Question 1

The FM station KDUL broadcasts music at 99.1 MHz. Find the wavelength of these waves.

Accepted Answer

A)  1.88 × 10-2 m 
B)  0.330 m 
C)  3.03 m 
D)  5.33 × 102 m 
E)  > 103 m 
A)  1.88 × 10-2 m 
B)  0.330 m 
C)  3.03 m 
D)  5.33 × 102 m 
E)  > 103 m

Question 2

Consider the following adjectives used to describe types of spectrum: continuous line atomic emission absorption
How many of them are appropriate to describe the spectrum of radiation absorbed by a sample of mercury vapor?

Accepted Answer

A)  one 
B)  two 
C)  three 
D)  four 
E)  five 
A)  one 
B)  two 
C)  three 
D)  four 
E)  five

Question 3

Who developed an empirical equation from which the wavelengths of lines in the spectrum of hydrogen atoms can be calculated?

Accepted Answer

A)  Planck 
B)  de Broglie 
C)  Bohr 
D)  Rutherford 
E)  Rydberg 
A)  Planck 
B)  de Broglie 
C)  Bohr 
D)  Rutherford 
E)  Rydberg

Question 4

Atomic orbitals developed using quantum mechanics

Accepted Answer

A)  describe regions of space in which one is most likely to find an electron. 
B)  describe exact paths for electron motion. 
C)  give a description of the atomic structure which is essentially the same as the Bohr model. 
D)  allow scientists to calculate an exact volume for the hydrogen atom. 
E)  are in conflict with the Heisenberg Uncertainty Principle. 
A)  describe regions of space in which one is most likely to find an electron. 
B)  describe exact paths for electron motion. 
C)  give a description of the atomic structure which is essentially the same as the Bohr model. 
D)  allow scientists to calculate an exact volume for the hydrogen atom. 
E)  are in conflict with the Heisenberg Uncertainty Principle.

Question 5

Select the arrangement of electromagnetic radiation which starts with the lowest energy and increases to greatest energy.

Accepted Answer

A)  radio, visible, infrared, ultraviolet 
B)  infrared, visible, ultraviolet, microwave 
C)  visible, ultraviolet, infrared, gamma rays 
D)  X-radiation, visible, infrared, microwave 
E)  microwave, infrared, visible, ultraviolet 
A)  radio, visible, infrared, ultraviolet 
B)  infrared, visible, ultraviolet, microwave 
C)  visible, ultraviolet, infrared, gamma rays 
D)  X-radiation, visible, infrared, microwave 
E)  microwave, infrared, visible, ultraviolet

Question 6

The Bohr theory of the hydrogen atom predicts the energy difference (in J) between the n = 3 and the n = 5 state to be

Accepted Answer

A)  8.72 × 10-20 J. 
B)  1.36 × 10-19 J. 
C)  2.42 × 10-19 J. 
D)  1.55 × 10-19 J. 
E)  1.09 × 10-18 J. 
A)  8.72 × 10-20 J. 
B)  1.36 × 10-19 J. 
C)  2.42 × 10-19 J. 
D)  1.55 × 10-19 J. 
E)  1.09 × 10-18 J.

Question 7

The energy of an electron in the hydrogen atom is determined by

Accepted Answer

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

Question 8

a. Use Bohr's equation to calculate how much energy (in J) is needed to promote an electron from the H-atom ground state to the n = 4 level.
b. If a photon provides the energy in (a), what is its wavelength in nm?

Accepted Answer

a. 2.04 ×

Question 9

Who was the first scientist to propose that an object could emit only certain amounts of energy?

Accepted Answer

A)  Planck 
B)  Einstein 
C)  Bohr 
D)  Rydberg 
E)  de Broglie 
A)  Planck 
B)  Einstein 
C)  Bohr 
D)  Rydberg 
E)  de Broglie

Question 10

Which one of the following sets of quantum numbers can correctly represent a 3p orbital?

Accepted Answer

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

Question 11

Who proposed the principle which states that one cannot simultaneously know the exact position and velocity of a particle?

Accepted Answer

A)  Einstein 
B)  Planck 
C)  Heisenberg 
D)  Compton 
E)  de Broglie 
A)  Einstein 
B)  Planck 
C)  Heisenberg 
D)  Compton 
E)  de Broglie

Question 12

Use the Rydberg equation to calculate the frequency of a photon absorbed when the hydrogen atom undergoes a transition from n1 = 2 to n2 = 4. (R = 1.096776 × 107 m-1)

Accepted Answer

A)  2.056 × 106 s-1 
B)  2.742 × 106 s-1 
C)  6.165 × 1014 s-1 
D)  8.226 × 1014 s-1 
E)  > 1015 s-1 
A)  2.056 × 106 s-1 
B)  2.742 × 106 s-1 
C)  6.165 × 1014 s-1 
D)  8.226 × 1014 s-1 
E)  > 1015 s-1

Question 13

The following combinations of quantum numbers are not allowed.

Accepted Answer

a. n = 3
b

Question 14

In the Bohr model of the hydrogen atom, the electron moves in a circular path which Bohr referred to as an orbital.

