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Topic 4 Chem Bonding

Total questions: 128

Worksheet time: 5hrs 28mins

Name
Class
Date
1.

Which is correct for all solid ionic compounds?

a)

High volatility

b)

Poor electrical conductivity

c)

Low melting point

d)

Good solubility in water

2.

How does a lithium atom form the most stable ion?

a)

The atom gains a proton to form a positive ion.

b)

The atom loses a proton to form a negative ion.

c)

The atom loses an electron to form a positive ion.

d)

The atom gains an electron to form a negative ion.

3.

What is the IUPAC name of NiCO3?

a)

nickel(II) carbonate

b)

nickel carbonate

c)

nickel(I) carbonate

d)

nitrogen(I) carbonate

4.

How does a lithium atom form the most stable ion?

a)

The atom gains a proton to form a positive ion.

b)

The atom loses a proton to form a negative ion.

c)

The atom loses an electron to form a positive ion.

d)

The atom gains an electron to form a negative ion.

5.

A substance has the above properties:

What is the most probable structure of this substance?

a)

Network covalent

b)

Polar covalent molecule

c)

Ionic lattice

d)

Metallic lattice

6.

Which bonds cause the boiling point of water to be significantly greater than that of hydrogen sulfide?

a)

London (dispersion)

b)

Covalent

c)

Ionic

d)

Hydrogen

7.

Which of the following does not react with dilute HCl(aq)?

a)

Na2CO3

b)

Cu

c)

Zn

d)

CuO

8.

Which compound contains both ionic and covalent bonds?

a)

SIH4

b)

NaNO3

c)

H2CO

d)

Na2S

9.

Which substance has the following properties?


• Low melting point

• Very soluble in water

• Does not conduct electricity when molten

a)

Glucose, C6H12O6

b)

Silicon dioxide, SiO2

c)

Sodium chloride, NaCl

d)

Tetrachloromethane, CCl4

10.

What is the formula of ammonium phosphate?

a)

(NH3)3PO4

b)

(NH4)3PO4

c)

(NH4)2PO4

d)

(NH3)2PO3

11.

What is the formula of magnesium nitride?

a)

MgN

b)

Mg2N3

c)

Mg3N

d)

Mg3N2

12.

The formula of gallium phosphate is GaPO4. What is the correct formula of gallium sulfate?

a)

GaSO4

b)

GaS

c)

Ga2(SO4)3

d)

Ga2S

13.

Which compound has the shortest C to O bond?

a)

CH3CHO

b)

CO

c)

CO2

d)

C2H5OC2H5

14.

Which species has the longest carbon to oxygen bond length?

a)

CO

b)

CH3OH

c)

CH3CO2−

d)

H2CO

15.

What are the predicted electron domain geometries around the carbon and both nitrogen atoms in urea, (NH2)2CO, applying VSEPR theory?

a)

A

b)

B

c)

C

d)

D

16.

Which compound has the shortest C–N bond?

a)

CH3NH2

b)

(CH3)3CNH2

c)

CH3CN

d)

CH3CHNH

17.

The electronegativity values of four elements are given.

What is the order of increasing polarity of the bonds in the following compounds?

a)

CO < OF2 < NO < CF4

b)

CF4 < CO < OF2 < NO

c)

NO < OF2 < CO < CF4

d)

CF4 < NO < OF2 < CO

18.

Which two atoms form the most polar bond?

a)

C and F

b)

C and Cl

c)

Si and F

d)

Si and Cl

19.

How many bonding electrons are there in the urea molecule?

a)

8

b)

16

c)

20

d)

24

20.

Which molecule is non-polar?

a)

OF2

b)

NH3

c)

BF3

d)

SO2

21.

How many electrons form the carbon–oxygen bond in methanal, HCHO?

a)

2

b)

4

c)

8

d)

12

22.

Which statement is correct about carbon-oxygen bond lengths?

a)

The C–O bond lengths are equal in propanoic acid, C2H5COOH.

b)

The C–O bond length in carbon dioxide, CO2, is longer than the C–O bond length in methanol, CH3OH.

c)

The C–O bond length in carbon dioxide, CO2, is longer than the C–O bond length in carbon monoxide, CO.

d)

The C–O bond lengths are equal in ethyl ethanoate, CH3COOC2H5.

