Q: A sodium vapor lamp emits light at a wavelength of $$589\,\text{nm}. $$What is the frequency of this light? ($$c = 3.00 \times 10^8$\,\text{m/s})$$

$$5.09 \times 10$$^{14}$$\,\text{Hz}$$

Question 1

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

Accepted Answer

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

Question 2

Arrange the following types of electromagnetic radiation in order of increasing energy: infrared, ultraviolet, radio waves, X-rays.

Accepted Answer

Radio waves \u003c Infrared \u003c Ultraviolet \u003c X-rays

Question 3

Albert Einstein explained the photoelectric effect by proposing that:

Accepted Answer

Light consists of particles called photons, each with energy $$E = h
u$$

Question 4

Which statement best describes the difference between an emission spectrum and an absorption spectrum?

Accepted Answer

An emission spectrum results from electrons releasing energy as they fall to lower energy levels, while an absorption spectrum results from electrons absorbing energy and moving to higher energy levels.

Question 5

Calculate the wavelength (in nm) of a photon emitted when an electron in a hydrogen atom transitions from $$n=4 to$$ $$n=2. $$Use $$R_H = 1.097 	imes 10^7$\,	ext{m}^{-1}.$$

Accepted Answer

$$\approx 486\,	ext{nm}$$

Question 6

According to the Heisenberg uncertainty principle, which of the following is true?

Accepted Answer

It is impossible to know both the exact position and exact momentum of a particle simultaneously.

Question 7

Which of the following is the correct condensed (noble gas) electron configuration for calcium ($$Z=20$$)?

Accepted Answer

$$[	ext{Ar}]\,4s^2$

Question 8

How many unpaired electrons are present in the ground state of an iron ($$Z=26) $$atom?

Accepted Answer

4

Question 9

Which set of quantum numbers is NOT allowed for an electron in a 3d orbital?

Accepted Answer

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

Question 10

Which of the following statements about s, p, and d orbitals is correct?

Accepted Answer

There are three p orbitals per energy level, each with a dumbbell shape.

Question 11

A sodium vapor lamp emits light at a wavelength of $$589\,	ext{nm}. $$What is the frequency of this light? ($$c = 3.00 	imes 10^8$\,	ext{m/s})$$

Accepted Answer

$$5.09 	imes 10$$^{14}$$\,	ext{Hz}$$

Question 12

Which element has the following ground-state electron configuration: $$1s^2$$\,$$2s^2$$\,$$2p^6$$\,$$3s^2$$\,$$3p^4$$?

Accepted Answer

Sulfur

Question 13

Which quantum number determines the shape of an orbital?

Accepted Answer

Azimuthal quantum number ($$l)$$

Question 14

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

Accepted Answer

$$n=3 to$$ $$n=1$$

Question 15

Which of the following best explains why the lines in the emission spectrum of hydrogen are not continuous?

Accepted Answer

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

Question 16

Which of the following is the correct set of quantum numbers for the last electron added to a phosphorus atom ($$Z=15) in $$its ground state?

Accepted Answer

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

Question 17

Which of the following statements about the electromagnetic spectrum is FALSE?

Accepted Answer

Visible light has a higher frequency than X-rays.

Question 18

Which of the following best describes the shape of a d orbital?

Accepted Answer

Cloverleaf

Question 19

How many total orbitals are present in the $$n=3$$ principal energy level?

Accepted Answer

9

Question 20

Which of the following electron configurations is NOT possible for a neutral atom in its ground state?

Accepted Answer

$$1s^2$$\,$$2s^2$$\,$$2p^6$$\,$$3s^2$$\,$$3p^6$$\,$$4s^2$$\,$$3d^5$$

Chapter 8 Review: The Quantum-Mechanical Model of the Atom

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