Holt: Modern Chemistry

Mickey Sarquis, Jerry L. Sarquis

Chapter 6 Chemical Bonding - all with Video Answers

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Chapter Questions

00:24

Problem 1

What is a chemical bond?

Kamryn Szot

Numerade Educator

02:07

Problem 2

Identify and define the three major types of chemical bonding.

Kamryn Szot

Numerade Educator

02:15

Problem 3

What is the relationship between electronegativity and the ionic character of a chemical bond?

Kamryn Szot

Numerade Educator

02:49

Problem 4

a. What is the meaning of the term polar, as applied to chemical bonding?
b. Distinguish between polar-covalent and nonpolar-covalent bonds.

Kamryn Szot

Numerade Educator

01:19

Problem 5

In general, what determines whether atoms will form chemical bonds?

Kaitlynn Wade

Numerade Educator

06:46

Determine the electronegativity difference, the probable bond type, and the more-electronegative atom with respect to bonds formed between the following pairs of atoms. (Hint: See Sample Problem A.)
a. $\mathrm{H}$ and $\mathrm{I}$
b. $\mathrm{S}$ and $\mathrm{O}$
c. $\mathrm{K}$ and $\mathrm{Br}$
d. $\mathrm{Si}$ and $\mathrm{Cl}$
e. $\mathrm{K}$ and $\mathrm{Cl}$
f. $\mathrm{Se}$ and $\mathrm{S}$
g.$\mathrm{C}$ and $\mathrm{H}$

Kamryn Szot

Numerade Educator

04:39

Problem 7

List the bonding pairs described in item 6 in order of increasing covalent character.

Dr. Satish Ingale

Numerade Educator

03:36

Problem 8

Use orbital notation to illustrate the bonding in each of the following molecules:
a. chlorine, $\mathrm{Cl}_{2}$
b. oxygen, $\mathrm{O}_{2}$
c. hydrogen fluoride, $\mathrm{HF}$

Rashmi Sinha

Numerade Educator

01:34

Problem 9

The lattice energy of sodium chloride, $\mathrm{NaCl}$, is $-787.5 \mathrm{kJ} / \mathrm{mol}$ . The lattice energy of potassium chloride, $\mathrm{KCl}$, is $-715 \mathrm{k} / / \mathrm{mol}$ . In which compound is the bonding between ions stronger? Why?

Kamryn Szot

Numerade Educator

00:37

Problem 10

What is a molecule?

Kamryn Szot

Numerade Educator

02:38

Problem 11

a. What determines bond length?
b. In general, how are bond energies and bond lengths related?

Kamryn Szot

Numerade Educator

01:06

Problem 12

Describe the general location of the electrons in a covalent bond.

Kaitlynn Wade

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01:52

Problem 13

As applied to covalent bonding, what is meant by an unshared or lone pair of electrons?

Kamryn Szot

Numerade Educator

01:26

Problem 14

Describe the octet rule in terms of noble-gas configurations and potential energy.

Kaitlynn Wade

Numerade Educator

05:18

Problem 15

Determine the number of valence electrons in an atom of each of the following elements:
a. $\mathrm{H}$
b. $\mathrm{F}$
c. $\mathrm{Mg}$
d. $\mathrm{0}$
e. $\mathrm{Al}$
f. $\mathrm{N}$
g. $\mathrm{C}$

Kamryn Szot

Numerade Educator

01:15

Problem 16

In a Lewis structure, which atom is usually the central atom?

Kamryn Szot

Numerade Educator

04:59

Problem 17

Distinguish between single, double, and triple covalent bonds by defining each and providing an illustration of each type.

Kamryn Szot

Numerade Educator

02:00

Problem 18

For Lewis structures, how is the need for multiple bonds generally determined?

