Deck 8: Chemical Bonds: What Makes a Gas a Greenhouse Gas

Question 1

Which statement A-D about chemical bonds is not correct?

A)The attraction of the negatively charged electrons to the positively charged nuclei causes the electrostatic potential energy to decrease as two atoms come together.
B)The repulsion of the negatively charged electrons with each other and the positively charged nuclei with each other causes the electrostatic potential energy to increase when the two atoms are very close together.
C)As two atoms come together, the electrostatic potential energy goes through a minimum.The distance between the atoms at which this minimum occurs is called the bond length.
D)The bond energy is the energy released when two atoms infinitely far apart come together at a distance that minimizes the electrostatic potential energy.
E)Statements A-D are all correct.

Answer 1

Statements A-D are all correct.

Question 2

Which of the following is the correct Lewis symbol for S?

A)
B)
C)
D)
E)

Answer 2

Question 3

An Si-Si linkage would be classified as what type of bonding interaction?

A)polar covalent
B)metallic
C)ionic
D)nonpolar covalent
E)homogeneous

Answer 3

nonpolar covalent

Question 4

Which of the following elements contains the fewest number of valence electrons?

A)N
B)Se
C)Si
D)Al
E)Br

Question 5

A covalent bond results when ________

A)electrons are transferred from one atom to another atom.
B)atoms pool their electrons to form a "sea" of electrons.
C)atoms have outer electrons with the same principal quantum number.
D)electrons are shared between a pair of atoms.
E)an atom has 8 valence electrons.

Question 6

Which statement A-D about chemical bonds is not correct?

A)Atoms combine to form molecules because the energy of the molecule is lower than the energy of the free atoms.
B)The electrostatic potential energy explains why atoms bond together.
C)The electrostatic potential energy is directly proportional to the charges on two particles.
D)The electrostatic potential energy is inversely proportional to the distance between two charged particles.
E)Statements A-D are all correct.

Question 7

Which type of bonding involves the sharing of valence electrons by two atoms?

A)covalent
B)ionic
C)polar ionic
D)intramolecular
E)metallic

Question 8

Which statement provides the best description of an ionic bond?

A)A high electron density between two positively charged atomic nuclei serves to attract the nuclei to each other.
B)The negative charge on one atom is attracted to the positive charge on a second atom.
C)Two or more electrons are attracted to each other, thereby holding the atoms together.
D)Two atomic nuclei are attracted to each other by the strong nuclear force.
E)Two atomic nuclei are attracted to each other by the Coulomb force.

Question 9

The following Lewis symbol corresponds to which element?

A)Be
B)B
C)C
D)N
E)O

Question 10

Indicate the ion that does not have 8 valence electrons.

A)O^-
B)Na⁺
C)Al³⁺
D)P^3-
E)Ar

Question 11

What type of bonding is present in NaCl?

A)polar covalent
B)metallic
C)ionic
D)nonpolar covalent
E)amorphous

Question 12

How many valence electrons does S^2- have?

A)8
B)6
C)16
D)4
E)14

Question 13

How many valence electrons does F have?

A)5
B)7
C)8
D)9
E)19

Question 14

Which statement provides the best description of a covalent bond?

A)A high electron density between two positively charged atomic nuclei serves to attract the nuclei to each other.
B)The negative charge on one atom is attracted to the positive charge on a second atom.
C)Two or more electrons are attracted to each other, thereby holding the atoms together.
D)Two atomic nuclei are attracted to each other by the strong nuclear force.
E)Two atomic nuclei are attracted to each other by the Coulomb force.

Question 15

Which of the following is most likely a polar covalent bond?

A)Na - Cl
B)H - H
C)C - N
D)K - F
E)Ca - O

Question 16

Based on electronegativities, which one of the following would have ionic bonds?

A)O₂
B)MgO
C)H₂O
D)CF₄
E)SiO₂

Question 17

Which of the following is an example of a nonpolar covalent bond?

A)C - S
B)C - N
C)C - F
D)C - C
E)C - O

Question 18

Which of the following elements has 6 valence electrons?

A)C
B)S
C)N
D)Br
E)Be

Question 19

Which of the following elements contains the largest number of valence electrons?

