Question 1

A photon has an energy of 5.53 × 10-17 J. What is its frequency in s-1 (h = 6.63 × 10-34 J • s)?

Accepted Answer

A)  3.66 × 10-50 s-1 
B)  1.20 × 10-17 s-1 
C)  3.59 × 10-9 s-1  
D)  2.78 × 108 s-1 
E)  8.34 × 1016 s-1 
A)  3.66 × 10-50 s-1 
B)  1.20 × 10-17 s-1 
C)  3.59 × 10-9 s-1  
D)  2.78 × 108 s-1 
E)  8.34 × 1016 s-1 E

Question 2

A radio wave has a frequency of 8.6 × 108 Hz. What is the energy of one photon of this radiation? (h = 6.63 × 10-34 J • s)

Accepted Answer

A)  7.7 × 10-43 J 
B)  2.3 × 10-34 J 
C)  5.7 × 10-25 J 
D)  1.7 × 10-16 J 
E)  > 10-15 J 
A)  7.7 × 10-43 J 
B)  2.3 × 10-34 J 
C)  5.7 × 10-25 J 
D)  1.7 × 10-16 J 
E)  > 10-15 J C

Question 3

A sprinter must average 24.0 mi/h to win a 100-m dash in 9.30 s. What is his de Broglie wavelength at this speed if his mass is 84.5 kg ? (h = 6.63 × 10-34 J • s)

Accepted Answer

A)  7.31 × 10-37 m 
B)  3.26 × 10-37 m 
C)  5.08 × 10-30 m 
D)  1.34 × 10-30 m 
E)  None of these choices is correct. 
A)  7.31 × 10-37 m 
B)  3.26 × 10-37 m 
C)  5.08 × 10-30 m 
D)  1.34 × 10-30 m 
E)  None of these choices is correct. A

Question 4

Which of the following elements has the largest number of unpaired electrons in the ground state?

Accepted Answer

A)  K 
B)  V 
C)  S 
D)  Si 
E)  Cl 
A)  K 
B)  V 
C)  S 
D)  Si 
E)  Cl

Question 5

Which one of the following sets of quantum numbers is not possible?

Accepted Answer

A)  A 
B)  B 
C)  C 
D)  D 
E)  E 
A)  A 
B)  B 
C)  C 
D)  D 
E)  E

Question 6

Select the correct electron configuration for Te (Z = 52).

Accepted Answer

A)  [Kr]5s25p64d8 
B)  [Kr]5s25d105p4 
C)  [Kr]5s24d105p6 
D)  [Kr]5s24f14 
E)  [Kr]5s24d105p4 
A)  [Kr]5s25p64d8 
B)  [Kr]5s25d105p4 
C)  [Kr]5s24d105p6 
D)  [Kr]5s24f14 
E)  [Kr]5s24d105p4

Question 7

Calculate the de Broglie wavelength of a neutron that has a velocity of 200. cm/s. (mass of a neutron = 1.675 × 10-27 kg and h = 6.63 × 10-34 J • s)

Accepted Answer

A)  1.98 × 10-9 m 
B)  216 nm 
C)  1.8 × 1050 m 
D)  198 nm 
E)  5.05 mm 
A)  1.98 × 10-9 m 
B)  216 nm 
C)  1.8 × 1050 m 
D)  198 nm 
E)  5.05 mm

Question 8

Which ground-state atom has an electron configuration described by the following orbital diagram?

Accepted Answer

A)  phosphorus 
B)  germanium 
C)  selenium 
D)  tellurium 
E)  potassium 
A)  phosphorus 
B)  germanium 
C)  selenium 
D)  tellurium 
E)  potassium

Question 9

What wavelength, in nm, can strike a metal surface and eject an electron with a kinetic energy of 1.89 × 10-19 J if the binding energy of the metal is 289 kJ/mol?

