Chemistry: The Molecular Nature of Matter

Neil D. Jespersen, James E. Brady, Alison Hyslop

Chapter 7 The Quantum Mechanical Atom - all with Video Answers

Educators

Chapter Questions

01:53

Problem 1

In general terms, why do we call light electromagnetic radiation?

Dr. Satish Ingale

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01:31

Problem 2

In general, what does the term frequency imply? What is meant by the term frequency of light? What symbol is used for it, and what is the SI unit (and symbol) for frequency?

Nicole Smina

Numerade Educator

00:36

Problem 3

What is meant by the term wavelength of light? What symbol is used for it?

Nicole Smina

Numerade Educator

01:14

Problem 4

Sketch a picture of a wave and label its wavelength and its amplitude. Indicate how frequency could be measured.

Nicole Smina

Numerade Educator

01:56

Problem 5

Which property of light waves is a measure of the brightness of the light? Which specifies the color of the light? Which is related to the energy of the light?

Nicole Smina

Numerade Educator

04:23

Arrange the following regions of the electromagnetic spectrum in order of increasing wavelength (i.e., shortest wavelength $\longrightarrow$ longest wavelength): microwave, TV, ultraviolet, visible, X rays, infrared, gamma rays. What are the general wavelengths associated with each region? Arrange them in terms of increasing frequency and in terms of increasing energy.

Dr. Satish Ingale

Numerade Educator

00:26

Problem 7

What wavelength range is covered by the visible spectrum?

Nicole Smina

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00:28

Problem 8

Arrange the following colors of visible light in order of increasing wavelength: orange, green, blue, yellow, violet, red.

Nicole Smina

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00:50

Problem 9

What is the equation that relates the wavelength and frequency of a light wave? (Define all symbols used.)

Nicole Smina

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00:38

Problem 10

How is the frequency of a particular type of radiation related to the energy associated with it? (Give an equation, defining all symbols.)

Nicole Smina

Numerade Educator

00:48

Problem 11

What is a photon?

Lottie Adams

Numerade Educator

02:48

Problem 12

Show that the energy of a photon is given by the equation
$$
E=\frac{h c}{\lambda}
$$

Nicole Smina

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01:18

Problem 13

Examine each of the following pairs and state which of the two has the higher energy: (a) microwaves and infrared,
(b) visible light and infrared, (c) ultraviolet light and $\mathrm{X}$ rays,
(d) visible light and ultraviolet light.

Nicole Smina

Numerade Educator

00:26

Problem 14

What is a quantum of energy?

Nicole Smina

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01:11

Problem 15

What is an atomic spectrum? How does it differ from a continuous spectrum?

Nicole Smina

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01:03

Problem 16

What fundamental fact is implied by the existence of atomic spectra?

Nicole Smina

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03:22

Problem 17

Describe Niels Bohr's model of the structure of the hydrogen atom.

Dr. Satish Ingale

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02:46

Problem 18

In qualitative terms, how did Bohr's model account for the atomic spectrum of hydrogen?

Dr. Satish Ingale

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00:56

Problem 19

Why does the equation for the energy of an electron in a Bohr atom have a negative sign?

Nicole Smina

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02:13

Problem 20

In what way was Bohr's theory a success? How was it a failure?

Dr. Satish Ingale

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02:29

Problem 21

How does the behavior of very small particles differ from that of the larger, more massive objects that we encounter in everyday life? Why don't we notice this same behavior for the larger, more massive objects?

Dr. Satish Ingale

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02:59

Problem 22

Describe the phenomenon called diffraction. How can this be used to demonstrate that de Broglie's theory was correct?

Dr. Satish Ingale

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01:30

Problem 23

What experiment could you perform to determine whether a beam was behaving as a wave or as a stream of particles?

Dr. Satish Ingale

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01:19

Problem 24

What is wave/particle duality?

Dr. Satish Ingale

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02:03

Problem 25

What is the difference between a traveling wave and a standing wave?

Dr. Satish Ingale

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01:53

Problem 26

What is the collapsing atom paradox?

Dr. Satish Ingale

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02:09

Problem 27

How does quantum mechanics resolve the collapsing atom paradox?

Dr. Satish Ingale

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01:30

Problem 28

What are the names used to refer to the theories that apply the matter-wave concept to electrons in atoms?

Dr. Satish Ingale

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01:28

Problem 29

What is the term used to describe a particular waveform of a standing wave for an electron?