A)P
B)Sr
C)C
D)B
E)F

Question 20

How many valence electrons does aluminum have?

A)1
B)2
C)3
D)11
E)13

Question 21

Which diatomic molecule has the least number of valence electrons?

A)O₂
B)N₂
C)NO
D)Cl₂
E)F₂

Question 22

How many valence electrons are there in a correctly drawn Lewis structure for formamide, HCONH₂?

A)12
B)14
C)16
D)18
E)20

Question 23

Which of the following has 13 valence electrons?

A)SH^-
B)IO
C)NO
D)ICl
E)Cl₂

Question 24

Which of the following molecular ions has 3 valence electrons?

A)H₂⁺
B)He₂⁺
C)C₂⁺
D)B₂⁺
E)O₂^-

Question 25

Describe the position of electrons around one N atom in the Lewis structure of N₂.

A)3 shared electron pairs, 1 lone pair
B)2 shared electron pairs, 2 lone pairs
C)1 shared electron pair, 3 lone pairs
D)3 shared electron pairs
E)2 shared electron pairs, 1 lone pair

Question 26

Triple bonds________

A)involve sharing of 3 total electrons between atoms.
B)involve sharing of 6 total electrons between atoms.
C)always occur between 2 metal atoms.
D)occur only between atoms with 3 valence electrons.
E)typically occur between hydrogen and another atom.

Question 27

Which of the following molecules does not contain a triple bond?

A)N₂
B)HCN
C)C₂H₂
D)SO₂
E)CO

Question 28

How many valence electrons are there in PO₄^3-?

A)10
B)14
C)23
D)29
E)32

Question 29

How many total shared electrons are there in the Lewis structure of CS₂?

A)2
B)6
C)4
D)8
E)10

Question 30

Which of the following has the most valence electrons?

A)HF
B)NS
C)CN^-
D)ArF
E)Ar⁺

Question 31

How many covalent bonds are there in CN^-?

A)1
B)2
C)3
D)0
E)4

Question 32

How many lone pairs are there in ClO^-?

A)1
B)2
C)3
D)4
E)6

Question 33

How many valence electrons are there in BrO^-?

A)7
B)6
C)13
D)14
E)18

Question 34

Which of the following species contains a double bond?

A)NO^-
B)F₂
C)CH
D)OH^-
E)Br₂

Question 35

Which of the following ions does not have a complete valence-shell octet?

A)Al³⁺
B)I^-
C)Ca²⁺
D)Pb²⁺
E)S^2-

Question 36

Indicate which of the following molecules has four shared electrons.

A)O₂
B)CO
C)HI
D)N₂
E)Cl₂

Question 37

The following Lewis symbol corresponds to which ion?

A)F^-
B)O^-
C)C^2-
D)B³⁺
E)N^2-

Question 38

How many shared electron pairs are there in the Lewis structure of CN^-?

A)3
B)6
C)4
D)2
E)10

Question 39

How many valence electrons are there in SF₄?

A)13
B)28
C)21
D)34
E)40

Question 40

Indicate which of the following molecules has only a single bond.

A)O₂
B)CO
C)CN^-
D)N₂
E)Cl₂

Question 41

Which of the following properties is typically used to identify whether a bond is polar, nonpolar, or ionic?

A)electronegativity
B)ionization energy
C)atomic radius
D)electron affinity
E)atomic mass

Question 42

Which statements correctly describe a polar covalent bond?
I. Electrons are shared but not equally by the two atoms.
II. One atom has a small negative charge, and the other atom has a small positive charge.
III. The bond dipole is zero.
IV. One or more electrons are transferred from one atom to a second atom.

A)I and II only
B)II and III only
C)III and IV only
D)I and III only
E)I and IV only

Question 43

Carbon dioxide is a greenhouse gas. Which of the following is the correct Lewis structure for carbon dioxide?

A)
B)
C)
D)

Question 44

How many lone-pair electrons are on the central oxygen atom in the Lewis structure for dinitrogen pentoxide (N₂O₅)? A skeleton of the molecule is provided below.

A)0
B)2
C)4
D)1
E)3

Question 45

The measure of an atom's ability to attract electrons in a chemical bond is called ________

A)hybridization.
B)ionization energy.
C)electron affinity.
D)electronegativity.
E)ionic radius.

