Deck 7: The Electronic Structure of Atoms

Question 1

What is the binding energy (in J/mol or kJ/mol)of an electron in a metal whose threshold frequency for photoelectrons is 2.50 * 10¹⁴ /s?

A)99.7 kJ/mol
B)1.66 * 10^-19 J/mol
C)2.75 * 10^-43 J/mol
D)7.22 * 10¹⁷ kJ/mol
E)1.20 * 10^-6 J/mol

Answer 1

99.7 kJ/mol

Question 2

What is the energy in joules of a mole of photons associated with red light of wavelength 7.00 * 10² nm?

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

Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 6 to the n = 3 principal energy level. Recall that for hydrogen E_n = -2.18 * 10^-18 J(1/n²).

A)1.64 * 10¹⁵ /s
B)9.13 * 10¹³ /s
C)3.65 * 10¹⁴ /s
D)1.82 * 10^-19 /s
E)2.74 * 10¹⁴/s

Answer 3

2.74 * 10¹⁴/s

Question 4

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 E_n = -2.18 * 10^-18 J(1/n²)

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

Question 5

Calculate the frequency of visible light having a wavelength of 686 nm.

A)4.37 * 10¹⁴ /s
B)4.37 * 10⁵ /s
C)6.17 * 10¹⁴ /s
D)2.29 * 10^-15 /s
E)2.29 * 10^-6 /s

Question 6

What is the energy in joules of a mole of photons associated with visible light of wavelength 486 nm?

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

In the following diagram of a wave

A)(a)is amplitude and (b)is wavelength
B)(a)is frequency and (b)is amplitude
C)(a)is wavelength and (b)is frequency
D)(a)is amplitude and (b)is frequency
E)(a)is wavelength and (b)is amplitude

Question 8

The second line of the Balmer series occurs at a wavelength of 486.1 nm. What is the energy difference between the initial and final levels of the hydrogen atom in this emission process?

A)2.44 * 10¹⁸ J
B)4.09 * 10^-19 J
C)4.09 * 10^-22 J
D)4.09 * 10^-28 J
E)1.07 * 10^-48 J

Question 9

A proton is roughly 1800 times more massive than an electron. If a proton and an electron are traveling at the same speed,

A)the wavelength of the photon will be about 1800 times longer than the wavelength of the electron.
B)the wavelength of the photon will be about times longer than the wavelength of the electron.
C)the wavelength of the photon will be roughly equal to the wavelength of the electron.
D)the wavelength of the electron will be about times longer than the wavelength of the photon.
E)the wavelength of the electron will be about 1800 times longer than the wavelength of the photon.

Question 10

If a hydrogen atom and a helium atom are traveling at the same speed,

A)the wavelength of the hydrogen atom will be about 4 times longer than the wavelength of the helium atom.
B)the wavelength of the hydrogen atom will be about 2 times longer than the wavelength of the helium.
C)the wavelength of the hydrogen atom will be roughly equal to the wavelength of the helium atom.
D)the wavelength of the helium atom will be about 2 times longer than the wavelength of the hydrogen atom.
E)the wavelength of the helium atom will be about 4 times longer than the wavelength of the hydrogen atom.

Question 11

What is the wavelength of radiation that has a frequency of 2.10 * 10¹⁴ s ^-1?

A)6.30 * 10²² m
B)7.00 * 10² nm
C)7.00 * 10⁵ m
D)1.43 * 10^-6 m
E)3.00 * 10⁸ m

Question 12

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 13

Complete this sentence: Atoms emit visible and ultraviolet light

A)as electrons jump from lower energy levels to higher levels.
B)as the atoms condense from a gas to a liquid.
C)as electrons jump from higher energy levels to lower levels.
D)as they are heated and the solid melts to form a liquid.
E)as the electrons move about the atom within an orbit.

Question 14

Calculate the frequency of visible light having a wavelength of 486 nm.