Dr. Satish Ingale

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01:06

Problem 31

What are the allowed values of the principal quantum number? Of the secondary quantum numbers? Of the magnetic quantum numbers?

Nicole Smina

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01:08

Problem 32

What information does each type of quantum number give for an atomic orbital?

Nicole Smina

Numerade Educator

00:42

Problem 33

How does the value of $n$ in the Rydberg equation relate to the principle quantum number, $n$ ?

Sam Limsuwannarot

Numerade Educator

01:51

Problem 34

Why is (a) the $d$ subshell in the Period 4 designated as $3 d$ and $(\mathbf{b})$ the $f$ subshell in Period 7 designated as $5 f ?$

Dr. Satish Ingale

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01:22

Problem 35

Why does every shell contain an $s$ subshell?

Dr. Satish Ingale

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00:34

Problem 36

How many orbitals are found in (a) an s subshell,
(b) a $p$ subshell, (c) a $d$ subshell, and (d) an $f$ subshell?

Nicole Smina

Numerade Educator

00:38

Problem 37

If the value of $m_{\ell}$ for an electron in an atom is $2,$ could another electron in the same subshell have $m_{\ell}=-3$ ?

Nicole Smina

Numerade Educator

02:33

Problem 38

What physical property of electrons leads us to propose that they spin like a toy top?

Dr. Satish Ingale

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03:03

Problem 39

Explain the two magnetic properties that are affected by the number of unpaired electrons.

Dr. Satish Ingale

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01:02

Problem 40

What is the Pauli exclusion principle? What effect does it have on the populating of orbitals by electrons?

Nicole Smina

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00:16

Problem 41

What are the possible values of the spin quantum number?

Nicole Smina

Numerade Educator

00:39

Problem 42

Suppose an electron in an atom has the following set of quantum numbers: $n=2, \ell=-1, m_{\ell}=-1, m_{s}=+1 / 2$.
What set of quantum numbers is impossible for another electron in this same atom?

Nicole Smina

Numerade Educator

01:13

Problem 43

What do we mean by the term electronic structure?

Dr. Satish Ingale

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01:03

Problem 44

What is the "ground state" of an atom?

Nicole Smina

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00:58

Problem 45

Within any given shell, how do the energies of the $s, p, d$, and $f$ subshells compare? How do the energies of the orbitals belonging to a given subshell compare?

Nicole Smina

Numerade Educator

01:37

Problem 46

What fact about the energies of subshells was responsible for the apparent success of Bohr's theory about electronic structure?

Dr. Satish Ingale

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01:42

Problem 47

Give the electron configurations of the elements in Period 2 of the periodic table.

Nicole Smina

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02:15

Problem 48

Using your own words, describe how to use the periodic table to write the electron configuration of an element.

Nicole Smina

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02:21

Problem 49

Give the correct electron configurations of (a) Cr and (b) Cu. Explain why they do not have the expected electron configurations.

Nicole Smina

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00:55

Problem 50

What is the correct electron configuration of silver? Why is this electron configuration different from the expected electron configuration.

Nicole Smina

Numerade Educator

01:43

Problem 51

How are the electron configurations of the elements in a given group similar? Illustrate your answer by writing shorthand configurations for the elements in Group $6 \mathrm{~A}$.

Nicole Smina

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01:13

Problem 52

Define the terms valence shell and valence electrons. Define core electrons.

Nicole Smina

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03:29

Problem 53

Why do we use probabilities when we discuss the position of an electron in the space surrounding the nucleus of an atom?

Crystal Wang

Numerade Educator

01:12

Problem 54

Sketch the approximate shape of (a) a $1 s$ orbital and (b) a $2 p$ orbital.

Anand Jangid

Numerade Educator

00:30

Problem 55

How does the size of a given type of orbital vary with $n$ ?

Nicole Smina

Numerade Educator

00:33

Problem 56

How are the $p$ orbitals of a given $p$ subshell oriented relative to each other?

Nicole Smina

Numerade Educator

01:56

Problem 57

What is a nodal plane? How are the number of nodal planes relate to the value of $\ell$ ?

Dr. Satish Ingale

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02:12

Problem 58

What is a radial node? How are the number of radial nodes related to the value of $n$ and $\ell$ ?

Dr. Satish Ingale

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01:16

Problem 59

How many nodal planes does a $p$ orbital have? How many does a $d$ orbital have?

