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

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

Q: A laser emits light with a frequency of $4.69 \times 10^{14}\ \mathrm{s}^{-1}$. What is the energy of one photon of this radiation? ($h = 6.626 \times 10^{-34}\ \mathrm{J\cdot s}$)

$3.11 \times 10^{-19}\ \mathrm{J}$

Q: What is the wavelength ($\lambda$) of an electron moving at $2.65 \times 10^6\ \mathrm{m/s}$? (Mass of electron $m = 9.11 \times 10^{-31}\ \mathrm{kg}$, $h = 6.626 \times 10^{-34}\ \mathrm{J\cdot s}$)

$2.74 \times 10^{-10}\ \mathrm{m}$

Question 1

Which of the following statements correctly describes the relationship between the frequency ($v$) and wavelength ($\lambda$) of electromagnetic radiation?

Accepted Answer

Frequency and wavelength are inversely proportional; as one increases, the other decreases.

Question 2

A sodium lamp emits yellow light with a wavelength of $589\ \mathrm{nm}$. What is the frequency ($v$) of this radiation? (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 relates the energy of a photon ($E$) to its frequency ($v$)?

Accepted Answer

$E = h v$

Question 4

A laser emits light with a frequency of $4.69 	imes 10^{14}\ \mathrm{s}^{-1}$. What is the energy of one photon of this radiation? ($h = 6.626 	imes 10^{-34}\ \mathrm{J\cdot s}$)

Accepted Answer

$3.11 	imes 10^{-19}\ \mathrm{J}$

Question 5

Which phenomenon provided evidence that light behaves as both a wave and a particle?

Accepted Answer

Photoelectric effect

Question 6

According to the Bohr model, what happens when an electron in a hydrogen atom transitions from $n=3$ to $n=2$?

Accepted Answer

A photon is emitted and the atom loses energy.

Question 7

Which equation is used to calculate the wavelength of light emitted during an electron transition in hydrogen according to the Rydberg formula?

Accepted Answer

$\dfrac{1}{\lambda} = R_H \left( \dfrac{1}{n_f^2} - \dfrac{1}{n_i^2} \right)$

Question 8

An electron in a hydrogen atom moves from $n=6$ to $n=2$. What is the sign of the energy change ($\Delta E$) and what does it indicate?

Accepted Answer

$\Delta E$ is negative; energy is emitted as a photon.

Question 9

Which quantum number determines the shape of an atomic orbital?

Accepted Answer

Angular momentum quantum number ($l$)

Question 10

What is the maximum number of electrons that can occupy the $n=3$ shell of an atom?

Accepted Answer

18

Question 11

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

Accepted Answer

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

Question 12

Which principle states that no two electrons in an atom can have the same set of four quantum numbers?

Accepted Answer

Pauli exclusion principle

Question 13

What is the condensed (noble-gas) electron configuration for calcium ($Z=20$)?

Accepted Answer

$[\mathrm{Ar}]\ 4s^2$

Question 14

Which of the following ions is isoelectronic with neon ($[\mathrm{Ne}]$)?

Accepted Answer

$\mathrm{Na}^+$

Question 15

Which rule states that electrons fill degenerate orbitals singly before pairing up?

Accepted Answer

Hund's rule

Question 16

What is the wavelength ($\lambda$) of an electron moving at $2.65 	imes 10^6\ \mathrm{m/s}$? (Mass of electron $m = 9.11 	imes 10^{-31}\ \mathrm{kg}$, $h = 6.626 	imes 10^{-34}\ \mathrm{J\cdot s}$)

Accepted Answer

$2.74 	imes 10^{-10}\ \mathrm{m}$

Question 17

Which orbital designation is impossible?

Accepted Answer

2d

Question 18

For the $3d$ subshell, what are the possible values of the magnetic quantum number ($m_l$)?

Accepted Answer

$-2, -1, 0, 1, 2$

Question 19

Which electron configuration represents a transition metal ion with a completely filled $d$-subshell?

Accepted Answer

$[\mathrm{Ar}]\ 3d^{10}$

Question 20

Which of the following best describes core electrons in an atom?

Accepted Answer

Electrons in inner energy levels that do not participate in bonding.

Chapter 6: Electronic Structure of Atoms – Study Notes

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