I -s'2o. 100 Chapter 3 Chemical Bonds UWL tnteractive versions of these problems may be assigned in OWL. Orange-numbered problems are applied. Section 3.2 What ls the Octet Rule? 3.17 Answer true or false. ' (a) The octet rule refers to the chemical bonding patterns of the first eight elements of the Periodic Table. (b) The octet rule refers to the tendency ofcertain elements to react in such a way that they achieve an outer shell ofeight valence electrons. (c) In gaining electrons, an atom becomes a posi- tively charged ion called a cation. (d) When an atom forms an ion, only the number of . valence electrons changes; the number ofprotons and neutrons in the nucleus does not change. (e) In forming ions, Group 2A elements typically lose two electrons to become cations with a charge of +2. (f) In forming an ion, a sodium atom (1s22s22p63s1) completes its valence shell by adding one elec- tron to filI its 3s shell (k22s22p63s2). (g) The elements of Group 6A typically react by ac- cepting two electrons to become anions with a charge of -2. (h) With the exception of hydrogen, the octet rule applies to all elements in periods 1,2, and 3. (i) Atoms and the ions derived from them have very similar physical and chemical properties. 3.18 How many electrons must each atom gain or lose to acquire an electron configuration identical to the noble gas nearest to it in atomic number? (a) Li (b) Cl (c) P (d) Al (e) Sr (f) S (e) Si (h) O 3.19 Show how each chemical change obeys the octet rule. (a) Lithium forms Li* (b) Oxygen forms O Show how each chemical change obeys the octet rule. (a) Hydrogen forms H- (hydride ion) (b) Aluminum forms Al3+ 3,2L Write the formula for the most stable ion formed by each element. (a) Mg (b) F (c) (d) s (e) K (I) 3.22 Why is Li- not a stable ion? 3.23 Predict which ions are stable: (a) I- (b) Se2+ (c) Na* (d) 52- (e) tr12+ (fl Ba8+ 3,24 Predict which ions are stable: (a) Br2- (b) C4- (c) Ca* (d) Ar* (e) Na* (I) Cs* a 3.25 Why are carbon and silicon reluctant to foil bonds? 3.26 Table 3.2 shows the following ions of co14m and Cu2*. Do these violate the octet rule? Section 3.3 How Do We Name Anions and Cations? 5.27 Answer true or false. (a) For Group 1A and Group 2A elements,fte of the ion each forms is simply the nare element followed by the word ion; for Mg2* is named magnesium ion. (b) H+ is named hydronium ion, and H is hydride ion. (c) The nucleus of H* consists of one proton neutron. (d) Many transition and inner transition form more than one positively charged irn I (e) In naming metal cations with two diffemed charges, the suffix -oas refers to the ion a charge of + 1 and -ic refers to the ion wift charge of +2. (f) Fe3* may be named either iron(III) ion or (g) The anion derived from a bromine atom is bromine ion. (h) The anion derived from an oxygen atomis named oxide ion. (i) HCO; is named hydrogen carbonate ion- . 0) The prefrx bi- in the name "bicarbonate'im indicates that this ion h.

1. I -s'2o.
100 Chapter 3 Chemical Bonds
UWL tnteractive versions of these problems may be assigned
in OWL.
Orange-numbered problems are applied.
Section 3.2 What ls the Octet Rule?
3.17 Answer true or false. '
(a) The octet rule refers to the chemical bonding
patterns of the first eight elements of the
Periodic Table.
(b) The octet rule refers to the tendency ofcertain
elements to react in such a way that they achieve
an outer shell ofeight valence electrons.
(c) In gaining electrons, an atom becomes a posi-
tively charged ion called a cation.
(d) When an atom forms an ion, only the number of
. valence electrons changes; the number ofprotons
and neutrons in the nucleus does not change.
(e) In forming ions, Group 2A elements typically
lose two electrons to become cations with a
charge of +2.