Dr. Satish Ingale

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02:45

Problem 60

On appropriate coordinate axes, sketch the shape of the
following $d$ orbitals: $\left(\right.$ a) $d_{x y},$ (b) $d_{x^{2}-y^{2}},$ (c) $d_{z^{2}}$.

Dr. Satish Ingale

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03:12

Problem 61

What is the meaning of effective nuclear charge? How does the effective nuclear charge felt by the outer electrons vary going down a group? How does it change as we go from left to right across a period?

Dr. Satish Ingale

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01:51

Problem 62

Explain why a $3 s$ electron in Al experiences a greater effective nuclear charge than a $3 p$ electron.
Atomic Size

Tim Blackstad

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01:09

Problem 63

Explain why the atomic size varies across the periodic table and down the periodic table.

Nicole Smina

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00:56

Problem 64

Explain why cations are smaller than their uncharged atoms and anions are larger than their uncharged atoms.

Nicole Smina

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00:55

Problem 65

In what region of the periodic table are the largest atoms found? Where are the smallest atoms found?

Nicole Smina

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02:33

Problem 66

Going from left to right in the periodic table, why are the size changes among the transition elements more gradual than those among the representative elements?

Dr. Satish Ingale

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01:33

Problem 67

Define ionization energy. Why are ionization energies of atoms and positive ions endothermic quantities?

Nicole Smina

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Problem 68

For oxygen, write an equation for the change associated with (a) its first ionization energy and (b) its third ionization energy.

Andrew Eddins

Emory University

03:06

Problem 69

Explain why ionization energy increases from left to right in a period and decreases from top to bottom in a group.

Dr. Satish Ingale

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01:05

Problem 70

Why is an atom's second ionization energy always larger than its first ionization energy?

Nicole Smina

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01:01

Problem 71

Why is the fifth ionization energy of carbon so much larger than its fourth?

Nicole Smina

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01:13

Problem 72

Why is the first ionization energy of aluminum less than the first ionization energy of magnesium?

Nicole Smina

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04:13

Problem 73

Why does phosphorus have a larger first ionization energy than sulfur?

Dr. Satish Ingale

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03:30

Problem 74

Define electron affinity. Why are electron affinities usually exothermic?

Dr. Satish Ingale

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03:02

Problem 75

For sulfur, write an equation for the change associated with
(a) its first electron affinity and
(b) its second electron affinity. How should they compare?

Dr. Satish Ingale

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02:11

Problem 76

Why does Cl have a more exothermic electron affinity than F? Why does Br have a less exothermic electron affinity than $\mathrm{Cl}$ ?

Dr. Satish Ingale

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01:35

Problem 77

Why is the second electron affinity of an atom always endothermic?

Dr. Satish Ingale

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03:26

Problem 78

How is electron affinity related to effective nuclear charge? On this basis, explain the relative magnitudes of the electron affinities of oxygen and fluorine.

Dr. Satish Ingale

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01:39

Problem 79

What is the frequency in hertz of blue light having a wavelength of $436 \mathrm{nm}$ ?

Dr. Satish Ingale

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01:39

Problem 80

Ultraviolet light with a wavelength of more than $295 \mathrm{nm}$ has little germicidal value. What is the frequency that corresponds to this wavelength?

Dr. Satish Ingale

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01:57

Problem 81

Ozone protects the earth's inhabitants from the harmful effects of ultraviolet light arriving from the sun. This shielding is a maximum for UV light having a wavelength of $295 \mathrm{nm}$. What is the frequency in hertz of this light?

Dr. Satish Ingale

Numerade Educator

03:20

Problem 82

The meter is defined as the length of the path light travels in a vacuum during the time interval of $1 / 299,792,458$ of a second. It is recommended that a helium-neon laser is used for defining the meter. The light from the laser has a wavelength of $632.99139822 \mathrm{nm}$. What is the frequency of this light, in hertz?

Dr. Satish Ingale

Numerade Educator

02:16

Problem 83

In New York City, radio station WCBS broadcasts its FM signal at a frequency of 101.1 megahertz $(\mathrm{MHz})$. What is the wavelength of this signal in meters?

Dr. Satish Ingale

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03:39

Problem 84

Sodium vapor lamps are often used in residential street lighting. Sodium gives off two yellow lines of light having frequencies of $5.09 \times 10^{14} \mathrm{~Hz}$ and $5.08 \times 10^{14} \mathrm{~Hz}$ as shown in Figure 7.7 . What are the wavelengths of light in nanometers?

