Question 1

Which orbital has the highest energy in a multielectron atom? The quantum numbers are given as (n, $\ell$ , ml).

Accepted Answer

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

Question 2

Which of the following photons has the highest frequency?

Accepted Answer

A)  a photon from a Nd:YAG laser with $\lambda$ = 1,064 nm 
B)  a photon from an Ar+ laser with $\lambda$ = 514.5 nm 
C)  a photon from a Kr+ laser with $\lambda$ = 647 nm 
D)  a photon from an ArF laser with $\lambda$= 193 nm 
E)  a photon from a He-Ne laser with $\lambda$= 633 nm 
A)  a photon from a Nd:YAG laser with $\lambda$ = 1,064 nm 
B)  a photon from an Ar+ laser with $\lambda$ = 514.5 nm 
C)  a photon from a Kr+ laser with $\lambda$ = 647 nm 
D)  a photon from an ArF laser with $\lambda$= 193 nm 
E)  a photon from a He-Ne laser with $\lambda$= 633 nm

Question 3

A shell consists of all ________

Accepted Answer

A)  electrons with the same $\ell$
Quantum number. 
B)  orbitals with the same quantum numbers. 
C)  orbitals with the same principal quantum number. 
D)  electrons with the same magnetic quantum number. 
E)  orbitals with the same $\ell$
And ml quantum numbers. 
A)  electrons with the same $\ell$
Quantum number. 
B)  orbitals with the same quantum numbers. 
C)  orbitals with the same principal quantum number. 
D)  electrons with the same magnetic quantum number. 
E)  orbitals with the same $\ell$
And ml quantum numbers.

Question 4

The fact that the absorption and emission spectra of atoms and their ions are different is evidence that the spectra are due to ________

Accepted Answer

A)  electrons. 
B)  protons. 
C)  neutrons. 
D)  the nuclei. 
E)  electromagnetic interactions. 
A)  electrons. 
B)  protons. 
C)  neutrons. 
D)  the nuclei. 
E)  electromagnetic interactions.

Question 5

Which one of the following diagrams represents the electron configuration of a nitrogen atom?

Accepted Answer

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

Question 6

Which listing has the orbitals in order of increasing energy in a multielectron atom?

Accepted Answer

A)  3s x y z 
E)  3s < 2p < 4s 
A)  3s x y z 
E)  3s < 2p < 4s

Question 7

In comparing the dark Fraunhofer lines with light emitted by elements in a flame, Bunsen and Kirchhoff demonstrated that ________

Accepted Answer

A)  atoms emit and absorb electromagnetic radiation at characteristic wavelengths. 
B)  the solar spectrum has dark lines. 
C)  helium may be found in minerals that contain uranium. 
D)  electrons are responsible for the absorption and emission of electromagnetic radiation. 
E)  the solar spectrum has bright lines. 
A)  atoms emit and absorb electromagnetic radiation at characteristic wavelengths. 
B)  the solar spectrum has dark lines. 
C)  helium may be found in minerals that contain uranium. 
D)  electrons are responsible for the absorption and emission of electromagnetic radiation. 
E)  the solar spectrum has bright lines.

Question 8

Early photoelectric light detectors were based on cesium. Cesium metal has a work function of 3.43 *10-19 J. What is the longest wavelength of light that could be detected with one of these detectors?

Accepted Answer

A)  759 nm 
B)  579 nm 
C)  679 nm 
D)  767 nm 
E)  455 nm 
A)  759 nm 
B)  579 nm 
C)  679 nm 
D)  767 nm 
E)  455 nm

Question 9

Which of the following sources produces the lowest energy photons?

Accepted Answer

A)  a doctor's X-ray source 
B)  the heat lamp in your bathroom 
C)  a microwave oven 
D)  gamma rays from a star 
E)  radio waves from your local station 
A)  a doctor's X-ray source 
B)  the heat lamp in your bathroom 
C)  a microwave oven 
D)  gamma rays from a star 
E)  radio waves from your local station

Question 10

Radiation with a wavelength of ________ nm is produced by the n = 5 to n = 2 transition in the hydrogen atom, and this transition occurs in the ________ region of the electromagnetic spectrum.

Accepted Answer

The answer of Radiation with a wavelength of ________ nm...

Question 11

Which statement A-D about the wave function for a single electron is not correct?

