Question 1

How many 2d electron states can an atom have?

Accepted Answer

A)  0 
B)  4 
C)  6 
D)  8 
E)  10 
A)  0 
B)  4 
C)  6 
D)  8 
E)  10

Question 2

In the n = 1 state, the energy of the hydrogen atom is -13.6 eV. What is its energy in the n = 2 state?

Accepted Answer

A)  -6.79 eV 
B)  -4.53 eV 
C)  -3.40 eV 
D)  -1.51 eV 
A)  -6.79 eV 
B)  -4.53 eV 
C)  -3.40 eV 
D)  -1.51 eV

Question 3

A hydrogen atom is in the 6h state. Which one of the following is not a magnetic quantum number for that state?

Accepted Answer

A)  0 
B)  1 
C)  2 
D)  4 
E)  6 
A)  0 
B)  1 
C)  2 
D)  4 
E)  6

Question 4

If n = 5, which one of the following is not an allowed magnetic quantum number m1?

Accepted Answer

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

Question 5

In a hydrogen atom, an electron with n = 7 can exist in how many different quantum states?

Accepted Answer

A)  6 
B)  7 
C)  15 
D)  98 
A)  6 
B)  7 
C)  15 
D)  98

Question 6

How many values can the magnetic quantum number have in a hydrogen atom for which the orbital angular momentum quantum number is equal to 8?

Accepted Answer

A)  9 
B)  15 
C)  5 
D)  8 
E)  17 
A)  9 
B)  15 
C)  5 
D)  8 
E)  17

Question 7

A hydrogen atom is in the 6h state. What is the principal quantum number.

Accepted Answer

A)  0 
B)  3 
C)  5 
D)  6 
E)  7 
A)  0 
B)  3 
C)  5 
D)  6 
E)  7

Question 8

What is the maximum number of electrons that can occupy the g subshell?

Accepted Answer

A)  10 
B)  14 
C)  18 
D)  22 
A)  10 
B)  14 
C)  18 
D)  22

Question 9

Neon has 10 electrons. What is the value of Z of the next higher element that has chemical properties very similar to those of neon?

Accepted Answer

A)  11 
B)  17 
C)  18 
D)  19 
E)  36 
A)  11 
B)  17 
C)  18 
D)  19 
E)  36

Question 10

The only valid electron state and shell designation among the following is

Accepted Answer

A)  1p, K (n = 1) shell. 
B)  2s, K (n = 1) shell. 
C)  1s, L (n = 2) shell. 
D)  2p, L (n = 2) shell. 
E)  3f, M (n = 3) shell. 
A)  1p, K (n = 1) shell. 
B)  2s, K (n = 1) shell. 
C)  1s, L (n = 2) shell. 
D)  2p, L (n = 2) shell. 
E)  3f, M (n = 3) shell.

Question 11

What is the longest wavelength in the Balmer series?

Accepted Answer

A)  240 nm 
B)  328 nm 
C)  365 nm 
D)  656 nm 
E)  820 nm 
A)  240 nm 
B)  328 nm 
C)  365 nm 
D)  656 nm 
E)  820 nm

Question 12

In a hydrogen atom, a given electron has ℓ = 7. How many possible values can m1 have?

Accepted Answer

A)  6 
B)  7 
C)  15 
D)  98 
A)  6 
B)  7 
C)  15 
D)  98

Question 13

How many values of the magnetic quantum number, mℓ, correspond to a value of ℓ = 4?

Accepted Answer

A)  3 
B)  5 
C)  8 
D)  9 
E)  7 
A)  3 
B)  5 
C)  8 
D)  9 
E)  7

Question 14

Which of the following statements are true for the Bohr model of the atom? (There could be more than one correct choice.)

Accepted Answer

A)  The spacing between all the electron shells is the same. 
B)  The energy difference between all the electron shells is the same. 
C)  As we look at higher and higher electron shells, they get closer and closer together, but the difference in energy between them gets greater and greater. 
D)  As we look at higher and higher electron shells, they get farther and farther apart, but the difference in energy between them gets smaller and smaller. 
E)  There is no general pattern in the spacing of the shells or their energy differences. 
A)  The spacing between all the electron shells is the same. 
B)  The energy difference between all the electron shells is the same. 
C)  As we look at higher and higher electron shells, they get closer and closer together, but the difference in energy between them gets greater and greater. 
D)  As we look at higher and higher electron shells, they get farther and farther apart, but the difference in energy between them gets smaller and smaller. 
E)  There is no general pattern in the spacing of the shells or their energy differences.

Question 15

What is the energy (in electron-volts) of the n = 3 state of atomic hydrogen?

