# Quiz 29: Atoms and Molecules

Physics & Astronomy

Q 1Q 1

To which of the following values of n does the longest wavelength in the Balmer series correspond?
A)3
B)5
C)1
D)7
E)∞ (very large)

Free

Multiple Choice

A

Q 2Q 2

To which of the following values of n does the shortest wavelength in the Balmer series correspond?
A)3
B)5
C)7
D)1
E)∞ (very large)

Free

Multiple Choice

E

Q 3Q 3

The Balmer series is formed by electron transitions in hydrogen that
A)end on the n = 1 shell.
B)begin on the n = 1 shell.
C)end on the n = 2 shell.
D)begin on the n = 2 shell.
E)are between the n = 1 and n = 3 shells.

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Multiple Choice

C

Q 4Q 4

The Lyman series is formed by electron transitions in hydrogen that
A)end on the n = 1 shell.
B)begin on the n = 1 shell.
C)end on the n = 2 shell.
D)begin on the n = 2 shell.
E)are between the n = 1 and n = 3 shells.

Free

Multiple Choice

Q 5Q 5

The Paschen series is formed by electron transitions that
A)end on the n = 1 shell.
B)begin on the n = 1 shell.
C)end on the n = 2 shell.
D)begin on the n = 3 shell.
E)end on the n = 3 shell.

Free

Multiple Choice

Q 6Q 6

Hydrogen atoms can emit four spectral lines with visible colors from red to violet. These four visible lines emitted by hydrogen atoms are produced by electrons
A)that start in the n = 2 level.
B)that end up in the n = 2 level.
C)that end up in the n = 3 level.
D)that end up in the ground state.
E)that start in the ground state.

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Multiple Choice

Q 7Q 7

When an electron jumps from an orbit where n = 4 to one where n = 2
A)a photon is emitted.
B)a photon is absorbed.
C)two photons are emitted.
D)two photons are absorbed.
E)None of the given answers are correct.

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Multiple Choice

Q 8Q 8

The energy difference between adjacent orbit radii in a hydrogen atom
A)increases with increasing values of n.
B)decreases with increasing values of n.
C)remains constant for all values of n.
D)varies randomly with increasing values of n.

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Multiple Choice

Q 9Q 9

The figure shows part of the energy level diagram of a certain atom. The energy spacing between levels 1 and 2 is twice that between 2 and 3. If an electron makes a transition from level 3 to level 2, the radiation of wavelength λ is emitted. What possible radiation wavelengths might be produced by other transitions between the three energy levels?
A)both λ/2 and λ/3
B)only λ/2
C)both 2λ and 3λ
D)only 2λ

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Multiple Choice

Q 10Q 10

The distance between adjacent orbits in a hydrogen atom
A)increases with increasing values of n.
B)decreases with increasing values of n.
C)remains constant for all values of n.
D)varies randomly with increasing values of n.

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Multiple Choice

Q 11Q 11

If a hydrogen atom originally in a state with principal quantum number n is excited to state n' = 2n, then
A)its radius and binding energy will double.
B)its radius will quadruple and the binding energy will double.
C)its radius will double and the binding energy will quadruple.
D)its radius will quadruple and the binding energy will be reduced by a factor of four.
E)its radius and binding energy will quadruple.

Free

Multiple Choice

Q 12Q 12

Which of the following statements are true for the Bohr model of the atom? (There could be more than one correct choice.)
A)The spacing between all the electron shells is the same.
B)The energy difference between all the electron shells is the same.
C)As we look at higher and higher electron shells, they get closer and closer together, but the difference in energy between them gets greater and greater.
D)As we look at higher and higher electron shells, they get farther and farther apart, but the difference in energy between them gets smaller and smaller.
E)There is no general pattern in the spacing of the shells or their energy differences.

