Question 1

Calculate the wavelength (in nm)of the light emitted by a neon sign with a frequency of 4.60 × 10¹⁴ Hz. A) 651 nm B) 1254 nm C) 730 nm D) 339 nm E) 440 nm

Accepted Answer

The wavelength can be calculated using the formula: wavelength = speed of light / frequency. The speed of light is approximately 3.00 × 10^8 m/s. Converting the frequency to wavelength: (3.00 × 10^8 m/s) / (4.60 × 10^14 Hz) = 6.52 × 10^-7 m, which is 652 nm. The closest option is 651 nm.

Question 2

How many orbitals are contained in the n = 2 level? Give thel and m_l values of each of them.

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Question 3

Give an example of a d orbital.

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Question 4

Each of the following sets of quantum numbers is supposed to specify an orbital.Choose the one set of quantum numbers that does NOT contain an error. A) n = 4, l = 4, m_l =0 B) n = 3, l = 2, m_l =-3 C) n = 4, l = 0, m_l =+1 D) n = 3, l = 1, m_l = -2 E) n = 5, l = 3, m_l =-3

Accepted Answer

The quantum numbers must satisfy the conditions: 0 ≤ l < n and -l ≤ m_l ≤ l. Option E satisfies these conditions: for n=5, l can be 0, 1, 2, or 3, and m_l can range from -3 to +3.

Question 5

For hydrogen,what is the wavelength of the photon emitted when an electron drops from a 4d orbital to a 2s orbital in a hydrogen atom? The Rydberg constant is 1.097 × 10^-2 nm^-1. A) 656.3 nm B) 486.2 nm C) 364.6 nm D) 2.057 × 10^-3 nm

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Question 6

In which orbital would an electron (on average)be closest to the nucleus?
A) 3p
B) 6f
C) 3s
D) 3d
E) 6d

Accepted Answer

The 3s orbital has the lowest energy and therefore the electron would be closest to the nucleus on average. The other options are higher energy orbitals and the electron would be farther away on average.

Question 7

Each of the following sets of quantum numbers is supposed to specify an orbital.Choose the one set of quantum numbers that does NOT contain an error. A) n = 2, l = 2, m_l =+1 B) n = 2, l = -1, m_l =0 C) n = 3, l = 2, m_l =+3 D) n = 4, l = 3, m_l =-2 E) n = 4, l = 2, m_l =+4

Accepted Answer

The quantum numbers must satisfy the conditions: 0 ≤ l < n and -l ≤ m_l ≤ +l. Option D satisfies these conditions: n = 4, l = 3, and m_l = -2.

Question 8

Define diffraction.

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Question 9

Why do atoms only emit certain wavelengths of light when they are excited?
 (Why do line spectra exist?)

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Question 10

What is the photoelectric effect?

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Question 11

Why don't we observe the wavelength of everyday macroscopic objects?

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Question 12

Calculate the frequency of the light emitted a photon with a wavelength of 120 nm. A) 1.03 × 10¹⁵s^-1 B) 2.50 × 10¹⁵s^-1 C) 5.38 × 10¹⁵s^-1 D) 2.36 × 10¹⁵s^-1 E) 7.42 × 10¹⁵s^-1

Accepted Answer

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Question 13

Describe how a neon light works.

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Question 14

Define constructive interference.

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Question 15

Choose the one set of quantum numbers that contains an error. A) n = 6, l = 3, m_l=+2 B) n = 3, l = 2, m_l =0 C) n = 4, l = 0, m_l = -3 D) n = 5, l = 4, m_l = -2 E) n = 3, l =1, m_l =-1

Accepted Answer

The value of m can range from -l to +l, but in choice C, the value of m is -3, which is outside the permissible range for l = 0.

Question 16

How many different values of m_l are possible in the 6f sublevel? A) 1 B) 7 C) 4 D) 6 E) 2

Accepted Answer

The magnetic quantum number $ m_l $ can take values from $-l$ to $+l$, where $ l $ is the azimuthal quantum number. For an f sublevel, $ l = 3 $, so $ m_l $ can be $-3, -2, -1, 0, 1, 2, 3$, giving 7 possible values.

Question 17

Give an example of a p orbital.

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Question 18

Choose the transition (in a hydrogen atom)below that represents the emission of the shortest wavelength photon.
A) n = 4 to n = 3
B) n = 1 to n = 2
C) n = 3 to n = 7
D) n = 8 to n = 12
E) n = 3 to n = 1

Accepted Answer

The shortest wavelength corresponds to the highest energy transition, which is from n = 3 to n = 1.

