General Chemistry: Principles and Modern Applications

Ralph H. Petrucci, F. Geoffrey Herring, Jeffry D. Madura

Chapter 10

Chemical Bonding I: Basic Concepts - all with Video Answers

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Chapter Questions

Problem 1

Write Lewis symbols for the following atoms. (a) $\mathrm{Kr}$;
(b) Ge; (c) $\mathrm{N} ;$ (d) Ga; (e) As; (f) Rb.

Alannah Byers

Alannah Byers

Numerade Educator

Problem 2

Write Lewis symbols for the following ions. (a) $\mathrm{H}^{-}$ (b) $\operatorname{Sn}^{2+} ;$ (c) $\mathrm{K}^{+} ;$ (d) $\mathrm{Br}^{-} ;$ (e) $\mathrm{Se}^{2-} ;$ (f) $\mathrm{Sc}^{3+}$.

Alannah Byers

Numerade Educator

Problem 3

Write plausible Lewis structures for the following molecules that contain only single covalent bonds.
(a) $\mathrm{FCl} ;$ (b) $\mathrm{I}_{2} ;$ (c) $\mathrm{SF}_{2} ;$ (d) $\mathrm{NF}_{3} ;$ (e) $\mathrm{H}_{2} \mathrm{Te}$.

Susan Hallstrom

Susan Hallstrom

Numerade Educator

Problem 4

Each of the following molecules contains at least one multiple (double or triple) covalent bond. Give a plausible Lewis structure for (a) $\mathrm{OCS} ;$ (b) $\mathrm{CH}_{3} \mathrm{CHO}$
(c) $\mathrm{F}_{2} \mathrm{CO} ;$ (d) $\mathrm{Cl}_{2} \mathrm{SO} ;$ (e) $\mathrm{C}_{2} \mathrm{H}_{2}$.

Vasu Makani

Numerade Educator

Problem 5

By means of Lewis structures, represent bonding between the following pairs of elements: (a) Cs and $\mathrm{Br} ;$ (b) $\mathrm{H}$ and $\mathrm{Sb} ;$ (c) $\mathrm{B}$ and $\mathrm{Cl} ;$ (d) $\mathrm{Cs}$ and $\mathrm{Cl}$; (e) Li and O; (f) Cl and L. Your structures should show whether the bonding is essentially ionic or covalent.

Carolina Acevedo

Carolina Acevedo

Numerade Educator

Problem 6

Which of the following have Lewis structures that $d o$ not obey the octet rule: $\mathrm{NF}_{3}, \mathrm{AlCl}_{3}, \mathrm{SiF}_{6}^{2-}, \mathrm{SO}_{3}, \mathrm{PH}_{4}^{+}$ $\mathrm{PO}_{4}^{3-}, \mathrm{ClO}_{2} ?$

Vasu Makani

Numerade Educator

Problem 7

Give several examples for which the following statement proves to be incorrect. "All atoms in a Lewis structure have an octet of electrons in their valence shells."

Alannah Byers

Numerade Educator

Problem 8

Suggest reasons why the following do not exist as stable molecules: (a) $\mathrm{H}_{3} ;$ (b) $\mathrm{HHe} ;$ (c) $\mathrm{He}_{2}$; (d) $\mathrm{H}_{3} \mathrm{O}$.

Carolina Acevedo

Carolina Acevedo

Numerade Educator

Problem 9

Describe what is wrong with each of the following Lewis structures.

Vasu Makani

Numerade Educator

Problem 10

Describe what is wrong with each of the following Lewis structures.

Alannah Byers

Numerade Educator

Problem 11

Only one of the following Lewis structures is correct. Select that one and indicate the errors in the others.
(a) cyanate ion
(b) carbide ion
(c) hypochlorite ion
(d) nitrogen(II) oxide

Alannah Byers

Numerade Educator

Problem 12

Indicate what is wrong with each of the following Lewis structures. Replace each one with a more acceptable structure.

Vasu Makani

Numerade Educator

Problem 13

Write Lewis structures for the following ionic compounds: (a) calcium chloride; (b) barium sulfide;
(c) lithium oxide; (d) sodium fluoride.

Alannah Byers

Numerade Educator

Problem 14

Under appropriate conditions, both hydrogen and nitrogen can form monatomic anions. What are the Lewis symbols for these ions? What are the Lewis structures of the compounds (a) lithium hydride;
(b) calcium hydride; (c) magnesium nitride?

Carolina Acevedo

Carolina Acevedo

Numerade Educator

Problem 15

Derive the correct formulas for the following ionic compounds by writing Lewis structures. (a) lithium sulfide; (b) sodium fluoride; (c) calcium iodide; (d) scandium chloride.

Alannah Byers

Numerade Educator

Problem 16

Each of the following ionic compounds consists of a combination of monatomic and polyatomic ions. Represent these compounds with Lewis structures.
(a) $\mathrm{Al}(\mathrm{OH})_{3}$;
(c) $\mathrm{NH}_{4} \mathrm{F}$;
(d) $\mathrm{KClO}_{3}$;
(b) $\mathrm{Ca}(\mathrm{CN})_{2}$;
(e) $\mathrm{Ba}_{3}\left(\mathrm{PO}_{4}\right)_{2}$.

Vasu Makani

Numerade Educator

Problem 17

Assign formal charges to each of the atoms in the following structures.

Sam Limsuwannarot

Sam Limsuwannarot

Numerade Educator

Problem 18

Assign formal charges to each of the atoms in the following structures.

Sam Limsuwannarot

Sam Limsuwannarot

Numerade Educator

Problem 19

Both oxidation state and formal charge involve conventions for assigning valence electrons to bonded atoms in compounds, but clearly they are not the same. Describe several ways in which these concepts differ.

Carolina Acevedo

Carolina Acevedo

Numerade Educator

Problem 20

Although the notion that a Lewis structure in which formal charges are zero or held to a minimum seems to apply in most instances, describe several significant situations in which this appears not to be the case.