Accepted Answer

The answer of What is the energy (in electron-volts) of...

Question 16

What is the longest wavelength in the Lyman Series?

Accepted Answer

A)  45.60 nm 
B)  91.20 nm 
C)  121.5 nm 
D)  240.1 nm 
E)  365 nm 
A)  45.60 nm 
B)  91.20 nm 
C)  121.5 nm 
D)  240.1 nm 
E)  365 nm

Question 17

The Lyman series is formed by electron transitions in hydrogen that

Accepted Answer

A)  end on the n = 1 shell. 
B)  begin on the n = 1 shell. 
C)  end on the n = 2 shell. 
D)  begin on the n = 2 shell. 
E)  are between the n = 1 and n = 3 shells. 
A)  end on the n = 1 shell. 
B)  begin on the n = 1 shell. 
C)  end on the n = 2 shell. 
D)  begin on the n = 2 shell. 
E)  are between the n = 1 and n = 3 shells.

Question 18

For the ground state of the hydrogen atom, which of the following numbers represents the correct value of the magnetic quantum number?

Accepted Answer

A)  -1 
B)  0 
C)  1 
D)  2 
E)  -2 
A)  -1 
B)  0 
C)  1 
D)  2 
E)  -2

Question 19

Given that the speed of an electron in the ground state of hydrogen is 2190 km/s, what is the speed of an electron in the n = 4 orbit of hydrogen?

Accepted Answer

A)  547 km/s 
B)  31,000 km/s 
C)  139 km/s 
D)  178 km/s 
E)  2180 km/s 
A)  547 km/s 
B)  31,000 km/s 
C)  139 km/s 
D)  178 km/s 
E)  2180 km/s

Question 20

A hydrogen atom is excited to the n = 11 level. Its decay to the n = 7 level is detected in a photographic plate. What is the wavelength of the light photographed? 
(c = 3.00 × 108 m/s, 1 eV = 1.60 × 10-19 J, h = 6.626 × 10-34 J ∙ s)

Accepted Answer

A)  7510 nm 
B)  4670 nm 
C)  12,400 nm 
D)  4380 nm 
A)  7510 nm 
B)  4670 nm 
C)  12,400 nm 
D)  4380 nm

Exam 29: Atoms and Molecules

How many 2d electron states can an atom have?

In the n = 1 state, the energy of the hydrogen atom is -13.6 eV. What is its energy in the n = 2 state?

A hydrogen atom is in the 6h state. Which one of the following is not a magnetic quantum number for that state?

If n = 5, which one of the following is not an allowed magnetic quantum number m1?

In a hydrogen atom, an electron with n = 7 can exist in how many different quantum states?

How many values can the magnetic quantum number have in a hydrogen atom for which the orbital angular momentum quantum number is equal to 8?

A hydrogen atom is in the 6h state. What is the principal quantum number.

What is the maximum number of electrons that can occupy the g subshell?

Neon has 10 electrons. What is the value of Z of the next higher element that has chemical properties very similar to those of neon?

The only valid electron state and shell designation among the following is

What is the longest wavelength in the Balmer series?

In a hydrogen atom, a given electron has ℓ = 7. How many possible values can m1 have?

How many values of the magnetic quantum number, mℓ, correspond to a value of ℓ = 4?

Which of the following statements are true for the Bohr model of the atom? (There could be more than one correct choice.)

What is the energy (in electron-volts) of the n = 3 state of atomic hydrogen?

What is the longest wavelength in the Lyman Series?

The Lyman series is formed by electron transitions in hydrogen that

For the ground state of the hydrogen atom, which of the following numbers represents the correct value of the magnetic quantum number?

Given that the speed of an electron in the ground state of hydrogen is 2190 km/s, what is the speed of an electron in the n = 4 orbit of hydrogen?

A hydrogen atom is excited to the n = 11 level. Its decay to the n = 7 level is detected in a photographic plate. What is the wavelength of the light photographed? (c = 3.00 × 108 m/s, 1 eV = 1.60 × 10-19 J, h = 6.626 × 10-34 J ∙ s)

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Filters

If n = 5, which one of the following is not an allowed magnetic quantum number m₁?

In a hydrogen atom, a given electron has ℓ = 7. How many possible values can m₁ have?

How many values of the magnetic quantum number, m_ℓ, correspond to a value of ℓ = 4?

A hydrogen atom is excited to the n = 11 level. Its decay to the n = 7 level is detected in a photographic plate. What is the wavelength of the light photographed? (c = 3.00 × 10⁸ m/s, 1 eV = 1.60 × 10^-19J, h = 6.626 × 10^-34 J ∙ s)