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Multiple Choice

Q 13Q 13

A hydrogen atom is in the 6h state. What is the principal quantum number.
A)0
B)3
C)5
D)6
E)7

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Multiple Choice

Q 14Q 14

The orbital angular momentum quantum number can take which of the following values for any given value of the principal quantum number, n?
A)ℓ = 0, 1, 2, . . .
B)ℓ = 0, 1, 2, . . . , n
C)ℓ = 0, 1, 2, . . . , (n - 1)
D)ℓ = 1, 2, 3, 4, . . .
E)ℓ = 1, 2, 3, 4, . . ., (n + 1)

Free

Multiple Choice

Q 15Q 15

Which of the following values can be taken by the electron spin quantum number, m

_{s}? A)±1/2 B)0 C)±1 D)±2 E)±3Free

Multiple Choice

Q 16Q 16

According to the quantum mechanical model of the hydrogen atom, if the orbital angular momentum quantum number is ℓ, there will be how many permitted magnetic quantum numbers?
A)ℓ/2
B)2ℓ
C)2ℓ + 1
D)2ℓ - 1
E)3ℓ

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Multiple Choice

Q 17Q 17

According to the quantum mechanical model of the hydrogen atom, if the principal quantum number is n, how many different orbital angular momentum quantum numbers are permitted?
A)n/2
B)n
C)2n
D)3n
E)4n

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Multiple Choice

Q 18Q 18

According to Pauli's exclusion principle, how many electrons in an atom may have a particular set of quantum numbers?
A)1
B)3
C)2
D)4
E)5

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Multiple Choice

Q 19Q 19

The principal quantum number n can have any integer value ranging from
A)-∞ to +∞.
B)0 to ∞.
C)1 to ∞.
D)1 to 100.

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Multiple Choice

Q 20Q 20

The orbital angular momentum quantum number ℓ can have any integer value ranging from
A)0 to n.
B)0 to (n-1).
C)1 to n.
D)1 to (n+1).
E)-n to n.

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Multiple Choice

Q 21Q 21

The magnetic quantum number m

_{1}can have any integer value ranging from A)-n to +n. B)-ℓ to +ℓ. C)0 to n. D)0 to ℓ. E)0 to (n-1)Free

Multiple Choice

Q 22Q 22

The electron spin quantum number can have values of
A)-1/2, -1, 0, +1, +1/2.
B)-1/2, -1, +1, +1/2.
C)-1/2, 0, +1/2.
D)-1/2, +1/2.
E)only +1/2.

Free

Multiple Choice

Q 23Q 23

What is the atomic number of a neutral atom that has an electron configuration of 1s

^{2 }2s^{2 }2p^{6 }3s^{2 }3p^{2}? A)5 B)11 C)14 D)20Free

Multiple Choice

Q 24Q 24

If ℓ = 4, which one of the following is a possible quantum number for n?
A)0
B)2
C)3
D)4
E)8

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Multiple Choice

Q 25Q 25

If n = 5, which one of the following is not an allowed magnetic quantum number m

_{1}? A)0 B)2 C)4 D)5Free

Multiple Choice

Q 26Q 26

In its ground state, the quantum numbers (n, ℓ, m

_{1}, m_{s})for hydrogen are, respectively, A)1, 1, 1, 1. B)1, 0, 0, 0. C)1, 0, 0, ±1/2. D)1, 1, 1, ±1/2.Free

Multiple Choice

Q 27Q 27

Consider ground-state helium having two electrons in orbit. If one of the electrons has quantum numbers (n, ℓl, m

_{1}, m_{s})of 1, 0, 0, -1/2 respectively, the quantum numbers for the other electron will be A)1, 1, 0, -1/2. B)1, 0, 0, +1/2. C)1, 1, 1, +1/2. D)none of the given answers.Free

Multiple Choice

Q 28Q 28

The elements in the periodic table that have completely filled shells or subshells are referred to as
A)noble gases.
B)halogens.
C)alkali metals.
D)transition elements.

