Chapter10 Chemical Bonding and Intermolecular Forces
Review—10.1 Covalent bonds
1.Match each label with the appropriate term. Note: there may be more than one correct answer.
nonbonding electrons
nonbonding electrons
a
b
single bond
single bond
represents two electrons
represents core electrons
nonbonding electrons
c
bonding electrons
single bond
2.Lewis structures cannot
A.show the number of valence electrons.
B.show the location of bonds.
C.show the strength of bonds.
D.show how many bonds are present in a molecule.
3.How many valence electrons are available for bonding in bromine (Br)?
A.one
B.two
C.five
D.seven
4.Which element has the fewest valence electrons available for bonding?
A.iodine B.aluminum C.carbon D.nitrogen
5.How many valence electrons are available for bonding in silicon?
A.four
B.five
C.eight
D.fourteen
6.Which type of bond will form between two chlorine atoms?
A.an ionic bond
B.a metallic bond
C.a polar covalent bond
D.a nonpolar covalent bond
7.Which pair of elements will form a covalent bond?
A.hydrogen and chlorine
B.sodium and chlorine
C.copper and bromine
.zinc and bromine
8.Which structure shows the correct electron arrangement in CCl4?
A
B
C
D
9.Based on its location in the periodic table, what can most likely be predicted about sulfur?
A.It has four valence electrons available for bonding.
B.It has four nonbonding electrons.
C.It has six valence electrons available for bonding.
D.It has six nonbonding electrons.
10.Which compound most likely contains polar covalent bonds?
A.NaCl
B.AlF3
C.Br2
D.NF3
11.Which of the following do Lewis structures help us understand?
A.the exact structure of a molecule
B.the number of electrons that are involved in the bonding of the molecule
C.the total number of electrons in a molecule
D.how electrons attract other electrons in a molecule
12.In this model of a molecule of ammonia, NH3, how many covalent
bonds are represented?
A.1 covalent bond
B.2 covalent bonds
C.3 covalent bonds
D.4 covalent bonds
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Review——10.2
Types of Chemical bonds
1.Sodium chloride is made up of clear, colorless crystals. A solution of sodium chloride in water is a
good conductor of electricity. Which statement describes sodium chloride?
A.It is made up of ions that are held together by ionic bonds.
B.It is made up of atoms that are held together by metallic bonds.
C.It is made up of atoms that are held together by covalent bonds with equal sharing of electrons.
D.It is made up of atoms that are held together by covalent bonds with unequal sharing of electrons.
2.Which of these is a typical property of a substance that is composed of atoms that are held together
by covalent bonds?
A.It conducts electricity when in solid form.
B.It conducts electricity when in molten form.
C.It conducts electricity when it is dissolved in water.
D.It does not conduct electricity in any form.
3.Which of these is a property of a substance that is composed of atoms that are held together by
metallic bonds?
A.It has a low melting point.
B.It can be flattened and bent.
C.It cannot be shaped into wires.
D.It does not conduct electricity.
4.Sugar is made up of clear, colorless crystals that dissolve easily in water, but the crystals and their
solution do not conduct electricity. Which statement describes sugar?
A.It is made up of atoms that are held together by metallic bonds.
B.It is made up of atoms that are held together by covalent bonds.
C.It is made up of atoms that are held together by weak ionic bonds.
D.It is made up of atoms that are held together by strong ionic bonds.
5.Which interaction is responsible for the force of attraction between the particles in a salt crystal?
A.proton-proton
B.proton-electron C.neutron-electron
D.electron-electron
6.The table below shows the electronegativity values of various elements on the periodic table.
Electronegativities
Which pair of elements would form an ionic bond?
A．carbon (C) and oxygen (O)
B.strontium (Sr) and chlorine (Cl)
C.cesium (Cs) and germanium (Ge)
D.magnesium (Mg) and aluminum (Al)
7.Which type of atom has the strongest attraction for electrons in bond formation?
