Question 1

An individual carbon-oxygen bond is polar. Yet carbon dioxide, CO2, which has two carbon-oxygen bonds, is nonpolar because

Accepted Answer

A) the molecule has an even number of electrons. 
B) it has a greater symmetry. 
C) the electron-pulls of the two oxygen atoms are equal and opposite. 
D) Two of the above are reasonable. 
A) the molecule has an even number of electrons. 
B) it has a greater symmetry. 
C) the electron-pulls of the two oxygen atoms are equal and opposite. 
D) Two of the above are reasonable.

Question 2

Which of the following molecules is the most polar?

Accepted Answer

A) HCl 
B) BrF 
C) CO 
D) Br2 
A) HCl 
B) BrF 
C) CO 
D) Br2

Question 3

What is a molecule?

Accepted Answer

A) a group of atoms that are held together by covalent bonds 
B) a group of atoms that are held together by ionic bonds 
C) pair of atoms sharing a set of valence electrons 
D) pair of shared valence electrons 
E) group of covalent compounds held together by ionic bonds 
A) a group of atoms that are held together by covalent bonds 
B) a group of atoms that are held together by ionic bonds 
C) pair of atoms sharing a set of valence electrons 
D) pair of shared valence electrons 
E) group of covalent compounds held together by ionic bonds

Question 4

Chlorine, Cl2, is a gas at room temperature, but bromine, Br2, is a liquid. Explain.

Accepted Answer

A) Chlorine atoms are larger and this makes the formation of induced dipole-induced dipole attractions more favorable. 
B) Bromine atoms are larger and this makes the formation of induced dipole-induced dipole attractions more favorable. 
C) The smaller chlorine molecules are able to pack together in a tighter physical orientation. 
D) The bromine ions are held together by ionic bonds. 
A) Chlorine atoms are larger and this makes the formation of induced dipole-induced dipole attractions more favorable. 
B) Bromine atoms are larger and this makes the formation of induced dipole-induced dipole attractions more favorable. 
C) The smaller chlorine molecules are able to pack together in a tighter physical orientation. 
D) The bromine ions are held together by ionic bonds.

Question 5

How many more electrons can fit within the valence shell of a hydrogen atom?

Accepted Answer

A) 1 
B) 2 
C) 7 
D) 0 
A) 1 
B) 2 
C) 7 
D) 0

Question 6

Which would you expect to have a higher melting point: sodium chloride, NaCl, or cesium chloride, CsCl? Why?

Accepted Answer

A) The cesium chloride has a higher melting point because larger ions of the same charge are able to attract more ions of the opposite charge. 
B) The cesium chloride has a higher melting point because its ions are smaller, which makes the charges more dense. 
C) The sodium chloride has a higher melting point because of the greater charges of the ions, and hence the greater force of attractions between them. 
D) The sodium chloride has a higher melting point because its ions are smaller, which allows oppositely charged ions to get closer. 
A) The cesium chloride has a higher melting point because larger ions of the same charge are able to attract more ions of the opposite charge. 
B) The cesium chloride has a higher melting point because its ions are smaller, which makes the charges more dense. 
C) The sodium chloride has a higher melting point because of the greater charges of the ions, and hence the greater force of attractions between them. 
D) The sodium chloride has a higher melting point because its ions are smaller, which allows oppositely charged ions to get closer.

Question 7

What molecule loses a proton to form the hydroxide ion, OH⁻?

Accepted Answer

A) The oxygen molecule, O2 
B) The water molecule, H2O 
C) The hydrogen peroxide molecule, H2O2 
D) The hydrogen molecule, H2 
A) The oxygen molecule, O2 
B) The water molecule, H2O 
C) The hydrogen peroxide molecule, H2O2 
D) The hydrogen molecule, H2

Question 8

If the concentration of gold in seawater is 2.0 milligram per ton of sea water and the mass of the ocean is 1.5 × 1018 tons, how much gold is in the ocean?

Accepted Answer

A) 3.0 × 1012 kg 
B) 3.0 kg 
C) 300 g 
D) 36 mg 
E) 3,000 lb 
A) 3.0 × 1012 kg 
B) 3.0 kg 
C) 300 g 
D) 36 mg 
E) 3,000 lb

Question 9

Which of the following molecules would you expect to be the most strongly attracted to a Cl- ion?

Accepted Answer

A) H-F 
B) H3C-CH3 
C) Cl-Cl 
D) F-F 
E) CCl4 
A) H-F 
B) H3C-CH3 
C) Cl-Cl 
D) F-F 
E) CCl4

Question 10

Which of the following has the greatest number of nonbonding pairs of electrons ?

