Deck 7: Electrons in Atoms and Periodic Properties

Question 1

What is the frequency (, in Hz) of the photons emitted by a He-Ne laser with a wavelength () of 632.8 nm?

A) 4.738  10⁵ Hz
B) 1.897  10² Hz
C) 1.897  10¹¹ Hz
D) 4.741  10¹⁴ Hz
E) 1.897  10¹⁴ Hz

Answer 1

4.741  10¹⁴ Hz

Question 2

Which of the following is quantized?

A) the trajectory of a baseball hit from home plate
B) the speed of a Formula-1 race car
C) the diameter of a redwood tree
D) the number of marbles in a bag
E) your age

Answer 2

the number of marbles in a bag

Question 3

What is the minimum frequency of a photon that can eject a photoelectron from Ba metal? (The work function of barium is  = 4.3  10^-19 J.)

A) 2.8  10^-52 Hz
B) 6.5  10¹⁴ Hz
C) 6.5  10⁴ Hz
D) 6.5  10¹³ Hz
E) 2.8  10¹⁴ Hz

Answer 3

6.5  10¹⁴ Hz

Question 4

Indicate which metal requires the shortest wavelength photons to eject photoelectrons based on the following graph.

A) a
B) b
C) c
D) d

Question 5

Which of the following types of electromagnetic radiation has the longest wavelength?

A) gamma rays
B) X-rays
C) radio waves
D) infrared
E) visible

Question 6

Based on the following graph, which metal will emit the highest energy photoelectron when a photon with a frequency of 3.9  10¹⁴ Hz is incident on the metal?

A) a
B) b
C) c
D) d

Question 7

Which of the following occurs only in discrete (quantized) increments?

A) the speed a car drives on the interstate
B) the altitude that an airplane flies
C) time
D) the level of water in a sink
E) money

Question 8

In comparing the Fraunhofer lines with light emitted by elements in a flame, Bunsen and Kirchhoff demonstrated that __________

A) atoms emit and absorb electromagnetic radiation at characteristic wavelengths.
B) the solar spectrum has dark lines.
C) helium may be found in minerals that contain uranium.
D) electrons are responsible for the absorption and emission of electromagnetic radiation.
E) the solar spectrum has bright lines.

Question 9

Indicate which of the following photons can cause emission of photoelectrons from a surface of gallium ( = 6.7  10^-19 J).

A) 350 nm
B) 400 nm
C) 200 nm
D) 650 nm
E) 500 nm

Question 10

What is the wavelength (, in m) of a radio station operating at a frequency of 99.6 MHz?

A) 3.01  10⁶ m
B) 3.01 m
C) 3.32  10^-7 m
D) 0.332 m
E) 3.32 m

Question 11

In refraction, polychromatic light is dispersed into its component wavelengths by __________

A) constructive and destructive interference of light waves in air.
B) internal reflections within a prism.
C) differences in the bending of different wavelengths of light by a prism.
D) constructive and destructive interference of light waves in a prism.
E) the reduction in the intensity of white light to reveal the colors.

Question 12

Which statement about electromagnetic radiation is not correct?

A) Electromagnetic radiation consists of oscillating electric and magnetic fields.
B) Electromagnetic radiation is emitted by all stars.
C) All electromagnetic radiation is visible to the eye.
D) Electromagnetic radiation spans a very wide range of wavelengths from gamma rays to radio waves.
E) The frequency and wavelength of electromagnetic radiation are related to each other.

Question 13

Which of the following types of electromagnetic radiation has the shortest wavelength?

A) gamma rays
B) X-rays
C) radio waves
D) infrared
E) visible

Question 14

Fraunhofer lines are due to __________

A) emission of radiation.
B) absorption of radiation.
C) the photoelectric effect.
D) constructive interference.
E) destructive interference.

Question 15

The Fraunhofer lines are evidence that __________

A) atoms contain nuclei.
B) atoms contain electrons.
C) waves interfere constructively.
D) elements absorb light.
E) elements emit light.

