Deck 8: Electrons in Atoms

Question 1

What is the frequency associated with radiation of 4.59 × 10-8 cm wavelength?

A) 6.54 × 1017 s-1
B) 6.54 × 1015 s-1
C) 1.53 × 10-8 s-1
D) 13.8 s-1
E) 2.18 × 107 s-1

Answer 1

6.54 × 1017 s-1

Question 2

Use Planck's equation to determine the energy, in J/photon, of radiation of frequency 5.8 × 1015 s-1.

A) 3.8 × 10-18 J
B) 1.7 × 1024 J
C) 5.8 × 10-25 J
D) 1.7 × 10-16 J
E) 5.2 × 10-8 J

Answer 2

3.8 × 10-18 J

Question 3

Frequency and wavelength are related by the equation:

A) λ = c ∙ v
B) λ = c/v
C) v = λ/c
D) λ = v/c
E) c = λ/v

Answer 3

λ = c/v

Question 4

The Bohr theory explains that an emission spectral line is due to an electron losing energy but keeping the same values of its four quantum numbers.

Question 5

A radiation detector exposed to sunlight records the energy falling on a given area each unit time. If such a detector has a reading of 0.698 cal cm-2 min-1, how many photons of sunlight are striking each cm2 in one minute? Assume the average wavelength of sunlight is 460. nm. (4.184 J = 1 calorie)

A) 1.62 × 1018 photons
B) 4.32 × 1019 photons
C) 6.76 × 1018 photons
D) 2.31 × 1018 photons
E) 9.63 × 1019 photons

Question 6

What is the frequency of radiation with a wavelength of 440. nm?

A) 6.81 × 1014 s-1
B) 6.81 × 105 s-1
C) 1.51 × 10-27 s-1
D) 4.95 × 10-12 s-1
E) 2.02 × 10-11 s-1

Question 7

A radiation detector exposed to sunlight records the energy falling on a given area each unit time. If such a detector has a reading of 0.430 cal cm-2 min-1, how many photons of sunlight are striking each cm2 in one minute? Assume the average wavelength of sunlight is 460. nm. (4.184 J = 1 calorie)

A) 2.02 × 107 photons
B) 8.46 × 107 photons
C) 4.17 × 1018 photons
D) 1.02 × 1027 photons
E) 4.25 × 1027 photons

Question 8

Four of the 3d orbitals are alike except for the orientation with respect to the axes.

Question 9

The order of subshells of increasing energy in a multiple-electron atom is 4f, 5d, 6s, 6p.

Question 10

When an electron goes from a high energy state to a low one, another electron goes from a low energy state to a high one.

Question 11

The order of subshells of increasing energy in a multiple-electron atom is 6s, 4f, 5d, 6p.

Question 12

The symbol "n" in the Bohr theory of atomic structure refers to the shell or orbit in which an electron is found.

Question 13

What is the wavelength in nm associated with radiation of frequency 2.8 × 1013 s-1?

A) 840 nm
B) 2.8 × 104 nm
C) 299 nm
D) 9.3 × 104 nm
E) 1.1 × 104 nm

Question 14

Choose the INCORRECT statement concerning electromagnetic radiation.

A) Infrared light has a longer wavelength than ultraviolet light.
B) The greater the frequency of the electromagnetic radiation, the greater the energy of the radiation.
C) A photon with a wavelength of 5000 Angstroms has one-half as much energy as a photon with a wavelength of 2500 Angstroms.
D) The speed of ultraviolet light rays is faster than X-rays in a vacuum.
E) Electromagnetic radiation is energy transmission in which electric and magnetic fields are propagated as waves.

Question 15

The symbol "n" in the Bohr theory of atomic structure refers to the number of electrons in a shell.

Question 16

The relationship between the frequency of light and the energy of the light was postulated by:

A) Max Planck
B) Johann Balmer
C) Johannes Rydberg
D) Albert Einstein
E) Robert Bunsen

Question 17

The Bohr theory explains that an emission spectral line is due to an interaction between electrons in atoms.

Question 18

When an electron in an atom goes from a high energy state to a low one, light is given off.

