Question 1

The FM station KDUL broadcasts music at 99.1 MHz.Find the wavelength of these waves.(c = 3.00 × 108 m/s)

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

Select the correct electron configuration for sulfur (Z = 16).

Accepted Answer

A) 1s21p62s22p6 
B) 1s22s22p83s23p4 
C) 1s22s22p83s23p2 
D) 1s22s22p63s23p4 
E) 1s22s22p63s23d4 
A) 1s21p62s22p6 
B) 1s22s22p83s23p4 
C) 1s22s22p83s23p2 
D) 1s22s22p63s23p4 
E) 1s22s22p63s23d4

Question 3

The size 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) the angular momentum and magnetic quantum numbers,together. 
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) the angular momentum and magnetic quantum numbers,together.

Question 4

What is the energy in joules of a mole of photons associated with visible light of wavelength 486 nm? (c = 3.00 × 108 m/s; h = 6.63 × 10-34 J • s; NA = 6.022 × 1023 moles-1)

Accepted Answer

A) 6.46 × 10-16 J 
B) 6.46 × 10-25 J 
C) 2.46 × 10-4 J 
D) 12.4 kJ 
E) 246 kJ 
A) 6.46 × 10-16 J 
B) 6.46 × 10-25 J 
C) 2.46 × 10-4 J 
D) 12.4 kJ 
E) 246 kJ

Question 5

a.Planck

Accepted Answer

b.A blackbody can only emit or

Question 6

How many electrons are in the 4p orbitals of selenium?

Accepted Answer

A) 0 
B) 2 
C) 4 
D) 5 
E) 6 
A) 0 
B) 2 
C) 4 
D) 5 
E) 6

Question 7

___________ is the quantum number which describes the orientation of the orbital in space.

Accepted Answer

The magnet

Question 8

If one electron is added to the outer shell of chlorine,to which element would the configuration be similar?

Accepted Answer

The answer of If one electron is added to the...

Question 9

The most stable arrangement of electrons in orbitals of equal energy is the one in which the number of electrons with the same spin is maximized is

Accepted Answer

A) the Pauli exclusion principle. 
B) Bohr's equation. 
C) Hund's rule. 
D) de Broglie's relation. 
E) Dalton's atomic theory. 
A) the Pauli exclusion principle. 
B) Bohr's equation. 
C) Hund's rule. 
D) de Broglie's relation. 
E) Dalton's atomic theory.

Question 10

An atom in its ground state contains 33 electrons.How many of these electrons are in p orbitals?

Accepted Answer

A) 15 
B) 12 
C) 3 
D) 33 
E) None of the 
A) 15 
B) 12 
C) 3 
D) 33 
E) None of the

Question 11

A radio wave has a frequency of 8.6 × 108 Hz.What is the energy of one photon of this radiation? (h = 6.63 × 10-34 J • s)

Accepted Answer

A) 7.7 × 10-43 J 
B) 2.3 × 10-34 J 
C) 5.7 × 10-25 J 
D) 1.7 × 10-16 J 
E) > 10-15 J 
A) 7.7 × 10-43 J 
B) 2.3 × 10-34 J 
C) 5.7 × 10-25 J 
D) 1.7 × 10-16 J 
E) > 10-15 J

Question 12

According to the Heisenberg uncertainty principle,if the uncertainty in the speed of an electron is 3.5 × 103 m/s,the uncertainty in its position (in m)is at least ___________.(mass of an electron = 9.11 × 10-28 g)

Accepted Answer

A) 1.7 × 10-8 m 
B) 6.6 × 10-8 m 
C) 17 m 
D) 66 m 
E) None of these choices is correct. 
A) 1.7 × 10-8 m 
B) 6.6 × 10-8 m 
C) 17 m 
D) 66 m 
E) None of these choices is correct.

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 ).(h = 6.63 × 10-34 J • s)

Accepted Answer

A) 3.08 × 1015 s-1 
B) 1.03 × 108 s-1 
C) 2.06 × 1014 s-1 
D) 1.35 × 10-51 s-1 
E) 8.22 × 1014 s-1 
A) 3.08 × 1015 s-1 
B) 1.03 × 108 s-1 
C) 2.06 × 1014 s-1 
D) 1.35 × 10-51 s-1 
E) 8.22 × 1014 s-1

Question 14

What wavelength,in nm,can strike a metal surface and eject an electron at 1.89 × 10-19 J if the binding energy of the metal is 289 kJ/mol?

Accepted Answer

A) 1.89 × 10-19 nm 
B) 2.75 nm 
C) 189 nm 
D) 290 nm 
E) 297 nm 
A) 1.89 × 10-19 nm 
B) 2.75 nm 
C) 189 nm 
D) 290 nm 
E) 297 nm

Question 15

List the following types of radiation from lowest frequency to highest frequency: microwave,X ray,ultraviolet,visible,and infrared

Accepted Answer

A) microwave < infrared < visible < ultraviolet < X ray 
B) X ray < ultraviolet < visible < infrared < microwave 
C) visible < ultraviolet < microwave < X ray < infrared 
D) infrared < X ray < microwave < ultraviolet < visible 
E) infrared < visible < microwave < ultraviolet < X ray 
A) microwave < infrared < visible < ultraviolet < X ray 
B) X ray < ultraviolet < visible < infrared < microwave 
C) visible < ultraviolet < microwave < X ray < infrared 
D) infrared < X ray < microwave < ultraviolet < visible 
E) infrared < visible < microwave < ultraviolet < X ray

Question 16

The magnetic quantum number designates the shape of the atomic orbital.

