Question 1

Which of the following types of electromagnetic radiation has the lowest frequency?

Accepted Answer

A)  yellow 
B)  blue 
C)  orange 
D)  green 
E)  purple 
A)  yellow 
B)  blue 
C)  orange 
D)  green 
E)  purple C

Question 2

Give all possible values of l if n = 3.

Accepted Answer

A)  3 
B)  +1/2 
C)  0, 1, 2 
D)  -1, 0, 1 
E)  1, 2, 3, 4 
A)  3 
B)  +1/2 
C)  0, 1, 2 
D)  -1, 0, 1 
E)  1, 2, 3, 4 C

Question 3

When an electric current is passed through a tube containing hydrogen,hydrogen atoms absorb some of the electrical energy and reemit it as a ________ color.

Accepted Answer

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

Question 4

The heat that is felt from a hot object is called ________ radiation.

Accepted Answer

A)  ultraviolet 
B)  gamma 
C)  infrared 
D)  x-ray 
E)  microwave 
A)  ultraviolet 
B)  gamma 
C)  infrared 
D)  x-ray 
E)  microwave

Question 5

Calculate the energy of the red light emitted by a neon atom with a wavelength of 703.2 nm.

Accepted Answer

A)  3.54 × 10-19 J 
B)  4.27 × 10-19 J 
C)  2.34 × 10-19 J 
D)  6.45 × 10-19 J 
E)  2.83 × 10-19 J 
A)  3.54 × 10-19 J 
B)  4.27 × 10-19 J 
C)  2.34 × 10-19 J 
D)  6.45 × 10-19 J 
E)  2.83 × 10-19 J

Question 6

Describe the shape of a 3s orbital.

Accepted Answer

A)  spherical 
B)  dumbbell shaped 
C)  two balls 
D)  six balls 
E)  eight balls 
A)  spherical 
B)  dumbbell shaped 
C)  two balls 
D)  six balls 
E)  eight balls

Question 7

What is the maximum number of s orbitals that are possible?

Accepted Answer

A)  1 
B)  2 
C)  7 
D)  0 
E)  12 
A)  1 
B)  2 
C)  7 
D)  0 
E)  12

Question 8

Determine the end (final)value of n in a hydrogen atom transition,if the electron starts in n = 2 and the atom absorbs a photon of light with a frequency of 4.57 × 1014 Hz.

Accepted Answer

A)  3 
B)  1 
C)  4 
D)  6 
E)  7 
A)  3 
B)  1 
C)  4 
D)  6 
E)  7

Question 9

Calculate the wavelength (in nm)of the blue light emitted by a mercury lamp with a frequency of 6.88 × 1014 Hz.

Accepted Answer

A)  229 nm 
B)  436 nm 
C)  206 nm 
D)  485 nm 
E)  675 nm 
A)  229 nm 
B)  436 nm 
C)  206 nm 
D)  485 nm 
E)  675 nm

Question 10

Identify the color that has a wavelength of 730 nm.

Accepted Answer

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

Question 11

Identify the color of a flame test for barium.

Accepted Answer

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

Question 12

Give the numbers for ml for a d orbital.

Accepted Answer

A)  0, +1 
B)  0 
C)  +1, +2, +3, +4 
D)  -2, -1, 0, +1, +2 
E)  -3, -2, -1, 0, +1, +2, +3 
A)  0, +1 
B)  0 
C)  +1, +2, +3, +4 
D)  -2, -1, 0, +1, +2 
E)  -3, -2, -1, 0, +1, +2, +3

Question 13

Which of the following statements is TRUE?

Accepted Answer

A)  We can sometimes know the exact location and speed of an electron at the same time. 
B)  All orbitals in a given atom are roughly the same size. 
C)  Since electrons have mass, we must always consider them to have particle properties and never wavelike properties. 
D)  Atoms are roughly spherical because when all of the different shaped orbitals are overlapped, they take on a spherical shape. 
E)  All of the above are true. 
A)  We can sometimes know the exact location and speed of an electron at the same time. 
B)  All orbitals in a given atom are roughly the same size. 
C)  Since electrons have mass, we must always consider them to have particle properties and never wavelike properties. 
D)  Atoms are roughly spherical because when all of the different shaped orbitals are overlapped, they take on a spherical shape. 
E)  All of the above are true.

