Question 1

In quantum mechanics, an atomic orbital _______.

Accepted Answer

A) provides the position of an electron at any instant of time in the space around an atomic nucleus. 
B) provides the probability of finding an electron at any point in the space around an atomic nucleus. 
C) is identical to the orbits Bohr used in his analysis of the hydrogen atom. 
D) identifies the most probable position of an atomic nucleus. 
E) locates all the electrons in an atom. 
A) provides the position of an electron at any instant of time in the space around an atomic nucleus. 
B) provides the probability of finding an electron at any point in the space around an atomic nucleus. 
C) is identical to the orbits Bohr used in his analysis of the hydrogen atom. 
D) identifies the most probable position of an atomic nucleus. 
E) locates all the electrons in an atom.

Question 2

If the electron (9.11 *10-31 kg) in the hydrogen atom is traveling at about 2.2 *106 m/s $\pm$ 5%, what is the uncertainty in the electron's position?

Accepted Answer

A) ($\pm$58 µm) 
B) ($\pm$220 nm) 
C) ($\pm$130 pm) 
D) ($\pm$260 pm) 
E) ($\pm$5.2 fm) 
A) ($\pm$58 µm) 
B) ($\pm$220 nm) 
C) ($\pm$130 pm) 
D) ($\pm$260 pm) 
E) ($\pm$5.2 fm)

Question 3

What is the longest wavelength of light emitted by an excited hydrogen atom when nfinal = 1?

Accepted Answer

A) 91.16 nm 
B) 121.5 nm 
C) 273.5 nm 
D) 364.6 nm 
E) 656.2 nm 
A) 91.16 nm 
B) 121.5 nm 
C) 273.5 nm 
D) 364.6 nm 
E) 656.2 nm

Question 4

What wavelength of light is required to cause the ejection of photoelectrons with kinetic energies of 5.0 *10-20 J from a calcium surface ($\varPhi$ = 4.60 * 10-19 J)?

Accepted Answer

A) 485 nm 
B) 390 nm 
C) 308 nm 
D) 632 nm 
E) 480 nm 
A) 485 nm 
B) 390 nm 
C) 308 nm 
D) 632 nm 
E) 480 nm

Question 5

Arrange the following elements in order of increasing atomic radius: 16S, 9F, 14Si, 19K, 12Mg.

Accepted Answer

The answer of Arrange the following elements in order of...

Question 6

Which of the following transitions emits the longest wavelength photon?

Accepted Answer

A) n1 = 14 to n2 = 13 
B) n1 = 6 to n2 = 4 
C) n1 = 4 to n2 = 3 
D) n1 = 7 to n2 = 5 
E) n1 = 4 to n2 = 2 
A) n1 = 14 to n2 = 13 
B) n1 = 6 to n2 = 4 
C) n1 = 4 to n2 = 3 
D) n1 = 7 to n2 = 5 
E) n1 = 4 to n2 = 2

Question 7

Which of the following elements has the ground-state electron configuration $ 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{3} ? $

Accepted Answer

A) Al 
B) S 
C) Cl 
D) P 
E) Ar 
A) Al 
B) S 
C) Cl 
D) P 
E) Ar

Question 8

What is the minimum frequency of a photon that can eject a photoelectron from Ba metal? (The work function of barium is $\varPhi$ = 4.3 *10-19 J.)

Accepted Answer

A) 2.8* 10-52 Hz 
B) 6.5 *1014 Hz 
C) 6.5 * 104 Hz 
D) 6.5*1013 Hz 
E) 2.8 * 1014 Hz 
A) 2.8* 10-52 Hz 
B) 6.5 *1014 Hz 
C) 6.5 * 104 Hz 
D) 6.5*1013 Hz 
E) 2.8 * 1014 Hz

Question 9

As the frequency of electromagnetic radiation decreases, which statement below is TRUE?

Accepted Answer

A) Its wavelength decreases. 
B) Its energy decreases. 
C) Its speed decreases. 
D) Its magnetic field component remains constant. 
E) Its electric field component remains constant. 
A) Its wavelength decreases. 
B) Its energy decreases. 
C) Its speed decreases. 
D) Its magnetic field component remains constant. 
E) Its electric field component remains constant.

Question 10

The emission spectra of Na and Na+ are different because _______.

Accepted Answer

A) Na+ has fewer electrons. 
B) Na has fewer electrons. 
C) Na+ has more protons. 
D) Na has fewer neutrons. 
E) Na has more protons. 
A) Na+ has fewer electrons. 
B) Na has fewer electrons. 
C) Na+ has more protons. 
D) Na has fewer neutrons. 
E) Na has more protons.

Question 11

Cesium has a work function of 2.1 eV.What is the kinetic energy of an electron produced when green light (540 nm) is incident on a cesium metal surface? (1 eV = 1.60 * 10-19 J.)