2. (f) In forming an ion, a sodium atom (1s22s22p63s1)
completes its valence shell by adding one elec-
tron to filI its 3s shell (k22s22p63s2).
(g) The elements of Group 6A typically react by ac-
cepting two electrons to become anions with a
charge of -2.
(h) With the exception of hydrogen, the octet rule
applies to all elements in periods 1,2, and 3.
(i) Atoms and the ions derived from them have very
similar physical and chemical properties.
3.18 How many electrons must each atom gain or lose
to acquire an electron configuration identical to the
noble gas nearest to it in atomic number?
(a) Li (b) Cl (c) P (d) Al
(e) Sr (f) S (e) Si (h) O
3.19 Show how each chemical change obeys the octet
rule.
(a) Lithium forms Li* (b) Oxygen forms O
Show how each chemical change obeys the octet rule.
(a) Hydrogen forms H- (hydride ion)
(b) Aluminum forms Al3+
3,2L Write the formula for the most stable ion formed by
each element.
(a) Mg (b) F (c)
(d) s (e) K (I)
3.22 Why is Li- not a stable ion?
3.23 Predict which ions are stable:
(a) I- (b) Se2+ (c) Na* (d) 52- (e) tr12+ (fl Ba8+

3. 3,24 Predict which ions are stable:
(a) Br2- (b) C4- (c) Ca*
(d) Ar* (e) Na* (I) Cs*
a
3.25 Why are carbon and silicon reluctant to foil
bonds?
3.26 Table 3.2 shows the following ions of co14m
and Cu2*. Do these violate the octet rule?
Section 3.3 How Do We Name Anions
and Cations?
5.27 Answer true or false.
(a) For Group 1A and Group 2A elements,fte
of the ion each forms is simply the nare
element followed by the word ion; for
Mg2* is named magnesium ion.
(b) H+ is named hydronium ion, and H is
hydride ion.
(c) The nucleus of H* consists of one proton
neutron.
(d) Many transition and inner transition
form more than one positively charged irn I
(e) In naming metal cations with two diffemed
charges, the suffix -oas refers to the ion
a charge of + 1 and -ic refers to the ion wift
charge of +2.

4. (f) Fe3* may be named either iron(III) ion or
(g) The anion derived from a bromine atom is
bromine ion.
(h) The anion derived from an oxygen atomis
named oxide ion.
(i) HCO; is named hydrogen carbonate ion- .
0) The prefrx bi- in the name "bicarbonate'im
indicates that this ion has a charge of -2-
(k) The hydrogen phosphate ion has a charge
and the dihydrogen phosphate ion has a
charge of +2.
(l) The phosphate ion is PO3a-.
(m) The nitrite ion is NOz , and the nitrate
ion is NO3-.
(n) The carbonate ion is CO32-, and the
carbonate ion is HCO3-.
3.28 Name each polyatomic ion.
(a) HCO; (b) NO; (c) SOr'-
(d) HSO4- (e) HzPOa-
Section 3.4 What Are the Two Major Types
participating in the bond acquires an outer<{
electron configuration matching that of the{
gas nearest to it in atomic number. I
(b) Atoms that lose electrons to achieve a filled t
valence shell become cations and form ionic

5. bonds with anions.
of Chemical Bonds? :
3.29 Answer true or false. j
(a) According to the Lewis model of bondi.g, d
bond together in such a way that each atom {
AI
Br
,-.-r lll
- '-' - -----'--- - - -'
-
3.87
3.86
3.88
i-'
3.89
(e) HzO and NH3 are polar molecules, but CHa is
nonpolar.
(f) In methanol, CH3OH, the O-H bond is more
polar than the C-O bond.
(g) Dichloromethane, CH.zCl2,is polar, but tetrachlo-
romethane, CCla, is nonpolar.

6. (h) Ethanol, CHBCH2OH, the alcohol of alcoholic bev-
erages, has polar bonds, has a net dipole, and is a
polar mo1ecule.
Both CO2 and SO2 have polar bonds. Account for the
fact that CO2 is nonpolar and SO2 is polar.
Consider the molecule boron trifluoride, BF3.
(a) Write a Lewis structure for BF3.
(b) Predict the F-B-F bond angles using the
VSEPR model.
(c) Does BF3 have polar bonds? Is it a polar
molecule?
Is it possible for a molecule to have polar bonds and
yet have no dipole? ExPlain.
Is it possible for a molecule to have no polar bonds
and yet have a dipole? ExPlain.
In each case, tell whether the bond is ionic, polar co-
valent, or nonpolar covalent.
(a) Brz (b) BrCI (c) HCI (d) SrFz
3.90
-
(e) SiHa (0 CO G) N, G) CsCl
3.91 Account for the fact that chloromethane, CH3CI,
which has only one polar C-Cl bond, is a polar mol-
ecule, but carbon tetrachloride, CCla, which has four
polar C-Cl bonds, is a nonpolar molecule.