Question 16

The fact that the absorption and emission spectra of atoms and their ions are different is evidence that the spectra are due to __________

A) electrons.
B) protons.
C) neutrons.
D) the nuclei.
E) electromagnetic interactions.

Question 17

The studies of light emitted by hot objects (Max Planck) and the photoelectric effect (Albert Einstein) revolutionized physics because they revealed __________

A) that energy is quantized.
B) that light intensity does not affect the number of electrons ejected from a metal.
C) that atomic spectra are due to the quantized transitions of electrons.
D) that blackbody radiation is continuous.
E) that atomic spectra are continuous.

Question 18

The work function of sodium is  = 2.9  10^-19 J. What is the maximum wavelength that can cause ejection of photoelectrons from a sodium surface?

A) 151 nm
B) 222 nm
C) 45.1 nm
D) 451 nm
E) 685 nm

Question 19

Atomic spectra are due to the changes in the energy of __________

A) protons.
B) neutrons.
C) nuclei.
D) electrons.
E) electromagnetic radiation.

Question 20

The emission spectra of Na and Na⁺ are different because __________

A) Na⁺ has fewer electrons.
B) Na has fewer electrons.
C) Na⁺ has more protons.
D) Na has fewer neutrons.
E) Na has more protons.

Question 21

Indicate which of the following sources produces the highest energy photons.

A) a radio station with  = 106.7 MHz
B) a dentist's X-ray source with  = 100 pm
C) the laser in a CD player with  = 650 nm
D) a microwave oven with  = 6.0  10¹⁰ Hz
E) your cell phone with  = 1.750 GHz

Question 22

Which of the following photons has the lowest frequency?

A) a photon from a Nd:YAG laser with  = 1064 nm
B) a photon from an Ar⁺ laser with  = 514.5 nm
C) a photon from a Kr⁺ laser with  = 647 nm
D) a photon from an ArF laser with  = 193 nm
E) a photon from a He-Ne laser with  = 633 nm

Question 23

Which of the following photons has the highest energy?

A) a photon from a Nd:YAG laser with  = 1064 nm
B) a photon from an Ar⁺ laser with  = 514.5 nm
C) a photon from a Kr⁺ laser with  = 647 nm
D) a photon from an ArF laser with  = 193 nm
E) a photon from a He-Ne laser with  = 633 nm

Question 24

The study of light emitted by the hydrogen atom by Johann Balmer, Johannes Rydberg, Niels Bohr and others revolutionized physics because it revealed that __________

A) energy is quantized.
B) light intensity does not affect the number of atoms excited.
C) the emitted light is produced by the electron making a transition between quantized energy levels.
D) blackbody radiation is continuous.
E) atomic spectra are continuous.

Question 25

If each of the following metals is exposed to light with a wavelength of 240 nm, which will emit photoelectrons with the greatest kinetic energy?

A) iron ( = 7.2  10^-19 J)
B) platinum ( = 9.1  10^-19 J)
C) nickel ( = 8.3  10^-19 J)
D) palladium ( = 8.2  10^-19 J)
E) sodium ( = 4.4  10^-19 J)

Question 26

Which of the following sources produces the lowest energy photons?

A) a doctor's X-ray source
B) the heat lamp in your bathroom
C) a microwave oven
D) gamma rays from a star
E) radio waves from your local station

Question 27

Which of the following will lead to an increase in the kinetic energies of photoelectrons emitted when light is incident on a metal surface?

A) decrease in the light's wavelength
B) increase in the light's intensity
C) increase in the light's wavelength
D) decrease in the light's frequency
E) decrease in the light's intensity

Question 28

What is the energy (E, in J) of the photons emitted by an Ar⁺ laser with a wavelength of  = 488 nm?

A) 2.46  10¹⁸ J
B) 9.69  10^-23 J
C) 1.36  10^-36 J
D) 4.07  10^-19 J
E) 2.46  10^-18 J

Question 29

Based on the following graph, which metal will emit the highest energy photoelectron when a photon with a wavelength of 650 nm is incident on the metal?