Accepted Answer

3.2 * 10<s

Question 12

Which of the following statements regarding orbitals and wave functions is true?

Accepted Answer

A) Wave functions are mathematical solutions to the Schrödinger wave equation. 
B) Wave functions specify where an electron is at any given time. 
C) An orbital encloses a region in space around the nucleus where the probability of finding an electron is 1. 
D) The square of the wave function describes how the electron matter wave varies in time and space. 
E) All sine functions are solutions to the Schrödinger equation for the hydrogen atom. 
A) Wave functions are mathematical solutions to the Schrödinger wave equation. 
B) Wave functions specify where an electron is at any given time. 
C) An orbital encloses a region in space around the nucleus where the probability of finding an electron is 1. 
D) The square of the wave function describes how the electron matter wave varies in time and space. 
E) All sine functions are solutions to the Schrödinger equation for the hydrogen atom.

Question 13

What is the minimum energy that a photon must have to ionize a ground= state hydrogen atom to the
n = 4 energy level?

Accepted Answer

2.04* 10<s

Question 14

Electromagnetic radiation with a frequency of 8.6* 1014 Hz incident on an unknown metal surface causes the ejection of photoelectrons with kinetic energies of 2.8 *10-19 J.What is the unknown metal?

Accepted Answer

A) rubidium ($\varPhi$ = 3.5 -10-19 J) 
B) gold ($\varPhi$= 8.2 * 10-19 J) 
C) nickel ($\varPhi$ = 8.3 *10-19 J) 
D) sodium ($\varPhi$= 2.9 * 10-19 J) 
E) platinum ($\varPhi$ = 9.1 *10-19 J) 
A) rubidium ($\varPhi$ = 3.5 -10-19 J) 
B) gold ($\varPhi$= 8.2 * 10-19 J) 
C) nickel ($\varPhi$ = 8.3 *10-19 J) 
D) sodium ($\varPhi$= 2.9 * 10-19 J) 
E) platinum ($\varPhi$ = 9.1 *10-19 J)

Question 15

Which statement below regarding electron affinity is FALSE?

Accepted Answer

A) Electron affinity values are usually negative because the association of an electron with a positive nucleus should produce an ion that is more stable. 
B) Zeff has no impact on electron affinity values. 
C) Electron affinities become more positive as atomic size increases. 
D) The electron affinities of the noble gases are positive or zero. 
E) Electron pairing in orbitals can have an impact on electron affinity. 
A) Electron affinity values are usually negative because the association of an electron with a positive nucleus should produce an ion that is more stable. 
B) Zeff has no impact on electron affinity values. 
C) Electron affinities become more positive as atomic size increases. 
D) The electron affinities of the noble gases are positive or zero. 
E) Electron pairing in orbitals can have an impact on electron affinity.

Question 16

Which set of quantum numbers below is NOT allowed?

Accepted Answer

A) n = 1, $ l $ = 0, ml = -1, ms = - ½ 
B) n = 3, $ l $ = 2, ml = 2, ms = + ½ 
C) n = 3, $ l $ = 1, ml = -1, ms = -½ 
D) n = 5, $ l $ = 4, ml = -4, ms = + ½ 
E) n = 6, $ l $ = 3, ml = 2, ms = - ½ 
A) n = 1, $ l $ = 0, ml = -1, ms = - ½ 
B) n = 3, $ l $ = 2, ml = 2, ms = + ½ 
C) n = 3, $ l $ = 1, ml = -1, ms = -½ 
D) n = 5, $ l $ = 4, ml = -4, ms = + ½ 
E) n = 6, $ l $ = 3, ml = 2, ms = - ½

Question 17

A mercury vapor lamp can be used as an 185 nm light source.What is the energy of one photon in joules? Of one mole of photons in kilojoules?

Accepted Answer

1.07 * 10<

Question 18

Write the condensed electron configuration of Po.

Accepted Answer

The answer of Write the condensed electron configuration of Po....

Question 19

Which transition in a hydrogen atom involves the largest change in energy?

Accepted Answer

A) n1 = 2 to n2 = 3 
B) n1 = 3 to n2 = 4 
C) n1 = 1 to n2 = 3 
D) n1 = 1 to n2 = 2 
E) n1 = 9 to n2 = 10 
A) n1 = 2 to n2 = 3 
B) n1 = 3 to n2 = 4 
C) n1 = 1 to n2 = 3 
D) n1 = 1 to n2 = 2 
E) n1 = 9 to n2 = 10

Question 20

The Swift explorer that NASA launched in 2004 can detect electromagnetic bursts with frequencies up to about 3.6 * 1019 Hz.What is the wavelength of this radiation, and in what region of the spectrum does it lie?

Accepted Answer

8.3 * 10<s

Exam 3: Atomic Structure Explaining the Properties of Elements

In quantum mechanics, an atomic orbital _______.

