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44 Chemistry: Matter and Change • Chapter 8 Study Guide for Content Mastery

Section 8.2 What is an ionic bond?In your textbook, read about forming ionic bonds and the characteristics of ionic compounds.

Circle the letter of the choice that best completes the statement or answers the question.

1. An ionic bond is

a. attraction of an atom for its electrons.

b. attraction of atoms for electrons they share.

c. a force that holds together atoms that are oppositely charged.

d. the movement of electrons from one atom to another.

2. The formula unit of an ionic compound shows the

a. total number of each kind of ion in a sample.

b. simplest ratio of the ions.

c. numbers of atoms within each molecule.

d. number of nearest neighboring ions surrounding each kind of ion.

3. The overall charge of a formula unit for an ionic compound

a. is always zero. c. is always positive.

b. is always negative. d. may have any value.

4. How many chloride (Cl�) ions are present in a formula unit of magnesium chloride,given that the charge on a Mg ion is 2�?

a. one-half b. one c. two d. four

5. Ionic bonds generally occur between

a. metals. c. a metal and a nonmetal.

b. nonmetals. d. noble gases.

6. Salts are examples of

a. nonionic compounds. b. metals. c. nonmetals. d. ionic compounds.

7. A three-dimensional arrangement of particles in an ionic solid is called a(n)

a. crystal lattice. b. sea of electrons. c. formula unit. d. electrolyte.

8. In a crystal lattice of an ionic compound,

a. ions of a given charge are clustered together, far from ions of the opposite charge.

b. ions are surrounded by ions of the opposite charge.

c. a sea of electrons surrounds the ions.

d. neutral molecules are present.

STUDY GUIDE FOR CONTENT MASTERYCHAPTER 8

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Study Guide for Content Mastery Chemistry: Matter and Change • Chapter 8 43

Ionic CompoundsIonic Compounds

Section 8.1 Forming Chemical BondsIn your textbook, read about chemical bonds and formation of ions.

Use each of the terms below just once to complete the passage.

The force that holds two atoms together is called a(n) (1) .

Such an attachment may form by the attraction of the positively charged

(2) of one atom for the negatively charged

(3) of another atom, or by the attraction of charged atoms,

which are called (4) . The attractions may also involve

(5) electrons, which are the electrons in the outermost

(6) . The (7) are a family of elements that

have very little tendency to react. Most of these elements have a set of eight outermost

electrons, which is called a stable (8) . The relatively stable electron

structures developed by loss of electrons in certain elements of groups 1B, 2B, 3A, and 4A

are called (9) .

For each statement below, write true or false.

10. A positively charged ion is called an anion.

11. Elements in group 1A lose their one valence electron, forming an ion witha 1� charge.

12. Elements tend to react so that they acquire the electron structure of ahalogen.

13. A sodium atom tends to lose one electron when it reacts.

14. The electron structure of a zinc ion (Zn2�) is an example of a pseudo-noble gas formation.

15. A Cl� ion is an example of a cation.

16. The ending -ide is used to designate an anion.

17. Nonmetals form a stable outer electron configuration by losing electronsand becoming anions.

false

true

false

true

true

false

true

false

pseudo-noble

octet

noble gasesenergy level

valence

ions

electrons

nucleus

chemical bond


chemical bond electrons energy level ions noble gases

nucleus octet pseudo-noble gas formations valence

gas formations

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Section 8.3 Chemical Formulas and Their NamesIn your textbook, read about communicating what is in a compound and naming ionsand ionic compounds.


A one-atom ion is called a(n) (1) ion. The charge of such an ion is

equal to the atom’s (2) , which is the number of (3)

transferred to or from the atom to form the ion. In ionic compounds, the sum of the charges of

all the ions equals (4) . Ions made up of more than one atom are called

(5) ions. If such an ion is negatively charged and includes one or more

oxygen atoms, it is called a(n) (6) . If two such ions can be formed that

contain different numbers of oxygen atoms, the name for the ion with more oxygen atoms ends

with the suffix (7) . The name for the ion with fewer oxygen atoms

ends with (8) .