Kamryn Szot

Numerade Educator

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Problem 19

Use electron-dot notation to illustrate the number of valence electrons present in one atom of each of the following elements. (Hint: See Sample Problem B.)
a. $\mathrm{Li} \quad$ e. $\mathrm{C}$
b. $\mathrm{Ca} \quad$ f. $\mathrm{P}$
c. $\mathrm{Cl} \quad$ g. $\mathrm{Al}$
d. $\mathrm{0} \qquad$ h. $\mathrm{S}$

Ronald Prasad

Numerade Educator

03:32

Problem 20

Use electron-dot structures to demonstrate the formation of ionic compounds involving the following elements:
a. $\mathrm{Na}$ and $\mathrm{S}$
b. $\mathrm{Ca}$ and $\mathrm{0}$
c. $\mathrm{Al}$ and $\mathrm{S}$

Dominique Jan Tan

Numerade Educator

06:06

Problem 21

Draw Lewis structures for each of the following molecules. (Hint: See Sample Problem D.)
a. contains one $\mathrm{C}$ and four $\mathrm{F}$ atoms
b. contains two$\mathrm{H}$ and one $\mathrm{Se}$ atom
c. contains one $\mathrm{N}$ and three $\mathrm{I}$ atoms
d. contains one $\mathrm{Si}$ and four $\mathrm{Br}$ atoms
e. contains one $\mathrm{C},$ one $\mathrm{C} 1,$ and three $\mathrm{H}$ atoms

Kamryn Szot

Numerade Educator

02:51

Problem 22

Determine the type of hybrid orbitals formed by the boron atom in a molecule of boron fluoride, $\mathrm{BF}_{3}$.

Susan Hallstrom

Numerade Educator

08:39

Problem 23

Draw Lewis structures for each of the following molecules. Show resonance structures, if they exist.
a. $\mathrm{O}_{2}$
b. $\mathrm{N}_{2}$
c. $\mathrm{CO}$
d. $\mathrm{SO}_{2}$

Kamryn Szot

Numerade Educator

04:52

Problem 24

Draw Lewis structures for each of the following polyatomic ions. Show resonance structures, if they exist.
a. $\mathrm{OH}^{-}$
b. $\mathrm{H}_{3} \mathrm{C}_{2} \mathrm{O}_{2}^{-}$
c. $\mathrm{BrO}_{3}^{-}$

David Collins

Numerade Educator

01:37

Problem 25

a. What is an ionic compound?
b. In what form do most ionic compounds occur?

Kamryn Szot

Numerade Educator

01:52

Problem 26

a. What is a formula unit?
b. What are the components of one formula unit of $\mathrm{CaF}_{2} ?$

Kamryn Szot

Numerade Educator

01:03

Problem 27

a. What is lattice energy?
b. In general, what is the relationship between lattice energy and the strength of ionic bonding?

Kaitlynn Wade

Numerade Educator

01:50

Problem 28

a. In general, how do ionic and molecular compounds compare in terms of melting points, boiling points, and ease of vaporization?
b. What accounts for the observed differences in the properties of ionic and molecular compounds?
c. Cite three physical properties of ionic compounds.

Kaitlynn Wade

Numerade Educator

01:28

Problem 29

a. What is a polyatomic ion?
b. Give two examples of polyatomic ions.
c. In what form do such ions often occur in nature?

David Collins

Numerade Educator

01:31

Problem 30

a. How do the properties of metals differ from those of both ionic and molecular compounds?
b. What specific property of metals accounts for their unusual electrical conductivity?

Kaitlynn Wade

Numerade Educator

01:08

Problem 31

What properties of metals contribute to their tendency to form metallic bonds?

Kaitlynn Wade

Numerade Educator

01:10

Problem 32

a. What is metallic bonding?
b. How can the strength of metallic bonding be measured?

Kaitlynn Wade

Numerade Educator

01:37

Problem 33

a. How is the VSEPR theory used to classify molecules?
b. What molecular geometry would be expected for $\mathrm{F}_{2}$ and $\mathrm{HF}$ ?

