2. Calculate the energy and wavelength of the photon. (The ionization energy of hydrogen is 13.6 eV, and h = 6.63 10

^{}^{34 }Js, c = 3.00 10^{8}m/s, 1 eV = 1.60 10^{}^{19}J, and 1 nm = 10^{}^{9}m) A) 2.21 eV, 563 nm B) 1.89 eV, 460 nm C) 2.58 10^{-19}J, 658 nm D) 3.02 10^{-19}J, 658 nmFree

Multiple Choice

Q 26Q 26

The speed of the electron in the Bohr theory of hydrogen is:
A) inversely proportional to n.
B) inversely proportional to n

^{2}. C) proportional to n. D) proportional to n^{2}.Free

Multiple Choice

Q 27Q 27

Which of the following transitions in hydrogen from an initial state (n

_{i}) to a final state (n_{f}) results in the least energy emitted? A) n_{i}= 3, n_{f}= 95 B) n_{i}= 80, n_{f}= 2 C) n_{i}= 2, n_{f}= 1 D) n_{i}= 1, n_{f}= 3Free

Multiple Choice

Q 28Q 28

In an analysis relating Bohr's theory to the de Broglie wavelength of electrons, when an electron moves from the n = 1 level to the n = 3 level, the circumference for its orbit becomes 9 times greater. This occurs because:
A) the wavelength of the electron becomes nine times as long.
B) there are triple as many wavelengths, and each wavelength is triple in length.
C) there are nine times as many wavelengths in the new orbit.
D) the electron is moving nine times as fast.

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Multiple Choice

Q 29Q 29

Characteristic K X-rays are the result of:
A) inner electron transitions.
B) outer electron transitions.
C) nuclear electron states.
D) buckytubes.

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Multiple Choice

Q 30Q 30

When a hydrogen atom absorbs a photon that raises it to the n = 5 state, how many different energies are possible for the photon(s) that may be emitted as the atom eventually returns to the ground state?
A) 5
B) 3
C) 4
D) The correct value is not given.

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Multiple Choice

Q 31Q 31

When a hydrogen atom absorbs a photon that raises it to the n = 4 state, what is the least number of photons that can be emitted by that atom as it returns to the ground state?
A) 4
B) 3
C) 5
D) The correct value is not given.

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Multiple Choice

Q 32Q 32

In the n = 5 shell, how many distinct values of are possible?
A) 5
B) 15
C) 10
D) The correct value is not given.

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Multiple Choice

Q 33Q 33

The Bohr theory does not predict that:
A) the approximate radius of a hydrogen atom is 5.3 10

^{}^{11}m. B) hydrogen atoms will give off the lines from the series ending in the n = 2 state. C) the ground state of hydrogen is spherically symmetric. D) it requires 13.6 eV to ionize hydrogen.Free

Multiple Choice

Q 34Q 34

The Bohr model of the hydrogen atom accounts for which quantum number?
A) orbital
B) principal
C) orbital magnetic
D) All of the above.

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Multiple Choice

Q 35Q 35

The quantum mechanical model of the hydrogen atom requires that if the principal quantum number is 5, there will be how many different permitted orbital quantum number(s)?
A) two
B) five
C) one
D) four

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Multiple Choice

Q 36Q 36

The quantum mechanical model of the hydrogen atom requires that if the orbital quantum number of the hydrogen atom is 3, there will be how many permitted orbital magnetic quantum numbers?
A) three
B) nine
C) four
D) seven

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Multiple Choice

Q 37Q 37

The quantum mechanical model of the hydrogen atom requires that if the orbital magnetic quantum number is 4, there will be how many permitted spin magnetic quantum numbers?
A) four
B) seven
C) three
D) two

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Multiple Choice

Q 38Q 38

How many possible substates are available in a hydrogen atom where the principal quantum number is 2?
A) 18
B) 8
C) 36
D) 9

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Multiple Choice

Q 39Q 39

The quantum mechanical model of the hydrogen atom requires that if the principal quantum number = 6, there will be how many permitted orbital quantum numbers?
A) 3
B) 16
C) 6
D) 5

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Multiple Choice

Q 40Q 40

The quantum mechanical model of the hydrogen atom requires that if the orbital quantum number = 5, there will be how many permitted orbital magnetic quantum numbers allowed?
A) 7
B) 15
C) 5
D) 11

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Multiple Choice

Q 41Q 41

The quantum mechanical model of the hydrogen atom requires that if the principal quantum number = 3, there will be permitted how many orbital magnetic quantum numbers?
A) 5
B) 8
C) 4
D) 7

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Multiple Choice

Q 42Q 42

The quantum mechanical model of the hydrogen atom requires that if the orbital quantum number = 4, there are permitted how many possible substates?
A) 22
B) 18
C) 8
D) 32

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Multiple Choice

Q 43Q 43

If the principal quantum number for hydrogen is 4, which one of the following is not a permitted orbital magnetic quantum number for that atom?
A) 2
B) 0
C) 3
D) 5

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Multiple Choice

Q 44Q 44

The quantum number that can have only two possible values is the:
A) orbital quantum number.
B) principal quantum number.
C) spin magnetic quantum number.
D) orbital magnetic quantum number.