Question 46

Acetonitrile (CH₃CN) is an important industrial chemical. Among other things, it is used to make plastic moldings, which have multiple uses, from car parts to Lego bricks. Which one of the following statements about acetonitrile is not correct?

A)Acetonitrile has 16 valence electrons.
B)Acetonitrile has one triple bond.
C)Acetonitrile has one pair of nonbonding electrons.
D)All atoms satisfy the octet rule in acetonitrile.
E)One carbon atom and the nitrogen atom have nonzero formal charges.

Question 47

Identify the molecule or ion that contains a polar covalent bond.

A)O₂
B)N₂
C)CN^-
D)H₂
E)I₂

Question 48

Identify the molecule below that contains a double bond.

A)HCN
B)O₃
C)C₂H₂
D)S₂
E)N₂

Question 49

Which of the following are listed in order of decreasing electronegativity?

A)F S Na H
B)F N P O
C)N P Si S
D)F Cl Br C
E)Te Se S O

Question 50

Indicate the element with the smallest electronegativity.

A)Cl
B)F
C)Be
D)K
E)C

Question 51

Indicate the element with the largest electronegativity.

A)K
B)Cs
C)Mg
D)B
E)Li

Question 52

Which statement A-D regarding electronegativity is not correct?

A)Electronegativity is a measure of an atom's ability to attract electrons in a molecule.
B)If the electronegativity difference is sufficiently large, then an ionic bond is formed.
C)All bonds are polar except those between the same atoms (e.g., CO vs.O₂).
D)Pauling assigned electronegativity values to atoms based on their ionization energies and electron affinities.
E)Statements A-D are all correct.

Question 53

Electronegativity increases from left to right across a period because of ________

A)increased shielding of valence electrons by the core electrons.
B)an increase in the number of protons in the nucleus.
C)a decrease in the effective nuclear charge (Z_eff).
D)an increase in the shielding of core electrons by the valence electrons.
E)a decrease in the ionization potential.

Question 54

Indicate which one of the following does not contain a polar covalent bond.

A)I₂
B)CO
C)HF
D)NO
E)CN^-

Question 55

In going down a column in the periodic table, the electronegativity ________

A)decreases because the valence electrons are further from the nucleus.
B)increases because the nuclear charge increases.
C)decreases because the atomic number increases.
D)increases because the ionization potential increases.
E)increases because the electron repulsion increases.

Question 56

Which group of elements is listed in order of increasing electronegativity?

A)F Cl Ge Sn
B)Rb Ca Sc Cs
C)Zr V Nb Ta
D)Sn P Cl F
E)Cl Br I F

Question 57

Trends in electronegativity are primarily a result of ________

A)the number of core electrons in an element.
B)an element's atomic number.
C)the effective nuclear charge (Z_eff) that an outer electron experiences.
D)the number of valence electrons of an element.
E)the atomic mass.

Question 58

What types of bonds form between the chlorine and oxygen atoms of the chlorite ion (ClO₂^-) to minimize the formal charge?

A)single
B)between single and double
C)double
D)triple
E)ionic

Question 59

Indicate which molecule contains the largest number of nonbonding electrons.

A)H₂
B)CO
C)N₂
D)NO
E)O₂

Question 60

How many lone-pair electrons are on each of the nitrogen atoms in the Lewis structure for dinitrogen tetroxide (N₂O₄)?

A)0
B)2
C)4
D)1
E)3

Question 61

In addition to CO₂, which of the gases in the atmosphere listed below can contribute to the greenhouse effect?

A)CH₄
B)N₂
C)O₂
D)Ar
E)None of these gases can contribute to the greenhouse effect.

Question 62

Which of these statements about greenhouse gases and the greenhouse effect is not correct?
I. Greenhouse gases prevent infrared radiation from escaping through the atmosphere.
II. To absorb infrared radiation, a molecule must have a vibration that produces a change in
The dipole moment of the molecule.
III. Argon is the third most abundant species in the atmosphere (after nitrogen and oxygen),
And therefore is a significant greenhouse gas.
IV. The average amount of carbon dioxide in the atmosphere increases when fossil fuels are
Burned, but not when ethanol (CH₃CH₂OH) produced from plants is burned.