Lottie Adams

Numerade Educator

Problem 21

What is the formal charge of the indicated atom in each of the following structures?
(a) the central $\mathrm{O}$ atom in $\mathrm{O}_{3}$
(b) $\mathrm{Al}$ in $\mathrm{AlH}_{4}^{-}$
(c) $\mathrm{Cl}$ in $\mathrm{ClO}_{3}^{-}$
(d) $\sin \sin ^{2} \theta^{-}$
(e) $\mathrm{Cl}$ in $\mathrm{Cl} \mathrm{F}_{3}$

Vasu Makani

Numerade Educator

Problem 22

Assign formal charges to the atoms in the following species, and then select the more likely skeletal structure.
(a) $\mathrm{H}_{2} \mathrm{NOH}$ or $\mathrm{H}_{2} \mathrm{ONH}$
(b) SCS or CSS
(c) NFO or FNO
(d) $\mathrm{SOCl}_{2}$ or $\mathrm{OSCl}_{2}$ or $\mathrm{OCl}_{2} \mathrm{S}$
(e) $\mathrm{F}_{3} \mathrm{SN}$ and $\mathrm{F}_{3} \mathrm{NS}$

Carolina Acevedo

Carolina Acevedo

Numerade Educator

Problem 23

The concept of formal charge helped us to choose the more plausible of the I ewis structures for $\mathrm{NO}_{2}^{+}$ given in expressions (10.14) and $(10.15) .$ Can it similarly help us to choose a single Lewis structure as most plausible for $\mathrm{CO}_{2} \mathrm{H}^{+} ?$ Explain.

Vasu Makani

Numerade Educator

Problem 24

Show that the idea of minimizing the formal charges in a structure is at times in conflict with the observation that compact, symmetrical structures are more commonly observed than elongated ones with many central atoms. Use $\mathrm{ClO}_{4}^{-}$ as an illustrative example.

Carolina Acevedo

Carolina Acevedo

Numerade Educator

Problem 25

Write acceptable Lewis structures for the following molecules: (a) $\mathrm{H}_{2} \mathrm{NNH}_{2}$; (b) HOClO; (c) (HO) $_{2}$ SO; (d) HOOH (e) SO $_{4}^{2-}$.

Carolina Acevedo

Carolina Acevedo

Numerade Educator

Problem 26

Two molecules that have the same formulas but different structures are said to be isomers. (In isomers, the same atoms are present but linked together in different ways.) Draw acceptable Lewis structures for two isomers of $\mathrm{S}_{2} \mathrm{F}_{2}$.

Vasu Makani

Numerade Educator

Problem 27

The following polyatomic anions involve covalent bonds between O atoms and the central nonmetal atom. Propose an acceptable Lewis structure for each.
(a) $\mathrm{SO}_{3}^{2-} ;$ (b) $\mathrm{NO}_{2}^{-} ;$ (c) $\mathrm{CO}_{3}^{2-} ;$ (d) $\mathrm{HO}_{2}^{-}$.

Carolina Acevedo

Carolina Acevedo

Numerade Educator

Problem 28

Represent the following ionic compounds by Lewis structures: (a) barium hydroxide; (b) sodium nitrite;
(c) magnesium iodate; (d) aluminum sulfate.

Carolina Acevedo

Carolina Acevedo

Numerade Educator

Problem 29

Write a plausible Lewis structure for crotonaldehyde, $\mathrm{CH}_{3} \mathrm{CHCHCHO},$ a substance used in tear gas and insecticides.

Lijeesh Krishnan

Lijeesh Krishnan

Numerade Educator

Problem 30

Write a plausible Lewis structure for $\mathrm{C}_{3} \mathrm{O}_{2},$ a substance known as carbon suboxide.

Alannah Byers

Numerade Educator

Problem 31

Write Lewis structures for the molecules represented by the following molecular models.

Vasu Makani

Numerade Educator

Problem 32

Write Lewis structures for the molecules represented by the following molecular models.

Vasu Makani

Numerade Educator

Problem 33

Write Lewis structures for the molecules represented by the following line-angle formulas. [Hint: Recall page $70 \text { and Figure } 3-2 .]$

Vasu Makani

Numerade Educator

Problem 34

Write Lewis structures for the molecules represented by the following line-angle formulas. [Hint: Recall page $70 \text { and Figure } 3-2 .]$

Vasu Makani

Numerade Educator

Problem 35

Identify the main group that the element $X$ belongs to in each of the following Lewis structures. For the types of molecule shown, give an example that exists.

David Collins

Numerade Educator

Problem 36

Identify the main group that the element $X$ belongs to in each of the following Lewis structures. For the types of molecule shown, give an example that exists.

Vasu Makani

Numerade Educator

Problem 37

Use your knowledge of electronegativities, but do not refer to tables or figures in the text, to arrange the following bonds in terms of increasing ionic character:
$\mathrm{C}-\mathrm{H}, \mathrm{F}-\mathrm{H}, \mathrm{Na}-\mathrm{Cl}, \mathrm{Br}-\mathrm{H}, \mathrm{K}-\mathrm{F}$.

Carolina Acevedo

Carolina Acevedo

Numerade Educator

Problem 38

Which of the following molecules would you expect to have a resultant dipole moment $(\mu) ;$ (a) $\mathrm{F}_{2}$, (b) $\mathrm{NO}_{2}$
(c) $\mathrm{BF}_{3},$ (d) $\mathrm{HBr},$ (e) $\mathrm{H}_{2} \mathrm{CCl}_{2}$, (f) $\mathrm{SiF}_{4},$ (g) OCS? Explain.

Carolina Acevedo

Carolina Acevedo

Numerade Educator

Problem 39

What is the percent ionic character of each of the following bonds: (a) $\mathrm{S}-\mathrm{H} ;$ (b) $\mathrm{O}-\mathrm{Cl} ;$ (c) $\mathrm{Al}-\mathrm{O}$
(d) As - O?

Lottie Adams

Numerade Educator

Problem 40

Plot the data of Figure $10-6$ as a function of atomic number. Does the property of electronegativity conform to the periodic law? Do you think it should?

Nicole Smina

Numerade Educator

Problem 41

Use a cross-base arrow $(\longrightarrow)$ to represent the polarity of the bond in each of the following diatomic molecules. Then use the data below to calculate, in the manner described on page $431,$ the partial charges ( $\delta$ ) on the atoms in each molecule. Express the partial charges as a decimal fraction of the elementary charge, $\mathrm{e}=1.602 \times 10^{-19} \mathrm{C},$ for example $\delta=+0.17 \mathrm{e}$
or $\delta=-0.17 \mathrm{e}$.

Vasu Makani

Numerade Educator

Problem 42

Use a cross-base arrow $(\longrightarrow)$ to represent the polarity of the bond in each of the following diatomic molecules. Then use the data below to calculate the partial charges ( $\delta$ ) on the atoms in each molecule. Express the partial charges in the manner described in Exercise 41.

Vasu Makani

Numerade Educator

Problem 43

Which electrostatic potential map corresponds to $\mathrm{F}_{2} \mathrm{C}=\mathrm{O},$ and which to $\mathrm{H}_{2} \mathrm{C}=\mathrm{O} ?$

Lottie Adams

Numerade Educator

Problem 44

Match the correct electrostatic potential map corresponding to HOCl, FOCl, and HOF.

Lottie Adams

Numerade Educator

Problem 45

Two electrostatic potential maps are shown, one corresponding to a molecule containing only S and $\mathrm{F}$, the other Si and F. Match them. What are the molecular formulas of the compounds?

