Deck 8: Bonding: General Concepts

Question 1

In the gaseous phase,which of the following diatomic molecules would be the most polar?

A)CsF
B)CsCl
C)NaCl
D)NaF
E)LiF

Answer 1

CsF

Question 2

In which case is the bond polarity incorrect?

A)( ^{$\delta$ +}H-F ^{$\delta$ -})
B)( ^{$\delta$ +}K-O ^{$\delta$ -})
C)( ^{$\delta$ +}Mg-H ^{$\delta$ -})
D)( ^{$\delta$ +}Cl-I ^{$\delta$ -})
E)( ^{$\delta$ +}Si-S ^{$\delta$ -})

Answer 2

( ^{$\delta$ +}Cl-I ^{$\delta$ -})

Question 3

A nonpolar covalent bond results from the unequal sharing of a pair of electrons between atoms in a molecule.

Answer 3

False

Question 4

In which pair do both compounds exhibit predominantly ionic bonding?

A)SCl₆ and HF
B)Na₂SO₃ and NH₃
C)KI and O₃
D)LiF and H₂O
E)LiBr and MgO

Question 5

Which of the following groups contains no ionic compounds?

A)HCN,NO₂,Ca(NO₃)₂
B)PCl₅,LiBr,Zn(OH)₂
C)KOH,CCl₄,SF₄
D)NaH,CaF₂,NaNH₂
E)CH₂O,H₂S,NH₃

Question 6

The force between two bodies having identical electric charges

A)is a force of repulsion
B)is a force of repulsion if the charges are negative,and one of attraction if they are positive
C)increases as the bodies are moved further apart
D)is independent of the distance between them
E)is directly proportional to the distance between them

Question 7

For the elements Cs,F,and Cl,the order of increasing electronegativity is:

A)F < Cl < Cs
B)Cs < Cl < F
C)Cl < Cs < F
D)F < Cs < Cl
E)none of these

Question 8

What is the correct order of the following bonds in terms of decreasing polarity?

A)N-Cl,P-Cl,As-Cl
B)P-Cl,N-Cl,As-Cl
C)As-Cl,N-Cl,P-Cl
D)P-Cl,As-Cl,N-Cl
E)As-Cl,P-Cl,N-Cl

Question 9

Which of the following bonds is least polar?

A)C-O
B)H-C
C)S-Cl
D)Br-Br
E)They are all nonpolar.

Question 10

When a metal reacts with a nonmetal a covalent bond is formed.

Question 11

Choose the compound with the most ionic bond.

A)LiCl
B)KF
C)NaCl
D)LiF
E)KCl

Question 12

Which of the following bonds would be the least polar,yet still be considered polar covalent?

A)Mg-O
B)C-O
C)O-O
D)Si-O
E)N-O

Question 13

Which of the following bonds would be the most polar without being considered ionic?

A)Mg-O
B)C-O
C)O-O
D)Si-O
E)N-O

Question 14

For the elements Cs,F,and P,the order of increasing electronegativity is:

A)Cs < F < P
B)Cs < P < F
C)P < F < Cs
D)F < Cs < P
E)none of these

Question 15

Metals typically have _______ electronegativity values.

A)high
B)low
C)negative
D)no
E)two of these

Question 16

Based on electronegativity differences,which of the following is most likely to be ionic?

A)CaF₂
B)Br₂
C)BH₃
D)NO
E)CF₄

Question 17

Atoms with greatly different electronegativity values are expected to form

A)no bonds
B)covalent bonds
C)triple bonds
D)ionic bonds
E)none of these

Question 18

The electron pair in a C-F bond could be considered

A)closer to C because carbon has a larger radius and thus exerts greater control over the shared electron pair
B)closer to F because fluorine has a higher electronegativity than carbon
C)closer to C because carbon has a lower electronegativity than fluorine
D)an inadequate model since the bond is ionic
E)centrally located directly between the C and F

Question 19

Atoms having equal or nearly equal electronegativities are expected to form

A)no bonds
B)polar covalent bonds
C)nonpolar covalent bonds
D)ionic bonds
E)covalent bonds

Question 20

Based on electronegativities,which of the following would you expect to be most ionic?

