Question 1

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

Question 2

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.

Question 3

Which of the following compounds has polar covalent bonds?

Accepted Answer

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

Question 4

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

Question 5

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.

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

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.

Question 8

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

Accepted Answer

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

Question 9

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.

Question 10

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

Question 11

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.

Question 12

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

Accepted Answer

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

Question 13

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.

Question 14

Which of the following elements has two valence electrons?

Accepted Answer

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

Question 15

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

Question 16

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

Question 17

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

Question 18

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.

Question 19

Which bond is most polar?

Accepted Answer

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

Question 20

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

Exam 15: How Atoms Bond and Molecules Attract

Which of the following statements describes a polar molecule?

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Which of the following would have the highest boiling point?

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

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

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

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Which of the following compounds has polar covalent bonds?

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

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What is the valence shell?

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

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

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

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Which of the following elements has two valence electrons?

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How are oxygen molecules attracted to water molecules?

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

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

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Does an ionic bond have a dipole?

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

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

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Which bond is most polar?

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

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

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