Deck 7: A Quantum Model of Atoms: Waves and Particles

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 Hz
B)1.897 Hz
C)1.897 Hz
D)4.738 Hz
E)1.897 Hz

Answer 1

4.738 Hz

Question 2

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

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

Answer 2

money

Question 3

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.

Answer 3

Na^ has fewer electrons.

Question 4

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 5

Which of the following photons has the highest frequency?

A)a photon from an Nd:YAG laser with   1,064 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 an He-Ne laser with   633 nm

Question 6

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 7

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 8

What color will a blue object appear when it is seen through a filter with the absorption spectrum shown below?

A)blue
B)yellow
C)red
D)black
E)white

Question 9

A radio station's operating frequency has a wavelength of 2.81 m. What is this frequency?

A)1.068 MHz
B)106.8 MHz
C)100.1 MHz
D)94.5 MHz
E)9.37 MHz

Question 10

Which of the following photons has the lowest frequency?

A)a photon from a lightbulb with   500 nm
B)a photon from a particle accelerator with   10 nm
C)a photon emitted from a nuclear reaction with   425 nm
D)a photon from an N laser with   337 nm
E)a photon from a KrF eximer laser with   248 nm

Question 11

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

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

Question 12

Which of the following photons has the lowest energy?

A)a photon from a green laser pointer with   532 nm
B)a photon from a tanning bed with   325 nm
C)a photon from a telescope with   700 nm
D)a photon from a quasar with   125 nm
E)a photon from a red LED bulb with   635 nm

Question 13

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 14

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

A)3.01 m
B)3.01 m
C)3.32 m
D)0.332 m
E)3.32 m

Question 15

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

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

Question 16

What color will a red object appear when it is seen through a filter with the absorption spectrum shown below?

A)blue
B)yellow
C)red
D)black
E)white

Question 17

In comparing the dark 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 18

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 19

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)one's age

Question 20

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

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

Question 21

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

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

Question 22

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 23

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

A)3.98 J
B)3.98 J
C)3.98 J
D)3.98 J
E)3.98 J

Question 24

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 25

Which of the following photons has the highest energy?

A)a photon from a lightbulb with   500 nm
B)a photon from a particle accelerator with   10 nm
C)a photon emitted from a nuclear reaction with   425 nm
D)a photon from an N laser with   337 nm
E)a photon from a KrF eximer laser with   248 nm

Question 26

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 J)
B)platinum (  9.1 J)
C)nickel (  8.3 J)
D)palladium (  8.2 J)
E)sodium (  4.4 J)

Question 27

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 J)
B)rubidium (  3.5 J)
C)barium (  4.3 J)
D)gold (  8.2 J)
E)platinum (  9.1 J)

Question 28

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 Hz
E)your cell phone with   1.750 GHz

Question 29

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 30

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

A)2.46 J
B)9.69 J
C)1.36 J
D)4.07 J
E)2.46 J

Question 31

An atom in its ground state absorbs a single photon of light and then relaxes back to the ground state by emitting an infrared photon (1,200 nm) followed by an orange photon (600 nm). What is the wavelength of the photon that was absorbed initially?

A)600 nm
B)1,200 nm
C)1,800 nm
D)900 nm
E)400 nm

Question 32

What is the wavelength of a photon emitted by a Kr^ laser with an energy of 3.07 J?

A)(  224 nm)
B)(  389 nm)
C)(  417 nm)
D)(  647 nm)
E)(  534 nm)

Question 33

What is the kinetic energy of the photoelectrons emitted from a sodium surface (  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 34

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 35

What is the photon energy of the yellow-orange light (  589 nm) produced by sodium vapor streetlights?

A)3.37 J
B)6.63 J
C)2.99 J
D)1.45 J
E)7.45 J

Question 36

What is the minimum frequency of a photon that can eject a photoelectron from Ba metal? (The work function of barium is   4.3 J.)

A)2.8 Hz
B)6.5 Hz
C)6.5 Hz
D)6.5 Hz
E)2.8 Hz

Question 37

Indicate which of the following photons can cause emission of photoelectrons from a surface of gallium (  6.7 J).

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

Question 38

Which of the following sources produces the lowest energy photons?

A)a dentist's X-ray source
B)the UV lamp at a tanning bed
C)radio waves from an MRI imager
D)gamma rays from a supernova
E)microwave radiation from a radiotelescope

Question 39

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

A)rubidium ( 3.5 J)
B)gold ( 8.2 J)
C)nickel ( 8.3 J)
D)sodium ( 4.4 J)
E)platinum ( 9.1 J)

Question 40

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 41

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

A)1,094 nm
B)1,875 nm
C)656 nm
D)335 nm
E)109 nm

Question 42

How much energy is required to ionize one mole of He^ ions in their ground state?

