Question 1

What color of visible light has the longest wavelength?

Accepted Answer

A) blue 
B) violet 
C) red 
D) yellow 
E) green 
A) blue 
B) violet 
C) red 
D) yellow 
E) green C

Question 2

Which one of the following is an incorrect orbital notation?

Accepted Answer

A) 2s 
B) 3py 
C) 3f 
D) 4dxy 
E) 4s 
A) 2s 
B) 3py 
C) 3f 
D) 4dxy 
E) 4s C

Question 3

Which electron configuration represents a violation of Hund's rule for an atom in its ground state?

Accepted Answer

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

Question 4

In a ground-state copper atom,the ________ subshell is partially filled.

Accepted Answer

A) 3s 
B) 4s 
C) 4p 
D) 3d 
E) 4d 
A) 3s 
B) 4s 
C) 4p 
D) 3d 
E) 4d

Question 5

The shape of an orbital is defined by the angular momentum quantum number which is represented as letter ________.

Accepted Answer

The answer of The shape of an orbital is defined...

Question 6

Which group in the periodic table contains elements with the valence electron configuration of ns2np1?

Accepted Answer

A) 1A 
B) 2A 
C) 3A 
D) 4A 
E) 8A 
A) 1A 
B) 2A 
C) 3A 
D) 4A 
E) 8A

Question 7

Which group is represented by a ns2np6 valence shell electron configuration?

Accepted Answer

Question 8

The total number of orbitals in a shell is given by ________.

Accepted Answer

A) I2 
B) n2 
C) 2n 
D) 2n + 1 
E) 2l + 1 
A) I2 
B) n2 
C) 2n 
D) 2n + 1 
E) 2l + 1

Question 9

The energy (J)required for an electronic transition in a Bohr hydrogen atom from n = 2 to n = 3 is ________ J.

Accepted Answer

A) 4.00 × 10-19 
B) 3.00 × 10-19 
C) -3.00 × 10-19 
D) -7.90 × 10-19 
E) 4.60 × 1014 
A) 4.00 × 10-19 
B) 3.00 × 10-19 
C) -3.00 × 10-19 
D) -7.90 × 10-19 
E) 4.60 × 1014

Question 10

What is the de Broglie wavelength (m)of a 1.0 × 109 kg train car traveling at 95 km/hr?

Accepted Answer

A) 2.51 × 10-41 
B) 2.51 × 10-47 
C) 6.97 × 10-45 
D) 2.51 × 10-44 
E) 6.97 × 10-48 
A) 2.51 × 10-41 
B) 2.51 × 10-47 
C) 6.97 × 10-45 
D) 2.51 × 10-44 
E) 6.97 × 10-48

Question 11

A photon that has an energy of 8.63 × 10-12 J would emit light at which wavelength (m)?

Accepted Answer

A) 230 
B) 2.30 × 10-14 
C) 2.30 
D) 3.48 × 1019 
E) 2.30 × 10-5 
A) 230 
B) 2.30 × 10-14 
C) 2.30 
D) 3.48 × 1019 
E) 2.30 × 10-5

Question 12

The n = 5 to n = 3 transition in the Bohr hydrogen atom corresponds to the ________ of a photon with a wavelength of ________ nm.

Accepted Answer

A) absorption, 657 
B) absorption, 1280 
C) emission, 657 
D) emission, 1280 
E) emission, 389 
A) absorption, 657 
B) absorption, 1280 
C) emission, 657 
D) emission, 1280 
E) emission, 389

Question 13

Which one of the following is an incorrect subshell notation?

Accepted Answer

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

Question 14

What is the wavelength (angstroms)of a photon that has an energy of 4.38 × 10-18 J?

Accepted Answer

A) 45.4 angstroms 
B) 2.30 × 107 angstroms 
C) 6.89 × 1015 angstroms 
D) 1.45 × 10-16 angstroms 
E) 1.31 × 10-9 angstroms 
A) 45.4 angstroms 
B) 2.30 × 107 angstroms 
C) 6.89 × 1015 angstroms 
D) 1.45 × 10-16 angstroms 
E) 1.31 × 10-9 angstroms

Question 15

An electron cannot have the quantum numbers n = ________,l = ________,ml = ________.