Dr. Satish Ingale

Numerade Educator

02:22

Problem 85

Calculate the energy in joules of a photon of red light having a frequency of $4.0 \times 10^{14} \mathrm{~Hz}$. What is the energy of one mole of these photons?

Dr. Satish Ingale

Numerade Educator

02:01

Problem 86

Calculate the energy in joules of a photon of green light having a wavelength of $563 \mathrm{nm}$.

Dr. Satish Ingale

Numerade Educator

02:56

Problem 87

In the spectrum of hydrogen, there is a line with a wavelength of $410.3 \mathrm{nm}$. (a) What color is this line?
(b) What is its frequency? (c) What is the energy of each of its photons?

Dr. Satish Ingale

Numerade Educator

02:19

Problem 88

In the spectrum of sodium, there is a line with a wavelength of $589 \mathrm{nm}$. (a) What color is this line? (b) What is its frequency?
(c) What is the energy of each of its photons?

Dr. Satish Ingale

Numerade Educator

01:09

Problem 89

Use the Rydberg equation to calculate the wavelength in nanometers of the spectral line of hydrogen for which $n_{2}=6$ and $n_{1}=3$. (Report your answer using three significant figures.) In what region of the electromagnetic spectrum would this line be found? Would we be expected to see the light corresponding to this spectral line? Explain
your answer.

Dr. Satish Ingale

Numerade Educator

02:24

Problem 90

Use the Rydberg equation to calculate the wavelength in nanometers of the spectral line of hydrogen for which $n_{2}=5$ and $n_{1}=2$. (Report your answer using three significant figures.) In what region of the electromagnetic spectrum would this line be found? Would we be expected to see the light corresponding to this spectral line? Explain your answer.

Dr. Satish Ingale

Numerade Educator

02:35

Problem 91

Calculate the wavelength and energy in joules of the spectral line produced in the hydrogen spectrum when an electron falls from the tenth Bohr orbit to the fourth. (Report your answer using three significant figures.) $\mathrm{In}$ which region of the electromagnetic spectrum (UV, visible, or infrared) is the line?

Dr. Satish Ingale

Numerade Educator

03:15

Problem 92

Calculate the energy in joules and the wavelength in nano- meters of the spectral line produced in the hydrogen spectrum when an electron falls from the fourth Bohr orbit to the first. (Report your answer using three significant figures.) In which region of the electromagnetic spectrum (UV, visible, or infrared) is the line?

Dr. Satish Ingale

Numerade Educator

00:17

Problem 93

What is the letter code for a subshell with (a) $\ell=1$ and
(b) $\ell=3 ?$

Nicole Smina

Numerade Educator

00:24

Problem 94

What is the letter code for a subshell with (a) $\ell=2$ and
(b) $\ell=4 ?$

Nicole Smina

Numerade Educator

00:19

Problem 95

What is the value of $\ell$ for (a) an $f$ orbital and (b) a d

Nicole Smina

Numerade Educator

00:17

Problem 96

What is the value of $\ell$ for (a) a $p$ orbital and
(b) a $g$ orbital?

Nicole Smina

Numerade Educator

00:33

Problem 97

What are the values of $n$ and $\ell$ for the subshells:
(a) $3 s$
(b) $5 d ?$

Nicole Smina

Numerade Educator

00:30

Problem 98

Give the values of $n$ and $\ell$ for the subshells:
(a) $4 p$,
(b) $6 f$.

Nicole Smina

Numerade Educator

00:18

Problem 99

For the shell with $n=6$, what are the possible values of $\ell ?$

Nicole Smina

Numerade Educator

00:28

Problem 100

What values of $\ell$ are possible for a shell with $n=4 ?$

Nicole Smina

Numerade Educator

00:31

Problem 101

In a particular shell, the largest value of $\ell$ is 7 . What is the value of $n$ for this shell?

Nicole Smina

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00:34

Problem 102

What is the value of $n$ for a shell if the largest value of $\ell$ is 5 ?

Nicole Smina

Numerade Educator

00:30

Problem 103

What are the possible values of $m_{\ell}$ for a subshell with
(a) $\ell=1$ and
(b) $\ell=3 ?$

Nicole Smina

Numerade Educator

00:27

Problem 104

If the value of $\ell$ for an electron in an atom is 5 , what are the possible values of $m_{\ell}$ that this electron could have?