In the chemical formula for any ionic compound, the chemical symbol for the

(9) is written first, followed by the chemical symbol for the

(10) . A(n) (11) is a small number used to

represent the number of ions of a given element in a chemical formula. Such numbers are

written to the (12) of the symbol for the element. If no number

appears, the assumption is that the number equals (13) .

For each formula in Column A, write the letter of the matching name in Column B.

Column A Column B

14. ClO2�

15. ClO4�

16. ClO�

17. Cl�

18. ClO3�a

c

b

d

e

one

lower right

subscriptanion

cation

-ite

-ate

oxyanion

polyatomic

zero

electronsoxidation number

monatomic


anion -ate cation electrons zero

lower right monatomic one oxidation number -ite

oxyanion polyatomic subscript

a. chlorate

b. hypochlorite

c. chloride

d. perchlorate

e. chlorite

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9. What is the relationship between lattice energy and the strength of the attractive forceholding ions in place?

a. The more positive the lattice energy is, the greater the force.

b. The more negative the lattice energy is, the greater the force.

c. The closer the lattice energy is to zero, the greater the force.

d. There is no relationship between the two quantities.

10. The formation of a stable ionic compound from ions

a. is always exothermic. c. is always endothermic.

b. may be either exothermic or endothermic. d. neither absorbs nor releases energy.

11. In electron transfer involving a metallic atom and a nonmetallic atom during ion forma-tion, which of the following is correct?

a. The metallic atom gains electrons from the nonmetallic atom.

b. The nonmetallic atom gains electrons from the metallic atom.

c. Both atoms gain electrons.

d. Neither atom gains electrons.

Underline the word that correctly describes each property in ionic compounds.

12. Melting point Low High

13. Boiling point Low High

14. Hardness Hard Soft

15. Brittleness Flexible Brittle

16. Electrical conductivity in the solid state Good Poor

17. Electrical conductivity in the liquid state Good Poor

18. Electrical conductivity when dissolved in water Good Poor


19. The crystal lattice of ionic compounds affects their melting and boilingpoints.

20. The lattice energy is the energy required to separate the ions of an ioniccompound.

21. The energy of an ionic compound is higher than that of the separateelements that formed it.

22. Large ions tend to produce a more negative value for lattice energy thansmaller ions do.

23. Ions that have larger charges tend to produce a more negative latticeenergy than ions with smaller charges do.

true

false

false

true

true

Section 8.2 continued


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Section 8.4 Metallic Bonds and Properties of MetalsIn your textbook, read about metallic bonds.

Use the diagram of metallic bonding to answer the following questions.

1. What is the name of the model of metallic bonding that is illustrated?

electron sea model

2. Why are the electrons in a metallic solid described as delocalized?

They are free to move from one atom to another.

3. Which electrons from the metal make up the delocalized electrons?

the valence electrons

4. Are the metal atoms that are shown cations or anions? How can you tell?

Cations; they are positively charged.

5. How do the metallic ions differ from the ions that exist in ionic solids?

The electrons are not completely lost by the metal atoms,

as they are in an ionic solid.

6. Explain what holds the metal atoms together in the solid.

They are bonded by the oppositely charged electron sea that surrounds them.

In your textbook, read about the properties of metals.

For each property, write yes if the property is characteristic of most metals, or no if it isnot. If the property is a characteristic of metals, explain how metallic bonding accountsfor the property.

7. Malleable

keeping the metallic bonds intact.

8. Brittle

9. Lustrous

10. High melting point

11. Low boiling point

12. Ductile

keeping the metallic bonds intact.

13. Poor conduction of heat

14. Good conduction of electricity Yes; the delocalized electrons are mobile.

no

Yes; when the metal is pulled, the delocalized electrons move,

no

Yes; the metallic bonds are strong.