A) a
B) b
C) c
D) d

Question 30

Which of the following photons has the lowest energy?

A) a photon from a Nd:YAG laser with  = 1064 nm
B) a photon from an Ar⁺ laser with  = 514.5 nm
C) a photon from a Kr⁺ laser with  = 647 nm
D) a photon from an ArF laser with  = 193 nm
E) a photon from a He-Ne laser with  = 633 nm

Question 31

Which of the following photons has the highest frequency?

A) a photon from a Nd:YAG laser with  = 1064 nm
B) a photon from an Ar⁺ laser with  = 514.5 nm
C) a photon from a Kr⁺ laser with  = 647 nm
D) a photon from an ArF laser with  = 193 nm
E) a photon from a He-Ne laser with  = 633 nm

Question 32

What wavelength of light is required to cause the ejection of photoelectrons with kinetic energies of 5.0  10^-20 J from a calcium surface ( = 4.60  10^-19 J)?

A) 485 nm
B) 390 nm
C) 308 nm
D) 632 nm
E) 480 nm

Question 33

Which of the following metals would be an appropriate choice for the construction of a photon detector for 550 nm light?

A) sodium ( = 4.4  10^-19 J)
B) rubidium ( = 3.5  10^-19J)
C) barium ( = 4.3  10^-19 J)
D) gold ( = 8.2  10^-19 J)
E) platinum ( = 9.1  10^-19 J)

Question 34

What is the energy (E, in J) of a photon from a microwave oven with a frequency of  = 6.0  10¹⁰ Hz?

A) 3.98  10^-30 J
B) 3.98  10^-39 J
C) 3.98  10^-23 J
D) 3.98  10^-17 J
E) 3.98  10^-13 J

Question 35

Electromagnetic radiation with a frequency of 8.6  10¹⁴ Hz incident on an unknown metal surface causes ejection of photoelectrons with kinetic energies of 1.3  10^-19 J. What is the unknown metal?

A) rubidium ( = 3.5  10^-19 J)
B) gold ( = 8.2  10^-19 J)
C) nickel ( = 8.3  10^-19 J)
D) sodium ( = 4.4  10^-19 J)
E) platinum ( = 9.1  10^-19 J)

Question 36

Which of the following sources produces the highest energy photons?

A) a doctor's X-ray source
B) the heat lamp in your bathroom
C) a microwave oven
D) gamma rays from a star
E) radio waves from your local station

Question 37

What is the kinetic energy of the photoelectrons emitted from a sodium surface ( = 2.9  10^-19 J) when it is irradiated by photons with a wavelength of 350 nm?

A) 2.9  10^-19 J
B) 5.7  10^-19 J
C) 0 J
D) 2.8  10^-19 J
E) 3.6  10^-19 J

Question 38

Which transition in a hydrogen atom requires the largest change in energy?

A) n₁ = 2 to n₂ = 3
B) n₁ = 2 to n₂ = 4
C) n₁ = 1 to n₂ = 3
D) n₁ = 1 to n₂ = 2
E) n₁ = 9 to n₂ = 10

Question 39

Indicate which of the following sources produces the lowest energy photons.

A) a radio station with  = 106.7 MHz
B) a dentist's X-ray source with  = 100 pm
C) the laser in a CD player with  = 650 nm
D) a microwave oven with  = 6.0  10¹⁰ Hz
E) your cell phone with  = 1.750 GHz

Question 40

Which of the transitions in the hydrogen atom energy-level diagram shown here is not possible?

A) a
B) b
C) c
D) d

Question 41

Which of the following is not an allowed value for the principal quantum number?

A) 1
B) 3
C) 10
D) 0
E) 2

Question 42

The change in energy of a one-electron atom or ion for an electronic transition from the initial energy level n_i to the final energy level n_f is given by E = -(2.18  10^-18 J) Z² Which of the following species will have the longest wavelength emission line for the transition between the n_i = 2 and n_f = 1 levels?

A) H
B) He⁺
C) Li²⁺
D) Be³⁺
E) B⁴⁺

Question 43

What quantum numbers are possible when n = 3?

