Question 1

The quantum numbers, n = 3, l = 1, ml = 0, ms = +1/2, represent an electron in a 3s subshell.

Accepted Answer

A) True 
 B)False

Question 2

The frequency of the emitted light from a cesium atom is an intensive property.

Accepted Answer

A) True 
 B)False

Question 3

Which one of the following sets of quantum numbers is not possible?

Accepted Answer

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

Question 4

What is the wavelength of radiation that has a frequency of 3.4 x 1011 s -1?

Accepted Answer

A) 8.8 x 10-4 nm 
B) 8.8 x 105 nm 
C) 8.8 x 10-13 nm 
D) 1.0 x 1011 nm 
E) 1.0 x 10-9 nm 
A) 8.8 x 10-4 nm 
B) 8.8 x 105 nm 
C) 8.8 x 10-13 nm 
D) 1.0 x 1011 nm 
E) 1.0 x 10-9 nm

Question 5

Calculate the wavelength of a neutron that has a velocity of 250 cm/s.(The mass of a neutron = 1.675 × 10-24 g)

Accepted Answer

A) 1.6 pm 
B) 0.016 nm 
C) 0.16 nm 
D) 160 nm 
E) 1.6 × 10-4 m 
A) 1.6 pm 
B) 0.016 nm 
C) 0.16 nm 
D) 160 nm 
E) 1.6 × 10-4 m

Question 6

In an electron microscope, electrons are accelerated to great velocities.Calculate the wavelength of an electron traveling with a velocity of 7.0 × 103 kilometers per second.The mass of an electron is 9.1 × 10-28 g.

Accepted Answer

A) 1.0 × 10-13 m 
B) 1.0 × 10-10 m 
C) 1.0 × 10-7 m 
D) 1.0 m 
A) 1.0 × 10-13 m 
B) 1.0 × 10-10 m 
C) 1.0 × 10-7 m 
D) 1.0 m

Question 7

Which ground-state atom has an electron configuration described by the following orbital diagram?

Accepted Answer

A) antimony 
B) germanium 
C) indium 
D) lead 
E) tin 
A) antimony 
B) germanium 
C) indium 
D) lead 
E) tin

Question 8

In the following diagram of a wave

Accepted Answer

A) (a)is amplitude and (b)is wavelength 
B) (a)is frequency and (b)is amplitude 
C) (a)is wavelength and (b)is frequency 
D) (a)is amplitude and (b)is frequency 
E) (a)is wavelength and (b)is amplitude 
A) (a)is amplitude and (b)is wavelength 
B) (a)is frequency and (b)is amplitude 
C) (a)is wavelength and (b)is frequency 
D) (a)is amplitude and (b)is frequency 
E) (a)is wavelength and (b)is amplitude

Question 9

When photons with a wavelength of 310.nm strike a magnesium plate, the maximum velocity of the ejected electrons is 3.45 × 105 m/s.Calculate the binding energy of electrons to the magnesium surface.

Accepted Answer

A) 32.7 kJ/mol 
B) 321 kJ/mol 
C) 353 kJ/mol 
D) 386 kJ/mol 
E) 419 kJ/mol 
A) 32.7 kJ/mol 
B) 321 kJ/mol 
C) 353 kJ/mol 
D) 386 kJ/mol 
E) 419 kJ/mol

Question 10

Write the ground state electron configuration for Cr.

Accepted Answer

[Ar] 4s¹3d⁵o

Question 11

The scattering of helium atoms by a solid can be used to gain information about the lattice of atoms, provided the wavelength of the helium atoms is comparable to the dimensions of the lattice.What is the wavelength, in picometers, of a helium-4 atom with a kinetic energy of 0.10 eV.(mass of 4He = 4.0026 amu; 1 amu = 1.67 × 10-24 g; 1 eV = 1.602 × 10-19 J. h = 6.626 × 10-34 J.s)

Accepted Answer

Question 12

What is the wavelength of radiation that has a frequency of 5.39 × 1014 s-1? (c = 2.9979 × 108 m/s)

Accepted Answer

A) 1.80 × 10-3 nm 
B) 556 nm 
C) 618 nm 
D) 6180 nm 
E) 1.61 × 1023 nm 
A) 1.80 × 10-3 nm 
B) 556 nm 
C) 618 nm 
D) 6180 nm 
E) 1.61 × 1023 nm

Question 13

Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level.Recall that for hydrogen En = -2.18 × 10 -18 J(1/n2)

Accepted Answer

A) 1.35 × 10-51 /s 
B) 1.03 × 108 /s 
C) 2.06 × 1014 /s 
D) 8.22 × 1014 /s 
E) 3.08 × 1015 /s 
A) 1.35 × 10-51 /s 
B) 1.03 × 108 /s 
C) 2.06 × 1014 /s 
D) 8.22 × 1014 /s 
E) 3.08 × 1015 /s

Question 14

Using the figure below, categorize electromagnetic radiation with an energy of 6.6 x 10-16 J/photon.

Accepted Answer

A) Gamma rays 
B) X rays 
C) Ultraviolet 
D) Infrared 
E) Microwave 
A) Gamma rays 
B) X rays 
C) Ultraviolet 
D) Infrared 
E) Microwave

Question 15

Electrons can be used to probe the arrangement of atoms on a solid surface if the wavelength of the electrons is comparable with the spacing between the atoms.Which of the following electron velocities would be appropriate for use in this application if the atoms are separated by 0.320 nm?

