Deck 8: Basic Concepts of Chemical Bonding

Question 1

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

A)HBr
B)HI
C)HCl
D)HF
E)H₂

Answer 1

HF

Question 2

The oxidation number of iron in Fe₂O₃ is ________.

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

Answer 2

+3

Question 3

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 3

increases, increase, decrease

Question 4

For ________ forms of a molecule or ion,the observed structure is an average of the ________ forms.

A)resonance, covalent
B)resonance, resonance
C)ionic, resonance
D)resonance, ionic
E)resonance, metallic

Question 5

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 6

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 7

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 8

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

Question 9

Which energy change corresponds to the first ionization energy of potassium?

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

Question 10

Which energy change corresponds to the electron affinity of fluorine?

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

Question 11

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 12

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

A)
B)
C)
D)
E)

Question 13

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 14

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 15

How many electrons are in the Lewis structure of a nitrite ion (NO₂^-)?

A)18
B)17
C)16
D)23
E)24

Question 16

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 17

Which of the following bonds would be considered non-polar covalent?

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

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

Which of the following has eight valence electrons?

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

Question 20

There can be two equivalent best resonance structures of ________.

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

Question 21

________ is an explosive made of nitroglycerine and an absorbent such as diatomaceous earth.

A)KOH
B)TNT
C)C-4
D)KBr
E)CFC

Question 22

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 23

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

A)NI₃
B)SO₂
C)ICl₅
D)SiF₄
E)CO₂

Question 24

Which of the following does not have eight valence electrons?

A)Cl^-
B)Xe
C)Ti⁺⁴
D)Rb⁺
E)Sr⁺

Question 25

Which of the following Lewis structures would be an incomplete octet?

A)NF₃
B)SO₂
C)BCl₃
D)CF₄
E)SO₃^2-

Question 26

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 27

There can be three equivalent best resonance structures of ________.

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

Question 28

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 29

Bond enthalpy is ________.

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

Question 30

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 31

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 32

Which of the following atoms may have an expansion to the octet?

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

Question 33

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 34

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 35

Dynamite consists of nitroglycerine mixed with diatomaceous earth or cellulose.What is another name for dynamite?

A)KBr
B)KOH
C)TNT
D)C-4
E)CFC

Question 36

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, is unpredictable

Question 37

Which of the following Lewis structures would be an expansion to the octet rule?

A)SiF₄
B)CF₄
C)CCl₄
D)PO₄^3-
E)NF₃

Question 38

Which of the following Lewis structures would be an expansion to the octet rule?

A)PH₃
B)PCl₃
C)CCl₄
D)CO₂
E)SO₃

Question 39

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 40

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

A)SF₄
B)KrF₂
C)CF₄
D)XeF₄
E)ICl₄^-

Question 41

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 42

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

A)Mn²⁺
B)Cr²⁺
C)V³⁺
D)Fe³⁺
E)K⁺

Question 43

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 44

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

A)I²⁺
B)I⁴⁺
C)I^4-
D)I⁺
E)I^-

Question 45

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 46

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

A)Al³⁺
B)Al⁴⁺
C)Al^4-
D)Al⁺
E)Al^-

Question 47

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

A)Mn²⁺
B)Cr²⁺
C)V³⁺
D)Fe³⁺
E)K⁺

Question 48

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 49

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

A)Mg²⁺
B)Mg^2-
C)Mg^6-
D)Mg⁶⁺
E)Mg^-

Question 50

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 51

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 52

What is the electron configuration for the Cu²⁺ ion?

A)[Ar]4s⁰3d¹⁰
B)[Ar]4s⁰3d¹⁰.
C)[Ar]4s⁰3d⁹
D)[Ar]4s²3d⁹.
E)[Ar]4s⁰3d¹¹

Question 53

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 54

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 55

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

A)P³⁺
B)P^3-
C)P⁵⁺
D)P^5-
E)P⁺

Question 56

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 57

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 58

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 59

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 60

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 61

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 62

The ion ICl₄^- has ________ valence electrons.

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

Question 63

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 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

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 66

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 67

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 68

The formula of palladium (IV)sulfide is ________.

A)Pd₂S₄
B)PdS₄
C)Pd₄S
D)PdS₂
E)Pd₂S₂

Question 69

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 70

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 71

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 72

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 73

The ion PO₄^3- has ________ valence electrons.

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

Question 74

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

Question 75

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 76

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

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

Question 77

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 78

The ion NO^- has ________ valence electrons.

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

Question 79

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

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

Question 80

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