A)2.06 * 10¹⁴ /s
B)2.06 * 10⁶ /s
C)6.17 * 10¹⁴ /s
D)1.20 * 10^-15 /s
E)4.86 * 10^-7 /s

Question 15

Calculate the wavelength 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)

A)97.2 nm
B)82.6 nm
C)365 nm
D)0.612 nm
E)6.8 * 10^-18 nm

Question 16

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)

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

Question 17

What is the energy in joules of one photon of microwave radiation with a wavelength 0.122 m? (c = 2.9979 * 10⁸ m/s; h = 6.626 * 10^-34 J.s)

A)2.70 * 10^-43 J
B)5.43 * 10^-33 J
C)1.63 * 10^-24 J
D)4.07 * 10^-10 J
E)2.46 * 10⁹ J

Question 18

What is the wavelength of radiation that has a frequency of 5.39 * 10¹⁴ s^-1? (c = 2.9979 * 10⁸ m/s)

A)1.80 * 10^-3 nm
B)556 nm
C)618 nm
D)6180 nm
E)1.61 * 10²³ nm

Question 19

A photon is roughly 1800 times more massive than an electron. If a proton and an electron have the same kinetic energy,

A)the wavelength of the photon will be about 1800 times longer than the wavelength of the electron.
B)the wavelength of the photon will be about times longer than the wavelength of the electron.
C)the wavelength of the photon will be roughly equal to the wavelength of the electron.
D)the wavelength of the electron will be about times longer than the wavelength of the photon.
E)the wavelength of the electron will be about 1800 times longer than the wavelength of the photon.

Question 20

As the frequency of an electromagnetic wave increases

A)its speed must increase.
B)its wavelength must increase.
C)its amplitude must increase.
D)its energy must increase.

Question 21

In an electron microscope, electrons are accelerated to great velocities. Calculate the wavelength of an electron traveling with a velocity of 7.0 * 10³ kilometers per second. The mass of an electron is 9.1 * 10^-28 g.

A)1.0 * 10^-13 m
B)1.0 * 10^-7 m
C)1.0 m
D)1.0 * 10^-10 m

Question 22

"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 23

Electrons can be used to probe the arrangement of atoms on a solid surface if the wavelength of the electrons is comparable with the spacing between the atoms. Which of the following electron velocities would be appropriate for use in this application if the atoms are separated by 0.320 nm?

A)2.27 * 10⁶ m/s
B)1.24 * 10³ m/s
C)3.00 * 10⁸ m/s
D)4.41 * 10⁶ m/s
E)8.06 * 10³ m/s

Question 24

A single pulse of a laser yields an average of 5.00 * 10¹⁸ photons with $\lambda$ = 633 nm. If melting ice to water at 0°C requires 6.01 kJ/mol, what is the fewest number of laser pulses need to melt 10.0 g of ice?

A)3830
B)3340
C)38300
D)2120
E)212

Question 25

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

A)
B)
C)
D)
E)

Question 26

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 27

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 28

When photons with a wavelength of 310. nm strike a magnesium plate, the maximum velocity of the ejected electrons is 3.45 *10⁵ m/s. Calculate the binding energy of electrons to the magnesium surface.

A)386 kJ/mol
B)419 kJ/mol
C)32.7 kJ/mol
D)321 kJ/mol
E)353 kJ/mol

Question 29

Calculate the wavelength of a neutron that has a velocity of 250 cm/s. (The mass of a neutron = 1.675 * 10^-24 g; h = 6.626 * 10^-34 J.s)

A)16 pm
B)0.016 nm
C)0.16 nm
D)160 nm
E)1.6 * 10^-4 m

Question 30

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

A)
B)
C)
D)
E)

Question 31

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

A)
B)
C)
D)
E)

Question 32

A common way of initiating certain chemical reactions with light involves the generation of free halogen atoms in solution. If $\Delta$ H for the reaction Cl₂(g) $\rarr$ 2Cl(g)is 242.8 kJ/mol, what is the longest wavelength of light that will produce free chlorine atoms in solution?