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Multiple Choice

Q 29Q 29

One of the emission lines described by the original version of Balmer's formula has wavelength What is the value of n in Balmer's formula that gives this emission line?
A)11
B)12
C)13
D)14

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Multiple Choice

Q 30Q 30

What is the value of n in the Balmer series for which the wavelength is 410.2 nm.
A)4
B)5
C)6
D)7
E)9

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Multiple Choice

Q 31Q 31

What is the wavelength in the Balmer series for n = 15?
A)277.1 nm
B)371.1 nm
C)188.6 nm
D)656 nm
E)754.2 nm

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Multiple Choice

Q 32Q 32

The value of a wavelength in the Balmer series is 372.1 nm. What is the corresponding value of n?
A)6
B)3
C)9
D)10
E)14

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Multiple Choice

Q 33Q 33

What is the longest wavelength in the Balmer series?
A)240 nm
B)328 nm
C)365 nm
D)656 nm
E)820 nm

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Multiple Choice

Q 34Q 34

What is the shortest wavelength in the Balmer series?
A)328 nm
B)365 nm
C)456 nm
D)656 nm
E)820 nm

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Multiple Choice

Q 35Q 35

What value of n corresponds to a wavelength of 922.7 nm in the Paschen series?
A)3
B)5
C)7
D)9
E)15

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Multiple Choice

Q 36Q 36

What value of n corresponds to a wavelength of 91.7 nm in the Lyman series?
A)1
B)3
C)5
D)9
E)13

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Multiple Choice

Q 37Q 37

What is the longest wavelength in the Paschen series?
A)2.01 nm
B)2.01 μm
C)365 nm
D)1.88 nm
E)1.88 μm

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Multiple Choice

Q 38Q 38

What is the shortest wavelength in the Paschen series?
A)410.2 nm
B)410.2 μm
C)365 nm
D)820.4 nm
E)820.4 μm

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Multiple Choice

Q 39Q 39

What is the shortest wavelength of the Lyman series?
A)91.16 nm
B)45.60 nm
C)121.5 nm
D)204.1 nm
E)365 nm

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Multiple Choice

Q 40Q 40

What is the longest wavelength in the Lyman Series?
A)45.60 nm
B)91.20 nm
C)121.5 nm
D)240.1 nm
E)365 nm

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Multiple Choice

Q 41Q 41

The wavelength of a ruby laser is 694.3 nm. What is the energy difference between the two energy states for the transition that produces this light? (c = 3.00 × 10

^{8}m/s, 1 eV = 1.60 × 10^{-19 }J, h = 6.626 × 10^{-34}J ∙ s) A)1.54 eV B)1.65 eV C)1.79 eV D)1.81 eVFree

Multiple Choice

Free

Essay

Q 43Q 43

Given that the energy levels of the hydrogen atom are given by E

_{n}= , where R = 1.097 × 10^{7}m^{-1}, what wavelength photon is emitted when the atom undergoes a transition from the n = 4 to the n = 6 level?Free

Essay

Q 44Q 44

Consider the Bohr model for the hydrogen atom. (c = 3.00 × 10

^{8}m/s, 1 eV = 1.60 × 10^{-19 }J, h = 6.626 × 10^{-34}J ∙ s) (a)How much energy (in eV)is needed to cause a transition of an electron from the second excited state to the third excited state? (b)What wavelength photon just has enough energy to initiate the transition in (a)?Free

Essay

Q 45Q 45

Given that the binding energy of the hydrogen atom in its ground state is -13.6 eV, what is the energy when it is in the n = 5 state?
A)2.72 eV
B)-2.72 eV
C)0.544 eV
D)-0.544 eV

Free

Multiple Choice

Q 46Q 46

If a hydrogen atom in the ground state absorbs a photon of energy 12.09 eV, to which state will the electron make a transition?
A)n = 2
B)n = 3
C)n = 4
D)n = 5

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Multiple Choice

Q 47Q 47

What is the ionization energy of the neutral hydrogen atom?
A)27.2 eV
B)13.6 eV
C)6.8 eV
D)none of the given answers

