Deck 8: Basic Concepts of Chemical Bonding

Question 1

In ionic bond formation, the lattice energy of ions ________ as the magnitude of the ion charges _______ and the radii ________.

A)increases, decrease, increase
B)increases, increase, increase
C)decreases, increase, increase
D)increases, increase, decrease
E)increases, decrease, decrease

Answer 1

increases, increase, decrease

Question 2

Lattice energy is ________.

A)the energy required to convert a mole of ionic solid into its constituent ions in the gas phase
B)the energy given off when gaseous ions combine to form one mole of an ionic solid
C)the energy required to produce one mole of an ionic compound from its constituent elements in their standard states
D)the sum of ionization energies of the components in an ionic solid
E)the sum of electron affinities of the components in an ionic solid

Answer 2

the energy required to convert a mole of ionic solid into its constituent ions in the gas phase

Question 3

In the nitrite ion (NO₂^-), ________.

A)both bonds are single bonds
B)both bonds are double bonds
C)one bond is a double bond and the other is a single bond
D)both bonds are the same
E)there are 20 valence electrons

Answer 3

both bonds are the same

Question 4

Resonance structures differ by ________.

A)number and placement of electrons
B)number of electrons only
C)placement of atoms only
D)number of atoms only
E)placement of electrons only

Question 5

For resonance forms of a molecule or ion, ________.

A)one always corresponds to the observed structure
B)all the resonance structures are observed in various proportions
C)the observed structure is an average of the resonance forms
D)the same atoms need not be bonded to each other in all resonance forms
E)there cannot be more than two resonance structures for a given species

Question 6

The Lewis structure of N₂H₂ shows ________.

A)a nitrogen-nitrogen triple bond
B)a nitrogen-nitrogen single bond
C)each nitrogen has one nonbonding electron pair
D)each nitrogen has two nonbonding electron pairs
E)each hydrogen has one nonbonding electron pair

Question 7

In which of the molecules below is the carbon-carbon distance the shortest?

A)H₂C CH₂
B)H-C≡C-H
C)H₃C-CH₃
D)H₂C C CH₂
E)H₃C-CH₂-CH₃

Question 8

Which of the following has the bonds correctly arranged in order of increasing polarity?

A)Be-F, Mg-F, N-F, O-F
B)O-F, N-F, Be-F, Mg-F
C)O-F, Be-F, Mg-F, N-F
D)N-F, Be-F, Mg-F, O-F
E)Mg-F, Be-F, N-F, O-F

Question 9

To convert from one resonance structure to another, ________.

A)only atoms can be moved
B)electrons and atoms can both be moved
C)only electrons can be moved
D)neither electrons nor atoms can be moved
E)electrons must be added

Question 10

The oxidation number of iron in Fe₂O₃ is ________.

A)-2
B)+1
C)+3
D)+2
E)-3

Question 11

The Lewis structure of the CO₃^2- ion is ________.

A)
B)
C)
D)
E)

Question 12

Which of the following has eight valence electrons?

A)Ti⁴⁺
B)Kr
C)Cl^-
D)Na⁺
E)all of the above

Question 13

Of the molecules below, the bond in ________ is the most polar.

A)HBr
B)HI
C)HCl
D)HF
E)H₂

Question 14

The type of compound that is most likely to contain a covalent bond is ________.

A)one that is composed of a metal from the far left of the periodic table and a nonmetal from the far right of the periodic table
B)a solid metal
C)one that is composed of only nonmetals
D)held together by the electrostatic forces between oppositely charged ions
E)There is no general rule to predict covalency in bonds.

Question 15

For the questions that follow, consider the BEST Lewis structures of the following oxyanions:
(i)NO₂^-
(ii)NO₃^-
(iii)SO₃^2-
(iv)SO₄^2-
(v)BrO₃^-
There can be four equivalent best resonance structures of ________.

A)(i)
B)(ii)
C)(iii)
D)(iv)
E)(v)

Question 16

The diagram below is the Born-Huber cycle for the formation of crystalline potassium fluoride.
Which energy change corresponds to the electron affinity of fluorine?

A)2
B)5
C)4
D)1
E)6

Question 17

Using the Born-Haber cycle, the ΔH°_f of KBr is equal to ________.

