Q: A laser emits light with a wavelength of $500\ \mathrm{nm}$. What is the frequency of this light? (Speed of light $c = 3.00 \times 10^8\ \mathrm{m/s}$)

$6.00 \times 10^{14}\ \mathrm{Hz}$

Q: Arrange the following types of electromagnetic radiation in order of increasing energy: infrared, ultraviolet, visible, radio.

Radio < Infrared < Visible < Ultraviolet

Q: Calculate the energy of a single photon of X-ray radiation with a wavelength of $1.00 \times 10^{-10}\ \mathrm{m}$. ($h = 6.626 \times 10^{-34}\ \mathrm{J\cdot s}$, $c = 3.00 \times 10^8\ \mathrm{m/s}$)

$1.99 \times 10^{-15}\ \mathrm{J}$

Q: Which quantum number determines the shape of an atomic orbital?

Angular momentum quantum number $l$

Q: Which of the following best explains why atomic emission spectra are discrete rather than continuous?

Electrons in atoms can only occupy specific energy levels, so only certain photon energies are emitted.

Q: A sodium street lamp emits yellow light at $589\ \mathrm{nm}$. How much energy is emitted per mole of photons at this wavelength? ($h = 6.626 \times 10^{-34}\ \mathrm{J\cdot s}$, $c = 3.00 \times 10^8\ \mathrm{m/s}$, $N_A = 6.022 \times 10^{23}\ \mathrm{mol}^{-1}$)

$2.03 \times 10^{5}\ \mathrm{J/mol}$

Q: Which set of quantum numbers is not allowed for an electron in an atom?

$n=2,\ l=2,\ m_l=0,\ m_s=+\frac{1}{2}$

Q: The work function ($\phi$) of a metal is $2.50\ \mathrm{eV}$. What is the minimum frequency of light required to eject electrons from this metal? ($1\ \mathrm{eV} = 1.602 \times 10^{-19}\ \mathrm{J}$, $h = 6.626 \times 10^{-34}\ \mathrm{J\cdot s}$)

$6.05 \times 10^{14}\ \mathrm{Hz}$

Question 1

Which of the following best describes the dual nature of electrons as discussed in the quantum-mechanical model?

Accepted Answer

Electrons exhibit both wave-like and particle-like properties depending on the experiment.

Question 2

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

Accepted Answer

$E = h 
u$

Question 3

A laser emits light with a wavelength of $500\ \mathrm{nm}$. What is the frequency of this light? (Speed of light $c = 3.00 	imes 10^8\ \mathrm{m/s}$)

Accepted Answer

$6.00 	imes 10^{14}\ \mathrm{Hz}$

Question 4

Which of the following statements about the photoelectric effect is correct?

Accepted Answer

Electrons are emitted from a metal surface only if the incident light has a frequency above a certain threshold.

Question 5

Arrange the following types of electromagnetic radiation in order of increasing energy: infrared, ultraviolet, visible, radio.

Accepted Answer

Radio < Infrared < Visible < Ultraviolet

Question 6

Calculate the energy of a single photon of X-ray radiation with a wavelength of $1.00 	imes 10^{-10}\ \mathrm{m}$. ($h = 6.626 	imes 10^{-34}\ \mathrm{J\cdot s}$, $c = 3.00 	imes 10^8\ \mathrm{m/s}$)

Accepted Answer

$1.99 	imes 10^{-15}\ \mathrm{J}$

Question 7

Which quantum number determines the shape of an atomic orbital?

Accepted Answer

Angular momentum quantum number $l$

Question 8

What is the maximum number of electrons that can occupy the $n=3$ principal energy level in an atom?

Accepted Answer

18

Question 9

Which of the following best explains why atomic emission spectra are discrete rather than continuous?

Accepted Answer

Electrons in atoms can only occupy specific energy levels, so only certain photon energies are emitted.

Question 10

A sodium street lamp emits yellow light at $589\ \mathrm{nm}$. How much energy is emitted per mole of photons at this wavelength? ($h = 6.626 	imes 10^{-34}\ \mathrm{J\cdot s}$, $c = 3.00 	imes 10^8\ \mathrm{m/s}$, $N_A = 6.022 	imes 10^{23}\ \mathrm{mol}^{-1}$)

Accepted Answer

$2.03 	imes 10^{5}\ \mathrm{J/mol}$

Question 11

Which set of quantum numbers is not allowed for an electron in an atom?

Accepted Answer

$n=2,\ l=2,\ m_l=0,\ m_s=+\frac{1}{2}$

Question 12

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

Accepted Answer

$n=3$ to $n=1$

Question 13

The work function ($\phi$) of a metal is $2.50\ \mathrm{eV}$. What is the minimum frequency of light required to eject electrons from this metal? ($1\ \mathrm{eV} = 1.602 	imes 10^{-19}\ \mathrm{J}$, $h = 6.626 	imes 10^{-34}\ \mathrm{J\cdot s}$)

Accepted Answer

$6.05 	imes 10^{14}\ \mathrm{Hz}$

Question 14

Which quantum number specifies the orientation of an orbital in space?

Accepted Answer

Magnetic quantum number $m_l$

Question 15

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

Accepted Answer

$c = \lambda 
u$

Question 16

Which of the following statements about the Bohr model of the atom is correct?

Accepted Answer

Electrons move in fixed orbits with quantized energies around the nucleus.

Question 17

A hospital uses ultraviolet light to sterilize equipment. If the UV light has a frequency of $1.00 	imes 10^{15}\ \mathrm{Hz}$, what is the energy of a single photon? ($h = 6.626 	imes 10^{-34}\ \mathrm{J\cdot s}$)

Accepted Answer

$6.63 	imes 10^{-19}\ \mathrm{J}$

Question 18

Which of the following is a correct statement about the principal quantum number $n$?

Accepted Answer

It determines the overall size and energy of an orbital.

Question 19

Which of the following best explains why X-rays are more dangerous to human tissue than visible light?

Accepted Answer

X-rays have much higher photon energies, which can ionize atoms and damage biological molecules.

Question 20

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

Accepted Answer

$n=2$ to $n=3$

The Quantum-Mechanical Model of the Atom: Study Guide

Study Guide - Practice Questions

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