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Multiple Choice

Q 48Q 48

What is the energy of the photon emitted when an electron drops from the state to the state in a hydrogen atom?
A)0.244 eV
B)0.264 eV
C)0.283 eV
D)0.303 eV

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Multiple Choice

Q 49Q 49

In a hydrogen atom, the electron makes a transition from the n = 8 to the n = 3 state. The wavelength of the emitted photon is closest to which one of the following values? (c = 3.00 × 10

^{8}m/s, 1 eV = 1.60 × 10^{-19 }J, h = 6.626 × 10^{-34}J ∙ s) A)9.57 × 10^{-7}m B)1.13 × 10^{-6}m C)3.12 × 10^{-7}m D)4.52 × 10^{-6}m E)6.34 × 10^{-7}mFree

Multiple Choice

Q 50Q 50

A hydrogen atom is excited to the n = 11 level. Its decay to the n = 7 level is detected in a photographic plate. What is the wavelength of the light photographed? (c = 3.00 × 10

^{8}m/s, 1 eV = 1.60 × 10^{-19 }J, h = 6.626 × 10^{-34}J ∙ s) A)7510 nm B)4670 nm C)12,400 nm D)4380 nmFree

Multiple Choice

Q 51Q 51

A hydrogen atom is excited to the n = 9 level. Its decay to the n = 6 level detected in a photographic plate. What is the frequency of the light photographed? (1 eV = 1.60 × 10

^{-19 }J, h = 6.626 × 10^{-34}J ∙ s) A)5.08 × 10^{13}Hz B)5910 Hz C)5910 nm D)3.28 × 10^{-9}kmFree

Multiple Choice

Q 52Q 52

A hydrogen atom is in its n = 2 excited state when its electron absorbs in an interaction with a photon. What is the energy of the resulting free electron?
A)6.1 eV
B)7.9 eV
C)8.2 eV
D)9.2 eV

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Multiple Choice

Q 53Q 53

A hydrogen atom makes a downward transition from the state to the state. Find the wavelength of the emitted photon. (c = 3.00 × 10

^{8}m/s, 1 eV = 1.60 × 10^{-19 }J, h = 6.626 × 10^{-}^{34}J ∙ s) A)2.56 μm B)1.54 μm C)2.05 μm D)3.07 μmFree

Multiple Choice

Q 54Q 54

The longest wavelength photon that can be emitted by a hydrogen atom, for which the final state is is closest to which one of the following values? (c = 3.0 × 10

^{8}m/s, A)39,000 nm B)22,000 nm C)7400 nm D)16,000 nm E)28,000 nmFree

Multiple Choice

Q 55Q 55

The shortest wavelength of a photon that can be emitted by a hydrogen atom, for which the initial state is is closest to which one of the following values?
A)92 nm
B)82 nm
C)72 nm
D)62 nm
E)52 nm

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Multiple Choice

Q 56Q 56

The longest wavelength of a photon that can be emitted by a hydrogen atom, for which the initial state is n = 3, is closest to which one of the following values? (c = 3.00 × 10

^{8}m/s, h = 6.626 × 10^{-34}J ∙ s, 1 eV = 1.60 × 10^{-19 }J) A)550 nm B)575 nm C)600 nm D)625 nm E)658 nmFree

Multiple Choice

Q 57Q 57

What is the shortest wavelength of a photon that can be emitted by a hydrogen atom, for which the initial state is n = 3? (c = 3.00 × 10

^{8}m/s, h = 6.626 × 10^{-34}J ∙ s, 1 eV = 1.60 × 10^{-19 }J) A)822 nm B)850 nm C)103 nm D)91.4 nm E)950 nmFree

Multiple Choice

Q 58Q 58

What is the energy required to remove the electron from a hydrogen atom in the n = 11 state?
A)0.112 eV
B)1.24 eV
C)13.5 eV
D)12.4 eV
E)0.141 eV

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Multiple Choice

Q 59Q 59

If light excites atomic hydrogen from its lowest energy level to the n = 12 level, what is the energy of the photons of this light?
A)13.5 eV
B)32.2 eV
C)13.6 eV
D)0.0944 eV
E)1.13 eV

