Question 1

According to the Bohr theory of the hydrogen atom, the minimum energy (in J) needed to ionize a hydrogen atom from the n = 2 state is

Accepted Answer

A)  2.18 × 10-18 J. 
B)  1.64 × 10-18 J. 
C)  5.45 × 10-19 J. 
D)  3.03 × 10-19 J. 
E)  None of these choices are correct. 
A)  2.18 × 10-18 J. 
B)  1.64 × 10-18 J. 
C)  5.45 × 10-19 J. 
D)  3.03 × 10-19 J. 
E)  None of these choices are correct. C

Question 2

Which of the following frequencies of electromagnetic radiation has the shortest wavelength?

Accepted Answer

A)  1 kilohertz 
B)  1 terahertz 
C)  1 dekahertz 
D)  1 gigahertz 
E)  1 megahertz 
A)  1 kilohertz 
B)  1 terahertz 
C)  1 dekahertz 
D)  1 gigahertz 
E)  1 megahertz B

Question 3

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  False

Question 4

Which of the following is a correct set of quantum numbers for an electron in a 3d orbital?

Accepted Answer

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

Question 5

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 6

A photon has an energy of 5.53 × 10-17 J. What is its frequency in s-1?

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)  8.35 × 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)  8.35 × 1016 s-1

Question 7

Continuous spectra are characteristic of heated solids.

Accepted Answer

A) True 
 B)False

Question 8

A sprinter must average 24.0 mi/h to win a 100-m dash in 9.30 s. What is his wavelength at this speed if his mass is 84.5 kg?

Accepted Answer

A)  7.29 × 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 are correct. 
A)  7.29 × 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 are correct.

Question 9

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 10

Which scientist first proposed that the electron in the hydrogen atom can have only certain energies?

Accepted Answer

A)  Planck 
B)  Einstein 
C)  Bohr 
D)  Rydberg 
E)  Heisenberg 
A)  Planck 
B)  Einstein 
C)  Bohr 
D)  Rydberg 
E)  Heisenberg

Question 11

Green light has a wavelength of 5200 Å. Calculate the energy of one photon of green light.

Accepted Answer

A)  3.4 × 10-40 J 
B)  3.4 × 10-30 J 
C)  3.8 × 10-29 J 
D)  3.4 × 10-27 J 
E)  3.8 × 10-19 J 
A)  3.4 × 10-40 J 
B)  3.4 × 10-30 J 
C)  3.8 × 10-29 J 
D)  3.4 × 10-27 J 
E)  3.8 × 10-19 J

Question 12

The de Broglie equation predicts that the wavelength (in m) of a proton moving at 1000. m/s is

Accepted Answer

A)  3.96 × 10-10 m. 
B)  3.96 × 10-7 m. 
C)  2.52 × 106 m. 
D)  2.52 × 109 m. 
E)  > 1010 m. 
A)  3.96 × 10-10 m. 
B)  3.96 × 10-7 m. 
C)  2.52 × 106 m. 
D)  2.52 × 109 m. 
E)  > 1010 m.

Question 13

Infrared radiation from the sun has a wavelength of 6200 nm. Calculate the energy of one photon of that radiation.

Accepted Answer

A)  4.l × 10-39 J 
B)  4.l × 10-30 J 
C)  3.2 × 10-29 J 
D)  3.2 × 10-26 J 
E)  between 10-20 and 10-19 J 
A)  4.l × 10-39 J 
B)  4.l × 10-30 J 
C)  3.2 × 10-29 J 
D)  3.2 × 10-26 J 
E)  between 10-20 and 10-19 J

Question 14

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?

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 15

The AM station KBOR plays your favorite music from the 20's and 30's at 1290 kHz. Find the wavelength of these waves.

Accepted Answer

A)  4.30 × 10-2 m 
B)  0.144 m 
C)  6.94 m 
D)  232 m 
E)  > 103 m 
A)  4.30 × 10-2 m 
B)  0.144 m 
C)  6.94 m 
D)  232 m 
E)  > 103 m

Question 16

In an atom, the square of an electron's wave function

Accepted Answer

A)  becomes zero at the nucleus. 
B)  is smallest near the nucleus. 
C)  is largest near the nucleus. 
D)  may be zero at more than one point. 
E)  tends to infinity at large distances from the nucleus. 
A)  becomes zero at the nucleus. 
B)  is smallest near the nucleus. 
C)  is largest near the nucleus. 
D)  may be zero at more than one point. 
E)  tends to infinity at large distances from the nucleus.

Question 17

The energy of a photon is directly proportional to the wavelength of the radiation.

Accepted Answer

A) True 
 B)False

Question 18

Line spectra are characteristic of atoms in the gas phase.

Accepted Answer

A) True 
 B)False

Question 19

Line spectra from all regions of the electromagnetic spectrum, including the Paschen series of infrared lines for hydrogen, are used by astronomers to identify elements present in the atmospheres of stars. Calculate the wavelength of the photon emitted when the hydrogen atom undergoes a transition from n = 5 to n = 3. (R = 1.096776 × 107 m-1)

Accepted Answer

A)  205.1 nm 
B)  384.6 nm 
C)  683.8 nm 
D)  1282 nm 
E)  > 1500 nm 
A)  205.1 nm 
B)  384.6 nm 
C)  683.8 nm 
D)  1282 nm 
E)  > 1500 nm

Question 20

The orientation in space 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)  None of these choices are correct. 
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)  None of these choices are correct.

Exam 7: Quantum Theory and Atomic Structure

According to the Bohr theory of the hydrogen atom, the minimum energy (in J) needed to ionize a hydrogen atom from the n = 2 state is

Which of the following frequencies of electromagnetic radiation has the shortest wavelength?

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

Which of the following is a correct set of quantum numbers for an electron in a 3d orbital?

Atomic orbitals developed using quantum mechanics

A photon has an energy of 5.53 × 10-17 J. What is its frequency in s-1?

Continuous spectra are characteristic of heated solids.

A sprinter must average 24.0 mi/h to win a 100-m dash in 9.30 s. What is his wavelength at this speed if his mass is 84.5 kg?

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)

Which scientist first proposed that the electron in the hydrogen atom can have only certain energies?

Green light has a wavelength of 5200 Å. Calculate the energy of one photon of green light.

The de Broglie equation predicts that the wavelength (in m) of a proton moving at 1000. m/s is

Infrared radiation from the sun has a wavelength of 6200 nm. Calculate the energy of one photon of that radiation.

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?

The AM station KBOR plays your favorite music from the 20's and 30's at 1290 kHz. Find the wavelength of these waves.

In an atom, the square of an electron's wave function

The energy of a photon is directly proportional to the wavelength of the radiation.

Line spectra are characteristic of atoms in the gas phase.

The orientation in space of an atomic orbital is associated with

Keys to Studying Chemistry Definitions, Units, and Problem Solving

The Components of Matter

Stoichiometry of Formulas and Equations

Three 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

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 Reaction Direction

Electrochemistry Chemical Change and Electrical Work

The Elements in Nature and Industry

Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

A photon has an energy of 5.53 × 10^-17 J. What is its frequency in s^-1?

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?