Q: A photon has a wavelength of $500\ \mathrm{nm}$. What is its frequency? (Speed of light $c = 3.00 \times 10^8\ \mathrm{m/s}$)

$6.00 \times 10^{14}\ \mathrm{Hz}$

Q: If the energy difference between two levels in a hydrogen atom is $2.18 \times 10^{-18}\ \mathrm{J}$, what is the wavelength of the photon emitted during this transition? ($h = 6.626 \times 10^{-34}\ \mathrm{J \cdot s}$, $c = 3.00 \times 10^8\ \mathrm{m/s}$)

$9.11 \times 10^{-8}\ \mathrm{m}$

Q: Calculate the energy (in joules) of a photon with a frequency of $7.50 \times 10^{14}\ \mathrm{Hz}$. ($h = 6.626 \times 10^{-34}\ \mathrm{J \cdot s}$)

$4.97 \times 10^{-19}\ \mathrm{J}$

Q: A medical imaging device uses photons with a wavelength of $1.00 \times 10^{-10}\ \mathrm{m}$. What is the energy of each photon? ($h = 6.626 \times 10^{-34}\ \mathrm{J \cdot s}$, $c = 3.00 \times 10^8\ \mathrm{m/s}$)

$1.99 \times 10^{-15}\ \mathrm{J}$

Q: A laser emits light at a wavelength of $632.8\ \mathrm{nm}$. What is the energy of one photon of this light? ($h = 6.626 \times 10^{-34}\ \mathrm{J \cdot s}$, $c = 3.00 \times 10^8\ \mathrm{m/s}$)

$3.14 \times 10^{-19}\ \mathrm{J}$

Question 1

Which of the following best describes the relationship between the energy of a photon and its frequency?

Accepted Answer

$E = h 
u$

Question 2

According to the Bohr model, which transition in a hydrogen atom would emit the highest energy photon?

Accepted Answer

From $n=2$ to $n=1$

Question 3

A photon has a wavelength of $500\ \mathrm{nm}$. What is its frequency? (Speed of light $c = 3.00 	imes 10^8\ \mathrm{m/s}$)

Accepted Answer

$6.00 	imes 10^{14}\ \mathrm{Hz}$

Question 4

Which equation correctly relates the energy of a photon to its wavelength?

Accepted Answer

$E = \frac{hc}{\lambda}$

Question 5

If the energy difference between two levels in a hydrogen atom is $2.18 	imes 10^{-18}\ \mathrm{J}$, what is the wavelength of the photon emitted during this transition? ($h = 6.626 	imes 10^{-34}\ \mathrm{J \cdot s}$, $c = 3.00 	imes 10^8\ \mathrm{m/s}$)

Accepted Answer

$9.11 	imes 10^{-8}\ \mathrm{m}$

Question 6

Which of the following statements about the Bohr model of the atom is correct?

Accepted Answer

Electrons occupy quantized energy levels and only emit or absorb energy when transitioning between these levels.

Question 7

A student observes a line in the hydrogen emission spectrum at $486\ \mathrm{nm}$. Which transition does this correspond to?

Accepted Answer

$n=4$ to $n=2$

Question 8

Which of the following best explains why only certain wavelengths are observed in the emission spectrum of hydrogen?

Accepted Answer

Electrons can only occupy specific energy levels, so only certain energy transitions (and thus wavelengths) are possible.

Question 9

Calculate the energy (in joules) of a photon with a frequency of $7.50 	imes 10^{14}\ \mathrm{Hz}$. ($h = 6.626 	imes 10^{-34}\ \mathrm{J \cdot s}$)

Accepted Answer

$4.97 	imes 10^{-19}\ \mathrm{J}$

Question 10

Which of the following is a limitation of the Bohr model?

Accepted Answer

It cannot explain the spectra of atoms with more than one electron.

Question 11

A medical imaging device uses photons with a wavelength of $1.00 	imes 10^{-10}\ \mathrm{m}$. What is the energy of each photon? ($h = 6.626 	imes 10^{-34}\ \mathrm{J \cdot s}$, $c = 3.00 	imes 10^8\ \mathrm{m/s}$)

Accepted Answer

$1.99 	imes 10^{-15}\ \mathrm{J}$

Question 12

Which of the following equations is used to calculate the frequency of light given its wavelength?

Accepted Answer

$
u = \frac{c}{\lambda}$

Question 13

If an electron in a hydrogen atom moves from $n=5$ to $n=2$, what happens?

Accepted Answer

A photon is emitted with energy equal to the difference between the two energy levels.

Question 14

Which of the following best describes the Balmer series in the hydrogen spectrum?

Accepted Answer

Transitions where electrons fall to $n=2$ from higher energy levels.

Question 15

A laser emits light at a wavelength of $632.8\ \mathrm{nm}$. What is the energy of one photon of this light? ($h = 6.626 	imes 10^{-34}\ \mathrm{J \cdot s}$, $c = 3.00 	imes 10^8\ \mathrm{m/s}$)

Accepted Answer

$3.14 	imes 10^{-19}\ \mathrm{J}$

Question 16

Which of the following is true about the quantization of energy in atoms?

Accepted Answer

Electrons can only have specific, discrete energy values.

Quantum Mechanics and Electron Configuration: Atomic Orbitals and Quantum Numbers

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