Lottie Adams

Numerade Educator

Problem 46

Two electrostatic potential maps are shown, one corresponding to a molecule containing only $\mathrm{Cl}$ and $\mathrm{F}$ the other $P$ and $F$. Match them. What are the molecular formulas of the compounds?

Lottie Adams

Numerade Educator

Problem 47

Through appropriate Lewis structures, show that the phenomenon of resonance is involved in the nitrite ion.

Alannah Byers

Numerade Educator

Problem 48

Which of the following species requires a resonance hybrid for its Lewis structure: (a) $\mathrm{CO}_{2},$ (b) $\mathrm{OCl}^{-}$ (c) $\mathrm{CO}_{3}^{2-},$ or $(\mathrm{d}) \mathrm{OH}^{-} ?$ Explain.

Lottie Adams

Numerade Educator

Problem 49

Dinitrogen oxide (nitrous oxide, or "laughing gas") is sometimes used as an anesthetic. Here are some data about the $\mathrm{N}_{2} \mathrm{O}$ molecule: $\mathrm{N}-\mathrm{N}$ bond length $=$ $113 \mathrm{pm} ; \mathrm{N}-\mathrm{O}$ bond length $=119 \mathrm{pm} .$ Use these data and other information from the chapter to comment on the plausibility of each of the following Lewis structures shown. Are they all valid? Which ones do you think contribute most to the resonance hybrid?

Lottie Adams

Numerade Educator

Problem 50

The Lewis structure of nitric acid, $\mathrm{HONO}_{2}$, is a resonance hybrid. How important do you think the contribution of the following structure is to the resonance hybrid? Explain.

Lottie Adams

Numerade Educator

Problem 51

Draw Lewis structures for the following species, indicating formal charges and resonance where applicable:
(a) $\mathrm{HCO}_{2}=$
(b) $\mathrm{HCO}_{3}^{-}$
(c) $\mathrm{FSO}_{3}^{-}$
(d) $\mathrm{N}_{2} \mathrm{O}_{3}^{2-}$ (the nitrogen atoms are joined centrally with one oxygen atom on one $\mathrm{N}$ and two on the other)

Carolina Acevedo

Carolina Acevedo

Numerade Educator

Problem 52

Draw Lewis structures for the following species, indicating formal charges and resonance where applicable:
(a) $\mathrm{HOSO}_{3}$
(b) $\mathrm{H}_{2} \mathrm{NCN}$
(c) $\mathrm{FCO}_{2}^{-}$
(d) $\mathrm{S}_{2} \mathrm{N}_{2}$ (a cyclic structure with $\mathrm{S}$ and $\mathrm{N}$ alternating)

Carolina Acevedo

Carolina Acevedo

Numerade Educator

Problem 53

Write plausible Lewis structures for the following odd-electron species: (a) $\mathrm{CH}_{3} ;$ (b) $\mathrm{ClO}_{2} ;$ (c) $\mathrm{NO}_{3}$.

Lottie Adams

Numerade Educator

Problem 54

Write plausible Lewis structures for the following free radicals: (a) $\cdot \mathrm{C}_{2} \mathrm{H}_{5} ;$ (b) $\mathrm{HO}_{2}$ "; (c) ClO?.

Lottie Adams

Numerade Educator

Problem 55

Which of the following species would you expect to be diamagnetic and which paramagnetic: (a) $\mathrm{OH}^{-} ;$ (b) $\mathrm{OH} ;(\mathrm{c}) \mathrm{NO}_{3} ;(\mathrm{d}) \mathrm{SO}_{3} ;(\mathrm{e}) \mathrm{SO}_{3}^{2-} ;(\mathrm{f}) \mathrm{HO}_{2} ?$

Lottie Adams

Numerade Educator

Problem 56

Write a plausible Lewis structure for $\mathrm{NO}_{2}$, and indicate whether the molecule is diamagnetic or paramagnetic. Two $\mathrm{NO}_{2}$ molecules can join together (dimerize) to form $\mathrm{N}_{2} \mathrm{O}_{4}$. Write a plausible Lewis structure for $\mathrm{N}_{2} \mathrm{O}_{4},$ and comment on the magnetic properties of the molecule.

Lottie Adams

Numerade Educator

Problem 57

In which of the following species is it necessary to employ an expanded valence shell to represent the Lewis structure: $\mathrm{PO}_{4}^{3-}, \mathrm{PI}_{3}, \mathrm{ICl}_{3}, \mathrm{OSCl}_{2}, \mathrm{SF}_{4}, \mathrm{ClO}_{4} ?$
Explain your choices.

Lottie Adams

Numerade Educator

Problem 58

Describe the carbon-to-sulfur bond in $\mathrm{H}_{2} \mathrm{CSF}_{4}$. That is, is it most likely a single, double, or triple bond?

Lottie Adams

Numerade Educator

Problem 59

Use VSEPR theory to predict the geometric shapes of the following molecules and ions: (a) $\mathrm{N}_{2}$; (b) HCN; (c) $\mathrm{NH}_{4}^{+} ;$ (d) $\mathrm{NO}_{3}^{-} ;$ (e) NSF.

Alannah Byers

Numerade Educator

Problem 60

Use VSEPR theory to predict the geometric shapes of the following molecules and ions: (a) $\mathrm{PCl}_{3} ;$ (b) $\mathrm{SO}_{4}^{2-}$;
(c) $\mathrm{SOCl}_{2} ;$ (d) $\mathrm{SO}_{3} ;$ (e) $\mathrm{BrF}_{4}^{+}$.

Alannah Byers

Numerade Educator

Problem 61

Each of the following is either linear, angular (bent), planar, tetrahedral, or octahedral. Indicate the correct shape of (a) $\mathrm{H}_{2} \mathrm{S} ;$ (b) $\mathrm{N}_{2} \mathrm{O}_{4} ;$ (c) $\mathrm{HCN} ;$ (d) $\mathrm{SbCl}_{6}^{-}$; (e) $\mathrm{BF}_{4}^{-}$

Alannah Byers

Numerade Educator

Problem 62

Predict the geometric shapes of (a) $\mathrm{CO} ;$ (b) $\mathrm{SiCl}_{4}$; (c) $\mathrm{PH}_{3} ;$ (d) $\mathrm{ICl}_{3} ;$ (e) $\mathrm{SbCl}_{5} ;$ (f) $\mathrm{SO}_{2} ;$ (g) $\mathrm{AlF}_{6}^{3-}$.

Alannah Byers

Numerade Educator

Problem 63

One of the following ions has a trigonal-planar shape: $\mathrm{SO}_{3}^{2-} ; \mathrm{PO}_{4}^{3-} ; \mathrm{PF}_{6}^{-} ; \mathrm{CO}_{3}^{2-} .$ Which ion is it? Explain.