Question 19

The Bohr theory explains that an emission spectral line is due to an electron losing energy and changing shells.

Question 20

Light passing through a transparent medium has a wavelength of 466 nm and a frequency of 6.20 × 1014 s-1. What is the speed of the light in the medium?

A) 2.89 × 108 m/s
B) 2.89 × 1017 m/s
C) 1.33 × 1012 m/s
D) 1.33 × 1021 m/s
E) 7.52 × 10-22 m/s

Question 21

How many photons of light with frequency 5.50 × 1015 Hz are required to provide 1 kJ of energy?

A) 3.64 × 10-18 photons
B) 2.74 × 1020 photons
C) 4.56 × 10-4 photons
D) 1.65 × 1044 photons
E) 3.64 × 10-16 photons

Question 22

Calculate the deBroglie wavelength of a ball of mass 125 grams and velocity 90 m/s.

A) 0.59 m
B) 5.9 × 10-31 m
C) 5.9 × 10-35 m
D) 590 m
E) 1.7 × 1034 m

Question 23

The fact that we cannot simultaneously measure the exact position and precise momentum of an electron is referred to as:

A) Pauli Exclusion Principle
B) The Aufbau Principle
C) Hund's Rule
D) The DeBroglie Relationship
E) Heisenberg Uncertainty Principle

Question 24

What is the wavelength of a bullet that is 0.450 g traveling at 2000. m/s?

A) 2000. m
B) 2.94 × 10-24 m
C) 7.36 × 10-34 m
D) 7.36 × 10-37 m
E) 1.49 × 10-40 m

Question 25

What is the energy in joules of the 656 nm spectral line of hydrogen?

A) 4.35 × 10-31 J
B) 3.03 × 10-19 J
C) 1.30 × 10-22 J
D) 3.03 × 10-28 J
E) 1.45 × 10-48 J

Question 26

When an electron in an atom goes from a high energy state to a low one, what occurs?

A) Another electron goes from a low energy state to a high one.
B) The atom moves faster.
C) Light is given off.
D) This process is not possible.
E) Light is absorbed.

Question 27

Calculate the wavelength in meters of light absorbed by an electron in an atom of hydrogen as it moves from n = 3 to n = 6.

A) 1.09 × 10-6 m
B) 8.22 × 10-7 m
C) 3.28 × 10-6 m
D) 1.83 × 10-7 m
E) 1.65 × 10-11 m

Question 28

For the Bohr hydrogen atom determine the energy level corresponding to n = 3.

A) 7.26 × 10-19 J
B) 7.36 × 10-35 J
C) -2.42 × 10-19 J
D) 3.33 × 107 J
E) 1.96 × 10-17 J

Question 29

The mathematical equation deduced by Johann Balmer and subsequently rewritten in another form by Johannes Rydberg gives us:

A) the relationship between wavelengths of spectral lines and the electrons' energies responsible for them
B) the relationship between wavelength and frequency of spectral lines
C) the relationship between frequencies of spectral lines and the energy values associated with them
D) a model for finding the limited numbers of wavelengths associated with atomic spectral lines
E) an explanation for the continuous range of energy values associated with atomic spectra

Question 30

The photoelectric effect:

A) was discovered by Max Planck
B) describes the phenomenon of producing light by shining a beam of electrons by on any metal surface
C) contradicted the view that light energy was dependent upon intensity only
D) is not the same principle used in modern electric eyes and solar calculators
E) results in a beam of electrons which increases in number, but not velocity, as the wavelength of incident light decreases

Question 31

The Bohr theory explains that an emission spectral line is:

A) due to an electron losing energy but keeping the same values of its four quantum numbers
B) due to an electron losing energy and changing shells
C) due to an interaction between electrons in two different principal shells
D) due to an electron gaining energy and changing shells
E) due to an increase in the principal quantum number n of an electron

Question 32

What is the energy in joules of the 434 nm spectral line of hydrogen?