7. Chemical Csnnections
9.92 (Chemical Connections 3A) What are the three main
inorganic components of one dry mixture currently
used to create sYnthetic bone?
3.93 (Chemical Connections 3B) Why is sodium iodide
often present in the table salt we buy at the grocery
store?
3.54 (Chemical Connections 38) What is a medical use of
barium sulfate?
3.95 (Chemical Connections 38) What is a medical use of
potassium permanganate?
3.96 (Chemical Connections 3A) What is the most preva-
lent metal ion in bone and tooth enamel?
3.97 (Chemical Connections 3C) In what way does the gas
nitric oxide, NO, contribute to the acidity of acid rain?
Additional Problems
3.98 Explain why argon does not form either (a) ionic
bonds or (b) covalent bonds.
3.99 Knowing what you do about covalent bonding in com-
pounds of carbon, nitrogen, and oxygen and given the
fact that silicon isjust below carbon in the Periodic
Table, phosphorus is just below nitrogen, and sulfur
Problems td.=
is just below oxygen, predict the molecular formula

8. for the compound formed by (a) silicon and chlorine'
(b) phosphorus and hYdrogen, and
(c) sulfur and hydrogen'
3.100 Use the valence-shell electron-pair repulsion model
to predict the shape of a molecule in which a cenhal
atom is surrounded by frve regions of electron
density-as, for example, in phosphorus pentaflue
ride, PF5. (Hint: Use molecular models or if you do
not have a set handy, use marshmallows or gum-
drops and toothpicks.)
3.101 Use the valence-shell electron-pair repulsion model
to predict the shape of a molecule in which a central
atom is surrounded by six regions ofelectron density,
as, for example, in sulfur hexa-fluoride, SF6'
3.102 Chlorine dioxide, ClO2, is a yellow to reddish yellow
gas at room temperature. This strong oxidizing
agent is used for bleaching cellulose, paper pulp,
and textiles and for water purifrcation. It was
the gas used to kill anthrax spores in the anthrax-
contaminated Hart Senate Office Building'
(a) How many valence electrons are present
in ClO2?
(b) Draw a Lewis structure for this molecule. (Hint:
The order of attachment of atoms in this molecule
is O-CI-O. Chlorine is a third-period element,
and its valence shell may contain more than eight
electrons.)
3.103 Using the information in Figure 2.16, estimate the

9. H-O and H-S distances (the atom-atom dis-
tances) in H2O and H2S, respectively.
3.104 Arrange the single covalent bonds within each set in
order of increasing PolaritY.
(a) C-H, O-H, N-H (b) C-H, C-Cl, C-I
(c) C-C, C-O, C-N
3.105 Consider the structure ofVitamin E shown below,
which is found most abundantly in wheat germ orl
sunflower, and safflower oils:
H.C"L Hz
"-q'"--g-"-?', H2 ?t' Ez !:' Hz !:'
,""-i-a-'c-o-?-c-cic-cH-a-cic'cH-( -c- -cH-i H3C H2 H2 H2 H2 i'
H, CE3HrC
Viramin tr
(a) Identify the various types ofgeometries present
in each central atom usingVSEPR theory-
(b) Determine the various relative bond angles as-
sociated with each central atom usingVSEPR
theorY.
(c) Which is the most polar bond tu lifamin E?
(d) Would you predict Vitamin E to be polar or
nonpolar?
Nitrousoxidedissolvesinfats.Thegasisaddedunderpressure
lo .rt, of whipped topping' When the valve is opened' the gas