Accepted Answer

A)  1.89 × 10-19 nm 
B)  2.75 nm 
C)  189 nm 
D)  290 nm 
E)  297 nm 
A)  1.89 × 10-19 nm 
B)  2.75 nm 
C)  189 nm 
D)  290 nm 
E)  297 nm

Question 10

The size of an atomic orbital is associated with

Accepted Answer

A)  the principal quantum number (n). 
B)  the angular momentum quantum number (l). 
C)  the magnetic quantum number (ml). 
D)  the spin quantum number (ms). 
E)  the angular momentum and magnetic quantum numbers, together. 
A)  the principal quantum number (n). 
B)  the angular momentum quantum number (l). 
C)  the magnetic quantum number (ml). 
D)  the spin quantum number (ms). 
E)  the angular momentum and magnetic quantum numbers, together.

Question 11

How many unpaired electrons does a ground-state atom of sulfur have?

Accepted Answer

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

Question 12

According to the Heisenberg uncertainty principle, if the uncertainty in the speed of an electron is 3.5 × 103 m/s, the uncertainty in its position (in m) is at least ________. (mass of an electron = 9.11 × 10-28 g)

Accepted Answer

A)  1.7 × 10-8 m 
B)  6.6 × 10-8 m 
C)  17 m 
D)  66 m 
E)  None of these choices is correct. 
A)  1.7 × 10-8 m 
B)  6.6 × 10-8 m 
C)  17 m 
D)  66 m 
E)  None of these choices is correct.

Question 13

How many electrons are in the 4p orbitals of vanadium?

Accepted Answer

A)  0 
B)  2 
C)  4 
D)  5 
E)  6 
A)  0 
B)  2 
C)  4 
D)  5 
E)  6

Question 14

The ground-state electron configuration of a calcium atom is

Accepted Answer

A)  [Ne]3s2. 
B)  [Ne]3s23p6. 
C)  [Ar]4s13d1. 
D)  [Ar]4s2. 
E)  [Ar]3d2. 
A)  [Ne]3s2. 
B)  [Ne]3s23p6. 
C)  [Ar]4s13d1. 
D)  [Ar]4s2. 
E)  [Ar]3d2.

Question 15

Hund's rule states that the most stable arrangement of electrons in orbitals of equal energy is the one in which the number of electrons with parallel spin is ________.

Accepted Answer

A)  minimized 
B)  nullified 
C)  neutral 
D)  maximized 
E)  not relevant 
A)  minimized 
B)  nullified 
C)  neutral 
D)  maximized 
E)  not relevant

Question 16

What is the frequency of electromagnetic radiation with wavelength 532 nm? (c = 3.00 × 108 m/s)

Accepted Answer

A)  5.64 × 1014 s-1 
B)  6.48 × 1012 s-1 
C)  4.18 × 1018 s-1  
D)  6.23 × 1014 s-1 
E)  3.75 × 1015 s-1 
A)  5.64 × 1014 s-1 
B)  6.48 × 1012 s-1 
C)  4.18 × 1018 s-1  
D)  6.23 × 1014 s-1 
E)  3.75 × 1015 s-1

Question 17

The ________ is the distance between identical points on successive waves.

Accepted Answer

The answer of The ________ is the distance between identical...

Question 18

Calculate the de Broglie wavelength associated with a 20Ne+ ion moving at a velocity of 2.0 × 105 m/s. The atomic mass of Ne-20 is 19.992 amu. (1 amu = 1.66 × 10-24 g and h = 6.63 × 10-34 J • s)

Accepted Answer

A)  1.0 × 10-13 m 
B)  1.0 × 10-16 m 
C)  1.0 × 10-18 m 
D)  9.7 × 1012 m 
E)  2.0 × 10-13 cm 
A)  1.0 × 10-13 m 
B)  1.0 × 10-16 m 
C)  1.0 × 10-18 m 
D)  9.7 × 1012 m 
E)  2.0 × 10-13 cm

Question 19

________ is an attempt to locate a subatomic particle acting as a wave even though it is impossible to know both the momentum and position of the particle simultaneously.

Accepted Answer

The Heisen

Question 20

In the ________ series, nf = 1 and you observe the ultraviolet region of the electromagnetic spectrum.

Accepted Answer

Exam 6: Quantum Theory and the Electronic Structure of Atoms

A photon has an energy of 5.53 × 10-17 J. What is its frequency in s-1 (h = 6.63 × 10-34 J • s)?