A)ΔH°_f [K (g)] + ΔH°_f [Br (g)] + I₁(K) + E(Br) + ΔH_lattice
B)ΔH°_f [K (g)] - ΔH°_f [Br (g)] - I₁(K) - E(Br) - ΔH_lattice
C)ΔH°_f [K (g)] - ΔH°_f [Br (g)] + I₁(K) - E(Br) + ΔH_lattice
D)ΔH°_f [K (g)] + ΔH°_f [Br (g)] - I₁ - E(Br) + ΔH_lattice
E)ΔH°_f [K (g)] + ΔH°_f [Br (g)] + I₁(K) + E(Br) - ΔH_lattice

Question 18

Which of the following does not have eight valence electrons?

A)Ca⁺
B)Rb⁺
C)Xe
D)Br^-
E)All of the above have eight valence electrons.

Question 19

The bond length in an HI molecule is 1.61 Å and the measured dipole moment is 0.44 D. What is the magnitude (in units of e)of the negative charge on I in HI? (1 debye = 3.34 × 10^-30 coulomb-meters; e = 1.6 × 10^-19 coulombs)

A)1.6 × 10^-19
B)0.057
C)9.1
D)1
E)0.22

Question 20

The diagram below is the Born-Huber cycle for the formation of crystalline potassium fluoride.
Which energy change corresponds to the first ionization energy of potassium?

A)2
B)5
C)4
D)3
E)6

Question 21

A valid Lewis structure of ________ cannot be drawn without violating the octet rule.

A)NF₃
B)IF₃
C)PF₃
D)SbF₃
E)SO₄^2-

Question 22

Of the possible bonds between carbon atoms (single, double, and triple), ________.

A)a triple bond is longer than a single bond
B)a double bond is stronger than a triple bond
C)a single bond is stronger than a triple bond
D)a double bond is longer than a triple bond
E)a single bond is stronger than a double bond

Question 23

A valid Lewis structure of ________ cannot be drawn without violating the octet rule.

A)PO₄^3-
B)SiF₄
C)CF₄
D)SeF₄
E)NF₃

Question 24

The central atom in ________ does not violate the octet rule.

A)SF₄
B)KrF₂
C)CF₄
D)XeF₄
E)ICl₄^-

Question 25

Given that the average bond energies for C-H and C-Br bonds are 413 and 276 kJ/mol, respectively, the heat of atomization of bromoform (CHBr₃)is ________ kJ/mol.

A)1241
B)689
C)-689
D)1378
E)-1378

Question 26

Dynamite ________.

A)was invented by Alfred Nobel
B)is made of nitroglycerine and an absorbent such as diatomaceous earth
C)is a much safer explosive than pure nitroglycerine
D)is an explosive
E)all of the above

Question 27

Of the bonds C-N, C N, and C≡N, the C-N bond is ________.

A)strongest/shortest
B)strongest/longest
C)weakest/shortest
D)weakest/longest
E)intermediate in both strength and length

Question 28

Dynamite consists of nitroglycerine mixed with ________.

A)potassium nitrate
B)damp KOH
C)TNT
D)diatomaceous earth or cellulose
E)solid carbon

Question 29

Why don't we draw double bonds between the Be atom and the Cl atoms in BeCl₂?

A)That would give positive formal charges to the chlorine atoms and a negative formal charge to the beryllium atom.
B)There aren't enough electrons.
C)That would result in more than eight electrons around beryllium.
D)That would result in more than eight electrons around each chlorine atom.
E)That would result in the formal charges not adding up to zero.

Question 30

Of the bonds C-C, C C, and C≡C, the C-C bond is ________.

A)strongest/shortest
B)strongest/longest
C)weakest/longest
D)weakest/shortest
E)intermediate in both strength and length

Question 31

A valid Lewis structure of ________ cannot be drawn without violating the octet rule.

A)ClF₃
B)PCl₃
C)SO₃
D)CCl₄
E)CO₂

Question 32

A valid Lewis structure of ________ cannot be drawn without violating the octet rule.

A)NI₃
B)SO₂
C)ICl₅
D)SiF₄
E)CO₂

Question 33

Based on the octet rule, boron will most likely form a ________ ion.

A)B^3-
B)B⁺
C)B³⁺
D)B²⁺
E)B^2-

Question 34

Which atom can accommodate an octet of electrons, but doesn't necessarily have to accommodate an octet?

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

Question 35

Bond enthalpy is ________.