Accepted Answer

A)  A French graduate student named Louis de Broglie first had the idea that an electron should be described as a wave 
B)  Louis de Broglie postulated that the wavelength of an electron is given in terms of Planck's constant and its momentum, $\lambda$ = h/p. 
C)  The square of the amplitude of the wave function at a particular point in space gives the probability density of finding the electron at that point. 
D)  An electronic wave function can never be 0 because that would mean the electron does not exist. 
E)  Statements A-D are all correct. 
A)  A French graduate student named Louis de Broglie first had the idea that an electron should be described as a wave 
B)  Louis de Broglie postulated that the wavelength of an electron is given in terms of Planck's constant and its momentum, $\lambda$ = h/p. 
C)  The square of the amplitude of the wave function at a particular point in space gives the probability density of finding the electron at that point. 
D)  An electronic wave function can never be 0 because that would mean the electron does not exist. 
E)  Statements A-D are all correct.

Question 12

Which of the following elements would you expect to have the lowest first ionization energy?

Accepted Answer

A)  F 
B)  Br 
C)  Cl 
D)  I 
E)  Xe 
A)  F 
B)  Br 
C)  Cl 
D)  I 
E)  Xe

Question 13

Place these types of radiation in order of increasing energy per photon.
I. Yellow light from a street lamp.
II. X-rays from a dental X-ray.
III. Microwaves from your cell phone.
IV. Radio waves from your favorite FM station.

Accepted Answer

The answer of Place these types of radiation in order...

Question 14

Which of the following is a possible set of quantum numbers for a 3d orbital?

Accepted Answer

A)  n = 3, $\ell$ = 1, me= -1 
B)  n = 3, $\ell$ = 0, me = 0 
C)  n = 3, $\ell$ = 2, me = 3 
D)  n = 3, $\ell$ = 2, me = 0 
E)  n = 3, $\ell$ = 1, me = 2 
A)  n = 3, $\ell$ = 1, me= -1 
B)  n = 3, $\ell$ = 0, me = 0 
C)  n = 3, $\ell$ = 2, me = 3 
D)  n = 3, $\ell$ = 2, me = 0 
E)  n = 3, $\ell$ = 1, me = 2

Question 15

What is the wavelength ($\lambda$, in m) of a radio station operating at a frequency of 99.6 MHz?

Accepted Answer

A)  3.01 * 106 m 
B)  3.01 m 
C)  3.32 *10 10-7 m 
D)  0.332 m 
E)  3.32 m 
A)  3.01 * 106 m 
B)  3.01 m 
C)  3.32 *10 10-7 m 
D)  0.332 m 
E)  3.32 m

Question 16

How much energy is required to ionize one mole of hydrogen atoms in their ground state?

Accepted Answer

A)  1,312 kJ 
B)  2.18 kJ 
C)  218 kJ 
D)  2,178 kJ 
E)  131.2 kJ 
A)  1,312 kJ 
B)  2.18 kJ 
C)  218 kJ 
D)  2,178 kJ 
E)  131.2 kJ

Question 17

The energy of a one-electron atom is given by E = -(2.18 *10-18 J) $$\left( \frac { z } { n } \right) ^ { 2 }$$ where Z is the atomic number of the element. Which of the following one-electron ions has the largest ionization energy?

Accepted Answer

A)  Li2+ 
B)  Be3+ 
C)  He+ 
D)  B4+ 
E)  C5+ 
A)  Li2+ 
B)  Be3+ 
C)  He+ 
D)  B4+ 
E)  C5+

Question 18

Write the electron configuration of Zn2+.

Accepted Answer

Question 19

How much energy is required to ionize a He+ ion in its ground state?

Accepted Answer

A)  2.18 * 10-18 J 
B)  4.36 *10-18 J 
C)  8.72 *10-18 J 
D)  1.74 *10-18 J 
A)  2.18 * 10-18 J 
B)  4.36 *10-18 J 
C)  8.72 *10-18 J 
D)  1.74 *10-18 J

Question 20

Electromagnetic radiation with a frequency of 8.6 *1014 Hz incident on an unknown metal surface causes ejection of photoelectrons with kinetic energies of 1.3 *10-19 J. What is the unknown metal?