A. barium (Ba)
B.chlorine (Cl)
C.iodine (I) D.strontium (Sr)
8.Consider the positions of barium (Ba), sulfur (S), silicon (Si), and calcium (Ca) on the periodic
table. The atoms of which element require the least amount of energy to give up an electron when
forming chemical bonds?
A.barium
B．sulfur
C.silicon
D.calcium
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9.Consider the positions of carbon, nitrogen, potassium, and calcium on the periodic table. The atoms
of which element attract electrons most strongly in chemical bonds?
A.carbon (C) B.calcium (Ca) C.nitrogen (N) D.potassium (K)
10.Which statement describes how the bond between two oxygen atoms is formed?
A.by sharing valence electrons with many other atoms
B.by the repulsion between ions of like charges
C.by the attraction of two oppositely charged ions
D. by sharing valence electrons between the two atoms
11.Which type of substances have chemical bonds that are not directional and valence electrons that
move freely between the atoms?
A. halogens
B. nonmetals
C. metals
D.salts
12.What will most likely happen when two bromine atoms bond together?
A.The atoms will become less stable.
B.An ionic bond will hold them together.
C.A covalent bond will hold them together.
D.A metallic bond will hold them together.
13.Which statement explains why the bonds between nonmetals tend to be covalent?
A.The bonds are found to be nondirectional. B.They have large differences in electronegativity.
C.They have small differences in electronegativity.
D.They have ions that produce an electrostatic pull.
14.Which statement is generally true about CaCl2?
A.It has only metallic bonds between the atoms. B.It has only covalent bonds between the atoms.
C.Its bonds are formed by large differences in electronegativity.
D.Its bonds are formed by small differences in electronegativity.
15.The incomplete table below shows selected properties of compounds that have ionic, covalent, or
metallic bonds.
Row
1
Bond
Ionic
Electrical conductivity
Yes
Likely property
High melting point
2
3
?
?
Yes
No
?
?
Which information would best fill the blanks in row 3?
A.metallic bond and low melting point
B.metallic bond and high melting point
C.covalent bond and low melting point
D.covalent bond and high melting point
16.Which statement describes the valence electrons in ionic bonds?
A.They are shared equally between two atoms.
B.They are shared unequally between two atoms.
C.They are shared among many atoms.
D.They are transferred from one atom to another.
17.How is electronegativity related to covalent bonding?
A.Atoms must have similar electronegativities in order to share electrons in a covalent bond.
B.Atoms must have very different electronegativities in order to transfer electrons in a covalent bond.
C.Atoms must have similar electronegativities in order to transfer electrons in a covalent bond.
D.Atoms must have very different electronegativities in order to share electrons in a covalent bond.
18.Which statement best explains why a metal atom and a nonmetal atom are most likely to form an
ionic bond?
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A.Metal atoms have low ionization energy, and nonmetal atoms have high electronegativity, so
electrons transfer easily from the nonmetal atom to the metal atom.
B.Metal atoms have low ionization energy, and nonmetal atoms have high electronegativity, so
electrons transfer easily from the metal atom to the nonmetal atom.
C.Metal atoms have high ionization energy, and nonmetal atoms have low electronegativity, so
electrons transfer easily from the nonmetal atom to the metal atom.
D.Metal atoms have high ionization energy, and nonmetal atoms have low electronegativity, so
electrons transfer easily from the metal atom to the nonmetal atom.
19.Which type of bonding involves the complete transfer of a valence electron from a less
electronegative atom to a more electronegative one?
A.ionic bonding
B.metallic bonding
C.covalent bonding
D.hydrogen bonding
20.Which element has the lowest ionization energy?
A.argon (Ar)
B.bromine (Br)
C.cesium (Cs)
D.nickel (Ni)
21.Which statement describes the valence electrons in metallic bonds?
A.They are shared equally between two atoms.
B. They are shared unequally between two atoms.
C.They are shared among many atoms.
D.They are transferred from one atom to another.
22.A substance conducts an electric current when it is in the liquid state. What would the
conductivity of the substance in solid form indicate about the type of bond in the substance?
A.If the solid is conductive, the bonds are ionic.
