Name Date Class

Chapter 6

SECTION 1

SHORT ANSWER

1. a

2. b

3. a

4. b

5. c

6. c

7. a

8. valence electrons

9. ionic bond

10. polar covalent

11. ionic bond

12. 1.7

13. a. H2

b. HCl

c. NaCl

14. A pair of electrons is attracted to both nuclei of the two atoms bonded together.

15. electronegativity

16. The difference between the electronegativity of the two atoms in a bond will
determine whether the bond is ionic or covalent. If the difference in
electronegativity is greater than 1.7, the bond is considered ionic.

17. The electron density is greater around the more electronegative atom, giving that
part of the compound a partial negative charge. The other part of the compound
has an equal partial positive charge.

Section 2

SHORT ANSWER

1. As the atoms involved in the formation of a covalent bond approach each other, the
electron-proton attraction is stronger than the electron-electron and proton-proton
repulsions. The atoms are drawn to each other and their potential energy decreases.
Eventually, a distance is reached at which the repulsions between the like charges
equals the attraction of the opposite charges. At this point, potential energy is at a
minimum and a stable molecule forms.

2. Choose from hydrogen, boron, beryllium, phosphorus, sulfur, and xenon.

3. Resonance structures show that one Lewis structure cannot correctly represent
the location of electrons in a bond. Resonance structures show delocalized
electrons, while Lewis structures depict electrons in a definite location.

4. a. H¾F, H¾Cl, H¾Br, H¾I

b. CºC, C=C, C¾C

5. a.

b.

c.

d.

e.

Section 3

SHORT ANSWER

1. a

2. d

3. b

4. b

5. b

6. The force of attraction between unlike charges holds a negative ion and a positive
ion together in an ionic bond.

7. lattice energy

8. The atoms in a polyatomic ion are held together with covalent bonds, but
polyatomic ions combine with ions of opposite charge to form ionic compounds.

9. KCl, NaCl, LiCl, CaO, MgO

10. a.

b.

11.

SECTION 4

SHORT ANSWER

1. b

2. a

3. d

4. d

5. a

6. c

7. Most metals have their outer electrons in s orbitals, while nonmetals have their
outer electrons in p orbitals.

8. The mobility of electrons in a network of metal atoms contributes to the
metal’s ability to conduct electricity and heat.

9. The amount of energy required to vaporize a metal is a measure of the strength
of the bonds that hold the metal together. The greater a metal’s enthalpy of
vaporization, the stronger the metallic bond.

10. a.

b.

11.

SECTION 5

SHORT ANSWER

1. Pairs of valence electrons repel one another.

2. The electron pairs that are not involved in bonding also take up space, creating
a tetrahedron of electron pairs and making the water molecule angular or bent.

3. the s orbital and all three p orbitals from the second energy level

4. electronegativity difference and molecular geometry or unshared electron pairs

5. 3

4

2

1

6. They are all forces of attraction between molecules. In all cases there is an attraction
between the slightly negatively-charged portion of one molecule and the slightly
positively charged portion of another molecule.

7.

MIXED REVIEW

SHORT ANSWER

1. a. lattice energy

b. bond energy

c. enthalpy of vaporization

2. a. ionic

b. ionic

c. polar covalent

d. nonpolar covalent

e. polar covalent

f. polar covalent

3. A hydrogen bond is a dipole-dipole attraction between a partially positive hydrogen
atom and the unshared electron pair of a strongly electronegative atom such as O,
N, or F. Unlike ionic or covalent bonds, in which electrons are given up or shared,
the hydrogen bond is a weaker attraction. Hydrogen bonds are generally
intermolecular, while ionic and covalent bonds occur between ions or atoms
respectively.

4. Oxygen has higher electronegativity than sulfur, which creates a highly polar bond.
Increased polarity in H2O bonds means a stronger intermolecular attraction, making
water a liquid at room temperature. Hydrogen bonding exists between water
molecules, but not between hydrogen sulfide molecules.

5. There is a difference between the electronegativities of the two atoms in both
types of bonds that results in electrons being more closely associated with the
more electronegative atom.

6. a. polar

b. polar

c. polar

d. polar

Chapter 7

SECTION 1

SHORT ANSWER

1. c

2. c

3. a. 4 elements

b. 6 oxygen atoms

c. 21 atoms

d. 4.2 ´ 1024 atoms

4. a. 11 atoms

b. 45 atoms

c. 10 atoms

d. 9 atoms

5. a. N2O5

b. iron(II) oxide

c. H2SO3

d. phosphoric acid

6. a. True

b. True

7. a. In general, if the anion name ends in -ate, the corresponding acid name will end in a
suffix of -ic. In general, if the anion name ends in -ite, the corresponding acid name
will end in a suffix of -ous.

b. In general, if the anion name ends in -ide, the corresponding acid name will end in a
suffix of -ic and begin with a prefix of hydro-. The prefix hydro- is never used for
anions ending in -ate or -ite.

8.

Compound name / Formula
Aluminum sulfide / Al2S3
Cesium carbonate / Cs2CO3
Lead(II) chloride / PbCl2
Ammonium phosphate / (NH4)3PO4
Hydroiodic acid / HI

Section 2

SHORT ANSWER

1. a. +4

b. +6

c. -2

d. +1

e. +6

f. +5

g. +4

h. -3

2. a. SCl2

b. nitrogen(IV) oxide

3. a. fluorine

b. 0; F2

4. a. tin(IV) oxide

b. SnO

5. a. NO, NO2

b. ClO

6. a. N2O3

b. +3

c. The three oxygen atoms have oxidation states of -6 total, and because the algebraic
sum of the oxidation states in a neutral compound must be zero, the two nitrogen
atoms must have oxidation states of +6 total,

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Modern Chemistry 206 Reaction Energy