Q: A sodium street lamp emits yellow light with a wavelength of $$589\ \mathrm{nm}. $$What is the frequency of this light? ($$c = 3.00 \times 10^8$\ \mathrm{m/s})$$

$$5.09 \times 10$$^{14}$$\ \mathrm{Hz}$$

Q: If the energy of a photon is $$3.0 \times 10$$^{-19}$$\ \mathrm{J}$$, what is its frequency? ($$h = 6.63 \times 10$$^{-34}$$\ \mathrm{J \cdot s})$$

$$4.5 \times 10$$^{14}$$\ \mathrm{Hz}$$

Question 1

Which of the following correctly describes the relationship between wavelength ($$\lambda$$), frequency ($$
u$$), and the speed of light ($$c$$)?

Accepted Answer

$$c = \lambda 
u$$

Question 2

A photon of red light has a wavelength of $$700\ \mathrm{nm}. $$Which of the following statements is true about its energy compared to a photon of blue light ($$450\ \mathrm{nm}$$)?

Accepted Answer

The red photon has less energy because energy is inversely proportional to wavelength.

Question 3

Which equation would you use to calculate the energy ($$E) of a $$photon given its frequency ($$
u$$)?

Accepted Answer

$$E = h 
u$$

Question 4

Which region of the electromagnetic spectrum has the highest energy photons?

Accepted Answer

Gamma rays

Question 5

What is the main reason each element has a unique emission spectrum?

Accepted Answer

Each element has a unique arrangement of electrons, leading to unique energy level differences.

Question 6

Which of the following best describes what happens when an electron in an atom absorbs energy?

Accepted Answer

The electron moves to a higher energy level (excited state).

Question 7

A sodium street lamp emits yellow light with a wavelength of $$589\ \mathrm{nm}. $$What is the frequency of this light? ($$c = 3.00 	imes 10^8$\ \mathrm{m/s})$$

Accepted Answer

$$5.09 	imes 10$$^{14}$$\ \mathrm{Hz}$$

Question 8

Which of the following electron configurations is correct for magnesium (atomic number 12)?

Accepted Answer

$$1s^2$$\ $$2s^2$$\ $$2p^6$$\ $$3s^2$$

Question 9

Which of the following best explains why ultraviolet light can cause sunburn but visible light cannot?

Accepted Answer

Ultraviolet photons have more energy than visible photons and can break chemical bonds in skin cells.

Question 10

Which of the following is true about absorption spectra?

Accepted Answer

They show dark lines where specific wavelengths are absorbed by a substance.

Question 11

If the energy of a photon is $$3.0 	imes 10$$^{-19}$$\ \mathrm{J}$$, what is its frequency? ($$h = 6.63 	imes 10$$^{-34}$$\ \mathrm{J \cdot s})$$

Accepted Answer

$$4.5 	imes 10$$^{14}$$\ \mathrm{Hz}$$

Question 12

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

Accepted Answer

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

Question 13

Which of the following best describes the difference between emission and absorption spectra?

Accepted Answer

Emission spectra show bright lines, absorption spectra show dark lines at the same wavelengths.

Question 14

Which of the following is the correct order of increasing energy for the following types of electromagnetic radiation: infrared, ultraviolet, visible?

Accepted Answer

Infrared \u003c Visible \u003c Ultraviolet

Question 15

Which of the following statements about the speed of light is correct?

Accepted Answer

The speed of light in a vacuum is constant for all wavelengths and frequencies.

Question 16

Which of the following best explains why each element emits only certain colors of light when heated?

Accepted Answer

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

Hsu Ch. 5.4 pgs 171-175, Atomic Structure, Electron Configuration, and Light: Study Notes

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