Question 1

How many valence electrons does gallium (Ga, atomic no. = 31)have?

Accepted Answer

A) 1 
B) 6 
C) 3 
D) 31 
E) 70 
A) 1 
B) 6 
C) 3 
D) 31 
E) 70

Question 2

Does an ionic bond have a dipole?

Accepted Answer

A) No, dipoles are only found in covalent compounds. 
B) No, but the electrical charges are relatively strong. 
C) Yes, the ionic bond is an example of a very strong dipole. 
D) Yes, but for ionic compounds they are referred to as monopoles. 
A) No, dipoles are only found in covalent compounds. 
B) No, but the electrical charges are relatively strong. 
C) Yes, the ionic bond is an example of a very strong dipole. 
D) Yes, but for ionic compounds they are referred to as monopoles.

Question 3

Given the following diagram, describe what happens electronically between these two molecules.

Accepted Answer

A) Oxygen A becomes slightly positively charged due to the protons on the water molecule. 
B) Oxygen B becomes slightly positively charged due to the protons on the water molecule. 
C) Oxygen A becomes slightly negatively charged due to the oxygen molecule. 
D) Hydrogens on oxygen W becomes slightly positively charged due to the oxygen molecule. 
E) none of the above 
A) Oxygen A becomes slightly positively charged due to the protons on the water molecule. 
B) Oxygen B becomes slightly positively charged due to the protons on the water molecule. 
C) Oxygen A becomes slightly negatively charged due to the oxygen molecule. 
D) Hydrogens on oxygen W becomes slightly positively charged due to the oxygen molecule. 
E) none of the above

Question 4

Which of the following would have the smallest number of induced dipole-induced dipole interactions?

Accepted Answer

A) C6H14 
B) C8H18 
C) C10H22 
D) C12H26 
E) not enough information given 
A) C6H14 
B) C8H18 
C) C10H22 
D) C12H26 
E) not enough information given

Question 5

How are oxygen molecules attracted to water molecules?

Accepted Answer

A) The attraction between oxygen and water molecules is a classic example of dipole-dipole interaction. 
B) The hydrogen bonding in water causes the attraction of the oxygen atoms in the O2 molecule to water. 
C) As a water molecule is brought close to an oxygen molecule an induced dipole results in the O2 molecule causing the attraction. 
D) The attraction of oxygen and water molecules for one another is part of the common atom effect. Since both molecules contain oxygen, there is a built-in attraction. 
A) The attraction between oxygen and water molecules is a classic example of dipole-dipole interaction. 
B) The hydrogen bonding in water causes the attraction of the oxygen atoms in the O2 molecule to water. 
C) As a water molecule is brought close to an oxygen molecule an induced dipole results in the O2 molecule causing the attraction. 
D) The attraction of oxygen and water molecules for one another is part of the common atom effect. Since both molecules contain oxygen, there is a built-in attraction.

Question 6

Which of the following would have the highest boiling point?

Accepted Answer

A) C6H14 
B) C8H18 
C) C10H22 
D) C12H26 
E) not enough information given 
A) C6H14 
B) C8H18 
C) C10H22 
D) C12H26 
E) not enough information given

Question 7

Which of the following compounds has polar covalent bonds?

Accepted Answer

A) H2O 
B) CsF2 
C) S8 
D) Ne 
E) CH4 
A) H2O 
B) CsF2 
C) S8 
D) Ne 
E) CH4

Question 8

What is happening at the molecular level when a polar molecule like water interacts with a typical sodium ion?

Accepted Answer

A) The water molecule aligns such that the oxygen interacts with the sodium. 
B) The water molecule aligns such that the hydrogens interact with the sodium. 
C) The polarity of the water molecule is altered making the oxygen more positively charged. 
D) The polarity of the water molecule is altered making the hydrogens more negatively charged. 
E) none of the above 
A) The water molecule aligns such that the oxygen interacts with the sodium. 
B) The water molecule aligns such that the hydrogens interact with the sodium. 
C) The polarity of the water molecule is altered making the oxygen more positively charged. 
D) The polarity of the water molecule is altered making the hydrogens more negatively charged. 
E) none of the above

Question 9

If carbonic acid (H2CO3)were to undergo ionization, what would one of the products be?

Accepted Answer

A) H- 
B) CO2 
C) H2O 
D) CO3-1 
E) CO3-2 
A) H- 
B) CO2 
C) H2O 
D) CO3-1 
E) CO3-2

Question 10

Which of the following elements has two valence electrons?

Accepted Answer

A) Na 
B) Mg 
C) H 
D) Ne 
E) Li 
A) Na 
B) Mg 
C) H 
D) Ne 
E) Li

Question 11

Which of the following would be an ion with a double positive charge?