A radio wave has a frequency of 8.6 × 108 Hz. What is the energy of one photon of this radiation? (h = 6.63 × 10-34 J • s)

A sprinter must average 24.0 mi/h to win a 100-m dash in 9.30 s. What is his de Broglie wavelength at this speed if his mass is 84.5 kg ? (h = 6.63 × 10-34 J • s)

Which of the following elements has the largest number of unpaired electrons in the ground state?

Which one of the following sets of quantum numbers is not possible?

Select the correct electron configuration for Te (Z = 52).

Calculate the de Broglie wavelength of a neutron that has a velocity of 200. cm/s. (mass of a neutron = 1.675 × 10-27 kg and h = 6.63 × 10-34 J • s)

Which ground-state atom has an electron configuration described by the following orbital diagram?

What wavelength, in nm, can strike a metal surface and eject an electron with a kinetic energy of 1.89 × 10-19 J if the binding energy of the metal is 289 kJ/mol?

The size of an atomic orbital is associated with

How many unpaired electrons does a ground-state atom of sulfur have?

According to the Heisenberg uncertainty principle, if the uncertainty in the speed of an electron is 3.5 × 103 m/s, the uncertainty in its position (in m) is at least ________. (mass of an electron = 9.11 × 10-28 g)

How many electrons are in the 4p orbitals of vanadium?

The ground-state electron configuration of a calcium atom is

Hund's rule states that the most stable arrangement of electrons in orbitals of equal energy is the one in which the number of electrons with parallel spin is ________.

What is the frequency of electromagnetic radiation with wavelength 532 nm? (c = 3.00 × 108 m/s)

The ________ is the distance between identical points on successive waves.

Calculate the de Broglie wavelength associated with a 20Ne+ ion moving at a velocity of 2.0 × 105 m/s. The atomic mass of Ne-20 is 19.992 amu. (1 amu = 1.66 × 10-24 g and h = 6.63 × 10-34 J • s)

________ is an attempt to locate a subatomic particle acting as a wave even though it is impossible to know both the momentum and position of the particle simultaneously.

In the ________ series, nf = 1 and you observe the ultraviolet region of the electromagnetic spectrum.

Chemistry: the Central Science

Atoms, Molecules, and Ions

Stoichiometry: Ratios of Combination

Reactions in Aqueous Solutions

Thermochemistry

Electron Configuration and the Periodic Table

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Molecular Geometry and Bonding Theories

Gases

Intermolecular Forces and the Physical Properties of Liquids and Solids

Modern Materials

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy, Free Energy, and Equilibrium

Electrochemistry

Nuclear Chemistry

Environmental Chemistry

Coordination Chemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Organic Chemistry

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A photon has an energy of 5.53 × 10^-17 J. What is its frequency in s^-1 (h = 6.63 × 10^-34 J • s)?

A radio wave has a frequency of 8.6 × 10⁸ Hz. What is the energy of one photon of this radiation? (h = 6.63 × 10^-34 J • s)

A sprinter must average 24.0 mi/h to win a 100-m dash in 9.30 s. What is his de Broglie wavelength at this speed if his mass is 84.5 kg ? (h = 6.63 × 10^-34 J • s)

Calculate the de Broglie wavelength of a neutron that has a velocity of 200. cm/s. (mass of a neutron = 1.675 × 10^-27 kg and h = 6.63 × 10^-34 J • s)

What wavelength, in nm, can strike a metal surface and eject an electron with a kinetic energy of 1.89 × 10^-19 J if the binding energy of the metal is 289 kJ/mol?

According to the Heisenberg uncertainty principle, if the uncertainty in the speed of an electron is 3.5 × 10³ m/s, the uncertainty in its position (in m) is at least ________. (mass of an electron = 9.11 × 10^-28 g)

What is the frequency of electromagnetic radiation with wavelength 532 nm? (c = 3.00 × 10⁸ m/s)

Calculate the de Broglie wavelength associated with a ²⁰Ne⁺ ion moving at a velocity of 2.0 × 10⁵ m/s. The atomic mass of Ne-20 is 19.992 amu. (1 amu = 1.66 × 10^-24 g and h = 6.63 × 10^-34 J • s)

In the ________ series, n_f= 1 and you observe the ultraviolet region of the electromagnetic spectrum.