A)N₂
B)CaF₂
C)CO₂
D)CH₄
E)CF₄

Question 21

In the reaction between magnesium and sulfur,the magnesium atoms

A)become anions
B)become cations
C)become part of polyatomic ions
D)share electrons with sulfur
E)crystallize

Question 22

Which of the following statements concerning lattice energy is false?

A)It is often defined as the energy released when an ionic solid forms from its ions.
B)MgO has a larger lattice energy than NaF.
C)The lattice energy for a solid with 2+ and 2- ions should be two times that for a solid with 1+ and 1- ions.
D)MgO has a larger lattice energy than LiF.
E)All of these are true.

Question 23

Which of the following species would be expected to have the lowest ionization energy?

A)F^-
B)Ne
C)O^2-
D)Mg²⁺
E)Na⁺

Question 24

Which of the following has the smallest radius?

A)F^-
B)Ne
C)O^2-
D)Mg²⁺
E)Na⁺

Question 25

Which of the following has the smallest radius?

A)K⁺
B)Cl^-
C)Rb⁺
D)S^2-
E)Ar

Question 26

Calculate the lattice energy for LiCl(s)given the following:

A)47 kJ/mol
B)171 kJ/mol
C)-580 kJ/mol
D)-865 kJ/mol
E)none of these

Question 27

When electrons in a molecule are not found between a pair of atoms but move throughout the molecule,this is called

A)ionic bonding
B)covalent bonding
C)polar covalent bonding
D)delocalization of the electrons
E)a dipole moment

Question 28

Which of the following has the smallest radius?

A)Br^-
B)S^2-
C)Xe
D)Ca²⁺
E)Kr

Question 29

Which of the following arrangements is in order of increasing size?

A)Ga³⁺ > Ca²⁺ > K⁺ > Cl^- > S^2-
B)S^2- > Cl^- > K⁺ > Ca²⁺ > Ga³⁺
C)Ga³⁺ > S^2- > Ca²⁺ > Cl^- > K⁺
D)Ga³⁺ > Ca²⁺ > S^2- > Cl^- > K⁺
E)Ga³⁺ > Ca²⁺ > S^2- > K⁺ > Cl^-

Question 30

Which of these is an isoelectronic series?

A)Na⁺,K⁺,Rb⁺,Cs⁺
B)K⁺,Ca²⁺,Ar,S^2-
C)Na⁺,Mg²⁺,S^2-,Cl^-
D)Li,Be,B,C
E)none of these (A-D)

Question 31

Which of the following statements are true concerning ionic bonding?

A)Ionic bonding occurs between a metal,which has a high affinity for electrons,and a nonmetal,which loses electrons relatively easy.
B)CaCl₂ forms because Ca²⁺ is always a more stable species than the calcium atom alone.
C)Compounds with ionic bonds tend to have low melting points.
D)The electronegativity difference between the bonding atoms of ionic compounds is small since the electrons are not shared but rather held together by electrostatic forces.
E)All of the above statements are false.

Question 32

The first electron affinity value for oxygen is _______ and the second electron affinity value is ________.

A)unfavorable (endothermic),favorable (exothermic)
B)unfavorable (endothermic),unfavorable (endothermic)
C)favorable (exothermic),favorable (exothermic)
D)favorable (exothermic),unfavorable (endothermic)
E)More information is needed.

Question 33

Which of the following statements is incorrect?

A)Ionic bonding results from the transfer of electrons from one atom to another.
B)Dipole moments result from the unequal distribution of electrons in a molecule.
C)The electrons in a polar bond are found nearer to the more electronegative element.
D)A molecule with very polar bonds can be nonpolar.
E)Linear molecules cannot have a net dipole moment.

Question 34

Which of the following molecules has no dipole moment?

A)CO₂
B)NH₃
C)H₂O
D)all
E)none

Question 35

Which of the following ionic compounds has the smallest lattice energy (i.e. ,the lattice energy least favorable to a stable lattice)?

A)LiF
B)CsI
C)NaCl
D)BaO
E)MgO

Question 36

The size in a series of isoelectronic ions increases as the nuclear charge increases.