Kaitlynn Wade

Numerade Educator

01:42

Problem 34

According to the VSEPR theory, what molecular geometries are associated with the following types of molecules?
a. $\mathrm{A} \mathrm{B}_{2}$
b. $\mathrm{A} \mathrm{B}_{3}$
C. $\mathrm{A} \mathrm{B}_{4}$
d. $\mathrm{A} \mathrm{B}_{5}$
e. $\mathrm{A} \mathrm{B}_{6}$

Kaitlynn Wade

Numerade Educator

02:55

Problem 35

Describe the role of each of the following in predicting molecular geometries:
a. unshared electron pairs
b. double bonds

Kamryn Szot

Numerade Educator

00:45

Problem 36

a. What are hybrid orbitals?
b. What determines the number of hybrid orbitals produced by the hybridization of an atom?

Kaitlynn Wade

Numerade Educator

01:59

Problem 37

a. What are intermolecular forces?
b. In general, how do these forces compare in strength with those in ionic and metallic bonding?
c. What types of molecules have the strongest intermolecular forces?

Kaitlynn Wade

Numerade Educator

01:47

Problem 38

What is the relationship between electronegativity and the polarity of a chemical bond?

Kamryn Szot

Numerade Educator

02:13

Problem 39

a. What are dipole-dipole forces?
b. What determines the polarity of a molecule?

Kaitlynn Wade

Numerade Educator

01:40

Problem 40

a. What is meant by an induced dipole?
b. What is the everyday importance of this type of intermolecular force?

Rachel Vallejo

Numerade Educator

01:52

Problem 41

a. What is hydrogen bonding?
b. What accounts for its extraordinary strength?

Kaitlynn Wade

Numerade Educator

01:31

Problem 42

What are London dispersion forces?

Kaitlynn Wade

Numerade Educator

04:16

Problem 43

According to the VSEPR theory, what molecular geometries are associated with the following types of molecules?
a. $\mathrm{AB}_{3} \mathrm{E}$
b. $\mathrm{AB}_{2} \mathrm{E}_{2}$
c. $\mathrm{AB}_{2} \mathrm{E}$

Kaitlynn Wade

Numerade Educator

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Problem 44

Use hybridization to explain the bonding in methane, $\mathrm{CH}_{4}$ .

David Collins

Numerade Educator

01:41

Problem 45

For each of the following polar molecules, indicate the direction of the resulting dipole:
a. $\mathrm{AB}_{3} \mathrm{E}$
b. $\mathrm{AB}_{2} \mathrm{E}_{2}$
c. $\mathrm{AB}_{2} \mathrm{E}$
a. $\mathrm{H}-\mathrm{F}$
b. $\mathrm{H}-\mathrm{C} 1$
c. $\mathrm{H}-\mathrm{Br}$
d. $\mathrm{H}-1$

Kaitlynn Wade

Numerade Educator

02:27

Problem 46

Determine whether each of the following bonds would be polar or nonpolar:
a. $\mathrm{H}-\mathrm{H}$
b. $\mathrm{H}-\mathrm{O}$
c. $\mathrm{H}-\mathrm{F}$
d. $\mathrm{Br}-\mathrm{Br}$
e. $\mathrm{H}-\mathrm{Cl}$
f. $\mathrm{H}-\mathrm{N}$

Kaitlynn Wade

Numerade Educator

03:06

Problem 47

On the basis of individual bond polarity and orientation, determine whether each of the following molecules would be polar or nonpolar:
a. $\mathrm{H}_{2} \mathrm{O}$
b. $\mathrm{I}_{2}$
c. $\mathrm{CF}_{4}$
d. $\mathrm{NH}_{3}$
e. $\mathrm{CO}_{2}$

Kaitlynn Wade

Numerade Educator

05:04

Problem 48

Draw a Lewis structure for each of the following molecules, and then use the VSEPR theory to predict the molecular geometry of each:
a. $\mathrm{SCl}_{2}$
b. $\mathrm{PI}_{3}$
c. $\mathrm{Cl}_{2} \mathrm{O}$
d. $\mathrm{NH}_{2} \mathrm{Cl}$
e. $\mathrm{SiCl}_{3} \mathrm{Br}$
f. $\mathrm{ONCl}$

