Q: A red laser pointer emits light with a wavelength of $650\ \mathrm{nm}$. What is the frequency of this light? (Speed of light $c = 3.00 \times 10^8\ \mathrm{m/s}$)

$4.62 \times 10^{14}\ \mathrm{Hz}$

Q: Calculate the energy of a photon with a frequency of $6.0 \times 10^{14}\ \mathrm{Hz}$. (Planck's constant $h = 6.626 \times 10^{-34}\ \mathrm{J \cdot s}$)

$3.98 \times 10^{-19}\ \mathrm{J}$

Q: A sodium street lamp emits yellow light with a wavelength of $589\ \mathrm{nm}$. What is the energy of one photon of this light? ($h = 6.626 \times 10^{-34}\ \mathrm{J \cdot s}$, $c = 3.00 \times 10^8\ \mathrm{m/s}$)

$3.38 \times 10^{-19}\ \mathrm{J}$

Question 1

A hospital uses ultraviolet (UV) light to sterilize surgical equipment. Which property of UV light makes it effective for this purpose?

Accepted Answer

UV light has a shorter wavelength and higher energy than visible light, which can break chemical bonds in microorganisms.

Question 2

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

Accepted Answer

$c = \lambda 
u$

Question 3

A red laser pointer emits light with a wavelength of $650\ \mathrm{nm}$. What is the frequency of this light? (Speed of light $c = 3.00 	imes 10^8\ \mathrm{m/s}$)

Accepted Answer

$4.62 	imes 10^{14}\ \mathrm{Hz}$

Question 4

Which of the following statements best explains the photoelectric effect?

Accepted Answer

Electrons are emitted from a metal surface only when the light's frequency is above a certain threshold, regardless of intensity.

Question 5

Calculate the energy of a photon with a frequency of $6.0 	imes 10^{14}\ \mathrm{Hz}$. (Planck's constant $h = 6.626 	imes 10^{-34}\ \mathrm{J \cdot s}$)

Accepted Answer

$3.98 	imes 10^{-19}\ \mathrm{J}$

Question 6

Which of the following sets of quantum numbers is NOT permitted for an electron in an atom?

Accepted Answer

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

Question 7

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 8

How many electrons can be accommodated in all the orbitals with $n=3$ in a neutral atom?

Accepted Answer

18

Question 9

Which of the following electron configurations represents the ground state of oxygen?

Accepted Answer

$1s^2\ 2s^2\ 2p^4$

Question 10

A sodium street lamp emits yellow light with a wavelength of $589\ \mathrm{nm}$. What is the energy of one photon of this light? ($h = 6.626 	imes 10^{-34}\ \mathrm{J \cdot s}$, $c = 3.00 	imes 10^8\ \mathrm{m/s}$)

Accepted Answer

$3.38 	imes 10^{-19}\ \mathrm{J}$

Question 11

Which quantum number determines the shape of an atomic orbital?

Accepted Answer

Angular momentum quantum number ($l$)

Question 12

Which of the following best describes Hund's Rule?

Accepted Answer

Electrons occupy all orbitals of a given subshell singly before pairing up.

Question 13

Which of the following elements has the abbreviated electron configuration $[Ne]\ 3s^2\ 3p^4$?

Accepted Answer

Sulfur

Question 14

A scientist analyzes the light emitted by a distant star and observes a unique set of spectral lines. What does this observation allow the scientist to determine?

Accepted Answer

The elements present in the star

Question 15

Which of the following statements about atomic orbitals is correct?

Accepted Answer

An s-orbital is spherical in shape.

Question 16

Which set of quantum numbers describes a 4f electron?

Accepted Answer

$n=4,\ l=3,\ m_l=2,\ m_s=+\frac{1}{2}$

Question 17

Which of the following is the correct order of filling for the first five atomic orbitals according to the Aufbau principle?

Accepted Answer

$1s,\ 2s,\ 2p,\ 3s,\ 3p$

Question 18

A transition metal ion is found to have the electron configuration $[Ar]\ 4s^0\ 3d^5$. Which ion is this most likely to be?

Accepted Answer

Mn$^{2+}$

Question 19

Which of the following statements about the relationship between wavelength, frequency, and energy of electromagnetic radiation is correct?

Accepted Answer

As wavelength increases, frequency decreases and energy decreases.

Chapter 6: Electronic Structure of Atoms – Study Notes

Study Guide - Practice Questions

Study Guide - Flashcards