Question 1

Which of the following elements will most likely form an ion with a -1 charge?

Accepted Answer

A) Na 
B) S 
C) Ne 
D) Mg 
E) Cl 
A) Na 
B) S 
C) Ne 
D) Mg 
E) Cl E

Question 2

Which of the following intermolecular forces best describes why molecules like sucrose (which has many OH groups)are very water soluble?

Accepted Answer

A) dipole-dipole 
B) induced dipole-induced dipole 
C) dipole-induced dipole 
D) ion-dipole 
E) hydrogen bonding 
A) dipole-dipole 
B) induced dipole-induced dipole 
C) dipole-induced dipole 
D) ion-dipole 
E) hydrogen bonding E

Question 3

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

Accepted Answer

A) the oxygen molecule, O2 
B) the water molecule, H2 O 
C) the hydrogen peroxide molecule, H2O2 
D) the hydrogen molecule, H2 
A) the oxygen molecule, O2 
B) the water molecule, H2 O 
C) the hydrogen peroxide molecule, H2O2 
D) the hydrogen molecule, H2 B

Question 4

Which of the following molecules should have the same molecular shape and approximate bond angles as ammonia,NH3 ?

Accepted Answer

A)  BH3 
B)  CH4 
C)  SO3 
D)  PH3 
E)  NO2 
A)  BH3 
B)  CH4 
C)  SO3 
D)  PH3 
E)  NO2

Question 5

Which of the following substances is pure?

Accepted Answer

A) an ionic compound consisting of sodium and chlorine ions 
B) a covalent compound consisting of one type of molecule 
C) an element 
D) all of the above 
E) none of the above 
A) an ionic compound consisting of sodium and chlorine ions 
B) a covalent compound consisting of one type of molecule 
C) an element 
D) all of the above 
E) none of the above

Question 6

How do the electron-dot structures of elements in the same group in the periodic table compare with one another?

Accepted Answer

A) The structures differ by exactly two electrons between vertically consecutive elements. 
B) The number of valence shell electrons increases by one for each element from the top to the bottom of the group. 
C) Elements of the same group have the same number of valence electrons. 
D) The number of electrons in the electron-dot-structure will equal the group number for each element of the group. 
A) The structures differ by exactly two electrons between vertically consecutive elements. 
B) The number of valence shell electrons increases by one for each element from the top to the bottom of the group. 
C) Elements of the same group have the same number of valence electrons. 
D) The number of electrons in the electron-dot-structure will equal the group number for each element of the group.

Question 7

Why is it so easy for a magnesium atom to lose two electrons?

Accepted Answer

A) The nuclear charge of the magnesium atoms is relatively weak. 
B) These two electrons are found relatively far from the nucleus. 
C) These two electrons are well shielded from the nuclear charge. 
D) There are lots of electron-electron repulsions that go on within the valence shell. 
A) The nuclear charge of the magnesium atoms is relatively weak. 
B) These two electrons are found relatively far from the nucleus. 
C) These two electrons are well shielded from the nuclear charge. 
D) There are lots of electron-electron repulsions that go on within the valence shell.

Question 8

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 9

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 10

MgCl2 crystals are composed of

Accepted Answer

A) units of MgCl2 molecules held together by dipole interactions. 
B) groups of Mg2+ ions and Cl2 molecules. 
C) units composed of six Mg atoms and six Cl21 molecules. 
D) a multitude of Mg2+ ions and Cl2 ions grouped together in a three-dimensional array with a 1:2 ratio of Mg2+ to Cl2 . 
E) a two-dimensional array of [-Mg-Cl-Cl-] units. 
A) units of MgCl2 molecules held together by dipole interactions. 
B) groups of Mg2+ ions and Cl2 molecules. 
C) units composed of six Mg atoms and six Cl21 molecules. 
D) a multitude of Mg2+ ions and Cl2 ions grouped together in a three-dimensional array with a 1:2 ratio of Mg2+ to Cl2 . 
E) a two-dimensional array of [-Mg-Cl-Cl-] units.

Question 11

Why is calcium fluoride,Ca $\mathrm { F } _ { 2 }$ ,a high melting point crystalline solid while stannic chloride, $\mathrm { SnCl } _ { 4 }$ ,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) Ca $\mathrm { F } _ { 2 }$ is a small,linear,non-polar molecule,while $\mathrm { SnCl } _ { 4 }$ 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 $\mathrm { CaF } _ { 2 }$ ,tend to have higher melting points than more covalently bonded structures,like $\mathrm { SnCl } _ { 4 }$ 
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) Ca $\mathrm { F } _ { 2 }$ is a small,linear,non-polar molecule,while $\mathrm { SnCl } _ { 4 }$ 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 $\mathrm { CaF } _ { 2 }$ ,tend to have higher melting points than more covalently bonded structures,like $\mathrm { SnCl } _ { 4 }$

Question 12

Which of the following intermolecular forces best describes why nonpolar molecules like gasoline (C8H18)have only limited solubility in water?

Accepted Answer

A) dipole-dipole 
B) induced dipole-induced dipole 
C) dipole-induced dipole 
D) ion-dipole 
E) Both A and B 
A) dipole-dipole 
B) induced dipole-induced dipole 
C) dipole-induced dipole 
D) ion-dipole 
E) Both A and B

Question 13

Why are the melting temperatures of most ionic compounds far greater than the melting temperatures of most covalent compounds?