Kaitlynn Wade

Numerade Educator

04:40

Problem 49

Draw a Lewis structure for each of the following polyatomic ions, and then use VSEPR theory to determine the geometry of each:
a. $\mathrm{NO}_{3}^{-}$
b. $\mathrm{NH}_{4}^{+}$
c. $\mathrm{SO}_{4}^{2-}$
d. $\mathrm{ClO}_{2}^{-}$

Kaitlynn Wade

Numerade Educator

01:15

Problem 50

Arrange the following pairs from strongest to weakest attraction:
a. polar molecule and polar molecule
b. nonpolar molecule and nonpolar molecule
c. polar molecule and ion
d. ion and ion

Alexander Cheng

Numerade Educator

01:55

Problem 51

Determine the geometry of the following molecules:
a. $\mathrm{CCl}_{4}$
b. $\mathrm{BeCl}_{2}$
c. $\mathrm{PH}_{3}$

Kaitlynn Wade

Numerade Educator

00:40

Problem 52

What types of atoms tend to form the following types of bonding?
a. ionic
b. covalent
c. metallic

Matthew Confer

Numerade Educator

02:14

Problem 53

What happens to the energy level and stability of two bonded atoms when they are separated and become individual atoms?

Kaitlynn Wade

Numerade Educator

02:29

Problem 54

Draw the three resonance structures for sulfur trioxide, $\mathrm{SO}_{3}$ .

Kaitlynn Wade

Numerade Educator

00:33

Problem 55

a. How do ionic and covalent bonding differ?
b. How does an ionic compound differ from a molecular compound?
c. How does an ionic compound differ from a metal?

David Collins

Numerade Educator

02:42

Problem 56

Write the electron-dot notation for each of the following elements:
a. $\mathrm{He}$
b. $\mathrm{C} 1$
C. $\mathrm{O}$
d. $\mathrm{P}$
e.$\mathrm{B}$

Kaitlynn Wade

Numerade Educator

01:18

Problem 57

Write the structural formula for methanol, $\mathrm{CH}_{3} \mathrm{OH}$.

Kaitlynn Wade

Numerade Educator

02:15

Problem 58

How many $\mathrm{K}^{+}$ and $\mathrm{S}^{2-}$ ions would be in one formula unit of the ionic compound formed by these ions?

Kaitlynn Wade

Numerade Educator

02:07

Problem 59

Explain metallic bonding in terms of the sparsely populated outermost orbitals of metal atoms.

Susan Hallstrom

Numerade Educator

03:23

Problem 60

Explain the role of molecular geometry in determining molecular polarity.

Kaitlynn Wade

Numerade Educator

00:44

Problem 61

How does the energy level of a hybrid orbital compare with the energy levels of the orbitals from which it was formed?

Nicole Smina

Numerade Educator

01:29

Problem 62

Aluminum's enthalpy of vaporization is 284 $\mathrm{kJ} / \mathrm{mol}$ . Beryllium's enthalpy of vaporization is 284 $\mathrm{kJ} / \mathrm{mol}$ . In which element is the bonding stronger between atoms?

Kaitlynn Wade

Numerade Educator

02:39

Problem 63

Determine the electronegativity difference, the probable bonding type, and the more-electronegative atom for each of the following pairs of atoms:
a. $\mathrm{Zn}$ and $\mathrm{O}$
b. $\mathrm{Br}$ and $\mathrm{I}$
c. $\mathrm{S}$ and $\mathrm{Cl}$

Kaitlynn Wade

Numerade Educator

02:53

Problem 64

Draw the Lewis structure for each of the following molecules:
a. $\mathrm{PCl}_{3}$
b. $\mathrm{CCl}_{2} \mathrm{F}_{2}$
c. $\mathrm{CH}_{3} \mathrm{NH}_{2}$

Kaitlynn Wade

Numerade Educator

01:16

Problem 65

Draw the Lewis structure for $\mathrm{BeCl}_{2}$.. (Hint: Beryllium do not follow the octet rule.)