Alannah Byers

Numerade Educator

Problem 64

Two of the following have the same shape. Which two, and what is their shape? What are the shapes of the other two? $\mathrm{NI}_{3}, \mathrm{HCN}, \mathrm{SO}_{3}^{2-}, \mathrm{NO}_{3}^{-}$.

Alannah Byers

Numerade Educator

Problem 65

Each of the following molecules contains one or more multiple covalent bonds. Draw plausible Lewis structures to represent this fact, and predict the shape of each molecule. (a) $\mathrm{CO}_{2} ;$ (b) $\mathrm{Cl}_{2} \mathrm{CO} ;$ (c) CINO $_{2}$.

Vasu Makani

Numerade Educator

Problem 66

Sketch the probable geometric shape of a molecule of
(a) $\mathrm{N}_{2} \mathrm{O}_{4}\left(\mathrm{O}_{2} \mathrm{NNO}_{2}\right) ;$ (b) $\mathrm{C}_{2} \mathrm{N}_{2}(\mathrm{NCCN}) ;$ (c) $\mathrm{C}_{2} \mathrm{H}_{6}$
$\left(\mathrm{H}_{3} \mathrm{CCH}_{3}\right) ;(\mathrm{d}) \mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}\left(\mathrm{H}_{3} \mathrm{COCH}_{3}\right)$.

Alannah Byers

Numerade Educator

Problem 67

Use the VSEPR theory to predict the shapes of the anions (a) $\mathrm{ClO}_{4}^{-} ;$ (b) $\mathrm{S}_{2} \mathrm{O}_{3}^{2-}\left(\text { that is, } \mathrm{SSO}_{3}^{2-}\right) ;$ (c) $\mathrm{PF}_{6}^{-}$;
(d) I $_{3}^{-}$.

Alannah Byers

Numerade Educator

Problem 68

Use the VSEPR theory to predict the shape of (a) the molecule OSF $_{2} ;$ (b) the molecule $\mathrm{O}_{2} \mathrm{SF}_{2} ;$ (c) the ion $\mathrm{SF}_{5}^{-} ;$ (d) the ion $\mathrm{ClO}_{4}^{-} ;$ (e) the ion $\mathrm{ClO}_{3}^{-}$.

Alannah Byers

Numerade Educator

Problem 69

The molecular shape of $\mathrm{BF}_{3}$ is planar (see Table 10.1 ). If a fluoride ion is attached to the $B$ atom of $B F_{3}$ through a coordinate covalent bond, the ion $\mathrm{BF}_{4}^{-}$ results. What is the shape of this ion?

Vasu Makani

Numerade Educator

Problem 70

Explain why it is not necessary to find the Lewis structure with the smallest formal charges to make a successful prediction of molecular geometry in the VSEPR theory. For example, write Lewis structures for $S O_{2}$ having different formal charges, and predict the molecular geometry based on these structures.

Lottie Adams

Numerade Educator

Problem 71

Comment on the similarities and differences in the molecular structure of the following triatomic species:
$\mathrm{CO}_{2}, \mathrm{NO}_{2}^{-}, \mathrm{O}_{3},$ and $\mathrm{ClO}_{2}^{-}$.

Lottie Adams

Numerade Educator

Problem 72

Comment on the similarities and differences in the molecular structure of the following four-atom species: $\mathrm{NO}_{3}^{-}, \mathrm{CO}_{3}^{2-}, \mathrm{SO}_{3}^{2-},$ and $\mathrm{ClO}_{3}^{-}$.

Lottie Adams

Numerade Educator

Problem 73

Draw a plausible Lewis structure for the following series of molecules and ions: (a) $\mathrm{ClF}_{2}^{-} ;$ (b) $\mathrm{ClF}_{3}$; (c) $\mathrm{ClF}_{4}^{-} ;$ (d) ClF $_{5} .$ Describe the electron group geometry and molecular structure of these species.

Alannah Byers

Numerade Educator

Problem 74

Draw a plausible Lewis structure for the following series of molecules and ions: $(a) \operatorname{SiF}_{6}^{2-} ;$ (b) $\mathrm{PF}_{5} ;$ (c) $\mathrm{SF}_{4}$;
(d) $\mathrm{XeF}_{4}$. Describe the electron group geometry and molecular structure of these species.

Vasu Makani

Numerade Educator

Problem 75

Sketch the propyne molecule, $\mathrm{CH}_{3} \mathrm{C} \equiv \mathrm{CH}$. Indicate the bond angles in this molecule. What is the maximum number of atoms that can be in the same plane?

Lottie Adams

Numerade Educator

Problem 76

Sketch the propene molecule, $\mathrm{CH}_{3} \mathrm{CH}=\mathrm{CH}_{2}$. Indicate the bond angles in this molecule. What is the maximum number of atoms that can be in the same plane?

Nicole Smina

Numerade Educator

Problem 77

Lactic acid has the formula $\mathrm{CH}_{3} \mathrm{CH}(\mathrm{OH}) \mathrm{COOH}$
Sketch the lactic acid molecule, and indicate the various bond angles.

Lottie Adams

Numerade Educator

Problem 78

Levulinic acid has the formula $\mathrm{CH}_{3}(\mathrm{CO}) \mathrm{CH}_{2} \mathrm{CH}_{2}$
COOH. Sketch the levulinic acid molecule, and indicate the various bond angles.

Vasu Makani

Numerade Educator

Problem 79

Sketch, by using the dash and wedge symbolism, the $\mathrm{H}_{2} \mathrm{NCH}_{2} \mathrm{CHO}$ molecule, and indicate the various bond angles.

Lottie Adams

Numerade Educator

Problem 80

One of the isomers of chloromethanol has the formula $\mathrm{ClCH}_{2} \mathrm{OH} .$ Sketch, by using the dash and wedge symbolism, this isomer of chloromethanol, and indicate the various bond angles.

Lottie Adams

Numerade Educator

Problem 81

Predict the shapes of the following molecules, and then predict which would have resultant dipolemoments: (a) $\mathrm{SO}_{2} ;$ (b) $\mathrm{NH}_{3} ;$ (c) $\mathrm{H}_{2} \mathrm{S} ;$ (d) $\mathrm{C}_{2} \mathrm{H}_{4} ;$ (e) $\mathrm{SF}_{6}$;
(f) $\mathrm{CH}_{2} \mathrm{Cl}_{2}$.