10. ""p."at,
ttrus
"*prnding
(whipping) the topping and forcing it out
ofthe can.
(a) How many valence electrons are present in a mol- 3'81
ecule of N2O?
(b) Write two equivalent contributing structures for
this molecule. The connectivity in nitrous oxide is
N-N-O.
(c) Exptain why the following is not an acceptable
contributing structure:
tN-N:0
Section 3.10 How Do We Predict Bond
Angles in Covalent Molecules?
3.79 Answer true or false'
(a) The letters VSEPR stand for valence-shell
electron-Pair rePulsion'
(b) In predicting bond angles about a central atom in
a covalent molecule, the VSEPR model considers
only shared electron pairs (electron pairs involved

11. in forming covalent bonds)'
(c) The VSEPR model treats the two electron pairs
r ofa double bond as one region ofelectron density
I und the three electron pairs ofa triple bond as
I one region ofelectron densitY'
(d) In carbon dioxide, O:C:O, carbon is sur-
rounded by four pairs ofelectrons and the
VSEPR model predicts 109'5" for the O-C-O
bond angle.
(e) For a central atom surrounded by three regions of
electron density, the VSEPR model predicts bond
angles of l-20'.
(f) The geometry about a carbon atom surrounded by
three regions ofelectron density is described as
trigonal Planar'
(g) For a central atom surrounded by four regions of
electron density, the VSEPR model predicts bond
angles of360"/4 : 90''
(h) For the ammonia molecule, NH3, theVSEPR
model predicts H-N-H bond angles of 109'5''
(i) For the ammonium ion, NHa+, theVSEPR model
predicts H-N-H bond angles of l'09'5''
0) The VSEPR model applies equally wellto cova-

12. lent compounds ofcarbon, nitrogen, and oxygen'
(k) In water, H-O-H, the oxygen atom forms cova-
lent bonds to two other atoms, and therefore' the
VSEPR model predicts an H-O-H bond angle
of 180".
(l) Ifyou fail to consider unshared pairs ofvalence
electrons when you use the VSEPR model' you
will arrive at an incorrect prediction'
(m) Given the assumptions of the VSEPR model' the
onlybond angles it predicts for compounds ofcarbon'
nitrogen, urd o*yg".t are 109'5', 120', and 180''
State the shape of a molecule whose central atom is
surrounded bY:
(a) T$o regions ofelectron density
(b) Three regions ofelectron density
(c) Four regions ofelectron density
Hydrogen and oxygen combine in different ratios to
for* rirO (water) and IIro, (hydrogen peroxide)'
(a) How many valence electrons are found in H2O? In
HzO2?
(b) Draw Lewis structures for each molecule in part
(a). Be certain to show all valence electrons'

13. (c) Using the VSEPR model, predict th9 bgnd angles
about the oxygen atom in water and about each
oxygen atom in hYdrogen Peroxide'
Hydrogen and nitrogen combine in different ratios
toform three compounds: NH3 (ammonia), NzHa
(hydrazine), and N2H2 (diimide)'
(a) How many valence electrons must the Lewis
structure of each molecule show?
(b) Draw a Lewis structure for each molecule'
(c) Predict the bond angles about the nitrogen
atom(s) in each molecule'
Predict the shape of each molecule'
(a) CHa G) PHB (c) CHFg (d) SO2
(e) SOs (0 CCIzF2 G) Ntt, ft) PCls
Predict the shaPe ofeach ion.
(a) NOz- &) NHa* (c) Cos'-
Section 3.11 How Do We Determine
lf a Molecule ls Polar?
3.85 Answer true or false.
(a) To predict whether a covalent molecule is polar or

14. nonpolar, you must know both the polarity of each
bond and the geometry (shape) of the molecule'
(b) A molecule may have two or more polar bonds
and still be nonPolar'
(c) A1I molecules with polar bonds are polar'
(d) If water were a linear molecule with an H-O-H
bond angle of 180", water would be a nonpolar
molecule.
104 ChaPter 3 Chemical Bonds
8.78 Nitrous oxide, N2O, Iaughing gas, is a colorless'
nontoxic, tasteless, and odorless gas' It is used as
an inhalation anesthetic in dental and other surger-
ies. Because nitrous oxide is soluble in vegetable
oils (fats), it is used commercially as a propellant in
whiPPed toPPings.
;
d
3.80
3.82
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