Nicole Smina

Numerade Educator

00:56

Problem 105

If the value of $m_{\ell}$ for an electron in an atom is $-4,$ what is the smallest value of $\ell$ that the electron could have? What is the smallest value of $n$ that the electron could have?

Nicole Smina

Numerade Educator

00:40

Problem 106

How many orbitals are there in an $h$ subshell $(\ell=5) ?$ What are the possible values of $m_{\ell} ?$

Nicole Smina

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01:28

Problem 107

Give the complete set of quantum numbers for all of the electrons that could populate the $2 p$ subshell of an atom.

Nicole Smina

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01:26

Problem 108

Give the complete set of quantum numbers for all of the electrons that could populate the $3 d$ subshell of an atom.

Nicole Smina

Numerade Educator

01:27

Problem 109

In an antimony atom, how many electrons have (a) $\ell=1$ ?
(b) $m_{\ell}=2$ ?

Dr. Satish Ingale

Numerade Educator

01:07

Problem 110

In an atom of barium, how many electrons have
(a) $\ell=0$ and $(\mathbf{b}) m_{\ell}=1 ?$

Dr. Satish Ingale

Numerade Educator

01:58

Problem 111

Give the electron configurations of (a) $S,$ (b) $K$,
(c) $\mathrm{Ti}$ and (d) Sn.
(c) $\mathrm{Ni}$

Dr. Satish Ingale

Numerade Educator

01:15

Problem 112

Write the electron configurations of (a) As, (b) Cl, and (d) $S i$.

Dr. Satish Ingale

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01:25

Problem 113

Which of the following atoms in their ground states are expected to be paramagnetic:
(a) $\mathrm{Mn}$
(b) As,
(c) S,
(d) Sr,
(e) $\mathrm{Ar}$ ?

Dr. Satish Ingale

Numerade Educator

01:37

Problem 114

Which of the following atoms in their ground states are expected to be diamagnetic:
(a) Ba,
(b) Se,
(c) $\mathrm{Zn}$
(d) Si?

Dr. Satish Ingale

Numerade Educator

00:54

Problem 115

How many unpaired electrons would be found in the ground state of (a) $\mathrm{Mg}$,
(b) $\mathrm{P}$, and $(\mathbf{c}) \mathrm{V}$ ?

Dr. Satish Ingale

Numerade Educator

01:50

Problem 116

How many unpaired electrons would be found in the ground state of (a) $\mathrm{Cs},(\mathbf{b}) \mathrm{S},$ and $(\mathbf{c}) \mathrm{Ni}$ ?

Dr. Satish Ingale

Numerade Educator

01:21

Problem 117

Write the abbreviated electron configurations for (a) Ni,
(b) $\mathrm{Cs},(\mathbf{c}) \mathrm{Ge}$
(d) $\mathrm{Br}$, and $(\mathrm{e}) \mathrm{Bi} .$

Dr. Satish Ingale

Numerade Educator

01:38

Problem 118

Write the abbreviated electron configurations for (a) Al,
(b) Se,
(c) $\mathrm{Ba}$
(d) $\mathrm{Sb},$ and $(\mathrm{e}) \mathrm{Gd}$

Dr. Satish Ingale

Numerade Educator

02:34

Problem 119

Draw complete orbital diagrams for (a) Mg and (b) Ti.

Dr. Satish Ingale

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02:46

Problem 120

Draw complete orbital diagrams for
(a) As and (b) Ni.

Dr. Satish Ingale

Numerade Educator

02:59

Problem 121

Draw orbital diagrams for the abbreviated configurations of (a) $\mathrm{Ni},(\mathbf{b}) \mathrm{Cs},(\mathbf{c}) \mathrm{Ge},$ and $(\mathbf{d}) \mathrm{Br}$

Dr. Satish Ingale

Numerade Educator

02:59

Problem 122

Draw orbital diagrams for the abbreviated configurations of $($ a $) \mathrm{Al},(\mathbf{b}) \mathrm{Se},(\mathbf{c}) \mathrm{Ba},$ and $(\mathbf{d}) \mathrm{Sb}_{-}$

Dr. Satish Ingale

Numerade Educator

00:42

Problem 123

What is the value of $n$ for the valence shells of (a) Sn,
(b) $\mathrm{K},(\mathbf{c}) \mathrm{Br},$ and $(\mathbf{d}) \mathrm{Bi}$ ?