Accepted Answer

A) 2, 0, 0 
B) 2, 1, -1 
C) 3, 1, -1 
D) 1, 1, 1 
E) 3, 2, 1 
A) 2, 0, 0 
B) 2, 1, -1 
C) 3, 1, -1 
D) 1, 1, 1 
E) 3, 2, 1

Question 16

An NMR spectrum results from photon irradiation in which the electron spin alignment is flipped.

Accepted Answer

A) True 
 B)False

Question 17

Which one of the following is considered to be ionizing radiation?

Accepted Answer

A) visible light 
B) radio waves 
C) X-rays 
D) microwaves 
E) infrared radiation 
A) visible light 
B) radio waves 
C) X-rays 
D) microwaves 
E) infrared radiation

Question 18

The ground-state electron configuration of the element ________ is [Kr]5s14d5.

Accepted Answer

A) Nb 
B) Mo 
C) Cr 
D) Mn 
E) Tc 
A) Nb 
B) Mo 
C) Cr 
D) Mn 
E) Tc

Question 19

Electromagnetic radiation travels through vacuum at a speed of ________ m/s.

Accepted Answer

A) 186,000 
B) 125 
C) 3.00 × 108 
D) 10,000 
E) It depends on wavelength. 
A) 186,000 
B) 125 
C) 3.00 × 108 
D) 10,000 
E) It depends on wavelength.

Question 20

Electromagnetic radiation with a wavelength of 641 nm appears as orange light to the human eye.The energy of one photon of this light is 3.10 ×   J.Thus,a laser that emits   of energy in a pulse of light at this wavelength produces ________ photons in each pulse.

Accepted Answer

A) 2.4 ×   
B) 6.3 × 10-24 
C) 2.7 ×   
D) 4.2 ×   
E) 6.5 ×   
A) 2.4 ×   
B) 6.3 × 10-24 
C) 2.7 ×   
D) 4.2 ×   
E) 6.5 ×

Exam 6: Electronic Structure of Atoms

What color of visible light has the longest wavelength?

Which one of the following is an incorrect orbital notation?

Which electron configuration represents a violation of Hund's rule for an atom in its ground state?

In a ground-state copper atom,the ________ subshell is partially filled.

The shape of an orbital is defined by the angular momentum quantum number which is represented as letter ________.

Which group in the periodic table contains elements with the valence electron configuration of ns2np1?

Which group is represented by a ns2np6 valence shell electron configuration?

The total number of orbitals in a shell is given by ________.

The energy (J)required for an electronic transition in a Bohr hydrogen atom from n = 2 to n = 3 is ________ J.

What is the de Broglie wavelength (m)of a 1.0 × 109 kg train car traveling at 95 km/hr?

A photon that has an energy of 8.63 × 10-12 J would emit light at which wavelength (m)?

The n = 5 to n = 3 transition in the Bohr hydrogen atom corresponds to the ________ of a photon with a wavelength of ________ nm.

Which one of the following is an incorrect subshell notation?

What is the wavelength (angstroms)of a photon that has an energy of 4.38 × 10-18 J?

An electron cannot have the quantum numbers n = ________,l = ________,ml = ________.

An NMR spectrum results from photon irradiation in which the electron spin alignment is flipped.

Which one of the following is considered to be ionizing radiation?

The ground-state electron configuration of the element ________ is [Kr]5s14d5.

Electromagnetic radiation travels through vacuum at a speed of ________ m/s.

Electromagnetic radiation with a wavelength of 641 nm appears as orange light to the human eye.The energy of one photon of this light is 3.10 × J.Thus,a laser that emits of energy in a pulse of light at this wavelength produces ________ photons in each pulse.

Introduction: Matter, energy, and Measurement

Atoms, molecules, and Ions

Chemical Reactions and Reaction Stoichiometry

Reactions in Aqueous Solution

Thermochemistry

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

Filters

Which group in the periodic table contains elements with the valence electron configuration of ns²np¹?

Which group is represented by a ns²np⁶ valence shell electron configuration?

What is the de Broglie wavelength (m)of a 1.0 × 10⁹ kg train car traveling at 95 km/hr?

A photon that has an energy of 8.63 × 10^-12 J would emit light at which wavelength (m)?

The n = 5 to n = 3 transition in the Bohr hydrogen atom corresponds to the of a photon with a wavelength of nm.

What is the wavelength (angstroms)of a photon that has an energy of 4.38 × 10^-18 J?

An electron cannot have the quantum numbers n = ,l = ,m_l = ________.

The ground-state electron configuration of the element ________ is [Kr]5s¹4d⁵.