A) 1 and 2
B) 1, 2, and 3
C) 0, 1, 2, and 3
D) 0, 1, and 2
E) any integer

Question 44

Which of the transitions in the hydrogen atom energy-level diagram shown here requires the longest wavelength photon?

A) a
B) b
C) c
D) d

Question 45

Which of the transitions in the following hydrogen atom energy-level diagram involves the shortest wavelength photon?

A) a
B) b
C) c
D) d

Question 46

The energy of a one-electron atom is given by E = -(2.18  10^-18 J) where Z is the atomic number of the element. Which of the following one-electron ions has the largest ionization energy?

A) Li²⁺
B) Be³⁺
C) He⁺
D) B⁴⁺
E) C⁵⁺

Question 47

A shell is defined by __________

A) the quantum number.
B) the m_l quantum number.
C) the m_s quantum number.
D) the n quantum number.
E) both the and m_l quantum numbers.

Question 48

In quantum mechanics, an atomic orbital __________

A) provides the position of an electron at any instant of time in the space around an atomic nucleus.
B) locates all the electrons in an atom.
C) is identical to the orbits Bohr used in his analysis of the hydrogen atom.
D) identifies the most probable position of an atomic nucleus.
E) provides the probability of finding an electron at any point in the space around an atomic nucleus.

Question 49

What is the speed of an argon atom that has a de Broglie wavelength of 5.2 pm?

A) 0.52 m/s
B) 5.2  10³ m/s
C) 1.9  10³ m/s
D) 1.9 m/s
E) 25 m/s

Question 50

Which transition in a hydrogen atom will cause emission of the shortest wavelength photon?

A) n₁ = 4 to n₂ = 3
B) n₁ = 4 to n₂ = 2
C) n₁ = 3 to n₂ = 2
D) n₁ = 3 to n₂ = 1
E) n₁ = 10 to n₂ = 9

Question 51

De Broglie reasoned that for the electron in the hydrogen atom to behave as a stable circular wave, the circumference of the electron's orbit must be __________

A) equal to the wavelength of the electron.
B) an integer multiple of the electron's wavelength.
C) a half integer multiple of the electron's wavelength.
D) twice the wavelength of the electron.
E) twice the diameter of the orbit.

Question 52

Recently, buckyballs (C₆₀) became the largest object with a measured de Broglie wavelength. If the mass of a C₆₀ molecule is 1.20  10^-24 kg, what will be its de Broglie wavelength if it is moving at a speed of 220 m/sec?

A) 2.52 pm
B) 2.52 fm
C) 2.52 m
D) 1.20 pm
E) 5.22 m

Question 53

Which of the following electrons will have the smallest de Broglie wavelength?

A) an electron moving 220 m/sec
B) an electron moving 20 mi/hr
C) an electron moving 75 km/hr
D) an electron moving at 25% the speed of light
E) an electron at rest with no velocity

Question 54

How much energy is required to ionize a He⁺ ion in its ground state?

A) 2.18  10^-18 J
B) 4.36  10^-18 J
C) 8.72  10^-18 J
D) 1.74  10^-18 J

Question 55

Subshells are __________

A) orbitals with the same principal and angular momentum quantum numbers.
B) orbitals with the same principal quantum numbers.
C) orbitals with the same angular momentum quantum numbers.
D) orbitals with the same angular momentum and magnetic quantum numbers.
E) orbitals with the same spin quantum number.

Question 56

According to de Broglie, if the circumference of the electron's orbit in the hydrogen atom is twice the electron's wavelength, the orbit will __________

A) decay until the electron falls into the nucleus.
B) diverge, allowing the electron to escape.
C) be stable.
D) cause the electron to emit a photon.
E) not be circular.

Question 57

A shell consists of all __________

A) electrons with the same quantum number.
B) orbitals with the same quantum numbers.
C) orbitals with the same principal quantum number.
D) electrons with the same magnetic quantum number.
E) orbitals with the same and m_l quantum numbers.