23.

Which diatomic molecule has the strongest bonding between its atoms?

a)

H2

b)

N2

c)

O2

d)

F2

24.

Which molecule is non-polar?

a)

CCl4

b)

CH2Cl2

c)

CH3Cl

d)

CO

25.

Which combination of length and strength of the carbon‒to‒carbon bonds in C2H2 and C2H4 is correct?

a)

A

b)

B

c)

C

d)

D

26.

Which compounds contain both ionic and covalent bonding?

I. CaCO3

II. NaCl

III. NaOH

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

27.

Which sequence has the molecules in order of increasing nitrogen-nitrogen bond length?

a)

N2 < N2H4 < N2H2

b)

N2 < N2H2 < N2H4

c)

N2H4 < N2H2 < N2

d)

N2H2 < N2H4 < N2

28.

A solid has a melting point of 1582 °C and does not dissolve in water. It does not conduct electricity in the molten state. What type of structure does the solid have?

a)

Ionic

b)

Metallic

c)

Giant molecular

d)

Simple molecular

29.

What is the difference between the strength and the length of the carbon-oxygen bond in butanal and in butan-1-ol?

a)

The bond in butanal is stronger and longer than in butan-1-ol.

b)

The bond in butanal is weaker and shorter than in butan-1-ol.

c)

The bond in butanal is weaker and longer than in butan-1-ol.

d)

The bond in butanal is stronger and shorter than in butan-1-ol.

30.

Which statements are correct for the bonds between two carbon atoms?

I. Single bonds are longer than triple bonds.

II. Single bonds are stronger than double bonds.

III. Triple bonds are stronger than double bonds.

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

31.

Which bond is the least polar?

a)

C–H

b)

F–H

c)

O–H

d)

N–H

32.

Which statement about the physical properties of substances is correct?

a)

The only solids that conduct electricity are metals.

b)

All substances with covalent bonds have low melting points.

c)

Ionic solids are always brittle.

d)

All metals have high densities.

33.

Which single covalent bond is the most polar, given the following electronegativity values?

a)

C–O

b)

S–H

c)

C–H

d)

O–H

34.

Which bonds are arranged in order of increasing polarity?

a)

H–F < H–Cl < H–Br < H–I

b)

H–I < H–Br < H–F < H–Cl

c)

H–I < H–Br < H–Cl <H–F

d)

H–Br < H–I < H–Cl < H–F

35.

When C2H2, C2H4 and C2H6 are arranged in order of increasing carbon-carbon bond strength (weakest bond first), what is the correct order?

a)

C2H2, C2H4, C2H6

b)

C2H2, C2H6, C2H4

c)

C2H6, C2H4, C2H2

d)

C2H6, C2H2, C2H4

36.

The number of electrons in the valence shell of elements A and B, are 6 and 7 respectively. What is the formula and type of bonding in a compound formed by these elements?

a)

A2B, covalent

b)

AB2, covalent

c)

A2B, ionic

d)

AB2, ionic

37.

Which describes a resonance structure?

a)

Double bond can be drawn in alternative positions.

b)

Bonds vibrate by absorbing IR radiation.

c)

A double and a single bond in the molecule

d)

A Lewis structure

38.

What is the structure and bonding in SiO2 (s)?

a)

A

b)

B

c)

C

d)

D

39.

Which species does not have resonance structures?

a)

C6H6

b)

NH4+

c)

CO32−

d)

O3

40.

Which molecule contains an incomplete octet of electrons?

a)

NF3

b)

BF3

c)

BrF

d)

SF2

41.

How many lone pairs and bonding pairs of electrons surround the central chlorine atom in ClF2+?

a)

A

b)

B

c)

C

d)

D

42.

Which molecule is polar?

a)

BeCl2

b)

BCl3

c)

NCl3

d)

CCl4

43.

Which species has the same molecular geometry as SO32−?

a)

BF3

b)

SO3

c)

PF3

d)

CO32−

44.

Which form of carbon is the poorest electrical conductor?

a)

Graphite

b)

Graphene

c)

Diamond

d)

Carbon nanotube

45.

What is the molecular geometry and bond angle in the molecular ion NO3−?

a)

A

b)

B

c)

C

d)

D

46.