Accepted Answer

A) an Mg atom that gains two electrons 
B) an Mg atom that gains one electron 
C) an Mg atom that loses two electrons 
D) an Mg atom that loses one electron 
E) none of the above 
A) an Mg atom that gains two electrons 
B) an Mg atom that gains one electron 
C) an Mg atom that loses two electrons 
D) an Mg atom that loses one electron 
E) none of the above

Question 12

How is the number of unpaired valence electrons in an atom related to the number of bonds that the atom can form?

Accepted Answer

A) There is no defined relationship between the number of unpaired valence electrons and number of bonds that the atom can form. 
B) The number of unpaired valence electrons in an atom is one-half the number of bonds that the atom can form. 
C) The number of unpaired valence electrons in an atom is twice the number of bonds that the atom can form. 
D) The number of unpaired valence electrons in an atom is the same as the number of bonds that the atom can form. 
A) There is no defined relationship between the number of unpaired valence electrons and number of bonds that the atom can form. 
B) The number of unpaired valence electrons in an atom is one-half the number of bonds that the atom can form. 
C) The number of unpaired valence electrons in an atom is twice the number of bonds that the atom can form. 
D) The number of unpaired valence electrons in an atom is the same as the number of bonds that the atom can form.

Question 13

Which of the following statements describes a polar molecule?

Accepted Answer

A) The electrons in the molecule are distributed evenly throughout the molecule. 
B) The molecules are usually not attracted to one another very strongly. 
C) Polar molecules have the weakest intermolecular interactions with ionic compounds. 
D) The molecules have a high degree of symmetry. 
E) None of these statements describe polar molecules. 
A) The electrons in the molecule are distributed evenly throughout the molecule. 
B) The molecules are usually not attracted to one another very strongly. 
C) Polar molecules have the weakest intermolecular interactions with ionic compounds. 
D) The molecules have a high degree of symmetry. 
E) None of these statements describe polar molecules.

Question 14

Which bond is most polar?

Accepted Answer

A) H-N 
B) N-C 
C) C-C 
D) O-H 
A) H-N 
B) N-C 
C) C-C 
D) O-H

Question 15

What is the valence shell?

Accepted Answer

A) It is the outermost shell of electrons in an atom. 
B) It is the shell of electrons in an atom that is the least reactive. 
C) It is the last partially filled orbital in an atom. 
D) It is the shell of electrons in element V (atomic no. = 23) 
E) It is the same as the orbital configuration. 
A) It is the outermost shell of electrons in an atom. 
B) It is the shell of electrons in an atom that is the least reactive. 
C) It is the last partially filled orbital in an atom. 
D) It is the shell of electrons in element V (atomic no. = 23) 
E) It is the same as the orbital configuration.

Question 16

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 17

Which of the following describes how a metal atoms behaves in a bulk metallic object?

Accepted Answer

A) The metal ion shares its outermost electrons freely with its neighbors. 
B) The metal atoms have limited interaction with neighboring atoms. 
C) The metal atom shares its electrons in a very directional manner. 
D) The metal atom shares its electrons with only one other atom. 
E) none of the above 
A) The metal ion shares its outermost electrons freely with its neighbors. 
B) The metal atoms have limited interaction with neighboring atoms. 
C) The metal atom shares its electrons in a very directional manner. 
D) The metal atom shares its electrons with only one other atom. 
E) none of the above

Question 18

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 19

How many valence electrons does bromine (Br, atomic no. = 35)have?

Accepted Answer

A) 1 
B) 7 
C) 21 
D) 28 
E) 35 
A) 1 
B) 7 
C) 21 
D) 28 
E) 35

Question 20

If a neutral atom loses one electron, what is the electrical charge of the atom?

Accepted Answer

A) -1 
B) +1 
C) -2 
D) +2 
E) neutral 
A) -1 
B) +1 
C) -2 
D) +2 
E) neutral

Exam 15: How Atoms Bond and Molecules Attract

How many valence electrons does gallium (Ga, atomic no. = 31)have?

Does an ionic bond have a dipole?

Given the following diagram, describe what happens electronically between these two molecules.

Which of the following would have the smallest number of induced dipole-induced dipole interactions?

How are oxygen molecules attracted to water molecules?

Which of the following would have the highest boiling point?

Which of the following compounds has polar covalent bonds?

What is happening at the molecular level when a polar molecule like water interacts with a typical sodium ion?

If carbonic acid (H2CO3)were to undergo ionization, what would one of the products be?

Which of the following elements has two valence electrons?

Which of the following would be an ion with a double positive charge?

How is the number of unpaired valence electrons in an atom related to the number of bonds that the atom can form?

Which of the following statements describes a polar molecule?

Which bond is most polar?

What is the valence shell?

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

Which of the following describes how a metal atoms behaves in a bulk metallic object?

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

How many valence electrons does bromine (Br, atomic no. = 35)have?

If a neutral atom loses one electron, what is the electrical charge of the atom?

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

If carbonic acid (H₂CO₃)were to undergo ionization, what would one of the products be?