Nicholas Sacco

Numerade Educator

Problem 82

Which of the following molecules would you expect to be polar: (a) $\mathrm{HCN} ;$ (b) $\mathrm{SO}_{3} ;$ (c) $\mathrm{CS}_{2} ;$ (d) OCS; (e) $\operatorname{SOCl}_{2} ;$ (f) $\operatorname{SiF}_{4} ;$ (g) $\operatorname{POF}_{3}$ ? Give reasons for your conclusions.

Lottie Adams

Numerade Educator

Problem 83

The molecule $\mathrm{H}_{2} \mathrm{O}_{2}$ has a resultant dipole moment of
2.2 D. Can this molecule be linear? If not, describe a shape that might account for this dipole moment.

Lottie Adams

Numerade Educator

Problem 84

Refer to the Integrative Example. A compound related to nitryl fluoride is nitrosyl fluoride, FNO. For this molecule, indicate (a) a plausible Lewis structure and (b) the geometric shape. (c) Explain why the measured resultant dipole moment for FNO is larger than the value for $\mathrm{FNO}_{2}$.

Lottie Adams

Numerade Educator

Problem 85

Without referring to tables in the text, indicate which of the following bonds you would expect to have the greatest bond length, and give your reasons. (a) $\mathrm{O}_{2}$;
(b) $\mathrm{N}_{2} ;$ (c) $\mathrm{Br}_{2} ;$ (d) $\mathrm{BrCl}$.

Carolina Acevedo

Carolina Acevedo

Numerade Educator

Problem 86

Estimate the lengths of the following bonds and indicate whether your estimate is likely to be too high or too low: (a) I $-\mathrm{Cl} ;$ (b) $\mathrm{C}-\mathrm{F}$.

Carolina Acevedo

Carolina Acevedo

Numerade Educator

Problem 87

A relationship between bond lengths and single covalent radii of atoms is given on page $443 .$ Use this relationship together with appropriate data from Table 10.2 to estimate these single-bond lengths. (a) $\mathrm{I}-\mathrm{Cl} ;$ (b) $\mathrm{O}-\mathrm{Cl} ;$ (c) $\mathrm{C}-\mathrm{F} ;$ (d) $\mathrm{C}-\mathrm{Br}$.

DC

Doreen Chan

Numerade Educator

Problem 88

In which of the following molecules would you expect the oxygen-to-oxygen bond to be the shortest:
(a) $\mathrm{H}_{2} \mathrm{O}_{2},$ (b) $\mathrm{O}_{2},$ (c) $\mathrm{O}_{3} ?$ Explain.

Carolina Acevedo

Carolina Acevedo

Numerade Educator

Problem 89

Refer to the Integrative Example. Use data from the chapter to estimate the length of the $\mathrm{N}-\mathrm{F}$ bond in $\mathrm{FNO}_{2}$.

Carolina Acevedo

Carolina Acevedo

Numerade Educator

Problem 90

Write a Lewis structure of the hydroxylamine molecule, $\mathrm{H}_{2}$ NOH. Then, with data from Table $10.2,$ determine all the bond lengths.

Carolina Acevedo

Carolina Acevedo

Numerade Educator

Problem 91

A reaction involved in the formation of ozone in the upper atmosphere is $\mathrm{O}_{2} \longrightarrow$ 2 O. Without referring to Table $10.3,$ indicate whether this reaction is endothermic or exothermic. Explain.

Carolina Acevedo

Carolina Acevedo

Numerade Educator

Problem 92

Use data from Table $10.3,$ but without per forming detailed calculations, determine whether each of the following reactions is exothermic or endothermic.
(a) $\mathrm{CH}_{4}(\mathrm{g})+\mathrm{I}(\mathrm{g}) \longrightarrow \cdot \mathrm{CH}_{3}(\mathrm{g})+\mathrm{HI}(\mathrm{g})$
(b) $\mathrm{H}_{2}(\mathrm{g})+\mathrm{I}_{2}(\mathrm{g}) \longrightarrow 2 \mathrm{HI}(\mathrm{g})$

Vasu Makani

Numerade Educator

Problem 93

Use data from Table 10.3 to estimate the enthalpy change ( $\Delta H$ ) for the following reaction.
$$\begin{aligned}
&\mathrm{C}_{2} \mathrm{H}_{6}(\mathrm{g})+\mathrm{Cl}_{2}(\mathrm{g}) \longrightarrow \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{Cl}(\mathrm{g})+\mathrm{HCl}(\mathrm{g})\\
&H=?
\end{aligned}$$

Vasu Makani

Numerade Educator

Problem 94

One of the chemical reactions that occurs in the formation of photochemical smog is $\mathrm{O}_{3}+\mathrm{NO} \longrightarrow \mathrm{NO}_{2}+$
$\mathrm{O}_{2} .$ Estimate the enthalpy change of this reaction by using appropriate Lewis structures and data from Table 10.3.

Vasu Makani

Numerade Educator

Problem 95

Estimate the standard enthalpies of formation at $25^{\circ} \mathrm{C}$ and 1 bar of $(a)$ OH(g); $(b)$ N $_{2} H_{4}(g)$. Write Lewis structures and use data from Table $10.3,$ as necessary.

Carolina Acevedo

Carolina Acevedo

Numerade Educator

Problem 96

Use $\Delta H$ for the reaction in Example $10-15$ and other data from Appendix D to estimate $\Delta H_{f}^{\circ}\left[\mathrm{CH}_{3} \mathrm{Cl}(g)\right]$.

Vasu Makani

Numerade Educator

Problem 97

Use bond energies from Table 10.3 to estimate the enthalpy change $(\Delta H)$ for the following reaction.
$$\mathrm{C}_{2} \mathrm{H}_{2}(\mathrm{g})+\mathrm{H}_{2}(\mathrm{g}) \longrightarrow \mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{g}) \quad \Delta H=?$$

Vasu Makani

Numerade Educator

Problem 98

Equations (1) and (2) can be combined to yield the equation for the formation of $\mathrm{CH}_{4}(\mathrm{g})$ from its elements.
Use the preceding data and a bond energy of $436 \mathrm{kJ} / \mathrm{mol}$ for $\mathrm{H}_{2}$ to estimate the $\mathrm{C}-\mathrm{H}$ bond
energy. Compare your result with the value listed in Table 10.3.

Vasu Makani

Numerade Educator

Problem 99

One reaction involved in the sequence of reactions leading to the destruction of ozone is
$$\mathrm{NO}_{2}(\mathrm{g})+\mathrm{O}(\mathrm{g}) \longrightarrow \mathrm{NO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g})$$
Calculate $\Delta H^{\circ}$ for this reaction by using the thermodynamic data in Appendix D. Use your $\Delta H^{\circ}$ value, plus data from Table $10.3,$ to estimate the nitrogenoxygen bond energy in $\mathrm{NO}_{2}$. [Hint: The structure of nitrogen dioxide, $\mathrm{NO}_{2}$, is best represented as a resonance hybrid of two equivalent Lewis structures.]