A) 1.53 × 10-27 J
B) 4.58 × 10-28 J
C) 1.04 × 1048 J
D) 4.58 × 10-19 J
E) 9.59 × 10-49 J

Question 33

The existence of discrete (quantized) energy levels in an atom may be inferred from:

A) diffraction of electrons by crystals
B) X-ray diffraction by crystals
C) atomic line spectra
D) experiments on the photoelectric effect
E) visible spectrum

Question 34

Calculate the energy in kJ/mol of light with a wavelength of 360 nm.

A) 5.52 × 10-22 kJ/mol
B) 5.52 × 10-19 kJ/mol
C) 332 kJ/mol
D) 6.63 × 103 kJ/mol
E) 0.332 kJ/mol

Question 35

The symbol "n" in the Bohr theory of atomic structure refers to:

A) the energy of the electrons.
B) the total energy of the atom.
C) the number of electrons in a shell.
D) the shell in which an electron is found.
E) the number of orbits in an atom.

Question 36

Which statement regarding the wave function as suggested by Erwin Schrodinger is INCORRECT?

A) It has fluctuating values at all points on the curve.
B) It is a mathematical equation.
C) It is denoted by psi (Ψ).
D) It can describe any particle with wavelike motions.
E) It corresponds to a standing wave within the boundary of the system.

Question 37

What is the energy in joules of a mole of photons with the energy of the 434 nm spectral line of hydrogen?

A) 2.76 × 105 J
B) 9.21 × 10-4 J
C) 2.76 × 10-4 J
D) 5.78 × 10-25 J
E) 434 J

Question 38

What is the wavelength, in nm, associated with a 2000. kg truck traveling at a speed of 20 m/s, that is, considering the truck to be a "matter" wave?

A) 1.33 × 10-29 nm
B) 2.65 × 10-29 nm
C) 6.02 × 10-29 nm
D) 7.50 × 103 nm
E) 1.66 × 10-29 nm

Question 39

What is the wavelength associated with electrons traveling at one one-hundredth the speed of light?

A) 243 nm
B) 0.243 nm
C) 412 nm
D) 7.98 × 10-2 nm
E) 12.5 nm

Question 40

What is the wavelength of a ball that is 25.0 g traveling at 40.2 m/s?

A) 6.59 × 10-37 m
B) 6.59 × 10-34 m
C) 1.07 × 10-30 m
D) 4.12 × 10-37 m
E) 2.42 × 10-11 m

Question 41

The possible values of the magnetic quantum number, mℓ , of a 3p electron are:

A) 0, 1, 2
B) 2, 1, 0, -1, -2
C) 0
D) -1, 0, +1
E) +1, -1

Question 42

What is the smallest acceptable value for the missing quantum number? n = ?, ℓ = 2, mℓ = 0, ms = +1/2

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

Question 43

Which of the following statements about the electron spin quantum number is FALSE?

A) ms denotes the spin quantum number.
B) The value of the spin quantum number can be +1/2 or -1/2.
C) The value of the spin quantum number does not depend on other quantum numbers.
D) The value of the spin quantum number can be indicated by arrows to the right and to the left.
E) The spin quantum number is an indication that electrons generate a magnetic field.

Question 44

All of the terms below are quantum numbers EXCEPT:

A) principal
B) magnetic
C) spin
D) valence
E) orbital angular momentum

Question 45

Which statement about the zero-point energy is INCORRECT?

A) It is the lowest energy value of a particle.
B) It's value can be zero.
C) Because the zero-point energy is not zero, the particle cannot be at rest.
D) Zero-point energy corresponds to n = 1.
E) The zero-point energy is an allowable value of the energy of the particle.

Question 46

Give the appropriate values of n and ℓ for the orbital designation 3p.

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

Question 47

An orbital: I) describes a region of high electron density.
II) describes a region in an atom where an electron is likely to be found.
III) is a wave function resulting from specific values assigned to quantum numbers in wave equations.
IV) describes a spherical region around a nucleus where an electron can be found.

A) II only
B) I and II
C) II and III
D) I, II, and III
E) I, II, III, and IV

Question 48

Which of the following statements about electron spin is FALSE?

A) An electron produces a magnetic field.
B) The electron's magnetic field can be oriented in two directions in the presence of an external magnetic field.
C) Paired electrons produced no net magnetic field.
D) An experiment with silver atoms passing through a magnetic field seems to prove that electron spin exists.
E) Electron spin only exists when mℓ = 0.