Kaitlynn Wade

Numerade Educator

03:23

Problem 66

Draw a Lewis structure for each of the following polyatomic ions and determine their geometries:
a. $\mathrm{NO}_{2}^{-}$
b. $\mathrm{NO}_{3}^{-}$
c. $\mathrm{NH}_{4}^{+}$

Kaitlynn Wade

Numerade Educator

01:33

Problem 67

Why do most atoms tend to be chemically bonded to other atoms?

Kaitlynn Wade

Numerade Educator

01:53

Problem 68

Inferring Relationships The length of a bond varies depending on the type of bond formed. Predict and
compare the lengths of the carbon-carbon bonds in the following molecules. Explain your answer. (Hint: See Figure 2.10)

Kaitlynn Wade

Numerade Educator

00:38

Problem 69

Why does F generally form covalent bonds with great polarity?

Matthew Confer

Numerade Educator

03:46

Problem 70

Explain what is wrong with the following Lewis structures, and then correct each one.

Kaitlynn Wade

Numerade Educator

02:52

Problem 71

Ionic compounds tend to have higher boiling points than covalent substances do. Both ammonia, $\mathrm{NH}_{3}$, and methane, $\mathrm{CH}_{4}$, are covalent compounds, yet the boiling point of ammonia is $130^{\circ} \mathrm{C}$ higher than that of methane. What might account for this large difference?

Kaitlynn Wade

Numerade Educator

03:25

Problem 72

Figure 4.1 shows a model for a body-centered cubic crystal. Review the Properties tables for all of the metals in the Elements Handbook (Appendix A). What metals exist in body-centered cubic structures?

Arpit Gupta

Numerade Educator

01:18

Problem 73

Group 14 of the Elements Handbook (Appendix A) contains a discussion of semiconductors and the band theory of metals. How does this model explain the electrical conductivity of metals?

Manish Kumar

Numerade Educator

01:29

Problem 74

Prepare a report on the work of Linus Pauling.
a. Discuss his work on the nature of the chemical bond.
b. Linus Pauling was an advocate of the use of vitamin $\mathrm{C}$ as a preventative for colds. Evaluate Pauling’s claims. Determine if there is any scientific evidence that indicates whether vitamin $\mathrm{C}$ helps prevent colds.

Varsha Aggarwal

Numerade Educator

02:11

Problem 75

Covalently bonded solids, such as silicon, an element used in computer components, are harder than pure metals. Research theories that explain the hardness of covalently bonded solids and their usefulness in the computer industry. Present your findings to the class.

Madi Sousa

Numerade Educator

01:24

Problem 76

Natural rubber consists of long chains of carbon and hydrogen atoms covalently bonded together. When Charles Goodyear accidentally dropped a mixture of sulfur and rubber on a hot stove, the energy from the stove joined these chains together to make vulcanized rubber (named for Vulcan, the Roman god of fire). The carbon-hydrogen chains in vulcanized rubber are held together by two sulfur atoms that form covalent bonds between the chains. These covalent bonds are commonly called disulfide bridges. Explore other molecules that have such disulfide bridges. Present your findings to the class.

Kaitlynn Wade

Numerade Educator

02:37

Problem 77

Searching for the perfect artificial sweetener—great taste with no Calories—has been the focus of chemical research for some time. Molecules such as sucralose, aspartamine, and saccharine owe their sweetness to their size and shape. One theory holds that any sweetener must have three sites that fit into the proper taste buds on the tongue. This theory is appropriately known as the “triangle theory.” Research artificial sweeteners to develop a model to show how the triangle theory operates.

Kevin Zaborsky

Numerade Educator

00:37

Problem 78

Devise a set of criteria that will allow you to classify the following substances as ionic or non-ionic: $\mathrm{CaCO}_{3}, \mathrm{Cu}, \mathrm{H}_{2} \mathrm{O}, \mathrm{NaBr}$ , and C(graphite). Show your criteriato your instructor.

Matthew Confer

Numerade Educator

02:26

Problem 79

Performance Assessment Identify 10 common substances in and around your home, and indicate whether you would expect these substances to contain ionic, covalent, or metallic bonds.

Kaitlynn Wade

Numerade Educator