Lottie Adams

Numerade Educator

Problem 100

A reaction involved in the sequence of reactions leading to the destruction of ozone is
$$\mathrm{O}_{3}(\mathrm{g})+\mathrm{O}(\mathrm{g}) \longrightarrow 2 \mathrm{O}_{2}(\mathrm{g}) \quad \Delta H^{\circ}=-394 \mathrm{kJ}$$
Estimate the oxygen-oxygen bond energy in ozone by using the oxygen-oxygen bond energy in dioxygen from Table $10.3 .$ Compare this value with the $\mathrm{O}-\mathrm{O}$ and $\mathrm{O}=\mathrm{O}$ bond energies in Table $10.3 .$ How could you explain any differences?

Lottie Adams

Numerade Educator

Problem 101

Given the bond-dissociation energies: nitrogen-tooxygen bond in $\mathrm{NO}, 631 \mathrm{kJ} / \mathrm{mol} ; \mathrm{H}-\mathrm{H}$ in $\mathrm{H}_{2}$,
$436 \mathrm{kJ} / \mathrm{mol} ; \mathrm{N}-\mathrm{H}$ in $\mathrm{NH}_{3}, 389 \mathrm{kJ} / \mathrm{mol} ; \mathrm{O}-\mathrm{H}$ in
$\mathrm{H}_{2} \mathrm{O}, 463 \mathrm{kJ} / \mathrm{mol} ;$ calculate $\Delta H$ for the reaction.

Vasu Makani

Numerade Educator

Problem 102

The following statements are not made as carefully as they might be. Criticize each one.
(a) Lewis structures with formal charges are incorrect.
(b) Triatomic molecules have a planar shape.
(c) Molecules in which there is an electronegativity difference between the bonded atoms are polar.

Lottie Adams

Numerade Educator

Problem 103

A compound consists of $47.5 \%$ S and $52.5 \%$ Cl, by mass. Write a Lewis structure based on the empirical formula of this compound, and comment on its deficiencies. Write a more plausible structure with the same ratio of $\mathrm{S}$ to $\mathrm{Cl}$.

Vasu Makani

Numerade Educator

Problem 104

A $0.325 \mathrm{g}$ sample of a gaseous hydrocarbon occupies a volume of $193 \mathrm{mL}$ at $749 \mathrm{mmHg}$ and $26.1^{\circ} \mathrm{C}$. Determine the molecular mass, and write a plausible condensed structural formula for this hydrocarbon.

Lottie Adams

Numerade Educator

Problem 105

A $1.24 \mathrm{g}$ sample of a hydrocarbon, when completely burned in an excess of $\mathrm{O}_{2}(\mathrm{g}),$ yields $4.04 \mathrm{g} \mathrm{CO}_{2}$ and $1.24 \mathrm{g} \mathrm{H}_{2} \mathrm{O} .$ Draw a plausible structural formula for the hydrocarbon molecule. [Hint: There is more than one possible arrangement of the C and H atoms.]

Lottie Adams

Numerade Educator

Problem 106

Draw Lewis structures for two different molecules with the formula $\mathrm{C}_{3} \mathrm{H}_{4}$. Is either of these molecules linear? Explain.

Alannah Byers

Numerade Educator

Problem 107

Sodium azide, $\mathrm{NaN}_{3}$, is the nitrogen gas-forming substance used in automobile air-bag systems. It is an ionic compound containing the azide ion, $\mathrm{N}_{3}^{-}$. In this ion, the two nitrogen-to-nitrogen bond lengths are $116 \mathrm{pm} .$ Describe the resonance hybrid Lewis structure of this ion.

Lottie Adams

Numerade Educator

Problem 108

Use the bond-dissociation energies of $\mathrm{N}_{2}(\mathrm{g})$ and $\mathrm{O}_{2}(\mathrm{g})$ in table $10.3,$ together with data from Appendix $D,$ to estimate the bond-dissociation energy of $\mathrm{NO}(\mathrm{g})$

Lottie Adams

Numerade Educator

Problem 109

Hydrogen azide, $\mathrm{HN}_{3}$, is a liquid that explodes violently when subjected to physical shock. In the $\mathrm{HN}_{3}$ molecule, one nitrogen-to-nitrogen bond length is $113 \mathrm{pm},$ and the other is $124 \mathrm{pm} .$ The $\mathrm{H}-\mathrm{N}-\mathrm{N}$
bond angle is $112^{\circ} .$ Draw Lewis structures and a sketch of the molecule consistent with these facts.

Lottie Adams

Numerade Educator

Problem 110

A few years ago the synthesis of a salt containing the $\mathrm{N}_{5}^{+}$ ion was reported. What is the likely shape of this ion-linear, bent, zigzag, tetrahedral, seesaw, or square-planar? Explain your choice.

Lottie Adams

Numerade Educator

Problem 111

Carbon suboxide has the formula $\mathrm{C}_{3} \mathrm{O}_{2} .$ The carbon-to-carbon bond lengths are $130 \mathrm{pm}$ and carbon-to-oxygen, $120 \mathrm{pm} .$ Propose a plausible Lewis structure to account for these bond lengths, and predict the shape of the molecule.

Vasu Makani

Numerade Educator

Problem 112

In certain polar solvents, $\mathrm{PCl}_{5}$ undergoes an ionization reaction in which a $\mathrm{Cl}^{-}$ ion leaves one $\mathrm{PCl}_{5}$ molecule and attaches itself to another. The products of the ionization are $\mathrm{PCl}_{4}^{+}$ and $\mathrm{PCl}_{6}^{-}$. Draw a sketch showing the changes in geometric shapes that occur in this ionization (that is, give the shapes of $\mathrm{PCl}_{5}$, $\mathrm{PCl}_{4}^{+},$ and $\mathrm{PCl}_{6}^{-}$ ).
$$2 \mathrm{PCl}_{5} \rightleftharpoons \mathrm{PCl}_{4}^{+}+\mathrm{PCl}_{6}^{-}$$

Alannah Byers

Numerade Educator

Problem 113

Estimate the enthalpy of formation of HCN using bond energies from Table $10.3,$ data from elsewhere in the text, and the reaction scheme outlined as follows.

Lottie Adams

Numerade Educator

Problem 114

The enthalpy of formation of $\mathrm{H}_{2} \mathrm{O}_{2}(\mathrm{g})$ is $-136 \mathrm{kJ} / \mathrm{mol} .$ Use this value, with other appropriate data from the text, to estimate the oxygen-to-oxygen single-bond energy. Compare your result with the value listed in Table $10.3 .$

Lottie Adams

Numerade Educator

Problem 115

Use the VSEPR theory to predict a probable shape of the molecule $\mathrm{F}_{4} \mathrm{SCH}_{2}$, and explain the source of any ambiguities in your prediction.

