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Materials Science Part 1 (Lewis Structures) Review

Total questions: 69

Worksheet time: 1hrs 13mins

Name
Class
Date
1.
If fluorine is stronger then carbon, what charge will the fluorine receive?
a)
negative
b)
slight negative
c)
positive
d)
slight positive
2.
Type of intermolecular force present in HF.
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
3.
H2S has what kind of intermolecular force?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
4.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
5.

The model used to describe and explain the bonding and arrangement of atoms in a solid metal is the

a)

ball and stick model

b)

electron sea model

c)

metalloid model

d)

valence shell electron pair repulsion theory

6.

Which is the strongest intermolecular force below?

a)

Ionic

b)

Dispersion

c)

Hydrogen bonding

d)

dipole-dipole

7.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
8.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
9.
This could be the dot diagram of
a)
Mg
b)
Cl
c)
C
d)
O
10.
This could be the dot diagram of
a)
O
b)
B
c)
Li
d)
Ne
11.
This could be the dot diagram of 
a)
Ne
b)
Si
c)
Al
d)
Be
12.
Rank these in order of strength:
covalent bond
London forces
hydrogen bond
dipole-dipole attraction
a)
dipole-dipole>covalent bond>hydrogen bond>London
b)
London>dipole-diple>hydrogen bond>covalent bond
c)
covalent bond>hydrogen bond>dipole-dipole>London
d)
hydrogen bond>dipole-dipole>London>covalent bond
13.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
14.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
15.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
16.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
17.
How many electrons can be used in the Lewis Structure for : NO3 -
a)
23
b)
20
c)
18
d)
24
18.
How many valence electrons are available for bonding in the sulfate ion (SO4-2)?
a)
30 electrons
b)
32 electrons
c)
28 electrons
d)
impossible to tell
19.
How many electrons does each line indicate are shared?
a)
1
b)
2
c)
3
d)
4
20.
A Lewis structure can be used for showing an ionic bond but instead for dashes for the bonds positive and negative _____ are represented.
a)
atoms
b)
ions
c)
molecules
d)
electrons
21.
If electrons are shared unequally then the bond is....
a)
Non-polar covalent
b)
Ionic
c)
Non-polar ionic
d)
Polar covalent
22.
If electrons are shared equally then the bond is....
a)
Non-polar covalent
b)
Ionic
c)
Non-polar ionic
d)
Polar covalent
23.
Metals and nonmetals form which kind of bond?
a)
Polar covalent
b)
Ionic
c)
Non-polar covalent
d)
Metallic
24.
How strongly an atom attracts electrons is called....................
a)
Ionization energy
b)
Electronegativity
c)
Electricity
d)
Nuclear force
25.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
26.
In the correct Lewis structure for CH4, how many unshared electron pairs surround the carbon?
a)
2
b)
8
c)
0
d)
4
27.
In CO2, how many UNSHARED pairs of electrons does each oxygen have?
a)
2
b)
1
c)
4
d)
6
28.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
29.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
30.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
31.

How many total valence electrons are participating in bonding in the molecule above?

a)

8

b)

4

c)

2

d)

3

32.

CO2 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

e)

4

33.

Carbonate (CO32-) has how many double bonds?

a)

0

b)

1

c)

2

d)

3

34.

In HCN (Carbon is usually the central atom) what kind of bond is between the C and N

a)

Single

b)

Double

c)

Triple

35.

Which of the following elements are an exception to the octet rule and require less than 8 valence electrons?

a)

H

b)

C

c)

N

d)

B

e)

F

36.

If you were drawing a Lewis dot diagram for the ion, Mg2+, how many dots would be on the drawing?

a)

2

b)

0

c)

8

d)

12

37.

If you were drawing a Lewis dot diagram for the O2- ion, how many dots would be drawn?

a)

2

b)

6

c)

8

d)

10

38.

Which of the following statements is TRUE of resonance structures?

a)

One bond will be shorter than the others

b)

The electrons flip (oscillate) from one bond to the other

c)

There is only one true version of the molecule

d)

Only one drawing is necessary

39.

which of the following elements will NEVER double bond?

a)

C

b)

H

c)

Cl

d)

I

40.