Which combination describes the sulfate(IV) ion, SO32– (also known as sulfite ion)?

a)

A

b)

B

c)

C

d)

D

47.

Which correctly states the strongest intermolecular forces in the compounds below?

a)

A

b)

B

c)

C

d)

D

48.

What are the approximate bond angles and structure of crystalline SiO2?

a)

A

b)

B

c)

C

d)

D

49.

Which compound has resonance structures?

a)

C6H12

b)

CH3CHO

c)

NaBr

d)

Na2CO3

50.

Which substance has a giant covalent structure?

a)

A

b)

B

c)

C

d)

D

51.

Which pair of molecules has the same bond angles?

a)

PCl3 and BCl3

b)

SO2 and CO2

c)

H2O and NH3

d)

CCl4 and SiH4

52.

Which molecules react to form a dative covalent (coordinate) bond?

a)

CH4 and NH3

b)

C2H2 and Cl2

c)

NH3 and HF

d)

Cl2 and HF

53.

What describes the relationship between diamond, graphite and C60 fullerene?

a)

Allotropes

b)

Isomers

c)

Isotopes

d)

Polymers

54.

What describes the structure of silicon and silicon dioxide?

a)

A

b)

B

c)

C

d)

D

55.

Which species contain a dative covalent (coordination or coordinate) bond?

I. Carbon monoxide, CO

II. Ammonia, NH3

III. Oxonium ion, H3O+

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

56.

Which combination of shape and bond angle best describes a molecule of sulfur dioxide, SO2?

a)

A

b)

B

c)

C

d)

D

57.

Which diagrams can be used to represent the Lewis (electron dot) structure of boron trifluoride?

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

58.

Which species contains a bond angle of approximately 107°?

a)

H2O

b)

CF4

c)

NCl3

d)

BF3

59.

Which species contains a dative covalent (coordinate) bond?

a)

HCN

b)

C2H2

c)

CO2

d)

CO

60.

What is the shape and the bond angle of the molecule BF3?

a)

A

b)

B

c)

C

d)

D

61.

Which pair has the same bond angles?

a)

CH4 and NH4+

b)

NH3 and H2O

c)

C2H4 and C2H2

d)

CO2 and SO2

62.

Which diagram represents the bonding in SiO2?

a)

A

b)

B

c)

C

d)

D

63.

Which group of ions and molecules has delocalized electrons in all the species?

a)

CH3COCH3, C2H5COO−, and O3

b)

NO−3, NO−2, and CO2

c)

C6H6, CO2−3, and graphite

d)

C6H6, CO2−3, and C2H2

64.

The Lewis (electron dot) structure of aspirin is represented above. What are the approximate values of the bond angles α, β, and γ, in the molecule?

a)

α = 90o; β = 104.5o; γ = 104.5o

b)

α = 90o; β = 120o; γ = 120o

c)

α = 109.5o; β = 120o; γ = 120o

d)

α = 109.5o; β = 104.5o; γ = 120o

65.

Which combination best describes the type of bonding present and the melting point of silicon and silicon dioxide?

a)

A

b)

B

c)

C

d)

D

66.

Which statements about graphite are correct?

I. Carbon atoms are held in layers with weak attractions between layers.

II. Graphite is a non-metal which conducts electricity.

III. Each carbon atom is covalently bonded to three other carbon atoms.

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

67.

Which statements about the structure and bonding of silicon dioxide are correct?

a)

A

b)

B

c)

C

d)

D

68.

Diamond, C60 fullerene and graphite are allotropes of carbon. Which statements are correct about these allotropes?

I. In diamond each carbon is held in a tetrahedral arrangement.

II. In C60 fullerene each carbon is held in a trigonal arrangement.

III. In graphite each carbon is held in a tetrahedral arrangement.

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

69.

The Lewis (electron dot) structure of paracetamol (acetaminophen) is above. What are the approximate values of the bond angles?

a)

α = 104.5o; β = 120o; γ = 109.5o

b)

α = 109.5o; β = 109.5o; γ = 109.5o

c)

α = 120o; β = 120o; γ = 90o

d)

α = 104.5o; β = 120o; γ = 90o

70.

C60 fullerene consists of a simple molecular structure. Silicon dioxide, SiO2, can be described as a giant covalent (macromolecular) structure. Which statements are correct?