Lottie Adams

Numerade Educator

Problem 116

The enthalpy of formation of methanethiol, $\mathrm{CH}_{3} \mathrm{SH}(\mathrm{g}),$ is $-22.9 \mathrm{kJ} / \mathrm{mol} .$ Methanethiol can be synthesized by the reaction of gaseous methanol and $\mathrm{H}_{2} \mathrm{S}(\mathrm{g}) .$ Water vapor is another product. Use this information and data from elsewhere in the text to estimate the carbon-to-sulfur bond energy in methanethiol.

Vasu Makani

Numerade Educator

Problem 117

For LiBr, the dipole moment (measured in the gas phase) and the bond length (measured in the solid state) are $7.268 \mathrm{D}$ and $217 \mathrm{pm},$ respectively. For $\mathrm{NaCl}$ the corresponding values are $9.001 \mathrm{D}$ and $236.1 \mathrm{pm}$.
(a) Calculate the percent ionic character for each bond. (b) Compare these values with the expected ionic character based on differences in electronegativity (see Figure $10-7$ ). (c) Account for any differences in the values obtained in these two different ways.

Lottie Adams

Numerade Educator

Problem 118

One possibility for the electron-group geometry for seven electron groups is pentagonal-bipyramidal, as found in the IF $_{7}$ molecule. Write the VSEPR notation for this molecule. Sketch the structure of the molecule, labeling all the bond angles.

Lottie Adams

Numerade Educator

Problem 119

The extent to which an acid (HA) dissociates in water depends upon the stability of the anion $\left(\mathrm{A}^{-}\right);$ the more stable the anion, the more extensive is the dissociation of the acid. The anion is most stable when the negative charge is distributed over the whole anion rather than localized at one particular atom. Consider the following acids: acetic acid, fluoroacetic acid, cyanoacetic acid, and nitroacetic acid. Draw Lewis structures for their anions, including contributing resonance structures. Rank the acids in order of increasing extent of dissociation. Electrostatic potential maps for the four anions are provided on the next page. Identify which map corresponds to which anion, and discuss whether the maps confirm conclusions based on Lewis structures.

Nicholas Sacco

Numerade Educator

Problem 120

R. S. Mulliken proposed that the electronegativity $(\chi)$ of an atom is given by
$$\chi=k \times(I-E A)$$
where $I$ and $E A$ are the ionization energy and electron affinity of the atom, respectively. Using the electron affinities and ionization energy values for the halogen atoms up to iodine, estimate the value of $k$ by employing the electronegativity values in Figure $10-6 .$ Estimate the electron affinity of At.

Susan Hallstrom

Susan Hallstrom

Numerade Educator

Problem 121

When molten sulfur reacts with chlorine gas, a vile-smelling orange liquid forms. When analyzed, the liquid compound has the empirical formula SCl. Several possible Lewis structures are shown below. Criticize these structures and choose the best one.

Nicholas Sacco

Numerade Educator

Problem 122

Hydrogen azide, $\mathrm{HN}_{3}$, can exist in two forms. One form has the three nitrogen atoms connected in a line; and the nitrogen atoms form a triangle in the other. Construct Lewis structures for these isomers and describe their shapes. Other interesting derivatives are nitrosyl azide ( $\mathrm{N}_{4} \mathrm{O}$ ) and trifluoromethyl azide $\left(\mathrm{CF}_{3} \mathrm{N}_{3}\right) .$ Describe the shapes of these molecules based on a line of nitrogen atoms.

Lottie Adams

Numerade Educator

Problem 123

A pair of isoelectronic species for $C$ and $N$ exist with the formula $\mathrm{X}_{2} \mathrm{O}_{4}$ in which there is an $\mathrm{X}-\mathrm{X}$ bond. $\mathrm{A}$ corresponding fluoride of boron also exists. Draw Lewis structures for these species and describe their shapes.

Lottie Adams

Numerade Educator

Problem 124

Acetone $\left(\mathrm{CH}_{3}\right) \mathrm{C}=\mathrm{O},$ a ketone, will react with a strong base $(\mathrm{A})$ to produce the enolate anion, $\mathrm{CH}_{3}(\mathrm{C}=\mathrm{O}) \mathrm{CH}_{2}^{-} .$ Draw the Lewis structure of the enolate anion, and describe the relative contributions of any resonance structures.

Vasu Makani

Numerade Educator

Problem 125

The species $\mathrm{PBr}_{4}^{-}$ has been synthesized and has been described as a tetrahedral anion. Comment on this description.

Lottie Adams

Numerade Educator

Problem 126

One of the allotropes of sulfur is a ring of eight sulfur atoms. Draw the Lewis structure for the $S_{8}$ ring. Is the ring likely to be planar? The $S_{8}$ ring can be oxidized to produce $S_{8}$ O. In $S_{8} O,$ the oxygen atom is bonded to one of the S atoms and the Sg ring is still intact. Draw the Lewis structure for $\mathrm{S}_{8} \mathrm{O}$.

Vasu Makani

Numerade Educator

Problem 127

where the origin is the point on the ground directly beneath the plane at the moment of the release. Graph the trajectory of the packet and find the coordinates of the point where the packet lands.

Lucas Finney

Numerade Educator

Problem 128

Pauling's reasoning in establishing his original electronegativity scale went something like this: If we assume that the bond $A-B$ is nonpolar, its bond energy is the average of the bond energies of $\mathrm{A}-\mathrm{A}$ and $\mathrm{B}-\mathrm{B}$. The di ference between the calculated and measured bond energies of the bond $A-B$ is attributable to the partial ionic character of the bond and is called the ionic resonance energy (IRE). If the IRE is expressed in kilojoules per mole, the relationship between IRE and the electronegativity difference is $(\Delta \mathrm{EN})^{2}=\mathrm{IRE} / 96 .$ To test this basis for an electronegativity scale,
(a) Use data from Table 10.3 to determine IRE for the $\mathrm{H}-\mathrm{Cl}$ bond.
(b) Determine $\Delta \mathrm{EN}$ for the $\mathrm{H}-\mathrm{Cl}$ bond.
(c) Establish the approximate percent ionic character in the $\mathrm{H}-\mathrm{Cl}$ bond by using the result of part (b) and Figure $10-7$. Compare this result with that obtained in Example $10-4$.