Accepted Answer

A) 1.24 × 103 m/s 
B) 8.06 × 103 m/s 
C) 2.27 × 106 m/s 
D) 4.41 × 106 m/s 
E) 3.00 × 108 m/s 
A) 1.24 × 103 m/s 
B) 8.06 × 103 m/s 
C) 2.27 × 106 m/s 
D) 4.41 × 106 m/s 
E) 3.00 × 108 m/s

Question 16

Which element has the following ground-state electron configuration? 1s22s22p63s2

Accepted Answer

A) Na 
B) Mg 
C) Al 
D) Si 
E) Ne 
A) Na 
B) Mg 
C) Al 
D) Si 
E) Ne

Question 17

The quantum numbers, n = 4, l = 3, ml = 2, ms = +1/2, represent an electron in a 4f subshell

Accepted Answer

A) True 
 B)False

Question 18

The electron in a hydrogen atom falls from an excited energy level to the ground state in two steps, causing the emission of photons with wavelengths of 2624 nm and 97.2 nm, respectively.What is the principal quantum number or shell of the initial excited energy level from which the electron falls?

Accepted Answer

A) 2 
B) 3 
C) 4 
D) 6 
E) 8 
A) 2 
B) 3 
C) 4 
D) 6 
E) 8

Question 19

Which one of the following sets of quantum numbers is not possible?

Accepted Answer

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

Question 20

How many unpaired electrons does an atom of sulfur have in its ground state?

Accepted Answer

A) 0 
B) 1 
C) 2 
D) 3 
E) 4 
A) 0 
B) 1 
C) 2 
D) 3 
E) 4

Exam 7: Quantum Theory and the Electronic Structure of Atoms

The quantum numbers, n = 3, l = 1, ml = 0, ms = +1/2, represent an electron in a 3s subshell.

The frequency of the emitted light from a cesium atom is an intensive property.

Which one of the following sets of quantum numbers is not possible?

What is the wavelength of radiation that has a frequency of 3.4 x 1011 s -1?

Calculate the wavelength of a neutron that has a velocity of 250 cm/s.(The mass of a neutron = 1.675 × 10-24 g)

In an electron microscope, electrons are accelerated to great velocities.Calculate the wavelength of an electron traveling with a velocity of 7.0 × 103 kilometers per second.The mass of an electron is 9.1 × 10-28 g.

Which ground-state atom has an electron configuration described by the following orbital diagram?

In the following diagram of a wave

When photons with a wavelength of 310.nm strike a magnesium plate, the maximum velocity of the ejected electrons is 3.45 × 105 m/s.Calculate the binding energy of electrons to the magnesium surface.

Write the ground state electron configuration for Cr.

What is the wavelength of radiation that has a frequency of 5.39 × 1014 s-1? (c = 2.9979 × 108 m/s)

Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level.Recall that for hydrogen En = -2.18 × 10 -18 J(1/n2)

Using the figure below, categorize electromagnetic radiation with an energy of 6.6 x 10-16 J/photon.

Electrons can be used to probe the arrangement of atoms on a solid surface if the wavelength of the electrons is comparable with the spacing between the atoms.Which of the following electron velocities would be appropriate for use in this application if the atoms are separated by 0.320 nm?

Which element has the following ground-state electron configuration? 1s22s22p63s2

The quantum numbers, n = 4, l = 3, ml = 2, ms = +1/2, represent an electron in a 4f subshell

The electron in a hydrogen atom falls from an excited energy level to the ground state in two steps, causing the emission of photons with wavelengths of 2624 nm and 97.2 nm, respectively.What is the principal quantum number or shell of the initial excited energy level from which the electron falls?

Which one of the following sets of quantum numbers is not possible?

How many unpaired electrons does an atom of sulfur have in its ground state?

Chemistry: the Study of Change

Atoms, Molecules, and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

Gases

Thermochemistry

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

Electrochemistry

Nuclear Chemistry

Chemistry in the Atmosphere

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metal Chemistry and Coordination Compounds

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

The quantum numbers, n = 3, l = 1, m_l= 0, m_s= +1/2, represent an electron in a 3s subshell.

What is the wavelength of radiation that has a frequency of 3.4 x 10¹¹ s^-1?

Calculate the wavelength of a neutron that has a velocity of 250 cm/s.(The mass of a neutron = 1.675 × 10^-24 g)

In an electron microscope, electrons are accelerated to great velocities.Calculate the wavelength of an electron traveling with a velocity of 7.0 × 10³ kilometers per second.The mass of an electron is 9.1 × 10^-28 g.

When photons with a wavelength of 310.nm strike a magnesium plate, the maximum velocity of the ejected electrons is 3.45 × 10⁵ m/s.Calculate the binding energy of electrons to the magnesium surface.

What is the wavelength of radiation that has a frequency of 5.39 × 10¹⁴ s^-1? (c = 2.9979 × 10⁸ m/s)

Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level.Recall that for hydrogen E_n = -2.18 × 10^-18 J(1/n²)

Using the figure below, categorize electromagnetic radiation with an energy of 6.6 x 10^-16 J/photon.

Which element has the following ground-state electron configuration? 1s²2s²2p⁶3s²

The quantum numbers, n = 4, l = 3, m_l= 2, m_s= +1/2, represent an electron in a 4f subshell