I. Each carbon atom in C60 fullerene is bonded in a sphere of 60 carbon atoms, consisting of pentagons and hexagons.

II. Each O–Si–O bond angle in SiO2 is 180°.

III. SiO2 is insoluble in water.

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

71.

Which species contain dative covalent bonds?

I. CO

II. NH3

III. H3O+

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

72.

Which row correctly describes the bonding type and melting point of carbon and carbon dioxide?

a)

A

b)

B

c)

C

d)

D

73.

How do the bond angles in CH4, NH3 and H2O compare?

a)

CH4 = NH3 = H2O

b)

CH4 < NH3 < H2O

c)

NH3 < CH4 < H2O

d)

H2O < NH3 < CH4

74.

What is the correct Lewis structure for hypochlorous acid, a compound containing chlorine, hydrogen and oxygen?

a)

A

b)

B

c)

C

d)

D

75.

Which molecule has a non-bonding (lone) pair of electrons on the central atom?

a)

BF3

b)

SO2

c)

CO2

d)

SiF4

76.

Lewis structures are represented in different ways in different parts of the world. Two ways of drawing the Lewis structure for H3O+ are shown here. Which statement is correct about H3O+?

a)

The ion has a tetrahedral shape.

b)

The H–O–H bond angle is 120°.

c)

The H–O–H bond angle is 90°.

d)

The ion has a trigonal pyramidal shape.

77.

The Lewis structure of SO2 is given here. What is the shape of the SO2 molecule?

a)

Bent (V-shaped)

b)

Linear

c)

T-shaped

d)

Triangular planar

78.

Which species contain a dative covalent bond?

I. HCHO

II. CO

III. H3O+

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

79.

What is the shape of the ammonia molecule, NH3?

a)

Trigonal planar

b)

Trigonal pyramidal

c)

Linear

d)

V-shaped (bent)

80.

Which molecule is polar?

a)

CH2Cl2

b)

BCl3

c)

Cl2

d)

CCl4

81.

Which compound has a covalent macromolecular (giant covalent) structure?

a)

MgO (s)

b)

Al2O3 (s)

c)

P4O10 (s)

d)

SiO2 (s)

82.

Which molecule has an octahedral shape?

a)

SF6

b)

PCl5

c)

XeF4

d)

BF3

83.

How many non-bonding pairs of electrons are there in a nitrogen molecule?

a)

0

b)

1

c)

2

d)

3

84.

Which molecule contains a bond angle of approximately 120°?

a)

CH4

b)

C2H2

c)

C2H4

d)

C2H6

85.

Which is the best description of the bonding present in silicon dioxide, SiO2?

a)

Each silicon atom forms four single covalent bonds to oxygen atoms.

b)

Each silicon atom forms two double covalent bonds to oxygen atoms.

c)

Each silicon atom forms two single covalent bonds to oxygen atoms.

d)

Each silicon atom forms four double covalent bonds to oxygen atoms.

86.

What is the bond angle in the H3O+ ion?

a)

104°

b)

107°

c)

109°

d)

120°

87.

How many atoms is each carbon directly bonded to in its allotropes?

a)

A

b)

B

c)

C

d)

D

88.

Which molecule contains a dative covalent (coordinate) bond?

a)

HCN

b)

H2O2

c)

CO2

d)

CO

89.

Which describes an ionic compound?

a)

A

b)

B

c)

C

d)

D

90.

What is the order of increasing boiling point?

a)

CH3CH2CH2CH3<CH3CH(OH)CH3<CH3COCH3<CH3CO2H

b)

CH3CH2CH2CH3<CH3COCH3<CH3CH(OH)CH3<CH3CO2H

c)

CH3CO2H<CH3COCH3<CH3CH(OH)CH3<CH3CH2CH2CH3

d)

CH3CH2CH2CH3<CH3COCH3<CH3CO2H<CH3CH(OH)CH3

91.

Which compound has hydrogen bonds between its molecules?

a)

CH4

b)

CH4O

c)

CH3Cl

d)

CH2O

92.

Which compound has the highest boiling point?

a)

CH3CHO

b)

CH3CH2F

c)

CH3OCH3

d)

CH3CH2NH2

93.