Accepted Answer

A) True 
 B)False

Question 17

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; c = 3.00 × 108 m/s)

Accepted Answer

A) 2.06 × 106 s-1 
B) 2.74 × 106 s-1 
C) 6.17 × 1014 s-1 
D) 8.23 × 1014 s-1 
E) > 1015 s-1 
A) 2.06 × 106 s-1 
B) 2.74 × 106 s-1 
C) 6.17 × 1014 s-1 
D) 8.23 × 1014 s-1 
E) > 1015 s-1

Question 18

How many electrons are there in the 2nd principal energy level (n = 2)of a phosphorus atom?

Accepted Answer

A) 3 
B) 5 
C) 6 
D) 8 
E) 10 
A) 3 
B) 5 
C) 6 
D) 8 
E) 10

Question 19

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

Accepted Answer

A) True 
 B)False

Question 20

Which of the following is a correct set of quantum numbers for an electron in a 5f orbital?

Accepted Answer

A) n = 5,l = 3,ml = +1 
B) n = 5,l = 2,ml = +3 
C) n = 4,l = 3,ml = 0 
D) n = 4,l = 2,ml = +1 
E) n = 5,l = 4,ml = 3. 
A) n = 5,l = 3,ml = +1 
B) n = 5,l = 2,ml = +3 
C) n = 4,l = 3,ml = 0 
D) n = 4,l = 2,ml = +1 
E) n = 5,l = 4,ml = 3.

Exam 6: Quantum Theory and the Electronic Structure of Atoms

The FM station KDUL broadcasts music at 99.1 MHz.Find the wavelength of these waves.(c = 3.00 × 108 m/s)

Select the correct electron configuration for sulfur (Z = 16).

The size of an atomic orbital is associated with

What is the energy in joules of a mole of photons associated with visible light of wavelength 486 nm? (c = 3.00 × 108 m/s; h = 6.63 × 10-34 J • s; NA = 6.022 × 1023 moles-1)

a.Planck

How many electrons are in the 4p orbitals of selenium?

___________ is the quantum number which describes the orientation of the orbital in space.

If one electron is added to the outer shell of chlorine,to which element would the configuration be similar?

The most stable arrangement of electrons in orbitals of equal energy is the one in which the number of electrons with the same spin is maximized is

An atom in its ground state contains 33 electrons.How many of these electrons are in p orbitals?

A radio wave has a frequency of 8.6 × 108 Hz.What is the energy of one photon of this radiation? (h = 6.63 × 10-34 J • s)

According to the Heisenberg uncertainty principle,if the uncertainty in the speed of an electron is 3.5 × 103 m/s,the uncertainty in its position (in m)is at least ___________.(mass of an electron = 9.11 × 10-28 g)

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 ).(h = 6.63 × 10-34 J • s)

What wavelength,in nm,can strike a metal surface and eject an electron at 1.89 × 10-19 J if the binding energy of the metal is 289 kJ/mol?

List the following types of radiation from lowest frequency to highest frequency: microwave,X ray,ultraviolet,visible,and infrared

The magnetic quantum number designates the shape of the atomic orbital.

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; c = 3.00 × 108 m/s)

How many electrons are there in the 2nd principal energy level (n = 2)of a phosphorus atom?

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

Which of the following is a correct set of quantum numbers for an electron in a 5f orbital?

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Electron Configuration and the Periodic Table

Chemical Bonding I Basic Concepts

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The FM station KDUL broadcasts music at 99.1 MHz.Find the wavelength of these waves.(c = 3.00 × 10⁸ m/s)

What is the energy in joules of a mole of photons associated with visible light of wavelength 486 nm? (c = 3.00 × 10⁸ m/s; h = 6.63 × 10^-34 J • s; NA = 6.0²² × 10²³ moles^-1)

A radio wave has a frequency of 8.6 × 10⁸ Hz.What is the energy of one photon of this radiation? (h = 6.63 × 10^-34 J • s)

According to the Heisenberg uncertainty principle,if the uncertainty in the speed of an electron is 3.5 × 10³ m/s,the uncertainty in its position (in m)is at least ___________.(mass of an electron = 9.11 × 10^-28 g)

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 ).(h = 6.63 × 10^-34 J • s)

What wavelength,in nm,can strike a metal surface and eject an electron at 1.89 × 10^-1⁹ J if the binding energy of the metal is 289 kJ/mol?

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; c = 3.00 × 10⁸ m/s)

How many electrons are there in the 2^nd principal energy level (n = 2)of a phosphorus atom?