Accepted Answer

A) C 
B) H 
C) He 
D) F 
E) S 
A) C 
B) H 
C) He 
D) F 
E) S

Question 11

The charges with sodium chloride are all balanced-for every positive sodium ion there is a corresponding negative chloride ion. Since its charges are balanced, how can sodium chloride be attracted to water, and vice versa?

Accepted Answer

A) Dispersion forces come into play as the sodium chloride and water come into close proximity. 
B) Hydrogen bonding in water allows the sodium chloride molecule to be attracted to the water molecule. 
C) As a water molecule gets close to the sodium chloride it can distinguish the various ions and it is thus attracted to an individual ion by ion-dipole forces. 
D) This is not a matter of attraction. Sodium chloride dissolves in water because water provides a medium in which the individual sodium and chloride ions can disperse. 
A) Dispersion forces come into play as the sodium chloride and water come into close proximity. 
B) Hydrogen bonding in water allows the sodium chloride molecule to be attracted to the water molecule. 
C) As a water molecule gets close to the sodium chloride it can distinguish the various ions and it is thus attracted to an individual ion by ion-dipole forces. 
D) This is not a matter of attraction. Sodium chloride dissolves in water because water provides a medium in which the individual sodium and chloride ions can disperse.

Question 12

If you mix a typical aluminum ion (Al, atomic no. = 13)with a typical oxygen ion (O, atomic no. = 8), what compound is formed?

Accepted Answer

A) Al2O3 
B) Al3O2 
C) Al13O8 
D) Al3O 
E) Al2O2 
A) Al2O3 
B) Al3O2 
C) Al13O8 
D) Al3O 
E) Al2O2

Question 13

Metals are often used for making designer jewelry because they

Accepted Answer

A) do not conduct heat well 
B) conduct electricity 
C) are shiny 
D) are strong but can be bent 
E) c and d 
A) do not conduct heat well 
B) conduct electricity 
C) are shiny 
D) are strong but can be bent 
E) c and d

Question 14

Which of the following best describes ionic bonding?

Accepted Answer

A) two atoms sharing a set of electrons 
B) two atoms exchanging a set of electrons 
C) one atom giving up some of its electrons to another atom 
D) when two elements with same charge are held together by electrostatic forces 
E) none of the above 
A) two atoms sharing a set of electrons 
B) two atoms exchanging a set of electrons 
C) one atom giving up some of its electrons to another atom 
D) when two elements with same charge are held together by electrostatic forces 
E) none of the above

Question 15

Which of the following substances contains F- ions?

Accepted Answer

A) PF3 
B) F2 
C) CF4 
D) CaF2 
E) all of the above 
A) PF3 
B) F2 
C) CF4 
D) CaF2 
E) all of the above

Question 16

A substance consisting of which molecule shown below should have a higher boiling point?

Accepted Answer

A) The molecule on the left, COCl2, because it has a fewer number of atoms. 
B) The molecule on the right, C2H2Cl, because it has a greater number of atoms. 
C) The molecule on the left, COCl2, because it is less symmetrical. 
D) The molecule on the right, C2H2Cl, because of electronegativity considerations. 
A) The molecule on the left, COCl2, because it has a fewer number of atoms. 
B) The molecule on the right, C2H2Cl, because it has a greater number of atoms. 
C) The molecule on the left, COCl2, because it is less symmetrical. 
D) The molecule on the right, C2H2Cl, because of electronegativity considerations.

Question 17

Why is calcium fluoride, CaF2, a high melting point crystalline solid while stannic chloride, SnCl4, is a volatile liquid?

Accepted Answer

A) There is no theory to predict the physical property of melting point. Melting point temperatures are empirically determined. 
B) Actually, we would predict these results to be the opposite. Since each metal is combined with a group 17 halogen, the heavier metal (tin)combination should have the higher melting point. 
C) CaF2 is a small, linear, non-polar molecule, while SnCl4 is a huge tetrahedral structure. Therefore the bonds in calcium fluoride tend to give it a higher melting point temperature. 
D) Ionic compounds formed by elements on opposite sides of the periodic table, like CaF2, tend to have higher melting points than more covalently bonded structures, like SnCl4. 
A) There is no theory to predict the physical property of melting point. Melting point temperatures are empirically determined. 
B) Actually, we would predict these results to be the opposite. Since each metal is combined with a group 17 halogen, the heavier metal (tin)combination should have the higher melting point. 
C) CaF2 is a small, linear, non-polar molecule, while SnCl4 is a huge tetrahedral structure. Therefore the bonds in calcium fluoride tend to give it a higher melting point temperature. 
D) Ionic compounds formed by elements on opposite sides of the periodic table, like CaF2, tend to have higher melting points than more covalently bonded structures, like SnCl4.