Question 19

For a hydrogen atom,which electronic transition would result in the emission of a photon with the highest energy?
A) 1s → 2p
B) 3p → 7d
C) 3p → 1s
D) 6f → 4d

Accepted Answer

The energy of the emitted photon is given by the difference in energy between the initial and final electronic states. The level of energy in a hydrogen atom follows the equation E = -13.6 eV/n^2, where n is the principal quantum number. Therefore, the transition from a higher energy level to a lower energy level will result in the emission of a photon with a higher energy. In option C, the electron transitions from the third energy level to the first energy level, resulting in the emission of a photon with the highest energy.

Question 20

Consider a 3p orbital.How is it different from a 2p orbital?

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Quiz 3: The Quantum Mechanical Model of the Atom

Calculate the wavelength (in nm) of the light emitted by a neon sign with a frequency of 4.60 × 10¹⁴ Hz.

How many orbitals are contained in the n = 2 level? Give thel and m_l values of each of them.

Give an example of a d orbital.

Each of the following sets of quantum numbers is supposed to specify an orbital.Choose the one set of quantum numbers that does NOT contain an error.

For hydrogen,what is the wavelength of the photon emitted when an electron drops from a 4d orbital to a 2s orbital in a hydrogen atom? The Rydberg constant is 1.097 × 10^-2 nm^-1.

In which orbital would an electron (on average) be closest to the nucleus?

Each of the following sets of quantum numbers is supposed to specify an orbital.Choose the one set of quantum numbers that does NOT contain an error.

Define diffraction.

Why do atoms only emit certain wavelengths of light when they are excited? (Why do line spectra exist?)

What is the photoelectric effect?

Why don't we observe the wavelength of everyday macroscopic objects?

Calculate the frequency of the light emitted a photon with a wavelength of 120 nm.

Describe how a neon light works.

Define constructive interference.

Choose the one set of quantum numbers that contains an error.

How many different values of m_l are possible in the 6f sublevel?

Give an example of a p orbital.

Choose the transition (in a hydrogen atom) below that represents the emission of the shortest wavelength photon.

For a hydrogen atom,which electronic transition would result in the emission of a photon with the highest energy?

Consider a 3p orbital.How is it different from a 2p orbital?

Quiz 3: The Quantum Mechanical Model of the Atom

Calculate the wavelength (in nm) of the light emitted by a neon sign with a frequency of 4.60 × 1014 Hz.

How many orbitals are contained in the n = 2 level? Give the l and ml values of each of them.

Give an example of a d orbital.

Each of the following sets of quantum numbers is supposed to specify an orbital.Choose the one set of quantum numbers that does NOT contain an error.

For hydrogen,what is the wavelength of the photon emitted when an electron drops from a 4d orbital to a 2s orbital in a hydrogen atom? The Rydberg constant is 1.097 × 10-2 nm-1.

In which orbital would an electron (on average) be closest to the nucleus?

Each of the following sets of quantum numbers is supposed to specify an orbital.Choose the one set of quantum numbers that does NOT contain an error.

Define diffraction.

Why do atoms only emit certain wavelengths of light when they are excited? (Why do line spectra exist?)

What is the photoelectric effect?

Why don't we observe the wavelength of everyday macroscopic objects?

Calculate the frequency of the light emitted a photon with a wavelength of 120 nm.

Describe how a neon light works.

Define constructive interference.

Choose the one set of quantum numbers that contains an error.

How many different values of ml are possible in the 6f sublevel?

Give an example of a p orbital.

Choose the transition (in a hydrogen atom) below that represents the emission of the shortest wavelength photon.

For a hydrogen atom,which electronic transition would result in the emission of a photon with the highest energy?

Consider a 3p orbital.How is it different from a 2p orbital?

Calculate the wavelength (in nm) of the light emitted by a neon sign with a frequency of 4.60 × 10¹⁴ Hz.

How many orbitals are contained in the n = 2 level? Give thel and m_l values of each of them.

For hydrogen,what is the wavelength of the photon emitted when an electron drops from a 4d orbital to a 2s orbital in a hydrogen atom? The Rydberg constant is 1.097 × 10^-2 nm^-1.

How many different values of m_l are possible in the 6f sublevel?