Accepted Answer

A)  rubidium (  = 3.5 *10-19 J) 
B)  gold (  = 8.2 *10-19 J) 
C)  nickel (  = 8.3 *10-19 J) 
D)  sodium (  = 4.4 *10-19 J) 
E)  platinum (  = 9.1 *10-19 J) 
A)  rubidium (  = 3.5 *10-19 J) 
B)  gold (  = 8.2 *10-19 J) 
C)  nickel (  = 8.3 *10-19 J) 
D)  sodium (  = 4.4 *10-19 J) 
E)  platinum (  = 9.1 *10-19 J)

Exam 7: A Quantum Model of Atoms: Waves and Particles

Which orbital has the highest energy in a multielectron atom? The quantum numbers are given as (n, ℓ\ellℓ , ml).

Which of the following photons has the highest frequency?

A shell consists of all ________

The fact that the absorption and emission spectra of atoms and their ions are different is evidence that the spectra are due to ________

Which one of the following diagrams represents the electron configuration of a nitrogen atom?

Which listing has the orbitals in order of increasing energy in a multielectron atom?

In comparing the dark Fraunhofer lines with light emitted by elements in a flame, Bunsen and Kirchhoff demonstrated that ________

Early photoelectric light detectors were based on cesium. Cesium metal has a work function of 3.43 *10-19 J. What is the longest wavelength of light that could be detected with one of these detectors?

Which of the following sources produces the lowest energy photons?

Radiation with a wavelength of ________ nm is produced by the n = 5 to n = 2 transition in the hydrogen atom, and this transition occurs in the ________ region of the electromagnetic spectrum.

Which statement A-D about the wave function for a single electron is not correct?

Which of the following elements would you expect to have the lowest first ionization energy?

Place these types of radiation in order of increasing energy per photon. I. Yellow light from a street lamp. II. X-rays from a dental X-ray. III. Microwaves from your cell phone. IV. Radio waves from your favorite FM station.

Which of the following is a possible set of quantum numbers for a 3d orbital?

What is the wavelength ( λ\lambdaλ , in m) of a radio station operating at a frequency of 99.6 MHz?

How much energy is required to ionize one mole of hydrogen atoms in their ground state?

The energy of a one-electron atom is given by E = -(2.18 *10-18 J) (zn)2\left( \frac { z } { n } \right) ^ { 2 }(nz​)2 where Z is the atomic number of the element. Which of the following one-electron ions has the largest ionization energy?

Write the electron configuration of Zn2+.

How much energy is required to ionize a He+ ion in its ground state?

Electromagnetic radiation with a frequency of 8.6 *1014 Hz incident on an unknown metal surface causes ejection of photoelectrons with kinetic energies of 1.3 *10-19 J. What is the unknown metal?

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: the Air We Breathe

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Structures and Applications

Organic Chemistry: Fuels, Pharmaceuticals, Materials, and Life

Chemical Kinetics: Reactions in the Air We Breathe

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acid-Base and Solubility Equilibria: Reactions in Soil and Water

Metal Ions: Colorful and Essential

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: the Quest for Clean Energy

Biochemistry: the Compounds of Life

Nuclear Chemistry: Applications to Energy and Medicine

Life and the Periodic Table

Filters

Which orbital has the highest energy in a multielectron atom? The quantum numbers are given as (n, $\ell$ , m_l).

Early photoelectric light detectors were based on cesium. Cesium metal has a work function of 3.43 *10^-¹⁹ J. What is the longest wavelength of light that could be detected with one of these detectors?

Radiation with a wavelength of nm is produced by the n = 5 to n = 2 transition in the hydrogen atom, and this transition occurs in the region of the electromagnetic spectrum.

What is the wavelength ( $\lambda$ , in m) of a radio station operating at a frequency of 99.6 MHz?

The energy of a one-electron atom is given by E = -(2.18 *10^-¹⁸ J) $\left( \frac { z } { n } \right) ^ { 2 }$ where Z is the atomic number of the element. Which of the following one-electron ions has the largest ionization energy?

Write the electron configuration of Zn²⁺.

How much energy is required to ionize a He⁺ ion in its ground state?

Electromagnetic radiation with a frequency of 8.6 10¹⁴ Hz incident on an unknown metal surface causes ejection of photoelectrons with kinetic energies of 1.3 10^-¹⁹ J. What is the unknown metal?