What are the strongest intermolecular forces between molecules of propanone, CH3COCH3, in the liquid phase?

a)

London (dispersion) forces

b)

Covalent bonding

c)

Hydrogen bonding

d)

Dipole–dipole forces

94.

The compounds shown below have similar relative molecular masses. What is the correct order of increasing boiling point?

a)

CH3COOH < (CH3)2CO < (CH3)2CHOH

b)

CH3COOH < (CH3)2CHOH < (CH3)2CO

c)

(CH3)2CO < CH3COOH < (CH3)2CHOH

d)

(CH3)2CO < (CH3)2CHOH < CH3COOH

95.

Which forces are present between molecules of carbon dioxide in the solid state?

a)

Permanent dipole-permanent dipole interactions

b)

Temporary dipole-induced dipole interactions (London/dispersion forces)

c)

Covalent bonding

d)

Ionic bonding

96.

The following compounds have similar molar masses:

CH3CH2COOH, CH3CH2CH2CH2OH and CH3CH2CH2CH2CH3


What is the order of increasing boiling points?

a)

CH3CH2CH2CH2OH<CH3CH2COOH<CH3CH2CH2CH2CH3

b)

CH3CH2COOH<CH3CH2CH2CH2CH3<CH3CH2CH2CH2OH

c)

CH3CH2COOH<CH3CH2CH2CH2OH<CH3CH2CH2CH2CH3

d)

CH3CH2CH2CH2CH3<CH3CH2CH2CH2OH<CH3CH2COOH

97.

Which correctly lists butane (Mr=58), propanone (Mr=58), propan-1-ol (Mr=60) and propan-2-ol (Mr=60) in order of increasing boiling point?

a)

C4H10 < CH3COCH3 < CH3CH(OH)CH3 < CH3CH2CH2OH

b)

CH3CH2CH2OH < CH3CH(OH)CH3 < CH3COCH3 < C4H10

c)

C4H10 < CH3CH(OH)CH3 < CH3CH2CH2OH < CH3COCH3

d)

C4H10 < CH3COCH3 < CH3CH2CH2OH < CH3CH(OH)CH3

98.

Which process involves the breaking of hydrogen bonds?

a)

2HI(g) → H2(g) + I2(g)

b)

CH4(g) → C(g) + 4H(g)

c)

H2(l) → H2(g)

d)

NH3(l) → NH3(g)

99.

What is the correct order of increasing boiling point?

a)

C2H6 < HCHO < CH3OH

b)

HCHO < C2H6 < CH3OH

c)

CH3OH < HCHO < C2H6

d)

C2H6 < CH3OH < HCHO

100.

Which combination of properties is correct?

a)

A

b)

B

c)

C

d)

D

101.

Which compound has the highest boiling point?

a)

CH3CH3

b)

CH3OH

c)

CH3CH2OH

d)

CH3CH2CH3

102.

Which statements are correct about hydrogen bonding?

I. It is an electrostatic attraction between molecules.

II. It is present in liquid ammonia.

III. It is a permanent dipole-permanent dipole attraction.

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

103.

Which compound has the lowest boiling point?

a)

CH3CH2CH2OH

b)

CH3CH2CH2BR

c)

CH3CH2COOH

d)

CH3CH2CH2CH3

104.

What is the correct order of increasing boiling points?

a)

CH3CH3<CH3CH2Cl<CH3CH2Br<CH3CH2I

b)

CH3CH2Cl<CH3CH2Br<CH3CH3<CH3CH2I

c)

CH3CH2I<CH3CH2Br<CH3CH2Cl<CH3CH3

d)

CH3CH2Br<CH3CH2Cl<CH3CH2I<CH3CH3

105.

Which compound forms hydrogen bonds in the liquid state?

a)

C2H5OH

b)

CHCl3

c)

CH3CHO

d)

(CH3CH2)3N

106.

Which change explains why the boiling points of the halogens increase as their molecular masses increase?

a)

The intermolecular attraction due to temporarily induced dipoles increases.

b)

The gravitational attraction between molecules increases.

c)

The polarity of the bond within the molecule increases.

d)

The strength of the bond within the molecule increases.

107.

Four identical sealed containers are prepared each containing 10 cm3 of an organic compound and at the temperature shown below. Which container will have the highest vapour pressure?

a)

A

b)

B

c)

C

d)

D

108.