A)always positive
B)always negative
C)sometimes positive, sometimes negative
D)always zero
E)unpredictable

Question 36

Which of the following does not have eight valence electrons?

A)Cl^-
B)Xe
C)Ti⁺⁴
D)Rb⁺
E)Sr⁺

Question 37

Most explosives are compounds that decompose rapidly to produce ________ products and a great deal of ________.

A)gaseous, gases
B)liquid, heat
C)soluble, heat
D)solid, gas
E)gaseous, heat

Question 38

For the questions that follow, consider the BEST Lewis structures of the following oxyanions:
(i)NO₂^-
(ii)NO₃^-
(iii)SO₃^2-
(iv)SO₄^2-
(v)BrO₃^-
In which of the ions do all X-O bonds (X indicates the central atom)have the same length?

A)none
B)all
C)(i)and (ii)
D)(iii)and (v)
E)(iii), (iv), and (v)

Question 39

As the number of covalent bonds between two atoms increases, the distance between the atoms ________ and the strength of the bond between them ________.

A)increases, increases
B)decreases, decreases
C)increases, decreases
D)decreases, increases
E)is unpredictable

Question 40

A valid Lewis structure of ________ cannot be drawn without violating the octet rule.

A)NF₃
B)BeH₂
C)SO₂
D)CF₄
E)SO₃^2-

Question 41

The electron configuration of the S^2- ion is ________.

A)[Ar]3s²3p⁶
B)[Ar]3s²3p²
C)[Ne]3s²3p²
D)[Ne]3s²3p⁶
E)[Kr]3s²2p⁶

Question 42

Which of the following would have to gain two electrons in order to achieve a noble gas electron configuration? O Sr Na Se Br

A)Br
B)Sr
C)Na
D)O, Se
E)Sr, O, Se

Question 43

What species has the electron configuration [Ar]3d²?

A)Mn²⁺
B)Cr²⁺
C)V³⁺
D)Fe³⁺
E)K⁺

Question 44

Which of the following would have to lose two electrons in order to achieve a noble gas electron configuration? O Sr Na Se Br

A)O, Se
B)Sr
C)Na
D)Br
E)Sr, O, Se

Question 45

The halogens, alkali metals, and alkaline earth metals have ________ valence electrons, respectively.

A)7, 4, and 6
B)1, 5, and 7
C)8, 2, and 3
D)7, 1, and 2
E)2, 7, and 4

Question 46

The electron configuration of the phosphide ion (P^3-)is ________.

A)[Ne]3s²
B)[Ne]3s²3p¹
C)[Ne]3s²3p³
D)[Ne]3p²
E)[Ne]3s²3p⁶

Question 47

What is the electron configuration for the Co²⁺ ion?

A)[Ar]4s¹3d⁶
B)[Ar]3d⁷
C)[Ar]3d⁵
D)[Ar]4s²3d⁹
E)[Ne]3s²3p¹⁰

Question 48

The electron configuration of the sulfide ion (S^2-)is ________.

A)[Ne]3s²
B)[Ne]3s²3p¹
C)[Ne]3s²3p⁴
D)[Ne]3p²
E)[Ne]3s²3p⁶

Question 49

For a given arrangement of ions, the lattice energy decreases as ionic radius ________ and as ionic charge ________.

A)decreases, increases
B)increases, decreases
C)increases, increases
D)decreases, decreases
E)This cannot be predicted.

Question 50

What is the electron configuration for the Fe³⁺ ion?

A)[Ar]4s¹3d⁶
B)[Ar]4s⁰3d⁷
C)[Ar]4s⁰3d⁵
D)[Ar]4s²3d⁹
E)[Ne]3s²3p¹⁰

Question 51

What is the electron configuration for the Fe²⁺ ion?

A)[Ar]4s⁰3d⁶
B)[Ar]4s²3d⁴
C)[Ar]4s⁰3d⁸
D)[Ar]4s²3d⁸
E)[Ar]4s⁶3d²

Question 52

The only noble gas without eight valence electrons is ________.

A)Ar
B)Ne
C)He
D)Kr
E)All noble gases have eight valence electrons.

Question 53

The electron configuration of the P^3- ion is ________.