Yes; the delocalized electrons absorb and release protons.

no

Yes; when the metal is hammered, the delocalized electrons move,


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For each of the following chemical formulas, write the correct name of the ionic com-pound represented. You may refer to the periodic table and Table 8.7 for help.

19. NaI

20. CaCl2

21. K2S

22. MgO

23. LiHSO4

24. NH4Br

25. Ca3N2

26. Cs3P

27. KBrO3

28. Mg(ClO)2

29. Li2O2

30. Be3(PO4)2

31. (NH4)2CO3

32. NaBrO3

33. Fe2O3

34. Fe(IO3)2

For each of the following ionic compounds, write the correct formula for the compound.You may refer to the periodic table and Table 8.7 for help.

35. beryllium nitride

36. nickel(II) chloride

37. potassium chlorite

38. copper(I) oxide

39. magnesium sulfite

40. ammonium sulfide

41. calcium iodate

42. iron(III) perchlorate

43. sodium nitride Na3N

Fe(ClO4)3

Ca(IO3)2

(NH4)2S

MgSO3

Cu2O

KClO2

NiCl2

Be3N2

iron(III) iodate

iron(III) oxide

sodium bromate

ammonium carbonate

beryllium phosphate

lithium peroxide

magnesium hypochlorite

potassium bromate

cesium phosphide

calcium nitride

ammonium bromide

lithium hydrogen sulfate

magnesium oxide

potassium sulfide

calcium chloride

sodium iodide



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Section 9.2 Naming MoleculesIn your textbook, read about how binary compounds and acids are named from theirformulas.


1. Binary molecular compounds are generally composed of a metal and anonmetal.

2. The second element in the formula of a binary compound is named usingthe suffix -ite.

3. The prefix tetra- indicates three atoms.

4. The prefix hexa- indicates six atoms.

5. In naming the first element in a formula, the prefix mono- is not used.

6. For binary acids, the hydrogen part of the compound is named using theprefix hydro-.

7. An oxyacid contains only two elements.

8. If the name of the anion of an oxyacid ends in -ate, the acid namecontains the suffix -ous.

In your textbook, read about naming molecular compounds and oxyacids.

For each item in Column A, write the letter of the matching item in Column B.

Column A Column B

9. CO

10. CO2

11. H2CO3

12. NH3

13. N2O4

14. HNO2

15. HNO3

16. HBr

17. HBrO3h

a

f

d

b

e

g

i

c

false

false

true

true

true

false

false

false


a. hydrobromic acid

b. dinitrogen tetroxide

c. carbon monoxide

d. nitrous acid

e. ammonia

f. nitric acid

g. carbonic acid

h. bromic acid

i. carbon dioxide

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Covalent BondingCovalent Bonding

Section 9.1 The Covalent BondIn your textbook, read about the nature of covalent bonds.


When sharing of electrons occurs, the attachment between atoms that results is called

a(n) (1) . When such an attachment is formed, bond dissociation

energy is released, and the process is (2) . When two or more

atoms bond by means of electron sharing, the resulting particle is called a(n)

(3) . If the electrons shared are centered between the two atoms, the

attachment is called a(n) (4) . If the sharing involves the overlap of

parallel orbitals, the attachment is called a(n) (5) .

In your textbook, read about single and multiple bonds and bond strength.

Circle the letter of the choice that best completes the statement or answers the question.

6. In what form do elements such as hydrogen, nitrogen, and oxygen normally occur?

a. as single atoms c. as molecules containing three atoms

b. as molecules containing two atoms d. as molecules containing four atoms

7. How many electrons are shared in a double covalent bond?

a. none b. one c. two d. four

8. Bond length is the distance between

a. two molecules of the same substance. c. the nuclei of two attached atoms.

b. the electrons in two attached atoms. d. the orbitals of two attached atoms.