Question 37

Given the following information:

Calculate the change in enthalpy for:
2Li(s)+ 2HBr(g) $\to$ H₂(g)+ 2LiBr(s)

A)262 kJ
B)-602 kJ
C)-517 kJ
D)-992 kJ
E)none of these

Question 38

In which of the following compounds does the bond between the central atom and bromine have the greatest ionic character?

A)LiBr
B)KBr
C)SeBr₂
D)AsBr₃
E)CaBr₂

Question 39

Which of the following pairs is isoelectronic?

A)Li⁺ and K⁺
B)Na⁺ and Ne
C)I^- and Cl^-
D)S^2- and Ne
E)Al³⁺ and B³⁺

Question 40

Which of the following ionic compounds has the largest lattice energy (i.e. ,the lattice energy most favorable to a stable lattice)?

A)BaO
B)BeO
C)CsI
D)NaBr
E)BaS

Question 41

Choose the molecule with the strongest bond.

A)F₂
B)Cl₂
C)Br₂
D)I₂
E)All are equal.

Question 42

Consider the following reaction: A₂ + B₂ $\to$ 2AB $\Delta$ H = -365 kJ
The bond energy for A₂ is half the amount of AB.The bond energy of B₂ = 447 kJ/mol.What is the bond energy of A₂?

A)812 kJ/mol
B)630 kJ/mol
C)271 kJ/mol
D)-183 kJ/mol
E)none of these

Question 43

Which carbon in this molecule has tetrahedral bonding?

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

Question 44

Consider the compound crotonaldehyde,whose skeleton is:
How many nonbonding electrons appear in the Lewis structure of this molecule?

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

Question 45

When molten sulfur reacts with chlorine gas,a vile-smelling orange liquid forms that is found to have the empirical formula SCl.Which of the following could be the correct Lewis structure for this compound?

A)
B)
C)
D)
E) ^:

Question 46

In the Lewis structure for elemental nitrogen there is (are)

A)a single bond between the nitrogens
B)a double bond between the nitrogens
C)a triple bond between the nitrogens
D)three unpaired electrons
E)none of the above

Question 47

As the number of bonds between two carbon atoms increases,which one of the following decreases?

A)number of electrons between the carbon atoms
B)bond energy
C)bond length
D)all of these
E)none of these

Question 48

Draw the Lewis structures of the molecules below and use them to answer the following questions:
I.BH₃
II.NO₂
III.SF₆
IV.O₃
V.PCl₅
How many of the molecules have no dipole moment?

A)1
B)2
C)3
D)4
E)They are all polar.

Question 49

Choose the molecule with the strongest bond.

A)CH₄
B)H₂O
C)NH₃
D)HF
E)All are equal

Question 50

Consider the compound crotonaldehyde,whose skeleton is:
How many electrons must be shown (as bonding or nonbonding electrons)in the Lewis structure of this molecule?

A)12
B)18
C)24
D)28
E)32

Question 51

Given the following information: Br₂ bond energy = 193 kJ/mol
F₂ bond energy = 154 kJ/mol Br₂(g)+ F₂(g) $\to$ BrF₃(g)
$\Delta$ H° = -384 kJ/mol
Calculate the Br-F bond energy.

A)244 kJ/mol
B)237 kJ/mol
C)712 kJ/mol
D)128 kJ/mol
E)none of these

Question 52

Which of the following statements is false?

A)Models are human interpretations,not the same as reality.
B)Models are often wrong.
C)Models usually start out simple and become more complex over time.
D)We often learn more when a model is wrong than when it is right.
E)A model should be discarded when any exception to it is found.

Question 53

Choose the molecule with the strongest bond.

A)HF
B)HCl
C)HBr
D)HI
E)All are equal.

Question 54

Which of the following molecules contains a double bond?

A)CO₂
B)NH₃
C)H₂O
D)all
E)none

Question 55

As indicated by Lewis structures,which of the following would probably not exist as a stable molecule?

A)CH₃OH
B)CH₂O
C)CH₃O
D)C₂H₂
E)C₃H₄

Question 56

Draw the Lewis structures of the molecules below and use them to answer the following questions:
I.BH₃
II.NO₂
III.SF₆
IV.O₃
V.PCl₅
Which of the molecules obeys the octet rule?

