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Chapter 6 Chemical Bonding

Total questions: 60

Worksheet time: 34mins

Name
Class
Date
1.

The diagram displayed is best titled a

a)

Chemical formula for ethanol

b)

Lewis structure for ethanol

c)

Molecular formula for ethanol

d)

Structure formula for ethanol

2.

The representation of Ethanol in the diagram could be best described as

a)

Chemical formula

b)

Resonance structure

c)

Structural formula

d)

Lewis structure

3.

McCl2 would be best considered as a

a)

Polyatomic ion

b)

Molecule

c)

Compound

d)

Diatomic compound

4.

Br2 would be described as a

a)

diatomic compound

b)

polyatomic compound

c)

diatomic molecule

d)

ionic compound

5.

The molecule in this diagram demonstrates

a)

polar covalent bonding

b)

ionic bonding

c)

non-polar covalent bonding

d)

metallic bonding

6.

The name of this molecule is

a)

Carbon oxide

b)

Carbon dioxide

c)

Carbon monoxide

d)

Carbonic acid

7.

How many bonds form between the carbon atom and an oxygen atom in the diagram

a)

1

b)

2

c)

3

d)

4

8.

The diagram is Formaldehyde. How many valance electrons are around the central atom?

a)

4

b)

6

c)

8

d)

2

9.

This molecule is an organic solvent. How would you describe the bonds in this molecule?

a)

Polar

b)

ionic

c)

non-polar

d)

metallic

10.

Which term best describes the lewis dot structure in the diagram

a)

ionic compound

b)

diatomic molecule

c)

polyatomic ion

d)

a large cation

11.

The yellow spheres in the diagram of the water molecule represent

a)

Lone pair electrons

b)

Double bonds

c)

Core electrons

d)

Empty space

12.

What is the main idea behind the VSEPR theory?

a)

electrons spread out as far as possible

b)

pairs of electrons spread out as far as possible

c)

electrons are attracted to protons

d)

neutrons block the attraction of electrons and protons

13.

According to VSEPR Theory and Molecular Geometry what describes the geometry of this molecule

a)

Linear

b)

Bent (angular)

c)

trigonal pyramidal

d)

Spiral

14.

The name of the molecule in the diagram is

a)

Ammonium

b)

Nitrate

c)

Ammonia

d)

Nitrogen ion

15.

According to VSEPR Theory and Molecular Geometry the molecule in the diagram would be

a)

Linear

b)

Trigonal planar

c)

Bent (angular)

d)

Trigonal pyramidal

16.

What is the name of the molecule in this diagram

a)

Carbon dioxide

b)

Carbohydrate

c)

Methane

d)

Ethane

17.

According to the VSEPR Theory and Molecular Geometry what is the shape of this molecule

a)

Linear

b)

Trigonal planer

c)

Bent (angular)

d)

Tetrahedral

18.

Typically, atoms gain, lose or share valence electrons to achieve

a)

an exchange of energy

b)

a stable valence electron configuration

c)

vaporization

d)

an exchange of protons

19.

What element has the highest electronegativity?

a)

neon

b)

hydrogen

c)

francium

d)

oxygen

20.

How many electrons on the outside shell make an atom stable?

a)

2

b)

4

c)

6

d)

8

21.

Which one is not a diatomic molecule?

a)

I2

b)

C2H6

c)

O2

d)

Br2

22.

What is the sum of valence electrons around Na, Mg, N and F?

a)

13

b)

14

c)

15

d)

16

23.

Which one of these can make 2 bonds?

a)

Al

b)

O

c)

N

d)

F

24.

Which of the following would have the greatest bond energy

a)

N2

b)

H2

c)

O2

d)

F2

25.

Bond length of atoms is normally measured in

a)

kilojoules/mole

b)

millimeters

c)

picometers

d)

nanoliters

26.

What determines bond strength?

a)

distance between atoms

b)

electronegativity

c)

ionization energy

d)

group # of atoms

27.

According to the VSEPR theory, which one is bent? Use the chart on page 190 of textbook

a)

AB3E

b)

AB2E2

c)

ABE

d)

AB2

28.

What would be the shape of an BeF2?

a)

trigonal planar

b)

bent

c)

linear

d)

polyhedral

29.

In order, say if these are polar or nonpolar: HF, HCl, CO and Br2. Charts on page 166 & 153

a)

Polar, Non-polar, Polar, Polar

b)

Polar, Polar, Non-polar, Polar

c)

Polar, Polar, Polar, Non-Polar

d)

Non-Polar,Polar, Polar, Polar

30.

In order, say if these are polar or nonpolar: HF, HCl, CO and Br2. Charts on page 166 & 153

a)

Polar, Non-polar, Polar, Polar

b)

Polar, Polar, Non-Polar, Polar

c)

Polar, Polar,Polar, Non-Polar

d)

Non-PolarPolar,Polar, Polar

31.