B. If the solid is not conductive, the bonds are covalent.
C. If the solid is conductive, the bonds are metallic.
D.If the solid is not conductive, the bonds are metallic.
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Reviwe——10.3
Ionic bonds
1.Which statement is true about ionic compounds?
A.Solid ionic compounds are good conductors of electricity.
B.Ionic compounds have varying solubilities in water.
C.Ionic compounds have very low melting points.
D.Ionic compounds are very easy to bend.
2.Which compound has the highest melting point?
A.Al2(CO3)3
B.C12H22O11
C.C8H18
D.H2O
3.Which of the following compounds would be expected to have the strongest ionic bonds?
A.the compound that has the largest ions with the greatest charge
B.the compound that has the largest ions with the least charge
C.the compound that has the smallest ions with the greatest charge
D.the compound that has the smallest ions with the least charge
4.How do ionic bonds affect the properties of ionic compounds?
A.The bonds weakly hold ions together, increasing the melting point.
B.The bonds strongly hold ions together, reducing the boiling point.
C.The bonds prevent ions from moving throughout the crystal, so a solid ionic compound is a poor
conductor.
D.The bonds prevent electrons from moving throughout the crystal, so a solid ionic compound is a
poor conductor.
6.Which of the following best describes a pair of elements that will form an ionic bond?
A.C and H: Hydrogen easily loses electrons, and carbon gains them.
B.Li and O: Oxygen easily loses electrons, and lithium gains them.
C.P and Cl: Phosphorus easily loses electrons, and chlorine gains them.
D.Ca and Br: Calcium easily loses electrons, and bromine gains them.
7.Which of these best describes an ionic bond?
A.a force that keeps two large molecules together
B.an attraction that occurs between two nonmetals
C.a force that holds two oppositely charged ions together
D.an electromagnetic attraction that occurs between two metals
8.Which statement describes a step in the formation of an ionic bond?
A.An attraction occurs between two ions that have the same charge.
B.A metal atom forms a cation, and a nonmetal atom forms an anion.
C.A more electronegative atom transfers electrons to a less electronegative atom.
D.A metal pulls electrons from another metal and produces a force of attraction.
9.Which statement is true about ionic compounds?
A.They are made up of many large molecules that are bonded together.
B.They are made up of atoms of only one type of element.
C.They are made up of particles that are arranged in a repeating pattern.
D.They are made up of a random ratio of elements that are bonded together.
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10.The diagram below shows the atoms involved in forming table salt.Which
statement best describes what happens next?
A.Sodium becomes an anion by losing an electron to chlorine.
B.Chlorine becomes a cation by losing an electron to sodium.
C.Sodium becomes a cation by gaining an electron from chlorine.
D.Chlorine becomes an anion by gaining an electron from sodium.
11.Which pair of elements will form an ionic bond?
A.N and O
B.K and Br
C.C and Cl
D.Fe and Ni
12.Which pair of ions can form an ionic bond with each other and why?
A.Cu+ and Ag+; They are both metal ions.
B.S2- and O2-; They have like charges.
C.Br- and At-; They are both halogen ions.
D.Li+ and Br-; They have unlike charges.
13.Each model shows bonding between a pair of atoms.
Model A
Model B
Which statement best explains how the models differ?
A.Model A shows the formation of ions, and model B does not show the formation of ions.
B.Model A does not show the formation of ions, and model B shows the sharing of electrons.
C.Model A shows the sharing of electrons, and model B shows the formation of ions.
D.Model A shows the transfer of an electron, and model B shows the sharing of electrons.
14.Which statement indicates that a substance may be an ionic compound?
A.It has a low melting point.
B．It is made up of molecules.
C.It can be flattened by a force.
D.It is made up of a crystal lattice.
15.Which statement is true about a polyatomic ion?
A.It forms metallic bonds with other ions.
B.It forms covalent bonds with other ions.
C.It is made of atoms that are covalently bonded together.
D.It has a charge that is distributed over part of the entire unit.
16.What leads to the formation of an ionic bond with Hg22+?