Question 49

Which one of the following set of quantum numbers would not be allowed?

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

Question 50

Which of the following is not possible?

A) 2p
B) 4d
C) 5p
D) 3f
E) 2s

Question 51

Which of the following statements about orbital shapes is NOT true?

A) A 1s orbital is spherical.
B) 2p orbitals have a node at r = 0.
C) There are only two 2p orbitals, each directed along and x or y axis.
D) There are 5 3d orbitals.
E) Four of the 3d orbitals are alike except for the orientation with respect to the axes.

Question 52

Which two orbitals are located between the axes of a coordinate system and not along the axes?

A) dxy, py
B) dyz, px
C) dx2-y2, pz
D) dxy, dz2
E) dxy, dyz

Question 53

An atomic orbital represents:

A) the shape of an atom
B) the repulsion of all the electrons among themselves
C) a fixed path that an electron follows around the nucleus of an atom
D) the region of electron density for a covalent bond
E) the region of high probability for an electron around the nucleus of an atom

Question 54

Which of the following statements concerning quantum numbers is NOT correct?

A) "n" relates the most probable distance from the nucleus.
B) "l" denotes geometric shape.
C) "m" denotes orientation of an orbital with respect to the others.
D) The fourth quantum number refers to electron spin.
E) The four quantum numbers are derived from wave mechanics.

Question 55

The possible values of the orbital angular momentum quantum number of a 3p electron are:

A) +1/2, -1/2
B) -1, 0, +1
C) -1
D) 0
E) 1

Question 56

What is the orbital designation for the quantum numbers n = 2, ℓ = 1?

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

Question 57

Which of the following orbitals have lobes aligned along the x axis?

A) dxy
B) dx2-y2
C) dxz
D) dyz
E) s

Question 58

In a hydrogen atom, orbitals with the same energy:
I. extend the same distance from the nucleus.
II. have the same principle quantum number, n.
III. are referred to as iso-electronic.
IV. are referred to as degenerate.
V. are represented by 1s and 2s orbitals.

A) I, III, IV
B) I, II, IV
C) I, IV, V
D) I, II, III
E) I, II, III, and IV

Question 59

Give the appropriate values of n and ℓ for the orbital designation 3s.

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

Question 60

Which of the following orbitals have their lobes aligned along the y axis? I) dxy
II) dx2-y2
III) py
IV) dyz

A) II and III
B) I and IV
C) I and II
D) II and IV
E) I and III

Question 61

What is an acceptable value for the missing quantum number? n = 4, ℓ = 2, mℓ = 0, ms = ?

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

Question 62

Which series of subshells is arranged in order of increasing energy in a multiple-electron atom?

A) 5d, 4f, 6s, 6p
B) 4f, 6s, 5d, 6p
C) 4f, 5d, 6s, 6p
D) 6s, 4f, 5d, 6p
E) 6s, 6p, 5d, 4s

Question 63

Arrange the following in order of increasing ENERGY: UV radiation, visible radiation, X-rays, and microwaves.

A) X-rays < microwave < UV < visible
B) X-ray < microwave < visible < UV
C) microwave < visible < UV < X-rays
D) visible < UV < X-rays < microwave
E) UV < X-rays < microwave < visible

Question 64

What is the wavelength, in nm, of light with an energy content of 550 kJ/mol?

A) 0.218 nm
B) 0.419 nm
C) 157 nm
D) 218 nm
E) 6579 nm

Question 65

What is the wavelength of the line in the Balmer series of hydrogen corresponding to the transition from n = 5 to n = 2? The constant for Balmer's equation is 3.2881 × 1015 s-1.

A) 304 nm
B) 30.4 nm
C) 329 nm
D) 535 nm
E) 434 nm

Question 66

Exceptions to ________ are represented by chromium and copper in the 4th row of the periodic table.

A) the Aufbau Principle
B) Hund's Rule
C) the Bohr Theory
D) the Heisenberg Principle
E) the Pauli Exclusion Principle

Question 67

A television signal has a wavelength of 10.0 km. What is its frequency in kilohertz?