Metal bonded to metal forms which type of bond?

a)

polar covalent

b)

ionic

c)

metallic

d)

nonpolar covalent

32.

Metal bonded to NONmetal would be which type of bond?

a)

ionic

b)

metallic

c)

polar covalent

d)

non polar covalent

33.

NONmetal bonded to nonmetal would be which type of bond?

a)

ionic

b)

covalent

c)

metallic

34.

Why do atoms bond?

a)

to become more stable

b)

to lose electrons

c)

to gain electrons

d)

to gain potential energy

35.

Which one is not an intermolecular force?

a)

London dispersion forces

b)

Dipole dipole forces

c)

hydrogen bonding

d)

ionic bonding

36.

As individual atoms, the atoms are

a)

high in energy

b)

low in energy

c)

have zero energy

d)

are highly explosive

37.

How many valence electrons in aluminum?

a)

1

b)

2

c)

3

d)

5

38.

The type of bond formed when electrons are shared equally is called

a)

ionic

b)

covalent nonpolar

c)

covalent polar

d)

metallic

39.

To draw a Lewis structure, what must you know?

a)

atomic number

b)

atomic mass

c)

the number of valence electrons

d)

the period it's from on the Periodic Table

40.

The greater the electronegativity difference in two bonded atoms, the greater the % of

a)

ionic character

b)

covalent character

c)

metallic character

d)

poor character

41.

What does the R stand for in VSEPR?

a)

Retraction

b)

Repair

c)

Repulsion

d)

Rectangle

e)

Revoluiton

42.

When a balloon rubbed on my head approaches the wall a temporary diplole is formed. which force hold the balloon on the wall? Read pages 193-197.

a)

london dispersion force

b)

dipole-dipole

c)

hydrogen bond

d)

intramolecular force

43.

In almost all cases, how many bonds can a sulfur atom make?

a)

1

b)

2

c)

3

d)

4

44.

What shape is a water molecule?

a)

trigonal planar

b)

bent

c)

linear

d)

tetrahedral

45.

Ca bonded to F, ionic or covalent?

a)

ionic

b)

covalent

46.

Nitrogen bonded to Oxygen, ionic or covalent?

a)

ionic

b)

covalent

47.

What is the steric number of the central atom in Carbon Dioxide

a)

0

b)

1

c)

2

d)

3

e)

4

48.

In a metal lattice, ____________________ are surrounded by a pool of shared electrons.

a)

cations

b)

oversized nuclei

c)

anions

d)

double bonds

e)

polyatomic ions

49.

Why are metals good conductors of electric current?

a)

Metals are strong

b)

Metals are malleable

c)

Metals are inert

d)

Metals contain a shared pool of electrons that move freely

50.

Which is most likely to shatter when hit - sodium chloride or an alloy of metals called bronze?

a)

sodium chloride

b)

bronze

51.

Which is the strongest of the intermolecular bonds?

a)

ion-ion

b)

Dipole-Dipole

c)

Hydrogen bonding

d)

London dispersion forces

52.

Hybridization refers to the mixing of (read page 191-193)

a)

2 or more atomic orbitals (s and p) to produce new orbitals

b)

mixing of intermolecular and intramolecular bonds

c)

2 or more electrons to produce new electrons

d)

2 or more protons to produce new atomic orbitals

53.

In an ionic crystal structure the ions

a)

maximize potential energy by forming a lattice structure

b)

maximize energy by forming an amorphous chaotic structure

c)

minimize potential energy by forming a lattice structure

d)

minimize energy by forming an amorphous structure

54.

The behavior of substances in the solid state are governed by the way ions are arranged and the

a)

forces that drive them apart

b)

the intramolecular bonds

c)

forces that hold them together

d)

the colour of the crystals formed

55.

Observing a pure crystal indicates how the atoms are arranged at the molecular level because

a)

of repeated pattern of hydrogen bonding

b)

the potential energy of bond is easy to observe

c)

the pattern of intramolecular bond keeps repeating itself

d)

The molecules stop moving so they are easy to observe

e)

the pattern of intermolecular bond keeps repeating itself

56.

The ability of metal to be drawn into wires.

a)

Moving Electrons

b)

Malleability

c)

Ductility

d)

Electrical conductivity

57.

The ability of metal to be hammered into sheets.

a)

Moving Electrons

b)

Malleability

c)

Ductility

d)

Thermal conductivity

58.
Which type of bond has an unequal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
59.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
60.

In chemical compounds, non covalent bonds form when

a)

the electronegativity difference between two atoms is very large.

b)

electrons are completely transferred between two metals.

c)

pairs of electrons are shared between two nonmetal atoms.

d)

two nonmetal atoms are attracted to each other by opposite charges.

e)

the electronegativity difference is equal to 1.75 according to the pauling scale.

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