James Irizarry

Numerade Educator

Problem 129

On page $431,$ the bond angle in the $\mathrm{H}_{2} \mathrm{O}$ molecule is given as $104^{\circ}$ and the resultant dipole moment as $\mu=1.84 \mathrm{D}$.
(a) By an appropriate geometric calculation, determine the value of the $\mathrm{H}-$ O bond dipole in $\mathrm{H}_{2} \mathrm{O}$.
(b) Use the same method as in part (a) to estimate the bond angle in $\mathrm{H}_{2} \mathrm{S},$ given that the $\mathrm{H}-\mathrm{S}$ bond dipole is $0.67 \mathrm{D}$ and that the resultant dipole moment is $\mu=0.93 \mathrm{D}$.
(c) Refer to Figure $10-15$. Given the bond dipoles 1.87 D for the $\mathrm{C}-\mathrm{Cl}$ bond and $0.30 \mathrm{D}$ for the $\mathrm{C}-\mathrm{H}$ bond, together with $\mu=1.04 \mathrm{D},$ estimate the $\mathrm{H}-\mathrm{C}-\mathrm{Cl}$ bond angle in $\mathrm{CHCl}_{3}$.

Muhammad Ahsan

Numerade Educator

Problem 130

Alternative strategies to the one used in this chapter have been proposed for applying the VSEPR theory to molecules or ions with a single central atom. In general, these strategies do not require writing Lewis structures. In one strategy, we write
(1) the total number of electron pairs $=[$ (number of valence electrons) $\pm$ (electrons required for ionic charge) $] / 2$
(2) the number of bonding electron pairs $=$ (number of atoms) -1
(3) the number of electron pairs around central atom $=$ total number of electron pairs $-3 \times[$ number of terminal atoms (excluding $\mathrm{H}$ )]
(4) the number of lone-pair electrons = number of central atom pairs - number of bonding pairs After evaluating items $2,3,$ and $4,$ establish the VSEPR notation and determine the molecular shape. Use this method to predict the geometrical shapes of the following: (a) $\mathrm{PCl}_{5} ;$ (b) $\mathrm{NH}_{3} ;$ (c) $\mathrm{ClF}_{3} ;$ (d) $\mathrm{SO}_{2} ;$ (e) $\mathrm{ClF}_{4}^{-}$;
(f) $\mathrm{PCl}_{4}^{+}$. Justify each of the steps in the strategy, and explain why it yields the same results as the VSEPR method based on Lewis structures. How does the strategy deal with multiple bonds?

Lottie Adams

Numerade Educator

Problem 131

In your own words, define the following terms: (a) valence electrons; (b) electronegativity; (c) bonddissociation energy; (d) double covalent bond;(e) coordinate covalent bond.

Lottie Adams

Numerade Educator

Problem 132

Briefly describe each of the following ideas: (a) formal charge; (b) resonance; (c) expanded valence shell; (d) bond energy.

Lottie Adams

Numerade Educator

Problem 133

Explain the important distinctions between (a) ionic and covalent bonds; (b) lone-pair and bond-pair electrons; (c) molecular geometry and electron-group geometry; (d) bond dipole and resultant dipole moment; (e) polar molecule and nonpolar molecule.

Vasu Makani

Numerade Educator

Problem 134

Of the following species, the one with a triple covalent bond is (a) $\mathrm{NO}_{3}^{-} ;$ (b) $\mathrm{CN}^{-} ;$ (c) $\mathrm{CO}_{2} ;$ (d) $\mathrm{AlCl}_{3}$.

Lottie Adams

Numerade Educator

Problem 135

The formal charges on the $\mathrm{O}$ atoms in the ion $[\mathrm{ONO}]^{+}$ is $(\mathrm{a})-2 ;(\mathrm{b})-1 ;(\mathrm{c}) 0 ;(\mathrm{d})+1$.

Lottie Adams

Numerade Educator

Problem 136

Which molecule is nonlinear? (a) $\mathrm{SO}_{2} ;$ (b) $\mathrm{CO}_{2}$;
(c) HCN; (d) NO.

Lottie Adams

Numerade Educator

Problem 137

Which molecule is nonpolar? (a) $\mathrm{SO}_{3} ;$ (b) $\mathrm{CH}_{2} \mathrm{Cl}_{2}$;
(c) $\mathrm{NH}_{3} ;$ (d) FNO.

Lottie Adams

Numerade Educator

Problem 138

The highest bond-dissociation energy is found in
(a) $\mathrm{O}_{2} ;$ (b) $\mathrm{N}_{2} ;$ (c) $\mathrm{Cl}_{2} ;$ (d) $\mathrm{I}_{2}$.

Lottie Adams

Numerade Educator

Problem 139

The greatest bond length is found in (a) $\mathrm{O}_{2} ;$ (b) $\mathrm{N}_{2}$
(c) $\mathrm{Br}_{2} ;$ (d) BrCl.

Lottie Adams

Numerade Educator

Problem 140

Draw plausible Lewis structures for the following species; use expanded valence shells where necessary. (a) $\mathrm{Cl}_{2} \mathrm{O} ;$ (b) $\mathrm{PF}_{3} ;$ (c) $\mathrm{CO}_{3}^{2-} ;$ (d) $\mathrm{BrF}_{5}$.

Lottie Adams

Numerade Educator

Problem 141

Predict the shapes of the following sulfur-containing species. (a) $\mathrm{SO}_{2} ;$ (b) $\mathrm{SO}_{3}^{2-} ;$ (c) $\mathrm{SO}_{4}^{2-}$.

Lottie Adams

Numerade Educator

Problem 142

Without referring to tables or figures in the text other than the periodic table, indicate which of the following atoms, $\mathrm{Bi}, \mathrm{S}, \mathrm{Ba}, \mathrm{As},$ or $\mathrm{Mg},$ has the intermediate value when they are arranged in order of increasing electronegativity.

Lottie Adams

Numerade Educator

Problem 143

Use data from Tables 10.2 and 10.3 to determine for each bond in this following structure (a) the bond length and (b) the bond energy.

Lottie Adams

Numerade Educator

Problem 144

What is the VSEPR theory? On what physical basis is the VSEPR theory founded?

Lottie Adams

Numerade Educator

Problem 145

Use the $\mathrm{NH}_{3}$ molecule as an example to explain the difference between molecular geometry and electron-group geometry.

Alannah Byers

Numerade Educator

Problem 146

If you have four electron pairs around a central atom, under what circumstances can you have a pyramidal molecule? Similarly, how can you have a bent molecule? What are the expected bond angles in each case?

Lottie Adams

Numerade Educator

Problem 147

Draw three resonance structures for the sulfine molecule, $\mathrm{H}_{2} \mathrm{CSO}$. Do not consider ring structures.

Lottie Adams

Numerade Educator

Problem 148

Construct a concept map illustrating the connections between Lewis dot structures, the shapes of molecules, and polarity.

Vasu Makani

Numerade Educator