A)I only
B)II only
C)III only
D)IV only
E)III and IV only

Question 63

In which bond does the Cl atom have the highest electron density?

A)H-Cl
B)O-Cl
C)S-Cl
D)N-Cl
E)Br-Cl

Question 64

In general, resonance ________ electrons and ________ molecules.

A)delocalizes; stabilizes
B)destabilizes; destabilizes
C)localizes; stabilizes
D)delocalizes; destabilizes
E)localizes; destabilizes

Question 65

Resonance structures indicate that ________

A)there is more than one allotropic form of a compound.
B)more than one ionic form of a compound exists.
C)the electronic structure is an average or superposition of the diagrams.
D)more than one isotopic form of an element exists in the molecule.
E)the molecule jumps back and forth between two or more different electronic structures.

Question 66

How many total bonding pairs of electrons exist in a single resonance structure for NO₃^-?

A)1
B)2
C)3
D)4
E)8

Question 67

Which of the following gases in the atmosphere does not contribute to the greenhouse effect?

A)CO₂
B)CO
C)H₂O
D)CH₄
E)Ar

Question 68

Which of the following bonds is most polar?

A)B-H
B)N-H
C)P-H
D)Al-H
E)C-H

Question 69

To absorb infrared radiation, a molecule must have ________

A)a vibrational motion that causes a change in dipole moment.
B)a double or triple bond.
C)no center of symmetry, so one side is different from the other.
D)atoms other than carbon and hydrogen.
E)at least one carbon and one hydrogen atom.

Question 70

Which of the following molecules cannot absorb infrared radiation?

A)HCl
B)CH₄
C)N₂
D)C₆H₆
E)CO

Question 71

Not all the vibrations of carbon dioxide can absorb infrared radiation because ________

A)the molecule is not polar.
B)the molecule possesses a permanent dipole moment.
C)only some of the vibrations produce a transient dipole moment.
D)there are no hydrogen atoms in carbon dioxide.
E)the molecule is linear.

Question 72

When sulfur-containing fuels are burned, sulfur trioxide (SO₃) is formed in the atmosphere and contributes to acid rain (sulfur trioxide plus water produces sulfuric acid). How many resonance structures are there for SO₃ when each atom satisfies the octet rule?

A)0
B)1
C)2
D)3
E)4

Question 73

How many total equivalent Lewis structures are needed to describe the carbonate anion, CO₃^2-?

A)1
B)2
C)3
D)4
E)5

Question 74

Sodium nitrite (NaNO₂) is often used in meat curing because it prevents bacterial growth. How many major resonance contributing Lewis structures can be drawn for the nitrite anion (NO₂^-) ?

A)0
B)1
C)2
D)3
E)4

Question 75

Which sequence does not have the elements arranged correctly in order of increasing electronegativity?

A)I Br Cl
B)B N O
C)H C N
D)H Li S
E)Al S Cl

Question 76

Which of these statements correctly describes why methane and carbon dioxide are considered to be significant greenhouse gases?
I. Both have permanent dipole moments that change with vibration of the molecule.
II. Neither has a permanent dipole moment, but a dipole moment is produced when the
Molecule vibrates.
III. The concentration of carbon dioxide in the atmosphere increases when fossil fuels are
Mined and burned.

A)I only
B)II only
C)III only
D)I and III only
E)II and III only

Question 77

Which of these statements correctly describes the electronic charge distribution in a molecule?
I. The charge density around each atom is the same as it is in the free atom.
II. The electronic charge is distributed equally around each atom in the molecule.
III. Electrons are attracted preferentially to atoms with high electronegativity.
IV. Electronic charge density is enhanced in the space between atoms to form a bond.
V. Electrons are always shared between atoms and never transferred from one atom to another.

A)I only
B)II and III only
C)III and IV only
D)II only
E)V only

Question 78

In which bond does the H atom have the highest electron density?

A)H-Cl
B)H-Li
C)H-N
D)H-O
E)H-C

Question 79

Which of the following bonds is least polar?

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

Question 80

Which of the following bonds is primarily ionic?

A)Li-C
B)Li-H
C)Li-O
D)Li-Li
E)C-O