Question 18

Which of the following compounds contains ionic bonds?

Accepted Answer

A) CH4 
B) K2O 
C) Cl2 
D) OF2 
E) none of the above 
A) CH4 
B) K2O 
C) Cl2 
D) OF2 
E) none of the above

Question 19

How many covalent bonds would the following atom usually form?

Accepted Answer

A) 3 
B) 2 
C) 1 
D) 5 
E) would usually not form any covalent bonds 
A) 3 
B) 2 
C) 1 
D) 5 
E) would usually not form any covalent bonds

Question 20

What does the line in the following example actually represent? H-H

Accepted Answer

A) a shared pair of electrons 
B) a covalent bond 
C) an ionic bond 
D) a pair of nonbonding electrons 
E) A and B 
A) a shared pair of electrons 
B) a covalent bond 
C) an ionic bond 
D) a pair of nonbonding electrons 
E) A and B

Exam 15: How Atoms Bond and Molecules Attract

An individual carbon-oxygen bond is polar. Yet carbon dioxide, CO2, which has two carbon-oxygen bonds, is nonpolar because

Which of the following molecules is the most polar?

What is a molecule?

Chlorine, Cl2, is a gas at room temperature, but bromine, Br2, is a liquid. Explain.

How many more electrons can fit within the valence shell of a hydrogen atom?

Which would you expect to have a higher melting point: sodium chloride, NaCl, or cesium chloride, CsCl? Why?

What molecule loses a proton to form the hydroxide ion, OH⁻?

If the concentration of gold in seawater is 2.0 milligram per ton of sea water and the mass of the ocean is 1.5 × 1018 tons, how much gold is in the ocean?

Which of the following molecules would you expect to be the most strongly attracted to a Cl- ion?

Which of the following has the greatest number of nonbonding pairs of electrons ?

The charges with sodium chloride are all balanced-for every positive sodium ion there is a corresponding negative chloride ion. Since its charges are balanced, how can sodium chloride be attracted to water, and vice versa?

If you mix a typical aluminum ion (Al, atomic no. = 13)with a typical oxygen ion (O, atomic no. = 8), what compound is formed?

Metals are often used for making designer jewelry because they

Which of the following best describes ionic bonding?

Which of the following substances contains F- ions?

A substance consisting of which molecule shown below should have a higher boiling point?

Why is calcium fluoride, CaF2, a high melting point crystalline solid while stannic chloride, SnCl4, is a volatile liquid?

Which of the following compounds contains ionic bonds?

How many covalent bonds would the following atom usually form?

What does the line in the following example actually represent? H-H

Patterns of Motion and Equilibrium

Newtons Laws of Motion

Momentum and Energy

Gravity, Projectiles, and Satellites

Fluid Mechanics

Thermal Energy and Thermodynamics

Heat Transfer and Change of Phase

Static and Current Electricity

Magnetism and Electromagnetic Induction

Waves and Sound

Light

Atoms and the Periodic Table

The Atomic Nucleus and Radioactivity

Elements of Chemistry

Mixtures

How Chemicals React

Two Classes of Chemical Reactions

Organic Compounds

Rocks and Minerals

Plate Tectonics and Earths Interior

Shaping Earths Surface

Geologic Timereading the Rock Record

The Oceans, Atmosphere, and Climatic Effects

Driving Forces of Weather

The Solar System

Stars and Galaxies

The Structure of Space and Time

Prologue: the Nature of Science

Filters

An individual carbon-oxygen bond is polar. Yet carbon dioxide, CO₂, which has two carbon-oxygen bonds, is nonpolar because

Chlorine, Cl₂, is a gas at room temperature, but bromine, Br₂, is a liquid. Explain.

If the concentration of gold in seawater is 2.0 milligram per ton of sea water and the mass of the ocean is 1.5 × 10¹⁸ tons, how much gold is in the ocean?

Which of the following molecules would you expect to be the most strongly attracted to a Cl^- ion?

Which of the following substances contains F^- ions?

Why is calcium fluoride, CaF₂, a high melting point crystalline solid while stannic chloride, SnCl₄, is a volatile liquid?