If the electron (9.11 *10-31 kg) in the hydrogen atom is traveling at about 2.2 *106 m/s ±\pm± 5%, what is the uncertainty in the electron's position?

What is the longest wavelength of light emitted by an excited hydrogen atom when nfinal = 1?

What wavelength of light is required to cause the ejection of photoelectrons with kinetic energies of 5.0 *10-20 J from a calcium surface ( Φ\varPhiΦ = 4.60 * 10-19 J)?

Arrange the following elements in order of increasing atomic radius: 16S, 9F, 14Si, 19K, 12Mg.

Which of the following transitions emits the longest wavelength photon?

Which of the following elements has the ground-state electron configuration 1s22s22p63s23p3? 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{3} ? 1s22s22p63s23p3?

What is the minimum frequency of a photon that can eject a photoelectron from Ba metal? (The work function of barium is Φ\varPhiΦ = 4.3 *10-19 J.)

As the frequency of electromagnetic radiation decreases, which statement below is TRUE?

The emission spectra of Na and Na+ are different because _______.

Cesium has a work function of 2.1 eV.What is the kinetic energy of an electron produced when green light (540 nm) is incident on a cesium metal surface? (1 eV = 1.60 * 10-19 J.)

Which of the following statements regarding orbitals and wave functions is true?

What is the minimum energy that a photon must have to ionize a ground= state hydrogen atom to the n = 4 energy level?

Electromagnetic radiation with a frequency of 8.6* 1014 Hz incident on an unknown metal surface causes the ejection of photoelectrons with kinetic energies of 2.8 *10-19 J.What is the unknown metal?

Which statement below regarding electron affinity is FALSE?

Which set of quantum numbers below is NOT allowed?

A mercury vapor lamp can be used as an 185 nm light source.What is the energy of one photon in joules? Of one mole of photons in kilojoules?

Write the condensed electron configuration of Po.

Which transition in a hydrogen atom involves the largest change in energy?

The Swift explorer that NASA launched in 2004 can detect electromagnetic bursts with frequencies up to about 3.6 * 1019 Hz.What is the wavelength of this radiation, and in what region of the spectrum does it lie?

Matter and Energy an Atomic Perspective

Atoms, Ions, and Molecules the Building Blocks of Matter

Chemical Bonding Understanding Climate Change

Bonding Theories Explaining Molecular Geometry

Intermolecular Forces Attractions Between Particles

Stoichiometry Mass Relationships and Chemical Reactions

Aqueous Solutions Chemistry of the Hydrosphere

Thermochemistry Energy Changes in Chemical Reactions

Properties of Gases the Air We Breathe

Properties of Solutions Their Concentrations and Colligative Properties

Thermodynamics Why Chemical Reactions Happen

Chemical Kinetics Clearing the Air

Chemical Equilibrium Equal but Opposite Reaction Rates

Acid-Base Equilibria Proton Transfer in Biological Systems

Additional Aqueous Equilibria Chemistry and the Oceans

Electrochemistry the Quest for Clean Energy

The Solid State a Particulate View

Organic Chemistry Fuels, Pharmaceuticals, and Modern Materials

Biochemistry the Compounds of Life

Nuclear Chemistry the Risks and Benefits

The Main Group Elements Life and the Periodic Table

Transition Metals Biological and Medical Applications

Filters

If the electron (9.11 10^-31 kg) in the hydrogen atom is traveling at about 2.2 10⁶ m/s $\pm$ 5%, what is the uncertainty in the electron's position?

What is the longest wavelength of light emitted by an excited hydrogen atom when n_final = 1?

What wavelength of light is required to cause the ejection of photoelectrons with kinetic energies of 5.0 10^-20 J from a calcium surface ( $\varPhi$ = 4.60 10^-19 J)?

Arrange the following elements in order of increasing atomic radius: ₁₆S, ₉F, ₁₄Si, ₁₉K, ₁₂Mg.

Which of the following elements has the ground-state electron configuration $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{3} ?$

What is the minimum frequency of a photon that can eject a photoelectron from Ba metal? (The work function of barium is $\varPhi$ = 4.3 *10^-19 J.)

The emission spectra of Na and Na⁺ are different because _______.

Cesium has a work function of 2.1 eV.What is the kinetic energy of an electron produced when green light (540 nm) is incident on a cesium metal surface? (1 eV = 1.60 * 10^-19 J.)

Electromagnetic radiation with a frequency of 8.6* 10¹⁴ Hz incident on an unknown metal surface causes the ejection of photoelectrons with kinetic energies of 2.8 *10^-19J.What is the unknown metal?

The Swift explorer that NASA launched in 2004 can detect electromagnetic bursts with frequencies up to about 3.6 * 10¹⁹ Hz.What is the wavelength of this radiation, and in what region of the spectrum does it lie?