Nicole Smina

Numerade Educator

00:37

Problem 124

What is the value of $n$ for the valence shells of (a) Al,
(b) Se,
(c) $\mathrm{Ba},$ and
(d) $\mathrm{Sb}$ ?

Nicole Smina

Numerade Educator

01:24

Problem 125

Give the configuration of the valence shell for (a) Na,
(b) $\mathrm{Al},(\mathbf{c}) \mathrm{Ge},$ and $(\mathbf{d}) \mathrm{P}$

Nicole Smina

Numerade Educator

01:12

Problem 126

Give the configuration of the valence shell for
(a) $\mathrm{Mg}$
(b) $\mathrm{Br}$
(c) $\mathrm{Ga}$, and $(\mathbf{d}) \mathrm{Pb}$.

Nicole Smina

Numerade Educator

01:18

Problem 127

Draw the orbital diagram for the valence shell of (a) Na,
(b) $\mathrm{Al},(\mathbf{c}) \mathrm{Ge},$ and $(\mathbf{d}) \mathrm{P}$

Dr. Satish Ingale

Numerade Educator

01:46

Problem 128

Draw the orbital diagram for the valence shell of (a) $\mathrm{Mg}$,
(b) $\mathrm{Br},(\mathbf{c}) \mathrm{Ga},$ and
(d) $\mathrm{Pb}$.

Dr. Satish Ingale

Numerade Educator

00:51

Problem 129

If the core electrons were $100 \%$ effective at shielding the valence electrons from the nuclear charge and the valence electrons provided no shielding for each other, what would be the effective nuclear charge felt by a valence electron in
(a) $\mathrm{Na}$
(b) $S,(\mathbf{c}) \mathrm{Cl} ?$

Dr. Satish Ingale

Numerade Educator

03:36

Problem 130

What are the three properties of orbitals in which we are most interested? Why?

Dr. Satish Ingale

Numerade Educator

01:07

Problem 130

Dr. Satish Ingale

Numerade Educator

01:10

Problem 131

Choose the larger atom in each pair: (a) $\mathrm{Mg}$ or $\mathrm{S} ;$ (b) As or Bi.

Nicole Smina

Numerade Educator

01:14

Problem 132

Choose the larger atom in each pair: (a) Al or Ar;
(b) $\mathrm{Tl}$ or In.

Dr. Satish Ingale

Numerade Educator

01:02

Problem 133

Place the following in order of expected increasing size: Ge, As, $\mathrm{Sn}, \mathrm{Sb}$.

Dr. Satish Ingale

Numerade Educator

00:57

Problem 134

Place the following in order of increasing size: $\mathrm{N}^{3-}, \mathrm{Mg}^{2+},$ $\mathrm{Na}^{+}, \mathrm{Ne}, \mathrm{F}^{-}, \mathrm{O}^{2-}$

Nicole Smina

Numerade Educator

00:44

Problem 135

Choose the larger particle in each pair:
(a) $\mathrm{Na}$ or $\mathrm{Na}^{+}$
(b) $\mathrm{Co}^{3+}$ or $\mathrm{Co}^{2+} ;$ (c) $\mathrm{Cl}$ or $\mathrm{Cl}^{-}$.

Nicole Smina

Numerade Educator

02:27

Problem 136

Choose the larger particle in each pair:
(a) $S$ or $S^{2-}$;
(b) $\mathrm{Al}^{3+}$ or $\mathrm{Al} ;$ (c) $\mathrm{Au}^{+}$ or $\mathrm{Au}^{3+}$.

Dr. Satish Ingale

Numerade Educator

03:30

Problem 137

Choose the atom with the larger ionization energy in each pair:
(a) $B$ or $\mathrm{N} ;$ (b) Se or $S ;$ (c) $\mathrm{Cl}$ or Ge.

Crystal Wang

Numerade Educator

03:13

Problem 138

Choose the atom with the larger ionization energy in each pair: (a) Li or Rb;
(b) Al or $\mathrm{F} ;(\mathrm{c}) \mathrm{F}$ or $\mathrm{C}$

Dr. Satish Ingale

Numerade Educator

02:06

Problem 139

Choose the atom with the more exothermic electron affinity in each pair: (a) I or Br; (b) Ga or As.

Dr. Satish Ingale

Numerade Educator

01:16

Problem 140

Choose the atom with the more exothermic electron affinity in each pair: (a) $S$ or $A s ;$ (b) $S$ i or $N$.