A.the attraction of a noble gas
B.the attraction of an NH4+ ion
C.the attraction of a group 1 element
D.the attraction of an SO42– ion
17.Which chemical species can easily form an ionic bond with a cation?
A.Sr
B.Ne
C.NH4+
D.PO43–
19.Which property best indicates that a compound contains an ionic bond?
A.It is insoluble in water.
B.It can be easily flattened.
C.It has a low boiling point. D.It conducts electricity when molten.
20.Which statement best describes how an ionic bond forms?
A.The transfer of electrons forms strong bonds between ions.
B.The sharing of electrons forms strong bonds between ions.
C.The transfer of electrons results in attractive forces between molecules.
D.The sharing of electrons results in attractive forces between molecules.
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22.Which statement correctly describes the phosphate ion, PO43-?
A.It is composed of one phosphorus atom and four oxygen atoms covalently bonded together, and
there is a –3 charge distributed over the entire ion.
B.It is composed of one phosphorus atom and four oxygen atoms covalently bonded together, and
there is a –3 charge on the phosphorus atom.
C.It is composed of one phosphorus atom and four oxygen atoms ionically bonded together, and there
is a –3 charge distributed over the entire ion.
D.It is composed of one phosphorus atom and four oxygen atoms ionically bonded together, and there
is a –3 charge on the phosphorus atom.
23.Which best describes why NH4+ can form an ionic bond with Cl–?
A.Its outermost shell gains one or more electrons from Cl–.
B.Its positive charge is attracted to the negative charge of Cl–.
C. It has a negative charge that is spread over the entire ion.
D. It has a nitrogen atom that is strongly attracted to Cl–.
25.Which describes a step in the process of forming an ionic bond?
A.A metal atom loses electrons and becomes a positive ion.
B.A metal atom gains electrons and becomes a negative ion.
C.A nonmetal atom loses electrons and becomes a negative ion.
D.A nonmetal atom gains electrons and becomes a positive ion.
26.What is a three-dimensional structure that represents the alternating pattern of particles in a
crystal?
A.a polyatomic ion
B.a crystal lattice
C.an ionic bond
D.a formula unit
27.What ion will be formed by the selenium atom shown below when it has a stable set
of valence electrons?
A.Se6+
B.Se2+
C.Se6−
D.Se2−
28.Which of the following is the best description of how electrons are transferred in an ionic bond?
A.A metal atom loses electrons and a nonmetal atom gains electrons.
B.A metal atom gains electrons and a nonmetal atom loses electrons.
C.A metal and a nonmetal atom lose electrons.
D.A metal and a nonmetal atom gain electrons.
29.A user is constructing an ionic bond between beryllium and chlorine and has reached the stage
below. What should the user do next to make the chlorine atom stable?
A.Transfer an electron from the beryllium atom to the chlorine atom.
B.Transfer an electron from the chlorine atom to the beryllium atom.
C.Add another beryllium atom.
D.Add another chlorine atom.
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Quiz—Covalent bond
1.An element has six valence electrons available for bonding. Which group of the periodic table does
this element most likely belong to?
A.group 2
B.group 4
C.group 16
D.group 18
2.Based on its location in the periodic table, what can most likely be predicted about phosphorus?
A.It has three valence electrons available for bonding.
B.It has three nonbonding electrons.
C.It has five valence electrons available for bonding.
D.It has five nonbonding electrons.
3.An element has five valence electrons available for bonding. This element is most likely which of
the following?
A.boron B.phosphorus C.tin
D.tellurium
4.Which compound contains only nonpolar covalent bonds?
A.O2
B.CO2
C.H2O
D.NO2
5.A solid compound in a sealed container was kept at a very low temperature in a freezer. When
placed at room temperature, the substance quickly turned into a liquid. This compound is most
likely which of the following?
A.an ionic compound because it has a low boiling point
B.a covalent compound because it has a low boiling point
C.an ionic compound because it has a low melting point
D.a covalent compound because it has a low melting point
6.Which statement about covalent compounds is true?
A.They are able to melt at high temperatures.
B.They are poor conductors of heat.
C.They have strong intermolecular attractions.
