Deck 8: Electrons in Atoms

Question 1

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.

Answer 1

The speed of ultraviolet light rays is faster than X-rays in a vacuum.

Question 2

A radiation detector exposed to sunlight records the energy falling on a given area per 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

Answer 2

4.17 × 10¹⁸ photons

Question 3

The following orbitals are placed in the correct filling order:
4f,5d,6s,6p.

Answer 3

False

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

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 6

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 7

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

Question 8

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

Question 9

The following orbitals are placed in the correct filling order:
6s,4f,5d,6p.

Question 10

A radiation detector exposed to sunlight records the energy falling on a given area per 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 11

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

Question 12

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 13

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

Question 14

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

Question 15

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

Question 16

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

Question 17

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

Question 18

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 19

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 20

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

Question 21

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 22

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

A)It is the lowest energy value of a particle.
B)It's value can be zero.
C)It is denoted by psi (Ψ).
D)Zero-point energy corresponds to n = 1.
E)The zero-point energy is an allowable value of the energy of the particle.

Question 23

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 24

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 25

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 26

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 27

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 28

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 29

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)Light is absorbed.
E)This process is not possible.

Question 30

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 31

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 32

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 33

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 an orbit
D)the orbit in which an electron is found
E)the number of orbits in an atom

Question 34

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 35

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 36

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 orbits
C)due to an interaction between electrons in two different principal orbits
D)due to an electron gaining energy and changing orbits
E)due to an increase in the principal quantum number n of an electron

Question 37

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 38

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 39

Calculate the wavelength in meters of light absorbed by an electron in an atom of hydrogen as it moves that makes a transition 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 40

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 41

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 m_ℓ = 0.

Question 42

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 43

All of the terms below are quantum numbers EXCEPT:

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

Question 44

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

Question 45

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 46

What is the smallest acceptable value for the missing quantum number?
N = ?,ℓ = 2,m_ℓ = 0,m_s = +1/2

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

Question 47

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 to exist near the nucleus of an atom

Question 48

Which of the following orbitals have their lobes aligned along the y axis?
I.d_xy
II.d_x ^2-2y
III.p_y
IV.d_yz

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

Question 49

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 50

The possible value(s)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 51

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

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

Question 52

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

A)m_s 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 53

An atomic 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 54

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

A)d_xy
B)d_x^2-y2
C)d_xz
D)d_yz
E)s

Question 55

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

A)d_xy,p_y
B)d_yz,p_x
C)d_x²-_y²,p_z
D)d_xy,d_z²
E)d_xy,d_yz

Question 56

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 57

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 58

Which of the following is not possible?

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

Question 59

The possible values of the magnetic quantum number,m_ℓ ,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 60

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

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

Question 61

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 orbit.
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 62

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 63

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

A)n = 3,ℓ = 2,m_ℓ = 0,m_s = -1/2
B)n = 4,ℓ = 2,m_ℓ = 0,m_s = +1/2
C)n = 3,ℓ = 1,m_ℓ = 0,m_s = +1/2
D)n = 3,ℓ = 2,m_ℓ = 0,m_s = 0
E)n = 3,ℓ = 2,m_ℓ = 1/2,m_s = +1/2

Question 64

Which series below represents the correct order of orbital filling in a multielectron 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 65

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 66

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 67

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 68

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 69

Use Planck's equation to determine the wavelength,in nm,of radiation with 200.0 kJ/mol of energy.

A)167 nm
B)598 nm
C)5.98 × 10⁵ nm
D)1.67 × 10⁵ nm
E)242 nm

Question 70

The fact that the valence orbital configuration of nitrogen in the ground state is 2s²,2p_x¹2p_y¹2p_z¹ 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

Question 71

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 72

What is an acceptable value for the missing quantum number?
N = 4,ℓ = 2,m_ℓ = 0,m_s = ?

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

Question 73

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 74

"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 75

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

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

Question 76

Which of the following subshells is correctly designated?

A)1p⁵
B)3s³
C)3f²
D)4d¹¹
E)2p⁶

Question 77

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

A)30.0 kHz
B)3.00 × 10^{4 kHz}
C)3.00 × 10^{7 kHz}
D)3.33 × 10^{-7 kHz}
E)3.33 × 10^{-2 kHz}

Question 78

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

A)n = 4,ℓ = 2,m_ℓ = 1,m_s = +1/2
B)n = 4,ℓ = 1,m_ℓ = 1,m_s = +1/2
C)n = 3,ℓ = 1,m_ℓ = 1,m_s = +1/2
D)n = 4,ℓ = 3,m_ℓ = 1,m_s = +1/2
E)n = 4,ℓ = 1,m_ℓ = 1/2,m_s = 0

Question 79

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 80

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