Question 1

Arrange the colors green, red, and blue light in order of increasing energy per photon.

Accepted Answer

Red \u003c Green \u003c Blue

Question 2

Which equation correctly expresses the energy of a photon in terms of its wavelength $$\lambda$$?

Accepted Answer

$$E = h c / \lambda$$

Question 3

According to the photoelectric effect, what happens when light of frequency $$v$$ strikes a metal surface and $$h v is $$less than the binding energy $$\phi$$?

Accepted Answer

No electrons are ejected.

Question 4

A metal surface is irradiated with three different wavelengths: 325 nm, 455 nm, and 632 nm. Observation B shows photoelectrons with kinetic energy of 155 kJ/m. Which wavelength most likely caused this observation?

Accepted Answer

325 nm

Question 5

If a metal surface is struck with violet light, compared to yellow light, what will happen to the kinetic energy of the ejected electrons?

Accepted Answer

Electrons will be ejected, and they will have greater kinetic energy than those ejected by yellow light.

Question 6

Which statement best describes the emission spectrum of hydrogen?

Accepted Answer

It consists of four distinct lines in the visible region.

Question 7

What is the physical meaning of the binding energy $$\phi in $$the context of the photoelectric effect?

Accepted Answer

It is the minimum energy required to remove an electron from the metal surface.

Question 8

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

Accepted Answer

Each element has electrons in specific energy levels, resulting in unique transitions and photon energies.

Question 9

According to Bohr’s model, what happens when an electron in a hydrogen atom jumps from a higher energy orbit to a lower energy orbit?

Accepted Answer

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

Question 10

Which of the following is true about the relationship between wavelength and energy per photon?

Accepted Answer

Energy per photon decreases as wavelength increases.

Question 11

A student shines light of wavelength 455 nm on a metal surface and observes photoelectrons with kinetic energy of 51 kJ/m. What is the correct expression for the kinetic energy of the ejected electrons?

Accepted Answer

$$KE = h v - \phi$$

Question 12

Which of the following best describes a continuous spectrum?

Accepted Answer

A spectrum that contains all wavelengths of visible light without interruption.

Question 13

Which of the following is NOT explained by the Rutherford nuclear model of the atom?

Accepted Answer

How the atom’s structure changes when it gains or loses energy.

Question 14

Which formula would you use to calculate the frequency $$v of $$light given its wavelength $$\lambda$$?

Accepted Answer

$$v = c / \lambda$$

Question 15

Which observation corresponds to the 325-nm light in the photoelectric experiment described?

Accepted Answer

Observation B: Photoelectrons with kinetic energy of 155 kJ/m are observed.

Question 16

Which of the following is a direct consequence of the quantization of energy in Bohr’s model?

Accepted Answer

Electrons can only occupy specific orbits with fixed energies.

Question 17

Which real-world application relies on the unique emission spectra of elements?

Accepted Answer

Identifying elements in distant stars using spectroscopy.

Question 18

If the energy of a photon is $$3.0 	imes 10$$^{-19}$$ J, what is its wavelength? (Use h = 6.626$$ 	imes $$10^{-34} J$$·s and $$c = 3.00 	imes 10^8$ m/s)

Accepted Answer

$$\lambda = \dfrac{h c}{E} = \dfrac{6.626 	imes 10$$^{-34}$$ 	imes 3.00 	imes 10^8$}{3.0 	imes 10$$^{-19}$$}$$

Question 19

Which statement about the kinetic energy of photoelectrons is correct?

Accepted Answer

It increases as the frequency of incident light increases, provided $$h v \u003e \phi.$$

Quantization of Light, Photoelectric Effect, and Atomic Spectra

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