D.They have atomic bonds that are easy to break.
7.What is the best reason for the difference in properties of LiCl and C6H14O?
A.LiCl and C6H14O have different atomic masses.
B.Cl and O belong to different groups of the periodic table.
C.One compound is ionic, and the other is metallic.
D.One compound is covalent, and the other is ionic.
8.The image below shows two nitrogen atoms. For these two atoms to
form a stable molecule, N2, how many electrons would have to be part
of covalent bonds?
A.0 electrons
B.2 electrons
C.4 electrons
D.6 electrons
9.How many covalent bonds are there in one molecule of silica, SiO2?
A.0 covalent bonds
B.2 covalent bonds
C.4 covalent bonds
10.Explain what is wrong with the following structure.
D.6 covalent bonds
11.Use the periodic table to identify the number of valence electrons available for bonding for each of
the following elements and write Lewis Structures for these elements
O：
N：
Na：
I：
Si：
Mg：
8
B:
Reviwes——10.4
Lewis Structures and
Molecular Geometry
For each of the following molecules: (1) draw the Lewis Structure, (2) use VSEPR theory to determine
the shape and bond angle, (3) sketch the molecule and label each dipole moment (
), and (4) state
whether the molecule is polar or nonpolar.
Molecule
Lewis Structure
Molecular Shape
& Bond Angle
1. AsH3
2. BF3
3. BeBr2
4. SCl2
5. CHCl3
6. PCl3
7. SF6
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Sketch
Molecular
Polarity
Reviews-10.5
Intermolecular Forces
1.Among the intermolecular forces, which forces are typically the weakest?
A.dipole-dipole interactions B.hydrogen bonds
C.dipole-induced dipole interactions
D.London dispersion forces
2.The diagram below shows DNA molecules.
What do the broken lines connected to hydrogen atoms represent in this diagram?
A.the weakest intermolecular forces
B.the weakest intramolecular forces
C.the strongest intermolecular forces
D.the strongest intramolecular forces
3.When applied to a dish, soap makes grease soluble in water. Which explanation correctly supports
the role of intermolecular forces in this common observation?
A.The nonpolar end of a soap molecule attaches itself to grease.
B.The nonpolar end of a soap molecule attaches itself to water.
C.The polar soap molecule attaches itself to the dish.
D.The polar soap molecule attaches itself to a nonpolar soap molecule.
4.Which statement best describes London dispersion forces?
A.repulsive intramolecular forces
B.attractive intramolecular forces
C.repulsive intermolecular forces
D.attractive intermolecular forces
5.In the molecules below, areas that have a partial negative charge
are pink and areas that have a partial positive charge are blue.The
attractive force between these two molecules has most likely been
produced by
A.covalent bonds.
B.dipole-dipole interactions.
C.dipole-induced dipole interactions.
D.London dispersion forces.
6.When chemists convert ethene (C2H2) to ethanol (CH3CH2OH), they have a mixture of the two
gaseous substances. Why do chemists then lower the temperature of the mixture?
A.to collect liquid ethene and leave ethanol as a gas because ethene has stronger dipole-dipole forces
B.to collect liquid ethene and leave ethanol as a gas because ethanol has stronger London dispersion
forces
C.to collect liquid ethanol and leave ethene as a gas because ethanol has hydrogen bonds
D.to collect liquid ethanol and leave ethene as a gas because ethene has stronger London dispersion
forces
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7.Which forces can be classified as intramolecular?
A.London dispersion forces
B.van der Waals forces
C.hydrogen bonds
D.covalent bonds
8.Which interaction produces dispersive forces by creating temporary dipoles that induce dipoles in
other molecules?
A.dipole-dipole
B.hydrogen bonds
C.dipole-induced dipole
D.induced dipole-induced dipole
9.When a polar molecule causes a charge redistribution in a nonpolar molecule, what are the
molecules of the mixture most likely experiencing?
A.dipole-dipole interactions
B.nonpolar-nonpolar interactions
C.dipole-induced dipole interactions D.induced dipole-induced dipole interactions
10.van der Waals forces can best be described as the attractive or repulsive forces that are formed
A.between oppositely charged ions in a crystal.