Question 58

Which of the following objects, all moving at the same speed, will have the largest de Broglie wavelength?

A) a proton
B) an electron
C) a bowling ball
D) a neon atom
E) a neutron

Question 59

The mathematical description of an electron as a wave was developed by __________

A) Bohr.
B) Heisenberg.
C) Einstein.
D) De Broglie.
E) Schrödinger.

Question 60

Determine the wavelength of the line in the hydrogen atom spectrum corresponding to the n₁ = 3 to n₂ = 4 transition.

A) 1094 nm
B) 1875 nm
C) 656 nm
D) 335 nm
E) 109 nm

Question 61

Which combination of quantum numbers is possible for an atom with five orbitals in one subshell?

A) n = 1, = 0
B)n = 2, = 4
C) n = 3, = 2
D) n = 4, = 4
E) n = 5, = 0

Question 62

Which of the following represents an s orbital?

A)
B)
C)
D)

Question 63

How many orbitals exist for the quantum numbers n = 4, = 1?

A) 1
B) 2
C) 3
D) 4
E) 7

Question 64

What are the principal and angular momentum quantum numbers for a 4f orbital?

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

Question 65

The size of a typical atomic orbital is on the order of __________

A) femtometers.
B) picometers.
C) nanometers.
D) micrometers.
E) millimeters.

Question 66

Which of the following is the ground-state electron configuration of the Mg²⁺ ion?

A) 1s²2s²2p⁶3s²
B) [Ne]3s²
C) [Ne]3s²3p²
D) [He]2s²2p⁶
E) [He]2s²2p⁸

Question 67

Which subshell only has five orbitals?

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

Question 68

Which of the following orbitals is the lowest in energy (assuming they are all in the same shell)?

A)
B)
C)
D)

Question 69

The atomic radius of germanium (Z = 32) is smaller than the atomic radius of potassium (Z = 19) because of __________

A) a change in the n quantum number.
B) an increase in the effective nuclear charge.
C) the fact that p and d orbitals have the same orbital penetration.
D) a decrease in the effective nuclear charge.
E) germanium having 32 rather than 19 electrons.

Question 70

Which of the following atoms has no unpaired electrons?

A) B
B) C
C) O
D) Mg
E) Na

Question 71

How many unpaired electrons does the nitride (N^3-) ion have?

A) 0
B) 1
C) 2
D) 3
E) 6

Question 72

If the principal quantum number is seven (n = 7) and the angular momentum quantum number is three ( = 3), which of the following values is not an allowed value of the magnetic quantum number (m_l)?

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

Question 73

Which of the following elements has the ground-state electron configuration 1s²2s²2p⁶3s²3p⁴?

A) Al
B) Cl
C) S
D) P
E) Ar

Question 74

Which of the following atoms or ions has a single unpaired electron?

A) He
B) Sr
C) Na⁺
D) Al
E) Be

Question 75

Which of the following is a possible set of quantum numbers for a 3d orbital?

A) n = 3, = 1, m
= -1
B) n = 3, = 0, m
= 0
C) n = 3, = 2, m
= 3
D) n = 3, = 2, m
= 0
E) n = 3, = 1, m
= 2

Question 76

A certain shell is known to have a total of 16 orbitals. Which shell is it?

A) n = 4
B) n = 16
C) n = 8
D) n = 2

Question 77

What is the ground-state electron configuration of a Cl^- ion?

A) 1s²2s²2p⁶3s²3p⁴
B) 1s²2s²2p⁶3s²3p⁵
C) 1s²2s²2p⁶3s²3p⁶
D) 1s²2s²2p⁶3s²3p²
E) 1s²2s²2p⁶3s²3p⁸

Question 78

Which arrangement is correct for increasing atomic radius?

A) C < N < F
B) Rb < K < Li
C) Sc < Ge < Br
D) Se < Cu < Ca
E) H < He

Question 79

What is the orbital designation for an electron with the quantum numbers n = 3, = 2?

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

Question 80

How many orbitals are possible for the n = 2 shell?

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