9. Which of the following relationships relating to bond length is generally correct?

a. the shorter the bond, the stronger the bond

b. the shorter the bond, the weaker the bond

c. the shorter the bond, the fewer the electrons in it

d. the shorter the bond, the lower the bond dissociation energy

pi bond

sigma bond

molecule

exothermic

covalent bond


covalent bond molecule sigma bond exothermic pi bond

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Section 9.4 Molecular ShapeIn your textbook, read about the VSEPR model.

Circle the letter of the choice that best completes the statement.

1. The VSEPR model is used mainly to

a. determine molecular shape. c. determine ionic charge.

b. write resonance structures. d. measure intermolecular distances.

2. The bond angle is the angle between

a. the sigma and pi bonds in a double bond. c. two terminal atoms and the central atom.

b. the nucleus and the bonding electrons. d. the orbitals of a bonding atom.

3. The VSEPR model is based on the idea that

a. there is always an octet of electrons around an atom in a molecule.

b. electrons are attracted to the nucleus.

c. molecules repel one another.

d. shared and unshared electron pairs repel each other as much as possible.

4. The shape of a molecule whose central atom has four pairs of bonding electrons is

a. tetrahedral. b. trigonal planar. c. trigonal pyramidal. d. linear.

5. The shape of a molecule that has two covalent single bonds and no lone pairs on the central atom is


6. The shape of a molecule that has three single covalent bonds and one lone pair on thecentral atom is


In your textbook, read about hybridization.


The formation of new orbitals from a combination or rearrangement of valence electrons

is called (7) . The orbitals that are produced in this way are

(8) to one another. An example of an element that commonly

undergoes such formation is (9) . When this atom combines its three

p orbitals and its one s orbital, the orbitals that result are called (10)

orbitals. An example of a molecule that has this type of orbital is (11) .methane

sp3

carbon

identical

hybridization


carbon carbon dioxide hybridization sp3

identical methane sp phosphorus trihydride

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Section 9.3 Molecular StructuresIn your textbook, read about Lewis structures.


1. A structural formula shows the arrangement of the atoms in a molecule.

2. The central atom in a molecule is the one with the highest electronaffinity.

3. In molecules, hydrogen is always a terminal atom.

4. The number of bonding pairs in a molecule is equal to the number ofelectrons.

5. To find the total number of electrons available for bonding in a positiveion, you should add the ion charge to the total number of valence electronsof the atoms present.

6. The electrons in a coordinate covalent bond are donated by both thebonded atoms.

7. Resonance occurs when more than one valid Lewis structure can bewritten for a molecule.

8. Nitrate is an example of an ion that forms resonance structures.

9. The carbon dioxide molecule contains two double bonds.

10. All electrons in an atom are available for bonding.

11. In the sulfate ion (SO42�), 32 electrons are available for bonding.

12. When carbon and oxygen bond, the molecule contains ten pairs ofbonding electrons.

In your textbook, read about resonance structures and exceptions to the octet rule.

For each item in Column A, write the letter of the matching item in Column B.

Column A Column B

13. Odd number of valence electrons

14. Fewer than 8 electrons around an atom

15. More than 8 electrons around central atom

16. More than one valid Lewis structurea

d

b

c

false

true

false

true

true

true

false

false

false

true

false

true


a. O3

b. BF3

c. NO

d. SF6


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In your textbook, read about bond polarity.

Using the table of electronegativities on the preceding page, circle the letter of the choicethat best completes the statement or answers the question.

8. Unequal sharing of electrons between two bonded atoms always indicates

a. a nonpolar covalent bond. c. a polar covalent bond.

b. an ionic bond. d. a polar molecule.

9. When electronegativities of two bonded atoms differ greatly, the bond is

a. polar covalent. b. coordinate covalent. c. polar covalent. d. ionic.