Dr. Satish Ingale

Numerade Educator

00:53

Problem 141

Use the periodic table to select the element in the following list for which there is the largest difference between the second and third ionization energies: $\mathrm{Na}, \mathrm{Mg}, \mathrm{Al}, \mathrm{Si}, \mathrm{P}, \mathrm{Se}, \mathrm{Cl}$.

Nicole Smina

Numerade Educator

00:50

Problem 142

Use the periodic table to select the element in the following list for which there is the largest difference between the fourth and fifth ionization energies: $\mathrm{Na}, \mathrm{Mg}, \mathrm{Al}, \mathrm{Si}, \mathrm{P}$ Se, Cl.

Nicole Smina

Numerade Educator

01:31

Problem 143

The human ear is sensitive to sound ranging from 20.0 to $2.00 \times 10^{4} \mathrm{~Hz}$. The speed of sound is $330 \mathrm{~m} / \mathrm{s}$ in air, and $1500 \mathrm{~m} / \mathrm{s}$ under water. What is the longest and the shortest wavelength that can be heard (a) in air and (b) under water?

Crystal Wang

Numerade Educator

01:31

Problem 144

Microwaves are used to heat food in microwave ovens.
The microwave radiation is absorbed by moisture in the food. This heats the water, and as the water becomes hot, so does the food. How many photons having a wavelength of $3.00 \mathrm{~mm}$ would have to be absorbed by $1.00 \mathrm{~g}$ of water to raise its temperature by $1.00^{\circ} \mathrm{C} ?$

Crystal Wang

Numerade Educator

01:16

Problem 145

In the spectrum of hydrogen, there is a line with a wavelength of $410.3 \mathrm{nm}$. Use the Rydberg equation to calculate the value of $n$ for the higher energy Bohr orbit involved in the emission of this light. Assume the value of $n$ for the lower energy orbit equals 2 .

Crystal Wang

Numerade Educator

02:35

Problem 146

Calculate the wavelength in nanometers of the shortest wavelength of light emitted by a hydrogen atom. In what region of the electromagnetic spectrum is this light?

Dr. Satish Ingale

Numerade Educator

01:44

Problem 147

Which of the following electronic transitions could lead to the emission of light from an atom? $1 s \longrightarrow 4 p \longrightarrow 3 d \longrightarrow 5 f \longrightarrow 4 d \longrightarrow 2 p$

Dr. Satish Ingale

Numerade Educator

09:02

Problem 148

Calculate the wavelength of an electron moving at
(a) the speed of light, (b) one-tenth the speed of light, and
(c) $3 \times 10^{3} \mathrm{~m} / \mathrm{s}$. Calculate the wavelength of a baseball weighing $145 \mathrm{~g}$ traveling at
(d) $85 \mathrm{mi} / \mathrm{hr}$ and $(\mathrm{e})$ onetenth the speed of light.

Shalini Tyagi

Numerade Educator

01:10

Problem 149

What, if anything, is wrong with the following electron configurations for atoms in their ground
states? (a) $1 s^{2} 2 s^{1} 2 p^{3},$ (b) $[\mathrm{Kr}] 3 d^{7} 4 s^{2},$ (c) $1 s^{2} 2 s^{2} 2 p^{4}$,
(d) $[\mathrm{Xe}] 4 f^{14} 5 d^{8} 6 s^{1}$

Nicole Smina

Numerade Educator

01:31

Problem 150

Suppose students gave the following orbital diagrams for the $2 s$ and $2 p$ subshell in the ground state of an atom. What, if anything, is wrong with them? Are any of these electron distributions impossible?
(a) $\begin{array}{lll}\text { (a) } & \text { (11) (11) } & \text { (b) (1) (1) }\end{array}$
(c) (1) (1) (1)
(d) (11) (1) (1)

Crystal Wang

Numerade Educator

00:20

Problem 151

How many electrons are in $p$ orbitals in an atom of gallium?

Nicole Smina

Numerade Educator

01:01

Problem 152

What are the quantum numbers of the electrons that are lost by an atom of cobalt when it forms the ion $\mathrm{Co}^{2+}$ ?

Nicole Smina

Numerade Educator

01:55

Problem 153

The removal of an electron from the hydrogen atom corresponds to raising the electron to the Bohr orbit that has $n=\infty$. On the basis of this statement, calculate the ionization energy of hydrogen in units of (a) joules per atom and (b) kilojoules per mole. Compare this number to the value given in Table 7.2 .

