Q: A photon of blue light has a frequency of $$6.4 \times 10$$^{14}$$\ \text{s}^{-1}. $$What is its wavelength in meters?

$$4.7 \times 10$$^{-7}$$\ \text{m}$$

Q: What is the energy of a photon with a wavelength of $$486\ \text{nm}$$? (Use $$h = 6.63 \times 10$$^{-34}$$\ \text{J}\cdot\text{s}$$ and $$c = 3.00 \times 10^8$\ \text{m/s})$$

$$4.09 \times 10$$^{-19}$$\ \text{J}$$

Question 1

Which equation correctly relates the speed of light ($$c$$), wavelength ($$\lambda$$), and frequency ($$
u) of $$electromagnetic radiation?

Accepted Answer

$$c = \lambda 
u$$

Question 2

A photon of blue light has a frequency of $$6.4 	imes 10$$^{14}$$\ 	ext{s}^{-1}. $$What is its wavelength in meters?

Accepted Answer

$$4.7 	imes 10$$^{-7}$$\ 	ext{m}$$

Question 3

Which statement best describes the photoelectric effect?

Accepted Answer

Electrons are emitted from a metal surface when it is exposed to light of sufficient frequency.

Question 4

According to Planck, the energy of a vibrating atom is quantized and given by which equation?

Accepted Answer

$$E = nh
u$$

Question 5

What is the energy of a photon with a wavelength of $$486\ 	ext{nm}$$? (Use $$h = 6.63 	imes 10$$^{-34}$$\ 	ext{J}\cdot	ext{s}$$ and $$c = 3.00 	imes 10^8$\ 	ext{m/s})$$

Accepted Answer

$$4.09 	imes 10$$^{-19}$$\ 	ext{J}$$

Question 6

Which of the following best explains why the Bohr model was necessary to describe the hydrogen atom?

Accepted Answer

Classical physics could not explain the stability of atoms and the existence of line spectra.

Question 7

An electron in a hydrogen atom transitions from $$n=3 to$$ $$n=2. $$Which statement is true about the energy change?

Accepted Answer

Energy is emitted and $$\Delta E is $$negative.

Question 8

Which equation gives the energy of an electron in the $$nth $$energy level of a hydrogen atom according to the Bohr model?

Accepted Answer

$$E_n = -\dfrac{R_y}{n^2$}$$

Question 9

If the frequency of light is doubled, what happens to its wavelength?

Accepted Answer

The wavelength is halved.

Question 10

Which phenomenon demonstrates the wave nature of light?

Accepted Answer

Diffraction of light through a narrow slit.

Question 11

Which equation is used to calculate the energy of a photon?

Accepted Answer

$$E = h
u$$

Question 12

A hydrogen atom emits a photon as its electron transitions from $$n=4 to$$ $$n=2. $$Which region of the electromagnetic spectrum is this photon most likely to be found?

Accepted Answer

Visible

Question 13

Which quantum number determines the shape of an atomic orbital?

Accepted Answer

Azimuthal quantum number ($$l)$$

Question 14

Which statement best describes the particle-wave duality of light?

Accepted Answer

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

Question 15

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

Accepted Answer

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

Question 16

Which of the following is true about the electromagnetic spectrum?

Accepted Answer

It consists of a range of frequencies and wavelengths of electromagnetic radiation.

Question 17

Which equation would you use to calculate the frequency of light given its wavelength?

Accepted Answer

$$
u = \dfrac{c}{\lambda}$$

Question 18

Which of the following best describes the difference between emission and absorption in atomic transitions?

Accepted Answer

Emission occurs when an electron moves to a lower energy level, releasing a photon; absorption occurs when an electron moves to a higher energy level, absorbing a photon.

Question 19

Which quantum number is responsible for specifying the orientation of an orbital in space?

Accepted Answer

Magnetic quantum number ($$m_l)$$

Question 20

Which of the following statements about atomic orbitals is correct?

Accepted Answer

s orbitals are spherical, p orbitals are dumbbell-shaped, and d orbitals have more complex shapes.

Quantum-Mechanical Model of the Atom: Waves, Photons, and Atomic Structure - Chap. 8 P1

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