How many covalent bonds will an element in Group 15 make?

a)

5

b)

8

c)

3

d)

0

41.

Which of the following bonds is the LONGEST?

a)

single

b)

double

c)

triple

42.

How many bonding pairs of electrons are found in a octahedral molecule?

a)

2

b)

6

c)

8

d)

4

43.

VSEPR model explains that the molecular geometry is formed to _________ electron repulsions and therefore __________ distance between electrons.

a)

minimize , maximize

b)

maximize, minimize

c)

minimize, minimize

d)

maximize, maximize

44.

Which of the following substances would have a polar, covalent bond?

a)

H2

b)

NH3

c)

NaCl

d)

Mg

45.

Which of the following would have a metallic bond?

a)

H2

b)

NaCl

c)

Al

d)

H2O

46.

Which of the following forces is the STRONGEST?

a)

Dipole-Dipole

b)

Hydrogen bonding

c)

Ion-Dipole

d)

London dispersion

47.

Which of the following forces in the WEAKEST?

a)

ionic bond

b)

covalent bond

c)

metallic bond

48.

Which of the following has a high melting and boiling point, is a good conductor in solution, soluble, hard, and brittle?

a)

ionic

b)

metallic

c)

covalent

d)

covalent network

49.

Moderately high melting point, high boiling point, conducts electricity, insoluble, malleable

a)

ionic

b)

covalent

c)

metallic

d)

covalent network

50.

Very high melting and boiling point, poor conductor, insoluble and extremely hard

a)

ionic

b)

covalent

c)

metallic

d)

covalent network

51.

Low melting and boiling points, not a conductor, insoluble in water, soft

a)

ionic

b)

covalent

c)

metallic

d)

covalent network

52.

What is the formal charge of fluorine in the following Lewis structure?

a)

FC = 7-8 = -1

b)

FC = 7 - 1 + 6 = 12

c)

FC = 7 - (1 + 6) = 0

d)

FC = 7 + (1 + 6) = 14

53.

Is the following molecule polar or non-polar?

a)

polar

b)

non-polar

54.

Is the following molecule polar or non-polar?

a)

polar

b)

non-polar

55.

Is the following molecule polar or non-polar?

a)

polar

b)

non-polar

56.

Why type of force is shown?

a)

ion-dipole

b)

dipole-dipole

c)

hydrogen bond

d)

london dispersion

57.

Why type of force is shown?

a)

ion-dipole

b)

dipole-dipole

c)

hydrogen bonding

d)

london dispersion

58.

Why type of force is shown?

a)

ion-dipole

b)

dipole-dipole

c)

hydrogen bonding

d)

london dispersion

59.

Why type of force is shown?

a)

ion-dipole

b)

dipole-dipole

c)

hydrogen bonding

d)

london dispersion

60.

What type of bond is shown here?

a)

ionic

b)

metallic

c)

covalent

d)

network covalent

61.

Why type of bond is shown here?

a)

ionic

b)

metallic

c)

covalent

d)

network covalent

62.

Why type of bond is shown?

a)

ionic

b)

metallic

c)

covalent

d)

network covalent

63.

Why type of bond is shown?

a)

ionic

b)

metallic

c)

covalent

d)

network covalent

64.

Draw the molecule NO2- . What is its molecular geometry?

a)

linear

b)

trigonal planar

c)

bent

65.

Draw the molecule, SF4. What is it's electron pair geometry and molecular geometry?

a)

tetrahedral, tetrahedral

b)

octahedral, square planar

c)

trigonal bipyramidal, T-shaped

d)

trigonal bipyramidal, see-saw

66.

Draw the molecule BrF3. What is its electron pair geometry and molecular geometry?

a)

trigonal planar, trigonal planar

b)

tetrahedral, trigonal pyramidal

c)

trigonal bipyramidal, T-shaped

d)

octahedral, T-shaped

67.

Which of the following is the correct Lewis diagram for NaCl?

a)

A

b)

B

c)

C

d)

D

68.

Which of the following is isoelectronic to Xe?

a)

Br-

b)

Sr2+

c)

Cs+

d)

As3-

69.

Which of the following Lewis diagrams for an ion is correct?

a)

a

b)

b

c)

c

d)

d

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