Accepted Answer

A) Ionic bonds are so much stronger than the molecular attractions between covalently bonded compounds. 
B) Covalent bonds are not as strong as ionic bonds. 
C) As a solid,salts have a very organized crystalline structure which takes a lot of energy to break apart. 
D) Most covalent compounds have at least one weak bond in their structure that is easily broken when heat is added. 
A) Ionic bonds are so much stronger than the molecular attractions between covalently bonded compounds. 
B) Covalent bonds are not as strong as ionic bonds. 
C) As a solid,salts have a very organized crystalline structure which takes a lot of energy to break apart. 
D) Most covalent compounds have at least one weak bond in their structure that is easily broken when heat is added.

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

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

Question 16

Which of the following would have the lowest melting point?

Accepted Answer

A) CCl4 
B) CBr4 
C) CF4 
D) CI4 
E) not enough information given 
A) CCl4 
B) CBr4 
C) CF4 
D) CI4 
E) not enough information given

Question 17

Why is the surface area of a gecko's foot so extensive?

Accepted Answer

A) A gecko,like all amphibians,needs extensive surface area under foot for stability on land as well as mobility in water. 
B) A gecko's foot acts like a large dipole and thus allows for ion-dipole interaction in water. 
C) The greater the surface area the greater the number of induced dipole-induced dipole forces of attraction that can occur between the gecko's foot and the surface. 
D) The extensive surface area,once charged by the gecko's body,allows for the dipole-dipole attraction of every contact surface. 
A) A gecko,like all amphibians,needs extensive surface area under foot for stability on land as well as mobility in water. 
B) A gecko's foot acts like a large dipole and thus allows for ion-dipole interaction in water. 
C) The greater the surface area the greater the number of induced dipole-induced dipole forces of attraction that can occur between the gecko's foot and the surface. 
D) The extensive surface area,once charged by the gecko's body,allows for the dipole-dipole attraction of every contact surface.

Question 18

What property of metal atoms account for many of the observed bulk phenomena seen in metal samples?

Accepted Answer

A) Metal atoms easily lose one or more outer electrons. 
B) Metal atoms easily gain one or more outer electrons. 
C) Metals readily form ionic bonds. 
D) Metals readily form covalent bonds. 
E) none of the above 
A) Metal atoms easily lose one or more outer electrons. 
B) Metal atoms easily gain one or more outer electrons. 
C) Metals readily form ionic bonds. 
D) Metals readily form covalent bonds. 
E) none of the above

Question 19

What is the main difference between a dipole-dipole interaction and a dipole-induced dipole interaction?

Accepted Answer

A) Both are similar,but one involves a temporary dipole created by a permanent dipole. 
B) Dipole-dipole interactions are weaker because the dipoles are permanent. 
C) Dipole-induced dipole interactions are stronger because the induced dipoles can be formed at any time. 
D) Both are identical. 
E) none of the above 
A) Both are similar,but one involves a temporary dipole created by a permanent dipole. 
B) Dipole-dipole interactions are weaker because the dipoles are permanent. 
C) Dipole-induced dipole interactions are stronger because the induced dipoles can be formed at any time. 
D) Both are identical. 
E) none of the above

Question 20

How many nonbonding pairs of electrons are in the following molecule? H-H

Accepted Answer

A) 1 pair 
B) 6 pairs 
C) 0 pairs 
D) 8 pairs 
E) none of the above 
A) 1 pair 
B) 6 pairs 
C) 0 pairs 
D) 8 pairs 
E) none of the above

Exam 15: How Atoms Bond and Molecules Attract

Which of the following elements will most likely form an ion with a -1 charge?

Which of the following intermolecular forces best describes why molecules like sucrose (which has many OH groups)are very water soluble?

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

Which of the following molecules should have the same molecular shape and approximate bond angles as ammonia,NH3 ?

Which of the following substances is pure?

How do the electron-dot structures of elements in the same group in the periodic table compare with one another?

Why is it so easy for a magnesium atom to lose two electrons?

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

What is a molecule?

MgCl2 crystals are composed of

Why is calcium fluoride,Ca F2\mathrm { F } _ { 2 }F2​ ,a high melting point crystalline solid while stannic chloride, SnCl4\mathrm { SnCl } _ { 4 }SnCl4​ ,is a volatile liquid?

Which of the following intermolecular forces best describes why nonpolar molecules like gasoline (C8H18)have only limited solubility in water?

Why are the melting temperatures of most ionic compounds far greater than the melting temperatures of most covalent compounds?

Which of the following best describes ionic bonding?

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

Which of the following would have the lowest melting point?

Why is the surface area of a gecko's foot so extensive?

What property of metal atoms account for many of the observed bulk phenomena seen in metal samples?

What is the main difference between a dipole-dipole interaction and a dipole-induced dipole interaction?

How many nonbonding pairs of electrons are in the following molecule? 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 Time - Reading 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

Which of the following molecules should have the same molecular shape and approximate bond angles as ammonia,NH₃ ?

MgCl₂ crystals are composed of

Why is calcium fluoride,Ca $\mathrm { F } _ { 2 }$ ,a high melting point crystalline solid while stannic chloride, $\mathrm { SnCl } _ { 4 }$ ,is a volatile liquid?

Which of the following intermolecular forces best describes why nonpolar molecules like gasoline (C₈H₁₈)have only limited solubility in water?