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

Question 57

Complete the Lewis structure for the molecule: This molecule has __________ single bonds and __________ multiple bonds.

A)4,2
B)6,3
C)11,5
D)11,2
E)13,0

Question 58

Draw the Lewis structures of the molecules below and use them to answer the following questions:
I.BH₃
II.NO₂
III.SF₆
IV.O₃
V.PCl₅
Which of these molecules show resonance?

A)I,II
B)II,IV
C)II,V
D)III,IV
E)III,V

Question 59

Which of the following molecules exhibits the greatest bond energy?

A)F₂
B)Cl₂
C)Br₂
D)I₂
E)all the same

Question 60

A double bond occurs when two atoms share two pairs of electrons.

Question 61

In the Lewis structure for SF₆,the central sulfur atom shares __________ electrons.

A)4
B)8
C)10
D)12
E)None of the above,because SF₆ is an ionic compound.

Question 62

As indicated by Lewis structures,which of the following species could probably not exist as a stable molecule?

A)NH₃
B)N₂H₂
C)N₂H₄
D)N₂H₆
E)N₂O₄

Question 63

Consider the following molecules.
I.BF₃
II.CHBr₃ (C is the central atom)
III.Br₂
IV.XeCl₂
V.CO
VI.SF₄
Select the molecule(s)that fit the given statement.
These molecules have a zero net dipole moment.

A)III,V
B)I,III,IV
C)III,IV,V
D)I,III,IV,VI
E)none of them

Question 64

Which of the following compounds contains only one unshared pair of valence electrons?

A)NH₃
B)H₂O
C)CH₄
D)NaCl
E)BF₃

Question 65

Which of the following Lewis structures best describes BF₃?

A)
B)
C)
D)
E)

Question 66

Which of the following atoms cannot exceed the octet rule in a molecule?

A)N
B)S
C)P
D)I
E)All of the atoms (A-D)can exceed the octet rule.

Question 67

Which of the following species is best described by drawing resonance structures?

A)PH₃
B)NH₄⁺
C)O₃
D)SO₃
E)HCN

Question 68

Which has the greater N-O bond length,NO₂^- or NO₃^-?

A)NO₂^-
B)NO₃^-
C)The bond lengths are the same.
D)More information is needed.
E)None of these (A-D).

Question 69

Consider the following molecules.
I.BF₃
II.CHBr₃ (C is the central atom)
III.Br₂
IV.XeCl₂
V.CO
VI.SF₄
Select the molecule(s)that fit the given statement.
These molecules have a trigonal bipyramidal electron pair arrangement.

A)II,IV,VI
B)I,IV
C)IV,VI
D)VI only
E)none of them

Question 70

Which of the following exhibits resonance?

A)NH₃
B)PCl₅
C)H₂O
D)O₃
E)At least two of the molecules (A-D)exhibit resonance.

Question 71

Given the following Lewis structure:
How many unshared pairs of electrons are present in this molecule?

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

Question 72

How many resonance structures can be drawn for the molecule O₃?

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

Question 73

Consider the following molecules.
I.BF₃
II.CHBr₃ (C is the central atom)
III.Br₂
IV.XeCl₂
V.CO
VI.SF₄
Select the molecule(s)that fit the given statement.
These molecules violate the octet rule.

A)I,II,IV
B)I,III,IV,VI
C)III,V,VI
D)I,IV,VI
E)I,II,IV,VI

Question 74

Select the best Lewis structure for acetone,CH₃COCH₃.

A)
B)
C)
D)
E)

Question 75

In the cyanide ion (CN^-),the nitrogen has a formal charge of

A)-2
B)-1
C)0
D)2
E)More information is needed.

Question 76

The Lewis structure for H₃BO₃ is

A)
B)
C)
D)
E)

Question 77

Which of the following has an incomplete octet in its Lewis structure?

A)SO₂
B)ICl
C)CO₂
D)F₂
E)NO

Question 78

The Lewis structure for CHCl₃ has nine lone electron pairs.

Question 79

In the Lewis structure for ICl₂^-,how many lone pairs of electrons are around the central iodine atom?

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

Question 80

Given the following Lewis structure:
How many electrons are shared between carbons 1 and 2?

A)0
B)2
C)4
D)6
E)8