Question 14

Why don't we observe the wavelength of everyday macroscopic objects?

Accepted Answer

Due to the large mass of macro

Question 15

A type of energy embodied in oscillating electric and magnetic fields is called

Accepted Answer

A)  infrared radiation. 
B)  microwave radiation. 
C)  magnetism. 
D)  electricity. 
E)  electromagnetic radiation. 
A)  infrared radiation. 
B)  microwave radiation. 
C)  magnetism. 
D)  electricity. 
E)  electromagnetic radiation.

Question 16

Give the value of l for a 3p orbital.

Accepted Answer

A)  1 
B)  +4 
C)  0 
D)  +2 
E)  -2 
A)  1 
B)  +4 
C)  0 
D)  +2 
E)  -2

Question 17

What is the maximum number of f orbitals that are possible?

Accepted Answer

A)  0 
B)  3 
C)  7 
D)  8 
E)  9 
A)  0 
B)  3 
C)  7 
D)  8 
E)  9

Question 18

The distance between adjacent crests is called

Accepted Answer

A)  wavelength. 
B)  amplitude. 
C)  frequency. 
D)  area. 
E)  median. 
A)  wavelength. 
B)  amplitude. 
C)  frequency. 
D)  area. 
E)  median.

Question 19

Calculate the wavelength of light associated with the transition from n = 1 to n = 3 in the hydrogen atom.

Accepted Answer

A)  103 nm 
B)  155 nm 
C)  646 nm 
D)  971 nm 
E)  136 nm 
A)  103 nm 
B)  155 nm 
C)  646 nm 
D)  971 nm 
E)  136 nm

Question 20

Determine the longest wavelength of light required to remove an electron from a sample of potassium metal,if the binding energy for an electron in K is 1.76 × 103 kJ/mol.

Accepted Answer

A)  147 nm 
B)  68.0 nm 
C)  113 nm 
D)  885 nm 
E)  387 nm 
A)  147 nm 
B)  68.0 nm 
C)  113 nm 
D)  885 nm 
E)  387 nm

Exam 7: The Quantum-Mechanical Model of the Atom

Which of the following types of electromagnetic radiation has the lowest frequency?

Give all possible values of l if n = 3.

When an electric current is passed through a tube containing hydrogen,hydrogen atoms absorb some of the electrical energy and reemit it as a ________ color.

The heat that is felt from a hot object is called ________ radiation.

Calculate the energy of the red light emitted by a neon atom with a wavelength of 703.2 nm.

Describe the shape of a 3s orbital.

What is the maximum number of s orbitals that are possible?

Determine the end (final)value of n in a hydrogen atom transition,if the electron starts in n = 2 and the atom absorbs a photon of light with a frequency of 4.57 × 1014 Hz.

Calculate the wavelength (in nm)of the blue light emitted by a mercury lamp with a frequency of 6.88 × 1014 Hz.

Identify the color that has a wavelength of 730 nm.

Identify the color of a flame test for barium.

Give the numbers for ml for a d orbital.

Which of the following statements is TRUE?

Why don't we observe the wavelength of everyday macroscopic objects?

A type of energy embodied in oscillating electric and magnetic fields is called

Give the value of l for a 3p orbital.

What is the maximum number of f orbitals that are possible?

The distance between adjacent crests is called

Calculate the wavelength of light associated with the transition from n = 1 to n = 3 in the hydrogen atom.

Determine the longest wavelength of light required to remove an electron from a sample of potassium metal,if the binding energy for an electron in K is 1.76 × 103 kJ/mol.

Matter, measurement, and Problem Solving

Atoms and Elements

Molecules,compounds,and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes,valence Bond Theory,

Liquids,solids,and Intermolecular Forces

Solids and Modern Materials

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

Determine the end (final)value of n in a hydrogen atom transition,if the electron starts in n = 2 and the atom absorbs a photon of light with a frequency of 4.57 × 10¹⁴ Hz.

Calculate the wavelength (in nm)of the blue light emitted by a mercury lamp with a frequency of 6.88 × 10¹⁴ Hz.

Give the numbers for m_l for a d orbital.

Determine the longest wavelength of light required to remove an electron from a sample of potassium metal,if the binding energy for an electron in K is 1.76 × 10³ kJ/mol.