B.during dipole-dipole interactions between molecules.
C.when molecules move apart in the absence of other forces.
D.by a random, short-lived redistribution of electrons.
11.In the molecule on the left, areas that have a partial negative charge are pink and areas that have a
partial positive charge are blue. The molecule on the right is nonpolar.
What will most likely happen when these molecules get closer?
A.The molecules will repel each other because of a dipole-dipole
interaction.
B.The molecules will attract each other because of a dipole-dipole
interaction.
C.An induced dipole will be produced in the molecule on the right.
D.An induced dipole will be produced in the molecule on the left.
12.In the figure below, two nonpolar molecules are interacting.Which interaction would most
likely cause these molecules to repel each other?
A.hydrogen bonding
B.dipole-dipole interaction
C.dipole-induced dipole interaction
D.induced dipole-induced dipole interaction
13.Hydrogen bonding is necessary for
A.bonding carbon to oxygen.
B.forming double-stranded DNA molecules.
C.decreasing the boiling point of liquids such as water.
D.causing van der Waals interactions.
14.Are hydrogen bonds formed between all molecules?
A.No because hydrogen can only form these bonds with oxygen atoms.
B.No because hydrogen can only form these bonds with highly electronegative atoms.
C.Yes because hydrogen can easily form bonds with atoms that have a neutral charge.
D.Yes because hydrogen can form these bonds with weakly electronegative atoms.
15.Which of the following most likely requires intermolecular forces?
A.a spider walking on the bottom of a leaf
B.a rock maintaining its solid shape
C.a koala using claws to hold onto a tree
D.a piece of fruit falling from a branch to the ground
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16.Which statement best explains why water has a higher boiling point than ethane?
A.Ethane molecules are smaller than water and can move faster.
B.Water molecules need relatively less heat energy to move.
C.Water molecules form hydrogen bonds, which cannot be broken by heating water.
D.Ethane molecules have no hydrogen bonds and need less energy to separate.
17.Which statement about van der Waals forces is true?
A.When the forces are weaker, a substance will have higher volatility.
B.When the forces are stronger, a substance will have lower viscosity.
C.When the forces are weaker, the boiling point of a substance will be higher.
D.When the forces are stronger, the melting point of a substance will be lower.
18.ICl has a higher boiling point than Br2. What is the best explanation for this?
A.Br2 experiences dipole-dipole interactions.
B.ICl experiences dipole-dipole interactions.
C.Br2 forms hydrogen bonds.
D.ICl experiences induced dipole-induced dipole interactions.
20.In comparison to molecules that interact by London dispersion forces only, the melting point of
similar-sized molecules forming hydrogen bonds would most likely be
A.about the same. B.unpredictable.
C.lower.
D.higher.
21.Which forces involve nonpolar molecules?
A.hydrogen bonds and London dispersion forces
B.London dispersion forces and dipole-induced dipole forces
C.dipole-dipole forces and hydrogen bonds
D.dipole-induced dipole forces and dipole-dipole forces
22.Ming has two unknown substances. One is nonpolar, and the other is polar.
Which process would most likely help Ming identify which substance is polar and which is
nonpolar?
A.Test the boiling points. The polar substance should have a lower boiling point because of its dipoledipole forces.
B.Test for an odor. The nonpolar substance should have a higher volatility and stronger odor because
of its London dispersion forces.
C.Test the boiling points. The nonpolar substance should have a higher boiling point because of its
hydrogen bonds.
D.Test for an odor. The polar substance should have a higher volatility and weaker odor because of
its dipole-dipole forces.
23. The water molecules are attracted to each other by
A.ionic bonds.
B.hydrogen bonds.
C.London dispersion forces.
D.dipole-induced dipole interactions.
24.Which statement about hydrogen bonds is true?
A.They are the only force that allows a gecko to climb up glass.
B.They are the weakest of the intermolecular forces.
C.They are much stronger than intramolecular forces.
D.They help water striders walk on water by creating surface tension.
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