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Multiple Choice

Q 60Q 60

Light shines through atomic hydrogen gas that was initially in its ground state. You observe that after awhile much of the hydrogen gas has been excited to its n = 5 state. What wavelength of light entering the gas caused this excitation? (c = 3.00 × 10

^{8}m/s, h = 6.626 × 10^{-34}J ∙ s, 1 eV = 1.60 × 10^{-19 }J) A)110 nm B)91.4 nm C)95.2 nm D)2280 nmFree

Multiple Choice

Q 61Q 61

Radio astronomers often study the radiation emitted by a hydrogen atom from a transition between the two hyperfine levels associated with the ground state. This radiation has a wavelength of 21 cm. What is the energy difference between the hyperfine levels? (1 eV = 1.60 × 10

^{-19}J) A)5.9 × 10^{-6}eV B)5.9 × 10^{-25}J C)1.7 × 10^{-24}J D)4.7 × 10^{-25}JFree

Multiple Choice

Q 62Q 62

In a transition from one vibrational state to another, a molecule emits a photon of wavelength 5.56 µm. What is the energy difference between these two states? (c = 3.00 × 10

^{8}m/s, h = 6.626 × 10^{-34}J ∙ s, 1 eV = 1.60 × 10^{-19 }J) A)0.223 eV B)2.23 MeV C)13.6 eV D)13.6 MeV E)0.223 MeVFree

Multiple Choice

Q 63Q 63

What is the wavelength of the photon emitted when an electron in a hydrogen atom which is in the initial state n

_{ }= 8 jumps to the final state n = 2? (c = 3.00 × 10^{8}m/s, h = 6.626 × 10^{-34}J ∙ s, 1 eV = 1.60 × 10^{-19 }J) A)205 nm B)104 nm C)389 nm D)486 nm E)610 nmFree

Multiple Choice

Q 64Q 64

What is the wavelength of the photon emitted when an electron in a hydrogen atom which is in the initial state n = 4 jumps to the final state n = 2? (c = 3.00 × 10

^{8}m/s, h = 6.626 × 10^{-34}J ∙ s, 1 eV = 1.60 × 10^{-19 }J) A)243 nm B)486 nm C)556 nm D)312 nm E)609 nmFree

Multiple Choice

Q 65Q 65

The wavelength of the emitted photon if an electron in the hydrogen atom makes a transition from the n = 2 state to the ground state is closest to which of the following values? (c = 3.0 × 10

^{8}m/s, h = 6.626 × 10^{-34}J ∙ s, 1 eV = 1.60 × 10^{-19 }J) A)122 nm B)203 nm C)243 nm D)389 nm E)411 nmFree

Multiple Choice

Q 66Q 66

What is the wavelength of the emitted photon if an electron in the hydrogen atom makes a transition from the n = 7 state to the n = 2 state? (c = 3.00 × 10

^{8}m/s, h = 6.626 × 10^{-34}J ∙ s, 1 eV = 1.60 × 10^{-19 }J) A)199 nm B)365 nm C)4480 nm D)398 nm E)796 nmFree

Multiple Choice

Q 67Q 67

What frequency must a photon have to raise an electron in a hydrogen atom from the n = 2 to the n = 4 state? (h = 6.626 × 10

^{-34}J ∙ s, 1 eV = 1.60 × 10^{-19 }J) A)3.06 × 10^{14}Hz B)6.16 × 10^{14}Hz C)4.11 × 10^{14}Hz D)5.20 × 10^{14}Hz E)9.24 × 10^{14}HzFree

Multiple Choice

Q 68Q 68

In making a transition from state n = 1 to state n = 2, the hydrogen atom must
A)absorb a photon of energy 10.2 eV.
B)emit a photon of energy 10.2 eV.
C)absorb a photon of energy 13.58 eV.
D)emit a photon of energy 13.58 eV.