A)246.3 nm
B)465.2 nm
C)349.3 nm
D)698.6 nm
E)492.6 nm

Question 33

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

A)
B)
C)
D)
E)

Question 34

The longest wavelength of light that causes electrons to be ejected from the surface of a copper plate is 243 nm. What is the maximum velocity of the electrons ejected when light of wavelength 200. nm shines on a copper plate?

A)1.48 * 10⁶ m/s
B)6.22 * 10⁵ m/s
C)4.67 * 10⁴ m/s
D)1.97 * 10⁴ m/s
E)1.34 * 10⁶ m/s

Question 35

If a hydrogen atom and a helium atom have the same kinetic energy,

A)the wavelength of the hydrogen atom will be about 4 times longer than the wavelength of the helium atom.
B)the wavelength of the hydrogen atom will be about 2 times longer than the wavelength of the helium.
C)the wavelength of the hydrogen atom will be roughly equal to the wavelength of the helium atom.
D)the wavelength of the helium atom will be about 2 times longer than the wavelength of the hydrogen atom.
E)the wavelength of the helium atom will be about 4 times longer than the wavelength of the hydrogen atom.

Question 36

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.

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 37

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 38

The orbital diagram for a ground-state nitrogen atom is

A)
B)
C)
D)

Question 39

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 40

The number of orbitals in a d subshell is

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

Question 41

Which element has the following ground-state electron configuration? 1s²2s²2p⁶3s²

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

Question 42

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 43

Which element has the following ground-state electron configuration? [Kr]5s¹4d⁵

A)Mn
B)Mo
C)Nb
D)Re
E)Tc

Question 44

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

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

Question 45

A ground-state atom of arsenic has

A)no unpaired electrons.
B)one unpaired electron.
C)two unpaired electrons.
D)three unpaired electrons.
E)four unpaired electrons.

Question 46

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

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

Question 47

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

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

Question 48

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 49

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

A)antimony
B)germanium
C)indium
D)lead
E)tin

Question 50

Which element has the following ground-state electron configuration? [Ar]4s²3d¹⁰4p⁵

A)aresnic
B)bromine
C)iodine
D)selenium
E)tellerium

Question 51

The orbital diagram for a ground-state oxygen atom is

A)
B)
C)
D)
E)

Question 52

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 53

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

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

Question 54

The electron configuration of a ground-state vanadium atom is

A)[Ar]4s²4d³.
B)[Ar]4s²4p³.
C)[Ar]4s²3d³.
D)[Ar]3d⁵.

Question 55

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

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

Question 56

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

A)phosphorus
B)nitrogen
C)arsenic
D)vanadium
E)none of these

Question 57

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

A)phosphorus
B)germanium
C)selenium
D)tellurium
E)none of these

Question 58

Which of the following is the ground-state electron configuration of a calcium atom?

A)[Ne]3s²
B)[Ne]3s²3p⁶
C)[Ar]4s¹3d¹
D)[Ar]4s²
E)[Ar]3d²

Question 59

The orbital diagram for a ground state carbon atom is

A)
B)
C)
D)

Question 60

A ground-state atom of manganese has ___ unpaired electrons and is _____.

A)0, diamagnetic
B)2, diamagnetic
C)3, paramagnetic
D)5, paramagnetic
E)7, paramagnetic

Question 61

The ground-state electron configuration of Cr, Mo, and Ag are exceptions to the Aufbau principle. Which of the following is the electron configuration for Mo?

A)[Kr]5s¹4d⁵
B)[Kr]5s²4d⁴
C)[Xe]6s²5d⁴
D)[Ar]4s²4d⁴
E)[Kr]5s²4d⁶

Question 62

Which choice lists two elements with ground-state electron configurations that are well known exceptions to the Aufbau principle?

A)Cu and C
B)Cr and Cu
C)Cs and Cl
D)Rb and Co
E)Fe and Co

Question 63

Transition metal elements have atoms or ions with partially filled

A)s subshells.
B)p subshells.
C)d subshells.
D)f subshells.
E)g subshells.