A) 30.0 kHz
B) 3.00 × 104 kHz
C) 3.00 × 107 kHz
D) 3.33 × 10-7 kHz
E) 3.33 × 10-2 kHz

Question 68

Calculate the wavelength, in nm, of the first line of the Balmer series. The constant for Balmer's equation is 3.2881 × 1015 s-1.

A) 18.3 nm
B) 656 nm
C) 547 nm
D) 152 nm
E) 252 nm

Question 69

Use the Balmer equation to determine the wavelength, in nm, of the line in the Balmer series corresponding to n = 4. The constant for Balmer's equation is 3.2881 × 1015 s-1.

A) 365 nm
B) 45.6 nm
C) 205 nm
D) 486 nm
E) 1459 nm

Question 70

Use the Balmer equation to determine n for the spectral line of wavelength 656 nm. The constant for Balmer's equation is 3.2881 × 1015 s-1.

A) 3
B) 4
C) 5
D) 6
E) 7

Question 71

The principle that is based on electrons attempting to be as far apart as possible is the:

A) Heisenberg Principle
B) Exclusion Principle
C) Bohr Theory
D) Hund's Rule
E) Aufbau principle

Question 72

Which of the following subshells is correctly designated?

A) 1p5
B) 3s3
C) 3f2
D) 4d11
E) 2p6

Question 73

Niels Bohr promoted the connection between the periodic table and quantum theory. Which of the following statements is INCORRECT?

A) The link between the table arrangement and quantum theory is electron configuration.
B) Elements in the same group have similar electron configurations.
C) Elements in the same group have the same number of electrons in the outer shell.
D) Elements in the same group have the same principle quantum number.
E) Elements in the same group have the same number of valence electrons.

Question 74

The quantum numbers of the last electron of nickel could be:

A) n = 3, ℓ = 2, mℓ = 0, ms = 1/2
B) n = 4, ℓ = 2, mℓ = 0, ms = 1/2
C) n = 3, ℓ = 1, mℓ = 0, ms = 1/2
D) n = 3, ℓ = 2, mℓ = 0, ms = 0
E) n = 3, ℓ = 2, mℓ = 1/2, ms = 1/2

Question 75

"One places electrons into orbitals one by one from low energy to high energy" is one way of stating the:

A) Aufbau principle
B) Hund's Rule
C) Heisenberg Principle
D) Pauli Exclusion Principle
E) Rydberg's Principle

Question 76

The quantum numbers of the last electron of arsenic could be:

A) n = 4, ℓ = 2, mℓ = 1, ms = 1/2
B) n = 4, ℓ = 1, mℓ = 1, ms = 1/2
C) n = 3, ℓ = 1, mℓ = 1, ms = 1/2
D) n = 4, ℓ = 3, mℓ = 1, ms = 1/2
E) n = 4, ℓ = 1, mℓ = 1/2, ms = 0

Question 77

Experimental evidence for electron spin:

A) has not yet been found
B) was provided by Uhlenbeck and Goudsmit in 1925
C) came as the result of an experiment with vaporized silver atoms, which was originally designed for another purpose
D) is provided each time we make mirror-image molecules, called left and right-handed isomers
E) is not needed because the concept is only for our convenience

Question 78

Use the Balmer equation to determine n for the spectral line of wavelength 434 nm. The constant for Balmer's equation is 3.2881 × 1015 s-1.

A) 3
B) 4
C) 5
D) 6
E) 7

Question 79

What is the wavelength, in nm, of the spectral line resulting from the transition of an electron from n = 3 to n = 2 in a Bohr hydrogen atom? The constant for Balmer's equation is 3.2881 × 1015 s-1.

A) 18.3 nm
B) 656 nm
C) 547 nm
D) 152 nm
E) 252 nm

Question 80

The fact that the valence orbital configuration of nitrogen in the ground state is 2s2, 2px12py12pz1 is an illustration of:

A) the Bohr Theory
B) Hund's Rule
C) the Aufbau Principle
D) the Pauli Exclusion Principle
E) the Heisenberg Uncertainty Principle