Question 1

Which of the following statements best describes the relationship between wavelength and frequency for electromagnetic radiation?

Accepted Answer

As wavelength increases, frequency decreases.

Question 2

A photon of light has a wavelength of $$4.00 	imes 10$$^{-7}$$ m. What is its frequency? (Speed of light c = 3.00$$ 	imes $$10^8 m/s)$$

Accepted Answer

$$1.33 	imes 10$$^{15}$$ Hz

Question 3

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

Accepted Answer

$$E = h 
u$$

Question 4

The emission spectrum of hydrogen contains several lines in the visible region. What causes these lines?

Accepted Answer

Electrons moving from higher to lower energy levels, emitting photons.

Question 5

Which series in the hydrogen emission spectrum corresponds to transitions ending at $$n=2$$?

Accepted Answer

Balmer series

Question 6

Given Planck's constant $$h = 6.626 	imes 10$$^{-34}$$ J·s and the speed of light c = 3.00$$ 	imes $$10^8 m/s$$, what is the energy of a photon with wavelength $$5.00 	imes 10$$^{-7}$$ m?

Accepted Answer

$$3.98 	imes 10$$^{-19}$$ J

Question 7

According to Bohr’s model, which equation gives the energy of an electron in the $$nth $$energy level of hydrogen?

Accepted Answer

$$E_n = -h c R_H \left( \dfrac{1}{n^2$} \right)$$

Question 8

An electron in a hydrogen atom transitions from $$n=4 to$$ $$n=2. $$Which of the following best describes the energy and wavelength of the emitted photon?

Accepted Answer

The photon has positive energy and a wavelength in the visible region.

Question 9

Which of the following best explains why fireworks display different colors?

Accepted Answer

Different metal ions emit photons of specific energies when their electrons return to lower energy levels.

Question 10

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

Accepted Answer

$$9.12 	imes 10$$^{-8}$$ m

Question 11

Which of the following transitions in the hydrogen atom would emit a photon with the highest energy?

Accepted Answer

$$n=3 to$$ $$n=1$$

Question 12

What is the frequency of light emitted when an electron in hydrogen transitions from $$n=3 to$$ $$n=2$$? ($$\Delta E = 3.03 	imes 10$$^{-19}$$ J, h = 6.626$$ 	imes $$10^{-34} J$$·s)

Accepted Answer

$$4.58 	imes 10$$^{14}$$ Hz

Question 13

Which of the following best describes quantization of energy in atoms?

Accepted Answer

Electrons can only occupy specific energy levels, not values in between.

Question 14

Which equation would you use to calculate the wavelength of light emitted when an electron transitions between two energy levels in hydrogen?

Accepted Answer

$$\lambda = \dfrac{hc}{\Delta E}$$

Question 15

Which of the following is true about the Lyman series in the hydrogen spectrum?

Accepted Answer

It involves transitions ending at $$n=1$$ and emits ultraviolet light.

Question 16

A sodium vapor lamp emits yellow light at a wavelength of $$5.89 	imes 10$$^{-7}$$ m. What is the energy of each photon emitted? (h = 6.626$$ 	imes $$10^{-34} J$$·s, $$c = 3.00 	imes 10^8$ m/s)

Accepted Answer

$$3.37 	imes 10$$^{-19}$$ J

Question 17

Which of the following best explains why the hydrogen atom emits only certain wavelengths of light?

Accepted Answer

Electrons can only transition between specific energy levels, resulting in discrete photon energies.

Question 18

If an electron in hydrogen absorbs a photon and moves from $$n=2 to$$ $$n=5$$, what happens to the energy of the electron?

Accepted Answer

The electron gains energy and moves to a higher energy level.

Question 19

Which of the following is a real-world application of atomic emission spectra?

Accepted Answer

Identifying elements in distant stars using their spectral lines.

Electrons, Energy, and Light: Quantum Mechanics and Atomic Spectra

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