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Multiple Choice

Q 69Q 69

In the n = 1 state, the energy of the hydrogen atom is -13.6 eV. What is its energy in the n = 2 state?
A)-6.79 eV
B)-4.53 eV
C)-3.40 eV
D)-1.51 eV

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Multiple Choice

Q 70Q 70

Consider the Bohr model for the hydrogen atom in its second excited state.
(a)Determine the binding energy (eV)of the electron.
(b)What is the radius of the electron orbit, given that r

_{1}= 0.0529 nm? (c)How far is it from the next higher excited orbit?Free

Essay

Q 71Q 71

A hydrogen atom with a barely bound electron may have an average radius as large as a bacterium, which is a radius of What is the nearest principal quantum number of the atom in this state? The radius for ground state hydrogen is 0.0529 nm.
A)514
B)51
C)16
D)264,650

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Multiple Choice

Q 72Q 72

Calculate the orbital Bohr radius of the excited state in a hydrogen atom.
A)0.212 nm
B)0.106 nm
C)0.170 nm
D)0.244 nm

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Multiple Choice

Q 73Q 73

Given that the speed of an electron in the ground state of hydrogen is 2190 km/s, what is the speed of an electron in the n = 4 orbit of hydrogen?
A)547 km/s
B)31,000 km/s
C)139 km/s
D)178 km/s
E)2180 km/s

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Multiple Choice

Q 74Q 74

For an electron in the M (n = 3)shell, find (a)the largest possible orbital angular momentum it can have, and (b)the smallest possible orbital angular momentum it can have. Express your answers in SI units, and for each case indicate the subshell (s, p, d, ...)of the electron. (h = 6.626 × 10

^{-34}J ∙ s)Free

Essay

Q 75Q 75

An atom has completely filled inner shells and a single valence electron in an excited p state. The filled inner shells have an orbital momentum equal to zero. What is the magnitude of the orbital angular momentum of the atom?
A)1.0
B)1.2
C)1.4
D)1.7
E)2.0

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Multiple Choice

Q 76Q 76

What is the greatest magnitude of the orbital angular momentum L that you can find in a state with
A)5.48
B)5.92
C)6
D)6.48

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Multiple Choice

Q 77Q 77

Consider the n = 10 shell.
(a)What is the largest value of the angular momentum quantum number, ℓ, in this shell?
(b)How many electrons can be placed in this shell?

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Essay

Q 78Q 78

An atom with atomic number 6 is in its ground state. How many electrons are in its outermost shell?

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Q 79Q 79

Write out the electron configuration for the ground state of the phosphorus atom, which has 15 electrons.

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Q 80Q 80

The only valid electron state and shell designation among the following is
A)1p, K (n = 1)shell.
B)2s, K (n = 1)shell.
C)1s, L (n = 2)shell.
D)2p, L (n = 2)shell.
E)3f, M (n = 3)shell.

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Multiple Choice

Q 81Q 81

The only invalid electron state and shell designation among the following is
A)1s, K (n = 1)shell.
B)2s, L (n = 2)shell.
C)2d, L (n = 2)shell.
D)3s, M (n = 3)shell.
E)3d, M (n = 3)shell.

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Multiple Choice

Q 82Q 82

What is the electron configuration for Li, which has 3 electrons?
A)1s

^{3}B)1s^{1}2s^{2}C)1s^{2 }2s^{1}D)1s^{2 }1p^{1}E)1s^{1}2s^{1}3s^{1}Free

Multiple Choice

Q 83Q 83

What is the correct ground state electron configuration of boron, which has 5 electrons?
A)1s

^{2 }2s^{2 }2p B)1s^{2 }2s^{2 }2p^{3}C)1s^{2 }1p^{2 }2s D)1s^{2 }2p^{2 }3s E)1s^{2 }2p^{3}Free

Multiple Choice

Q 84Q 84

Which one of the following is the correct electronic configuration for carbon, which has 6 electrons?
A)1s