10. What is the electronegativity difference that usually is the dividing line between covalentand ionic bonds?

a. 1.0 b. 1.7 c. 2.7 d. 4.0

11. The symbol �� is placed next to which of the following?

a. the less electronegative atom in a polar covalent bond c. a positive ion

b. the more electronegative atom in a polar covalent bond d. the nucleus

12. A nonpolar covalent bond is one in which

a. electrons are transferred. c. electrons are shared equally.

b. electrons are shared unequally. d. both electrons are provided by the same atom.

13. Molecules containing only polar covalent bonds

a. are always polar. c. are always ionic.

b. may or may not be polar. d. are always nonpolar.

14. What factor other than electronegativity determines whether a molecule as a whole ispolar or not?

a. temperature b. its geometry c. its physical state d. its mass

15. Which of the following correctly describes the compound water, H2O?

a. ionic c. polar overall, with nonpolar covalent bonds

b. nonpolar overall, with polar covalent bonds d. polar overall, with polar covalent bonds

16. Which of the following correctly describes the compound carbon tetrachloride, CCl4?

a. ionic c. polar overall, with nonpolar covalent bonds

b. nonpolar overall, with polar covalent bonds d. polar overall, with polar covalent bonds

17. A molecule of ammonia, NH3, is

a. nonpolar because it is linear.

b. polar because it is linear.

c. nonpolar because there is no electronegativity difference.

d. polar because there is an electronegativity difference and the molecule is trigonal pyramidal.



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Section 9.5 Electronegativity and PolarityIn your textbook, read about electronegativity.

Use the table of electronegativities below to answer the following questions.

1. What is the meaning of the term electronegativity?

the tendency of an atom to attract electrons

2. Which element has the highest electronegativity? What is the numerical value? What are thename and group number of the chemical family that has the highest overall electronegativities?

fluorine; 3.98; halogens; group 7A

3. Which element has the lowest electronegativity? What is the numerical value? What are thename and group number of the chemical family that has the lowest overall electronegativities?

francium; 0.7; alkali metals; group 1A

4. What general trend in electronegativity do you note going down a group? Across a period?

Electronegativity tends to decrease. Electronegativity tends to increase.

5. How are the electronegativity values used to determine the type of bond that existsbetween two atoms?

The values are subtracted.

In your textbook, read about the properties of covalent compounds.


6. Ionic compounds are usually soluble in polar substances.

7. In a covalent molecular compound, the attraction between molecules tendsto be strong.

false

true

Electronegativities of Some Elements

MetalMetalloidNonmetal

78Pt2.2

79Au2.4

80Hg1.9

81Tl

1.8

82Pb1.8

83Bi1.9

85At2.2

28Ni

1.91

29Cu

1.90

30Zn

1.65

31Ga

1.81

32Ge

2.01

33As

2.18

34Se

2.55

35Br

2.96

46Pd

2.20

47Ag

1.93

48Cd

1.69

49In

1.78

50Sn

1.96

51Sb

2.05

52Te2.1

53I

2.66

13Al

1.61

14Si

1.90

15P

2.19

16S

2.58

17Cl

3.16

5B

2.04

6C

2.55

7N

3.04

8O

3.44

9F

3.98

84Po2.0

1H

2.203Li

0.98

11Na

0.9319K

0.82

37Rb

0.82

55Cs

0.7987Fr0.7

88Ra0.9

89Ac1.1

56Ba

0.89

57La

1.10

72Hf1.3

73Ta1.5

74W1.7

75Re1.9

76Os2.2

77Ir

2.2

38Sr

0.95

39Y

1.22

40Zr

1.33

41Nb1.6

42Mo2.16

20Ca

1.00

21Sc

1.36

22Ti

1.54

23V

1.63

24Cr

1.66

43Tc

2.10

44Ru2.2

25Mn1.55

26Fe

1.83

27Co

1.88

45Rh

2.28

12Mg1.31

4Be

1.57


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