David Collins

Numerade Educator

02:30

Problem 154

Use orbital diagrams to illustrate what happens when an oxygen atom gains two electrons. On the basis of what you have learned about electron affinities and electron configurations, why is it extremely difficult to place a third electron on the oxygen atom?

Crystal Wang

Numerade Educator

03:10

Problem 155

From the data available in this chapter, determine the ionization energy of (a) $\mathrm{F}^{-},$ (b) $\mathrm{O}^{-},$ and
(c) $\mathrm{O}^{2-} \cdot$ Are any of these energies exothermic?

Dr. Satish Ingale

Numerade Educator

03:48

Problem 156

For an oxygen atom, which requires more energy, the addition of two electrons or the removal of one electron?

Dr. Satish Ingale

Numerade Educator

01:21

Problem 157

Write out the orbital diagram of $N$ in the ground state. Without adding any more orbitals, write out all the different excited state electron configurations that can be written for $\mathrm{N}$.

Nicole Smina

Numerade Educator

01:10

Problem 158

The ions $\mathrm{He}^{+}$ and $\mathrm{Li}^{2+}$ have line spectra that can be calculated using a modified Bohr equation. The difference is that the nuclear charge, $Z$, must be incorporated into the equation
$$
\frac{1}{\lambda}=\frac{b}{h c}\left(\frac{Z^{2}}{n_{\text {low }}^{2}}-\frac{Z^{2}}{n_{\text {high }}^{2}}\right)
$$
What would be the wavelengths of light emitted for an electron dropping from $n=5$ to $n=1$ for $\mathrm{Li}^{2+}$ and $\mathrm{He}^{+}$ and $\mathrm{H}$ ? What are the corresponding energies?

Morgan Sizemore

Numerade Educator

03:00

Problem 159

A neon sign is a gas discharge tube in which electrons traveling from the cathode to the anode collide with neon atoms in the tube and knock electrons off of them. As electrons return to the neon ions and drop to lower energy levels, light is given off. How fast would an electron have to be moving to eject an electron from an atom of neon, which has a first ionization energy equal to $2080 \mathrm{~kJ} \mathrm{~mol}^{-1}$ ?

Dr. Satish Ingale

Numerade Educator

01:29

Problem 160

How many grams of water could have its temperature raised by $5.0^{\circ} \mathrm{C}$ by a mole of photons that have a wavelength of (a) $600 \mathrm{nm}$ and
(b) $300 \mathrm{nm}$ ?

Crystal Wang

Numerade Educator

02:15

Problem 161

It has been found that when the chemical bond between chlorine atoms in $\mathrm{Cl}_{2}$ is formed, $328 \mathrm{~kJ}$ is released per mole of $\mathrm{Cl}_{2}$ formed. What is the wavelength of light that would be required to break chemical bonds between chlorine atoms?

Dr. Satish Ingale

Numerade Educator

01:37

Problem 162

Using the ionization energy for sodium, would a photon with a wavelength of $23.7 \mathrm{nm}$ be able to transfer enough energy to an electron in a sodium atom to cause it to ionize if all of the energy of the photon is transferred to the $3 s^{1}$ electron of sodium? What is the maximum kinetic energy of the ejected electron?

Crystal Wang

Numerade Educator

03:22

Problem 163

Using photons with a wavelength of $23.7 \mathrm{nm}$, determine the kinetic energies of all of the electrons that can be observed from a sample of boron.

Guilherme Barros

Numerade Educator

03:15

Problem 164

Our understanding of the quantum mechanical atom has been developing since the early 1900 s. Has quantum mechanics had any effect on the daily lives of people?

Crystal Wang

Numerade Educator

00:59

Problem 165

When a copper atom loses an electron to become a $\mathrm{Cu}^{+}$ ion, what are the possible quantum numbers of the electron that was lost?

Nicole Smina

Numerade Educator

00:49

Problem 166

Paired electrons cancel each other's magnetic fields. Why can't unpaired electrons have opposite spins and cancel each other's magnetic fields also?

Nicole Smina

Numerade Educator

01:33

Problem 167

Placing a small piece of an element from Group $1 \mathrm{~A}$ in water results in increasingly rapid and violently spectacular reactions as we progress from lithium down to cesium. What information in this chapter makes this behavior understandable?

Nicole Smina

Numerade Educator