Accepted Answer

A) True 
 B)False

Question 15

In the quantum mechanical treatment of the hydrogen atom, which one of the following combinations of quantum numbers is not allowed?

Accepted Answer

The answer of In the quantum mechanical treatment of the...

Question 16

a. Calculate the momentum of a photon of green light, wavelength 515 nm.
b. If this photon is traveling in a vacuum, what is its "mass"?

Accepted Answer

a. 1.29 ×

Question 17

Platinum, which is widely used as a catalyst, has a work function F1F1F1S1F1F1F10 (the minimum energy needed to eject an electron from the metal surface) of 9.05 × 10-19 J. What is the longest wavelength of light which will cause electrons to be emitted?

Accepted Answer

A)  2.196 × 10-7 m 
B)  4.553 × 10-6 m 
C)  5.654 × 102 m 
D)  1.370 × 1015 m 
E)  > 106 m 
A)  2.196 × 10-7 m 
B)  4.553 × 10-6 m 
C)  5.654 × 102 m 
D)  1.370 × 1015 m 
E)  > 106 m

Question 18

A modern compact fluorescent lamp contains 1.4 mg of mercury. If each mercury atom in the lamp were to emit a single photon of wavelength 254 nm, how many joules of energy would be emitted?

Accepted Answer

A)  7.8 × 10-19 J 
B)  3.3 J 
C)  6.6 × 102 J 
D)  3.3 × 103 J 
E)  4.2 × 1018 J 
A)  7.8 × 10-19 J 
B)  3.3 J 
C)  6.6 × 102 J 
D)  3.3 × 103 J 
E)  4.2 × 1018 J

Question 19

Use the Bohr equation to calculate the energy of
a. the largest energy absorption or emission process involving the n = 2 state of the hydrogen atom.
b. the smallest energy absorption or emission process involving the n = 2 state of the hydrogen atom.

Accepted Answer

a. 1.64 × 10^-18 J (n =

Question 20

An electron in the n = 6 level emits a photon with a wavelength of 410.2 nm. To what energy level does the electron move?

Accepted Answer

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

Exam 7: Quantum Theory and Atomic Structure

The FM station KDUL broadcasts music at 99.1 MHz. Find the wavelength of these waves.

Consider the following adjectives used to describe types of spectrum: continuous line atomic emission absorption How many of them are appropriate to describe the spectrum of radiation absorbed by a sample of mercury vapor?

Who developed an empirical equation from which the wavelengths of lines in the spectrum of hydrogen atoms can be calculated?

Atomic orbitals developed using quantum mechanics

Select the arrangement of electromagnetic radiation which starts with the lowest energy and increases to greatest energy.

The Bohr theory of the hydrogen atom predicts the energy difference (in J) between the n = 3 and the n = 5 state to be

The energy of an electron in the hydrogen atom is determined by

a. Use Bohr's equation to calculate how much energy (in J) is needed to promote an electron from the H-atom ground state to the n = 4 level. b. If a photon provides the energy in (a), what is its wavelength in nm?

Who was the first scientist to propose that an object could emit only certain amounts of energy?

Which one of the following sets of quantum numbers can correctly represent a 3p orbital?

Who proposed the principle which states that one cannot simultaneously know the exact position and velocity of a particle?

Use the Rydberg equation to calculate the frequency of a photon absorbed when the hydrogen atom undergoes a transition from n1 = 2 to n2 = 4. (R = 1.096776 × 107 m-1)

The following combinations of quantum numbers are not allowed.

In the Bohr model of the hydrogen atom, the electron moves in a circular path which Bohr referred to as an orbital.

In the quantum mechanical treatment of the hydrogen atom, which one of the following combinations of quantum numbers is not allowed?

a. Calculate the momentum of a photon of green light, wavelength 515 nm. b. If this photon is traveling in a vacuum, what is its "mass"?

Platinum, which is widely used as a catalyst, has a work function  (the minimum energy needed to eject an electron from the metal surface) of 9.05 × 10-19 J. What is the longest wavelength of light which will cause electrons to be emitted?

A modern compact fluorescent lamp contains 1.4 mg of mercury. If each mercury atom in the lamp were to emit a single photon of wavelength 254 nm, how many joules of energy would be emitted?

Use the Bohr equation to calculate the energy of a. the largest energy absorption or emission process involving the n = 2 state of the hydrogen atom. b. the smallest energy absorption or emission process involving the n = 2 state of the hydrogen atom.

An electron in the n = 6 level emits a photon with a wavelength of 410.2 nm. To what energy level does the electron move?

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

The Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

The Properties of Mixtures: Solutions and Colloids

Periodic Patterns in the Main Group Elements: Bonding, Structure, and Reactivity

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Use the Rydberg equation to calculate the frequency of a photon absorbed when the hydrogen atom undergoes a transition from n₁ = 2 to n₂ = 4. (R = 1.096776 × 10⁷ m^-1)

Platinum, which is widely used as a catalyst, has a work function  (the minimum energy needed to eject an electron from the metal surface) of 9.05 × 10^-19 J. What is the longest wavelength of light which will cause electrons to be emitted?