Q: According to the photoelectric effect, what happens when light of frequency $$\nu$$ greater than the threshold frequency $$\nu_0$ shines on a metal surface?

Electrons are emitted with kinetic energy $$KE = h\nu - \phi.$$

Q: A photon has a wavelength of $$250\ \mathrm{nm}. $$What is the energy of this photon in joules? ($$h = 6.626 \times 10$$^{-34}$$\ \mathrm{J\cdot s}$$, $$c = 3.00 \times 10^8$\ \mathrm{m/s})$$

$$7.95 \times 10$$^{-19}$$\ \mathrm{J}$$

Q: A certain metal has a work function ($$\phi) of$$ $$2.50 \times 10$$^{-19}$$\ \mathrm{J}. $$What is the minimum frequency of light required to eject electrons from this metal? ($$h = 6.626 \times 10$$^{-34}$$\ \mathrm{J\cdot s})$$

$$3.78 \times 10$$^{14}$$\ \mathrm{Hz}$$

Q: If the speed of light is $$3.00 \times 10^8$\ \mathrm{m/s}$$, what is the frequency of green light with a wavelength of $$520\ \mathrm{nm}$$?

$$5.77 \times 10$$^{14}$$\ \mathrm{Hz}$$

Q: A sodium street lamp emits yellow light at $$589\ \mathrm{nm}. $$What is the energy of one photon of this light? ($$h = 6.626 \times 10$$^{-34}$$\ \mathrm{J\cdot s}$$, $$c = 3.00 \times 10^8$\ \mathrm{m/s})$$

$$3.37 \times 10$$^{-19}$$\ \mathrm{J}$$

Question 1

Which of the following statements best describes the relationship between wavelength ($$\lambda) $$and frequency ($$
u) of $$electromagnetic radiation?

Accepted Answer

They are inversely proportional; as wavelength increases, frequency decreases.

Question 2

A barcode scanner emits red light with a frequency of $$4.62 	imes 10$$^{14}$$\ \mathrm{s}^{-1}. $$What is the wavelength of this light in nanometers ($$\mathrm{nm}$$)? (Speed of light $$c = 3.00 	imes 10^8$\ \mathrm{m/s})$$

Accepted Answer

$$649\ \mathrm{nm}$$

Question 3

Which of the following types of electromagnetic radiation has the highest energy per photon?

Accepted Answer

Gamma rays

Question 4

According to the photoelectric effect, what happens when light of frequency $$
u$$ greater than the threshold frequency $$
u_0$ shines on a metal surface?

Accepted Answer

Electrons are emitted with kinetic energy $$KE = h
u - \phi.$$

Question 5

A photon has a wavelength of $$250\ \mathrm{nm}. $$What is the energy of this photon in joules? ($$h = 6.626 	imes 10$$^{-34}$$\ \mathrm{J\cdot s}$$, $$c = 3.00 	imes 10^8$\ \mathrm{m/s})$$

Accepted Answer

$$7.95 	imes 10$$^{-19}$$\ \mathrm{J}$$

Question 6

Which transition in a hydrogen atom would result in the emission of the highest energy photon?

Accepted Answer

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

Question 7

Which of the following best explains why the emission spectrum of hydrogen is not continuous?

Accepted Answer

Electrons in hydrogen can only occupy certain discrete energy levels.

Question 8

A certain metal has a work function ($$\phi) of$$ $$2.50 	imes 10$$^{-19}$$\ \mathrm{J}. $$What is the minimum frequency of light required to eject electrons from this metal? ($$h = 6.626 	imes 10$$^{-34}$$\ \mathrm{J\cdot s})$$

Accepted Answer

$$3.78 	imes 10$$^{14}$$\ \mathrm{Hz}$$

Question 9

Which of the following correctly ranks the regions of the electromagnetic spectrum from lowest to highest frequency?

Accepted Answer

Radio \u003c Infrared \u003c Visible \u003c Ultraviolet \u003c Gamma rays

Question 10

A carbon-carbon bond requires $$348\ \mathrm{kJ/mol} to $$break. What is the shortest wavelength of light (in nm) that can break this bond? ($$h = 6.626 	imes 10$$^{-34}$$\ \mathrm{J\cdot s}$$, $$c = 3.00 	imes 10^8$\ \mathrm{m/s}$$, $$N_A = 6.022 	imes 10$$^{23}$$\ \mathrm{mol}^{-1})$$

Accepted Answer

Question 11

Which of the following best describes the concept of quantization of energy in the context of electromagnetic radiation?

Accepted Answer

Energy is absorbed or emitted only in discrete packets called quanta.

Question 12

If the speed of light is $$3.00 	imes 10^8$\ \mathrm{m/s}$$, what is the frequency of green light with a wavelength of $$520\ \mathrm{nm}$$?

Accepted Answer

$$5.77 	imes 10$$^{14}$$\ \mathrm{Hz}$$

Question 13

Which of the following transitions in a hydrogen atom would result in the absorption of a photon of the shortest wavelength?

Accepted Answer

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

Question 14

Which property of electromagnetic radiation is responsible for the different colors observed in visible light?

Accepted Answer

Wavelength

Question 15

Which of the following best describes the dual nature of light?

Accepted Answer

Light exhibits both wave-like and particle-like properties.

Question 16

A sodium street lamp emits yellow light at $$589\ \mathrm{nm}. $$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

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

Question 17

Which of the following is true about the ground state of the hydrogen atom?

Accepted Answer

It is the lowest energy level available to the electron.

Question 18

Which of the following best explains why each element has a unique emission spectrum?

Accepted Answer

Each element has a unique set of allowed energy levels for its electrons.

Question 19

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

Accepted Answer

$$E = h
u$$

Atomic Structure, Electromagnetic Radiation, and the Bohr Model: Study Notes

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