Q: A hydrogen atom transitions from $$n=4 to$$ $$n=2. $$What is the energy of the emitted photon?

$$E = 13.6\,\text{eV} \left( \frac{1}{2^2$} - \frac{1}{4^2$} \right )$$

Q: What is the value of the Rydberg constant $$R$$ used in the Balmer formula?

$$1.097 \times 10^7$\,\text{m}^{-1}$$

Question 1

Which experiment provided direct evidence for the particle nature of light, as opposed to its wave nature?

Accepted Answer

The photoelectric effect

Question 2

A digital camera sensor detects light by counting the number of photons that hit each pixel. What property of light does this illustrate?

Accepted Answer

Particle nature of light

Question 3

Which of the following best describes the difference between a continuous spectrum and a line spectrum?

Accepted Answer

A continuous spectrum contains all wavelengths, while a line spectrum contains only specific wavelengths.

Question 4

According to Bohr’s hypothesis, what is the energy of a photon emitted when an atom transitions from an initial energy level $$E_i to a $$final energy level $$E_f$$?

Accepted Answer

$$h f = E_i - E_f$$

Question 5

The Rydberg formula for the Balmer series is $$\frac{1}{\lambda} = R \left( \frac{1}{2^2$} - \frac{1}{n^2$} \right). $$What does the integer $$n$$ represent?

Accepted Answer

The principal quantum number of the higher energy level

Question 6

What is the energy (in electron volts) of the $$n=3$$ energy level in a hydrogen atom, given $$E_n = -\frac{13.6\,	ext{eV}}{n^2$}$$?

Accepted Answer

$$-1.51\,	ext{eV}$$

Question 7

A hydrogen atom transitions from $$n=4 to$$ $$n=2. $$What is the energy of the emitted photon?

Accepted Answer

$$E = 13.6\,	ext{eV} \left( \frac{1}{2^2$} - \frac{1}{4^2$} ight )$$

Question 8

Which of the following transitions in a hydrogen atom would emit a photon in the visible region of the spectrum?

Accepted Answer

From $$n=3 to$$ $$n=2$$

Question 9

If a photon with energy less than the work function of a metal strikes its surface, what will happen?

Accepted Answer

No electron will be ejected.

Question 10

A solar panel generates electricity when photons strike its surface. Which concept explains why only photons above a certain energy can generate current?

Accepted Answer

The work function of the material

Question 11

Given the energy levels $$E_1 = 0$$\,	ext{eV}$$, E_2$ = 1.00\,	ext{eV}$$, and $$E_3 = 3.00$$\,	ext{eV}$$ for a hypothetical atom, what is the energy of a photon emitted when the atom transitions from E_3$ to E_2$?

Accepted Answer

$$2.00\,	ext{eV}$$

Question 12

What is the wavelength (in nm) of the $$H_\alpha$$ line in the Balmer series of hydrogen?

Accepted Answer

$$656.3\,	ext{nm}$$

Question 13

Which of the following best describes the ground state of an atom?

Accepted Answer

The state with the lowest possible energy

Question 14

If a hydrogen atom is in the $$n=4$$ state, how much energy is required to ionize it?

Accepted Answer

$$0.85\,	ext{eV}$$

Question 15

Which of the following transitions corresponds to the absorption of a photon by a hydrogen atom?

Accepted Answer

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

Question 16

What is the value of the Rydberg constant $$R$$ used in the Balmer formula?

Accepted Answer

$$1.097 	imes 10^7$\,	ext{m}^{-1}$$

Question 17

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

Accepted Answer

Electrons in hydrogen atoms can only occupy specific energy levels.

Question 18

A photon is absorbed by an atom, causing a transition from $$E_i to$$ $$E_f. $$What is the relationship between the photon energy and the energy levels?

Accepted Answer

$$h f = E_f - E_i$$

Question 19

Which of the following is a real-world application that relies on the photoelectric effect?

Accepted Answer

Solar panels generating electricity

Chapter 28: Photons, Electrons, and Atoms – Study Notes

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