^{2}2s^{2}2p^{2}B)1s^{1}2p^{1}C)1s^{1}2s^{2}2p^{1}D)1s^{1}2s^{1}2p^{1}E)1s^{2}2s^{2}2p^{4}Free

Multiple Choice

Q 85Q 85

Which one of the following is the correct electronic configuration for the sodium atom, which has 11 electrons?
A)1s

^{1}2s^{2}3p^{6}2s^{2}B)1s^{2}2s^{1}3p^{6}2s^{2}C)1s^{1}2s^{2}2p^{6}2s^{2}D)1s^{2}2s^{2}2p^{6}3s^{2}E)1s^{2}2s^{2}2p^{6}3s^{1}Free

Multiple Choice

Q 86Q 86

A hydrogen atom is in the 6h state. How many electrons are allowed in this state?
A)22
B)18
C)14
D)10
E)6

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Multiple Choice

Q 87Q 87

A hydrogen atom is in the 6h state. Which one of the following numbers could be an orbital angular momentum quantum number ℓ for that state?
A)5
B)6
C)7
D)8
E)9

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Multiple Choice

Q 88Q 88

A hydrogen atom is in the 6h state. Which one of the following is not a magnetic quantum number for that state?
A)0
B)1
C)2
D)4
E)6

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Multiple Choice

Q 89Q 89

In a hydrogen atom, a given electron has n = 7. How many possible values can ℓ have?
A)6
B)7
C)15
D)98

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Multiple Choice

Q 90Q 90

In a hydrogen atom, a given electron has ℓ = 7. How many possible values can m

_{1}have? A)6 B)7 C)15 D)98Free

Multiple Choice

Q 91Q 91

In a hydrogen atom, an electron with n = 7 can exist in how many different quantum states?
A)6
B)7
C)15
D)98

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Multiple Choice

Q 92Q 92

How many values of the magnetic quantum number, m

_{ℓ}, are possible if the orbital angular momentum quantum number is ℓ = 2? A)1 B)2 C)3 D)4 E)5Free

Multiple Choice

Q 93Q 93

How many values of the magnetic quantum number, m

_{ℓ}, correspond to a value of ℓ = 4? A)3 B)5 C)8 D)9 E)7Free

Multiple Choice

Q 94Q 94

For the ground state of the hydrogen atom, which of the following numbers represents the correct value of the orbital angular momentum quantum number?
A)-1
B)1
C)0
D)2
E)-2

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Multiple Choice

Q 95Q 95

For the ground state of the hydrogen atom, which of the following numbers represents the correct value of the magnetic quantum number?
A)-1
B)0
C)1
D)2
E)-2

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Multiple Choice

Q 96Q 96

How many values can the magnetic quantum number have in a hydrogen atom for which the orbital angular momentum quantum number is equal to 8?
A)9
B)15
C)5
D)8
E)17

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Multiple Choice

Q 97Q 97

How many unique quantum states correspond to the lowest possible energy level of an electron in the hydrogen atom?
A)3
B)0
C)1
D)4
E)2

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Multiple Choice

Q 98Q 98

How many electrons can be found with principal quantum number in a suitably heavy atom?
A)18
B)6
C)20
D)9

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Multiple Choice

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Multiple Choice

Q 101Q 101

What is the maximum number of electrons that can occupy the g subshell?
A)10
B)14
C)18
D)22

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Multiple Choice

Q 102Q 102

How many possible sets of electron states (or quantum numbers)are there in the 5f subshell?
A)2
B)8
C)10
D)14

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Multiple Choice

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Multiple Choice

Q 104Q 104

The values of n and ℓ for a 4f subshell are
A)n = 4, ℓ = 4.
B)n = 4, ℓ = 3.
C)n = 3, ℓ = 3.
D)n = 4, ℓ = 2.
E)n = 3, ℓ = -3.

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Multiple Choice

Q 105Q 105

Neon has 10 electrons. What is the value of Z of the next higher element that has chemical properties very similar to those of neon?
A)11
B)17
C)18
D)19
E)36

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Multiple Choice