A)5,251 kJ
B)2,178 kJ
C)3,764 kJ
D)1,234 kJ
E)757 kJ

Question 43

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 44

Early photoelectric light detectors were based on cesium. Cesium metal has a work function of 3.43 J. What is the longest wavelength of light that could be detected with one of these detectors?

A)759 nm
B)579 nm
C)679 nm
D)767 nm
E)455 nm

Question 45

How much energy is required to ionize an He^ ion in its ground state?

A)2.18 J
B)4.36 J
C)8.72 J
D)1.74 J

Question 46

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 47

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 48

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 49

How much energy is required to ionize one mole of hydrogen atoms in their ground state?

A)1,312 kJ
B)2.18 kJ
C)218 kJ
D)2,178 kJ
E)131.2 kJ

Question 50

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 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)Li^2
D)Be^3
E)B^4

Question 51

Recently, buckyballs (C₆₀) became the largest objects with a measured de Broglie wavelength. If the mass of a C₆₀ molecule is 1.20 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 52

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

A)n₁ 1 to n₂ 2
B)n₁ 3 to n₂ 4
C)n₁ 2 to n₂ 3
D)n₁ 3 to n₂ 5
E)n₁ 4 to n₂ 5

Question 53

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 54

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 55

What wavelength of light is required to cause the ejection of photoelectrons with kinetic energies of 5.0 J from a calcium surface (  4.60 J)?

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

Question 56

Determine the wavelength of the line in the hydrogen atom spectrum corresponding to the n₁  2 to n₂  6 transition.

A)1,275 nm
B)1,034 nm
C)595 nm
D)410 nm
E)225 nm

Question 57

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 58

The energy of a one-electron atom is given by where Z is the atomic number of the element. Which of the following one-electron ions has the largest ionization energy?

A)Li^2
B)Be^3
C)He^
D)B^4
E)C^5

Question 59

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 60

Determine the wavelength of the line in the hydrogen atom spectrum corresponding to the n₁  4 to n₂  8 transition.

A)1,947 nm
B)1,632 nm
C)1,058 nm
D)725 nm
E)421 nm

Question 61

Which statement A-D about the wave function for a single electron is not correct?

A)A French graduate student named Louis de Broglie first had the idea that an electron should be described as a wave.
B)Since   c, an expression for the wavelength of an electron can be found by combining Einstein's equation that relates mass and energy ( ) with his equation that gives the energy of a photon in terms of its frequency ( ).
C)The square of the wave function's amplitude at a particular point in space gives the probability density of finding the electron at that point.
D)Wave functions can have nodes, which are points where the amplitude is zero.
E)Statements A-D are all correct.

Question 62

The 2 subshell contains how many total orbitals?

A)1
B)3
C)5
D)7
E)9

Question 63

An orbital's orientation in space is determined 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 64

Which statement about the quantum numbers that identify an atomic orbital is not correct?

A)The principal quantum number, n, identifies the size of an atomic orbital.
B)The angular momentum quantum number, , identifies the shape of an atomic orbital.
C)The magnetic quantum number, m_l, identifies the orientation of the orbital in space.
D)The magnetic quantum number can have values that range from to in integer steps.
E)The principal quantum number alone, n, identifies the energy of an atomic orbital.

Question 65

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 66

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 67

An orbital's shape is determined 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 n and quantum numbers.

Question 68

Which statement about the quantum numbers that identify an atomic orbital is not correct?

A)The angular momentum quantum number, , identifies the shape of an orbital.
B)The value of the angular momentum quantum number can range from 0 to n, where n is the principal quantum number for the orbital.
C)Orbitals with the same value for the principal quantum number and the angular momentum quantum number are said to be in the same subshell.
D)Orbitals with the same values for the principal quantum number and the angular momentum quantum number have the same energy.
E)The value for the angular momentum quantum number also is designated by a letter: s  0, p  1, d  2, f  3, and so on.

Question 69

How many orbitals are possible for the n  4 shell?

A)4
B)9
C)16
D)25
E)36

Question 70

The 3 subshell contains how many total electrons?

A)2
B)6
C)10
D)14
E)18

Question 71

A proton in a cyclotron has a velocity of 2 m/s, which is nearly the speed of light. The uncertainty in the velocity is 1%. What is the minimum uncertainty in the position of the proton in meters? The proton mass is 2 kg.

A)3 m
B)1 m
C)1 m
D)3 m
E)1 m

Question 72

Which subshell only has five orbitals?

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

Question 73

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 74

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

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

Question 75

Which subshell contains six total electrons?

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

Question 76

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 77

Which statement about the quantum numbers that identify an atomic orbital is not correct?

A)The magnetic quantum number, m_l, identifies the orientation of the orbital in space.
B)The magnetic quantum number can have values that range from to in integer steps.
C)An s orbital of any given shell has only one possible m_l value.
D)For p orbitals of any given shell, there are five possible m_l values.
E)Statements A-D are all correct.

Question 78

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 79

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

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

Question 80

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.