Question 64

A ground-state chromium atom has how many unpaired electrons?

A)1
B)2
C)4
D)5
E)6

Question 65

Lanthanide (or rare earth elements)have atoms or ions with partially filled

A)s subshells.
B)p subshells.
C)d subshells.
D)f subshells.
E)g subshells.

Question 66

When the electron in a hydrogen atom falls from its first excited energy level to the ground state energy level, a photon with wavelength $\lambda$ is emitted. A proton having this same wavelength would have a velocity of

A)3.87 m/s.
B)5990 m/s.
C)1.21 * 10^-7 m/s.
D)3.26 m/s.
E)5.99 m/s.

Question 67

Which of the following is the electron configuration of an excited state of a copper atom?

A)[Ar]4s²3d⁹
B)[Ar]4s¹3d¹⁰
C)[Ar]4s¹3d⁸
D)[Ar]4s²3d⁸
E)[Ar]4s⁰3d¹⁰

Question 68

How many electrons in a ground-state cadmium atom are in orbitals labeled by m_l = -1?

A)2
B)10
C)12
D)18
E)36

Question 69

The electron in a hydrogen atom falls from an excited energy level to the ground state in two steps, causing the emission of photons with wavelengths of 1870 and 102.5 nm. What is the quantum number of the initial excited energy level from which the electron falls?

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

Question 70

Which of the following is the electron configuration of an excited state of an iron atom?

A)[Ar]4s²3d⁷
B)[Ar]4s²3d⁶
C)[Ar]4s²3d⁸
D)[Ar]4s¹3d⁷
E)[Ar]4s¹3d⁵

Question 71

Which of the following ground-state atoms is diamagnetic?

A)Ca
B)As
C)Cu
D)Fe
E)none of these

Question 72

Which of the following is diamagnetic both in its ground state and in all of its excited states?

A)Mg
B)Ne
C)Cu
D)Zn
E)none of these

Question 73

A ground-state atom of iron has ___ unpaired electrons and is _____.

A)0, diamagnetic
B)6, diamagnetic
C)3, paramagnetic
D)5, paramagnetic
E)4, paramagnetic

Question 74

When the electron in a hydrogen atom falls from the n = 3 excited energy level to the ground state energy level, a photon with wavelength $\lambda$ is emitted. An electron having this same wavelength would have a velocity of

A)7.10 * 10³ m/s.
B)2.93* 10⁶ m/s.
C)2.93 * 10³ m/s.
D)7.10 m/s.
E)3.00 * 10⁸ m/s.

Question 75

How many electrons in a ground-state tellurium atom are in orbitals labeled by l = 1?

A)4
B)10
C)12
D)16
E)22

Question 76

Which of the following is the electron configuration of an excited state of an oxygen atom?

A)1s²2s²2p⁴
B)1s²2s²2p⁵
C)1s²2s²2p³3s¹
D)1s²2s²2p⁶
E)1s²2s²2p³

Question 77

Which of the following atoms is paramagnetic both in its ground state and in all of its excited states?

A)C
B)N
C)O
D)Ti
E)Cr

Question 78

A ground-state atom of vanadium has ___ unpaired electrons and is _____.

A)0, diamagnetic
B)2, diamagnetic
C)3, paramagnetic
D)5, paramagnetic
E)4, diamagnetic

Question 79

The electron in a hydrogen atom falls from an excited energy level to the ground state in two steps, causing the emission of photons with wavelengths of 2624 and 97.2 nm. What is the quantum number of the initial excited energy level from which the electron falls?

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

Question 80

Breaking the oxygen-oxygen bond in hydrogen peroxide requires 210 kJ/mol. What is the longest wavelength of light that can cause this bond to be broken?

A)5.7 * 10^-4 m
B)9.5 * 10^-31 m
C)2.8 * 10^-7 m
D)9.5 * 10^-28 m
E)5.7 * 10^-7 m