Q: A sodium street lamp emits yellow light with a wavelength of $589 \ \mathrm{nm}$. What is the frequency of this light? (Speed of light $c = 3.00 \times 10^8 \ \mathrm{m/s}$)

$5.09 \times 10^{14} \ \mathrm{Hz}$

Q: According to the Bohr model, what is the energy of an electron in the $n=3$ level of a hydrogen atom? (Use $E_n = -2.18 \times 10^{-18} \ \mathrm{J}/n^2$)

$-2.42 \times 10^{-19} \ \mathrm{J}$

Q: A hydrogen atom absorbs a photon and its electron moves from $n=2$ to $n=5$. What is the energy of the absorbed photon? (Use $\Delta E = 2.18 \times 10^{-18} \left( \dfrac{1}{n_i^2} - \dfrac{1}{n_f^2} \right) \ \mathrm{J}$)

$4.58 \times 10^{-19} \ \mathrm{J}$

Q: A medical imaging device uses X-rays with a wavelength of $1.00 \times 10^{-10} \ \mathrm{m}$. What is the energy of a single photon of this X-ray? ($h = 6.626 \times 10^{-34} \ \mathrm{J \cdot s}$, $c = 3.00 \times 10^8 \ \mathrm{m/s}$)

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

Question 1

Which of the following statements best describes the relationship between wavelength, frequency, and energy for electromagnetic radiation?

Accepted Answer

As wavelength decreases, frequency and energy both increase.

Question 2

A sodium street lamp emits yellow light with a wavelength of $589 \ \mathrm{nm}$. What is the frequency of this light? (Speed of light $c = 3.00 	imes 10^8 \ \mathrm{m/s}$)

Accepted Answer

$5.09 	imes 10^{14} \ \mathrm{Hz}$

Question 3

Which equation correctly expresses the energy of a photon in terms of its frequency?

Accepted Answer

$E = h 
u$

Question 4

According to the Bohr model, what is the energy of an electron in the $n=3$ level of a hydrogen atom? (Use $E_n = -2.18 	imes 10^{-18} \ \mathrm{J}/n^2$)

Accepted Answer

$-2.42 	imes 10^{-19} \ \mathrm{J}$

Question 5

Which of the following best explains why atomic emission spectra consist of discrete lines rather than a continuous spectrum?

Accepted Answer

Electrons can only occupy certain quantized energy levels, so only specific energy transitions (and thus photon energies) are possible.

Question 6

A hydrogen atom absorbs a photon and its electron moves from $n=2$ to $n=5$. What is the energy of the absorbed photon? (Use $\Delta E = 2.18 	imes 10^{-18} \left( \dfrac{1}{n_i^2} - \dfrac{1}{n_f^2} ight) \ \mathrm{J}$)

Accepted Answer

$4.58 	imes 10^{-19} \ \mathrm{J}$

Question 7

Which quantum number determines the shape of an atomic orbital?

Accepted Answer

Azimuthal quantum number ($l$)

Question 8

How many different orbitals are possible for the $n=3$ shell?

Accepted Answer

9

Question 9

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

Accepted Answer

$n=2, \ l=2, \ m_l=0, \ m_s=+1/2$

Question 10

Which statement about the Heisenberg Uncertainty Principle is correct?

Accepted Answer

It is impossible to know both the exact position and exact velocity of an electron at the same time.

Question 11

Which of the following best describes the difference between excitation and ionization of an electron in an atom?

Accepted Answer

Excitation moves the electron to a higher energy level within the atom, while ionization removes the electron from the atom.

Question 12

Which of the following is the correct expression for the de Broglie wavelength of an electron?

Accepted Answer

$\lambda = \dfrac{h}{mv}$

Question 13

A medical imaging device uses X-rays with a wavelength of $1.00 	imes 10^{-10} \ \mathrm{m}$. What is the energy of a single photon of this X-ray? ($h = 6.626 	imes 10^{-34} \ \mathrm{J \cdot s}$, $c = 3.00 	imes 10^8 \ \mathrm{m/s}$)

Accepted Answer

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

Question 14

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

Accepted Answer

Magnetic quantum number ($m_l$)

Question 15

How many electrons can occupy all the $p$ orbitals in the $n=2$ shell?

Accepted Answer

6

Question 16

Which of the following is a correct set of quantum numbers for an electron in a $3d$ orbital?

Accepted Answer

$n=3, \ l=2, \ m_l=1, \ m_s=+1/2$

Question 17

Which of the following statements about atomic orbitals is true?

Accepted Answer

An orbital is a region in space where there is a high probability of finding an electron.

Question 18

A firework emits a green color due to the emission of light from excited barium atoms. What process is responsible for the green color observed?

Accepted Answer

Electrons in barium atoms fall from higher to lower energy levels, emitting photons of specific energy.

Question 19

Which of the following best describes the principal quantum number ($n$)?

Accepted Answer

It determines the energy and relative size of an orbital.

Question 20

Which of the following is a possible value for the magnetic quantum number ($m_l$) for a $4f$ orbital?

Accepted Answer

3

Chapter 8: Electronic Structure of Atoms – Study Notes

Study Guide - Practice Questions

Study Guide - Flashcards