Question 1

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

Accepted Answer

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 
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 2

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

Accepted Answer

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 
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 3

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)

Accepted Answer

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 
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 4

To what uncertainty, in pm, can the position of an electron traveling at 1.89 × 105 m/s be measured if the uncertainty of the speed is 2.00%?

Accepted Answer

A)  765 
B)  654 
C)  8.33 × 104 
D)  1.53 × 105 
E)  1.53 × 104 
A)  765 
B)  654 
C)  8.33 × 104 
D)  1.53 × 105 
E)  1.53 × 104

Question 5

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

Accepted Answer

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 
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 6

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

Accepted Answer

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. 
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 7

Use the basic rules for electron configuration to indicate the number of unpaired electrons in phosphorus.

Accepted Answer

A)  0 
B)  1 
C)  3 
D)  5 
E)  2 
A)  0 
B)  1 
C)  3 
D)  5 
E)  2

Question 8

The Bohr theory explains that an emission spectral line is:

Accepted Answer

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 
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 9

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

Accepted Answer

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 
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 10

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

Accepted Answer

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

Question 11

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

Accepted Answer

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

Question 12

Chlorine (atomic number = 17) has the electronic configuration: ________.

Accepted Answer

A)  1s22s22p63s23d5 
B)  1s22s22p62d53s2 
C)  1s22s22p63s23p5 
D)  1s22s22d103s2 
E)  1s22s22p62d63s1 
A)  1s22s22p63s23d5 
B)  1s22s22p62d53s2 
C)  1s22s22p63s23p5 
D)  1s22s22d103s2 
E)  1s22s22p62d63s1

Question 13

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

Accepted Answer

A) True 
 B)False

Question 14

The quantum numbers of the last electron of cesium are ________.

Accepted Answer

A)  n = 5, ℓ = 0, mℓ = 0, ms = 1/2 
B)  n = 6, ℓ = 1, mℓ = 0, ms = 1/2 
C)  n = 6, ℓ = 1, mℓ = 1, ms = 1/2 
D)  n = 6, ℓ = 0, mℓ = 0, ms = 1/2 
E)  n = 6, ℓ = 2, mℓ = 2, ms = 1/2 
A)  n = 5, ℓ = 0, mℓ = 0, ms = 1/2 
B)  n = 6, ℓ = 1, mℓ = 0, ms = 1/2 
C)  n = 6, ℓ = 1, mℓ = 1, ms = 1/2 
D)  n = 6, ℓ = 0, mℓ = 0, ms = 1/2 
E)  n = 6, ℓ = 2, mℓ = 2, ms = 1/2

Question 15

Choose the INCORRECT statement concerning electromagnetic radiation.

Accepted Answer

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. 
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 16

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

Accepted Answer

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

Question 17

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

Accepted Answer

A) True 
 B)False

Question 18

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

Accepted Answer

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 
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 19

Which of the following statements about electron spin is FALSE?

Accepted Answer

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. 
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 20

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

Accepted Answer

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

Exam 8: Electrons in Atoms

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

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

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)

To what uncertainty, in pm, can the position of an electron traveling at 1.89 × 105 m/s be measured if the uncertainty of the speed is 2.00%?

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

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

Use the basic rules for electron configuration to indicate the number of unpaired electrons in phosphorus.

The Bohr theory explains that an emission spectral line is:

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

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

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

Chlorine (atomic number = 17) has the electronic configuration: ________.

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

The quantum numbers of the last electron of cesium are ________.

Choose the INCORRECT statement concerning electromagnetic radiation.

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

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

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

Which of the following statements about electron spin is FALSE?

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

Matter - Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Additional Aspects

Intermolecular Forces: Liquids and Solids

Solutions and Their Physical Properties

Chemical Kinetics

Principles of Chemical Equilibrium

Acids and Bases

Additional Aspects of Acid-Base Equilibria

Solubility and Complex-Ion Equilibria

Spontaneous Change: Entropy and Free Energy

Electrochemistry

Main Group Elements I: Groups 1, 2, 13, and 14

Main Group Elements II: Groups 18, 17, 16, 15, and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry 1-41

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

Filters

To what uncertainty, in pm, can the position of an electron traveling at 1.89 × 10⁵ m/s be measured if the uncertainty of the speed is 2.00%?