A)[Ar]3s²3p⁶
B)[Ar]3s²3p²
C)[Ne]3s²3p⁶
D)[Ne]3s²3p²
E)[Kr]3s²2p⁶

Question 54

For a given arrangement of ions, the lattice energy increases as ionic radius ________ and as ionic charge ________.

A)decreases, increases
B)increases, decreases
C)increases, increases
D)decreases, decreases
E)This cannot be predicted.

Question 55

Which of the following would have to lose three electrons in order to achieve a noble gas electron configuration? Si Mg Al Cl P

A)Si, P
B)Al
C)P
D)Cl
E)Mg, Al, P

Question 56

Based on the octet rule, magnesium most likely forms a ________ ion.

A)Mg²⁺
B)Mg^2-
C)Mg^6-
D)Mg⁶⁺
E)Mg^-

Question 57

What species has the electron configuration [Ar]3d⁴?

A)Mn²⁺
B)Cr²⁺
C)V³⁺
D)Fe³⁺
E)K⁺

Question 58

Based on the octet rule, phosphorus most likely forms a ________ ion.

A)P³⁺
B)P^3-
C)P⁵⁺
D)P^5-
E)P⁺

Question 59

Based on the octet rule, aluminum most likely forms an ________ ion.

A)Al³⁺
B)Al⁴⁺
C)Al^4-
D)Al⁺
E)Al^-

Question 60

Based on the octet rule, iodine most likely forms an ________ ion.

A)I²⁺
B)I⁴⁺
C)I^4-
D)I⁺
E)I^-

Question 61

The ion PO₄^3- has ________ valence electrons.

A)14
B)24
C)27
D)29
E)32

Question 62

Elements from opposite sides of the periodic table tend to form ________.

A)covalent compounds
B)ionic compounds
C)compounds that are gaseous at room temperature
D)homonuclear diatomic compounds
E)covalent compounds that are gaseous at room temperature

Question 63

What is the maximum number of double bonds that a hydrogen atom can form?

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

Question 64

In the molecule below, which atom has the largest partial negative charge? Cl
∣
F- C -Br
∣
I

A)Cl
B)F
C)Br
D)I
E)C

Question 65

Electronegativity ________ from left to right within a period and ________ from top to bottom within a group.

A)decreases, increases
B)increases, increases
C)increases, decreases
D)stays the same, increases
E)increases, stays the same

Question 66

A triple bond consists of ________ pairs of electrons shared between two atoms.

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

Question 67

The formula of palladium (IV)sulfide is ________.

A)Pd₂S₄
B)PdS₄
C)Pd₄S
D)PdS₂
E)Pd₂S₂

Question 68

The ability of an atom in a molecule to attract electrons is best quantified by the ________.

A)paramagnetism
B)diamagnetism
C)electronegativity
D)electron charge-to-mass ratio
E)first ionization potential

Question 69

A double bond consists of ________ pairs of electrons shared between two atoms.

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

Question 70

The Lewis structure of AsH₃ shows ________ nonbonding electron pair(s)on As.

A)0
B)1
C)2
D)3
E)This cannot be determined from the data given.

Question 71

The ion ICl₄^- has ________ valence electrons.

A)34
B)35
C)36
D)28
E)8

Question 72

Given the electronegativities below, which covalent single bond is most polar? Element: H C N O
Electronegativity: 2.1 2.5 3.0 3.5

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

Question 73

A ________ covalent bond between the same two atoms is the longest.

A)single
B)double
C)triple
D)strong
E)They are all the same length.

Question 74

A nonpolar bond will form between two ________ atoms of ________ electronegativity.

A)different, opposite
B)identical, different
C)different, different
D)similar, different
E)identical, equal

Question 75

How many hydrogen atoms must bond to silicon to give it an octet of valence electrons?

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

Question 76

What is the maximum number of double bonds that a carbon atom can form?

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

Question 77

What is the maximum number of triple bonds that a carbon atom can form?

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

Question 78

The ion NO^- has ________ valence electrons.

A)15
B)14
C)16
D)10
E)12

Question 79

Determining lattice energy from Born-Haber cycle data requires the use of ________.

A)the octet rule
B)Coulomb's law
C)Periodic law
D)Hess's law
E)Avogadro's number

Question 80

Electropositivity ________ from left to right within a period and ________ from top to bottom within a group.

A)decreases, increases
B)increases, increases
C)increases, decreases
D)stays the same, increases
E)increases, stays the same