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Multiple Choice

Q 45Q 45

The quantum mechanical model of the hydrogen atom suggests a visual picture of the electron as which of the following?
A) planetary orbiting body
B) probability cloud
C) raisin in pudding
D) light quantum

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Multiple Choice

Q 46Q 46

What is the lowest value for n of a shell that can contain a g electron?
A) 5
B) 4
C) 3
D) 6

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Multiple Choice

Q 47Q 47

For n = 6, what are the maximum orbital quantum number and the maximum orbital magnetic quantum number?
A) 7, 6
B) 5, 4
C) 6, 5
D) 5, 5

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Multiple Choice

Q 48Q 48

For n = 5, how many allowed values are possible for the orbital quantum number and the orbital magnetic quantum number?
A) 5, 11
B) 6, 12
C) 5, 9
D) 4, 9

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Multiple Choice

Q 49Q 49

Magnesium has atomic number 12. In its ground state, how many electrons are in its n = 3 shell?
A) 2
B) 8
C) 16
D) 10

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Multiple Choice

Q 50Q 50

For the n = 5 shell, what are the lowest values possible for and respectively?
A) -5, -5
B) 4, -4
C) 0, -4
D) 0, 0

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Multiple Choice

Q 51Q 51

The restriction that no more than one electron may occupy a given quantum state in an atom was first stated by which of the following scientists?
A) Bohr
B) Pauli
C) de Broglie
D) Heisenberg

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Multiple Choice

Q 52Q 52

How many electrons are in chlorine's (atomic number 17) next to outer shell (n = 2)?
A) 18
B) 4
C) 2
D) 8

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Multiple Choice

Q 53Q 53

The ground state electronic configuration for sodium is 1s

^{2}2s^{2}2p^{6}3s^{1}. What is the orbital quantum number of the last (3s^{1}) electron? A) 3 B) 1 C) 2 D) 0Free

Multiple Choice

Q 54Q 54

What is the next energy level that fills after the 4d energy level is full?
A) 5p
B) 4s
C) 6s
D) 4f

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Multiple Choice

Q 55Q 55

The ground state electronic configuration for silicon is 1s

^{2}2s^{2}2p^{6}3s^{2}3p^{2}. Which of the following elements would be expected to be chemically similar to silicon? A) boron with configuration 1s^{2}2s^{2}2p^{1}B) lithium with configuration 1s^{2}2s^{1}C) carbon with configuration 1s^{2}2s^{2}2p^{2}D) sodium with configuration 1s^{2}2s^{2}2p^{6}3s^{1}Free

Multiple Choice

Q 56Q 56

The ground state electronic configuration for magnesium is 1s

^{2}2s^{2}2p^{6}3s^{2}. Which of the following would most likely result in an element being chemically similar to magnesium? A) the valence subshell having 2 electrons B) the valence electron being an s^{2}electron C) the valence electron being a p^{2}electron D) the valence electron having principal quantum number 3Free

Multiple Choice

Q 57Q 57

The ground state configuration for an element is . What is the atomic number of the element?
A) 11
B) 9
C) 24
D) 13

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Multiple Choice

Q 58Q 58

What is the maximum number of electrons that can occupy a 3d subshell?
A) 5
B) 14
C) 10
D) 18

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Multiple Choice

Q 59Q 59

The stimulated emission of photons from the excited atoms in a gas laser is prompted by which of the following?
A) nearby presence of photons of same wavelength as those emitted
B) high flux of electrons
C) high voltage
D) high temperature

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Multiple Choice

Q 60Q 60

The red light from a HeNe laboratory laser results from a transition in Ne. Determine the energy difference between the states if the wavelength of the light given off is 634 nm. (h = 6.63 10

^{}^{34 }Js, c = 3.00 10^{8}m/s, 1 eV = 1.60 10^{}^{19}J, and 1 nm = 10^{}^{9}m) A) 2.22 eV B) 1.43 eV C) 1.96 eV D) 2.04 eVFree

Multiple Choice

Q 61Q 61

The wavelength of a coherent laser is 628 nm. What energy difference exists between the upper excited state involved and the lower unexcited ground state? (h = 6.63 10

^{}^{34 }Js, c = 3.00 10^{8}m/s, 1 eV = 1.60 10^{}^{19}J, and 1 nm = 10^{}^{9}m) A) 1.86 eV B) 1.81 eV C) 1.75 eV D) 1.98 eVFree

Multiple Choice

Q 62Q 62

A ruby laser delivers a 2.28-J pulse in approximately 50 nanoseconds. The wavelength of the light is 694.4 nm. At least how many atoms within the ruby rod had to be excited to allow this high-energy laser pulse? (h = 6.63 10

^{}^{34 }Js, c = 3.00 10^{8}m/s, 1 eV = 1.6 10^{}^{19}J, and 1 nm = 10^{}^{9}m) A) 3 10^{19}B) 4 10^{18}C) 8 10^{18}D) 6 10^{20}Free

Multiple Choice

Q 63Q 63

In neon, the 20.66-eV level can undergo lasing action to the 18.70-eV level. What is the energy of the resulting photons?
A) 18.70 eV
B) 20.66 eV
C) 1.96 eV
D) 39.36 eV

Free

Multiple Choice