Which order is correct when the following compounds are arranged in order of increasing melting point?

a)

CH4 < H2S < H2O

b)

H2S < H2O < CH4

c)

CH4 < H2O < H2S

d)

H2S < CH4 < H2O

109.

Which substance can form intermolecular hydrogen bonds in the liquid state?

a)

CH3OCH3

b)

CH3CH2OH

c)

CH3CHO

d)

CH3CH2CH

110.

Which compound does not form hydrogen bonds between its molecules?

a)

CH3NH2

b)

CH3COCH3

c)

CH3COOH

d)

CH3CH2OH

111.

Which statement best describes the intramolecular bonding in HCN(l)?

a)

Electrostatic attractions between H+ and CN− ions

b)

Only van der Waals’ forces

c)

Van der Waals’ forces and hydrogen bonding

d)

Electrostatic attractions between pairs of electrons and positively charged nuclei

112.

What is the correct order if the compounds are arranged in order of increasing boiling point?

a)

H4 < CH3Cl < SiH4 < CH3OH

b)

CH3OH < CH4 < CH3Cl < SiH4

c)

CH3OH < CH3Cl < SiH4 < CH4

d)

CCH4 < SiH4 < CH3Cl < CH3OH

113.

Which combination corresponds to a strong metallic bond?

a)

A

b)

B

c)

C

d)

D

114.

Which combination causes the strength of metallic bonding to increase?

a)

A

b)

B

c)

C

d)

D

115.

Which combination corresponds to a strong metallic bond?

a)

A

b)

B

c)

C

d)

D

116.

Which metal has the strongest metallic bonding?

a)

Na

b)

Mg

c)

Al

d)

Ca

117.

A substance has the above properties:


What is the most probable structure of this substance?

a)

Network covalent

b)

Polar covalent molecule

c)

Ionic lattice

d)

Metallic lattice

118.

Which metal has the strongest metallic bond?

a)

Li

b)

Na

c)

K

d)

Rb

119.

Which particles are present in the lattice of a metal?

a)

Negative ions

b)

Positive and negative ions

c)

Positive ions

d)

Molecules

120.

A solid has a melting point of 1582 °C and does not dissolve in water. It does not conduct electricity in the molten state. What type of structure does the solid have?

a)

Ionic

b)

Metallic

c)

Giant molecular

d)

Simple molecular

121.

Which is the best description of a metallic bond?

a)

Electrostatic attraction between oppositely charged ions

b)

Electrostatic attraction between a pair of electrons and positively charged nuclei

c)

Electrostatic attraction between a lattice of positive ions and delocalized electrons

d)

Electrostatic attraction for a bonding pair of electrons which have been supplied by one of the atoms

122.

Which statement about the physical properties of substances is correct?

a)

The only solids that conduct electricity are metals.

b)

All substances with covalent bonds have low melting points.

c)

Ionic solids are always brittle.

d)

All metals have high densities.

123.

Zinc metal contains metallic bonding. Which is the best description of a metallic bond?

a)

The electrostatic attraction between a pair of electrons and positively charged nuclei.

b)

The electrostatic attraction between oppositely charged ions.

c)

The electrostatic attraction between a lattice of positive ions and delocalized electrons.

d)

The bond formed when one atom provides both electrons in a shared pair.

124.

Which particles are responsible for electrical conductivity in metals?

a)

Anions

b)

Cations

c)

Electrons

d)

Protons

125.

Which particles are responsible for the conduction of electricity in molten aluminium?

a)

Cations

b)

Anions

c)

Electrons

d)

Protons

126.

Which substance is made up of a lattice of positive ions and free moving electrons?

a)

Graphite

b)

Sodium chloride

c)

Sulfur

d)

Sodium

127.

Which substance does not conduct electricity?

a)

Solid zinc

b)

Molten zinc

c)

Solid zinc chloride

d)

Molten zinc chloride

128.

Which statement best describes metallic bonding?

a)

Electrostatic attractions between oppositely charged ions

b)

Electrostatic attractions between a lattice of positive ions and delocalized electrons

c)

Electrostatic attractions between a lattice of negative ions and delocalized protons

d)

Electrostatic attractions between protons and electrons

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