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LEWIS STRUCTURE

Total questions: 45

Worksheet time: 56mins

Name
Class
Date
1.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
2.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
3.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
4.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
5.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
6.
How many electrons should Oxygen have around its Lewis dot model?
a)
5
b)
6
c)
7
d)
8
7.
This is the correct dot diagram for sodium (Na)
a)
true
b)
false
8.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
9.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
10.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
11.
When writing Lewis Structures, only __________ electrons are used.
a)
Inner shell
b)
Core 
c)
Valence
d)
Stable
12.
A molecule of water has what shape?
a)
Linear
b)
Tetrahedral
c)
Bent
d)
Triangular
13.
A molecule of methane has what shape?
a)
Tetrahedral
b)
Triangular
c)
Pyramidal
d)
Octahedral
14.
The theory that is used to predict the arrangement of atoms about a central atom is called?
a)
Valence shell repulsion
b)
Valence shell electron sharing
c)
Valence shell electron pair repulsion
d)
Valence electron shell repulsion pair
15.
Multiple bonds are possible if _______, ______, and ________ are present in a molecule.
a)
C,H,O
b)
H,O,N
c)
C,N,S
d)
C,N,O
16.

XENON has _________ valence electrons.

a)

18

b)

8

c)

17

d)

7

17.

IODINE has _______ valence electrons.

a)

7

b)

17

c)

5

d)

8

18.

Between C, H, O and N, which atom is more electropositive?

a)

C

b)

H

c)

O

d)

N

19.

Draw a Lewis structure of IF3 molecules. Identify how many lone pair electrons around the central atom.

a)

1

b)

2

c)

3

d)

0

20.

Elements A and E have two and seven valence electrons respectively. The most likely formula of the compound formed between A and E is

a)

A2E

b)

AE2

c)

A2E2

d)

A2E7

21.

What is the meaning of Dative Bond?

a)

a covalent bond between two atoms where one of the atoms provides both electrons that form the bond.

b)

a covalent bond between two atoms where both of the atoms provides both electrons that form the bond.

c)

same with an ionic bond

d)

not exist

22.
Ionic bonds are between...
a)
nonmetals and nonmetals
b)
carbon and oxygen
c)
metals and nonmentals
d)
hydrogen and chlorine
23.
Covalent bonds are between...
a)
two or more nonmetals
b)
sodium and chlorine
c)
metals and metals
d)
metals and nonmetals
24.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
25.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
26.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
27.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
28.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
29.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
30.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Trigonal planar
31.

The geometry of a molecule with 5 bonded pairs of electrons and 0 lone pairs of electrons, AB5

a)

Tetrahedral

b)

Trigonal Planar

c)

Bent

d)

Trigonal bipyramidal

e)

Linear

32.

The geometry of a molecule with 2 bonded pairs of electrons and 2 lone pairs of electrons, AB2E2

a)

Tetrahedral

b)

Trigonal Planar

c)

Bent

d)

Trigonal Pyramidal

e)

Linear

33.

The geometry of a molecule with 3 bonded pairs of electrons and 2 lone pairs of electrons, AB3E2

a)

T-shaped

b)

Trigonal Planar

c)

Bent

d)

Trigonal Pyramidal

e)

Linear

34.

Which of the following compound has linear molecular shape?

a)

OCl2

b)

SCl2

c)

CO32-

d)

SnCl2

e)

XeF2

35.

Determine the molecular shape of CH3+

a)

Tetrahedral

b)

Linear

c)

Trigonal planar

d)

Trigonal pyramidal

36.

Which of the central atoms given below has only one lone pair of electron?

a)

BF3

b)

SO2

c)

H2O

d)

Cl2

37.

Choose a compound given with dipole moment NOT equal to zero ( μ\mu ≠\ne  0)

a)

SF4

b)

CCl4

c)

PCl5

d)

AlBr3

38.

The polarity of a substance depends on

i- the presence of lone pairs electrons

ii- the difference in electronegativity

iii- the molecular geometry

a)

i only

b)

i and ii

c)

ii and iii

d)

i, ii and iii

39.

Sulphur can form 3 compounds with fluorine. Which of these molecules is/are polar?

a)

SF2

b)

SF4

c)

SF6

40.

The F-P-F bond angle in PF5 in degree are

i-180

ii-90

iii-120

a)

i only

b)

i and ii

c)

ii and iii

d)

i,ii and iii

41.

Which of the following molecule pairs has the same molecular shape?

a)

BF3 and PCl3

b)

PCl3 and NBr3

c)

NBr3 and AlCl3

d)

BeCl2 and O3

42.

CCl4 and POCl3 both have the same molecular geometry. However CCl4 is non polar molecule whereas POCl3 is a polar molecule. What makes POCl3 a polar molecule?

a)

the bond dipoles cancel each other

b)

the bond dipoles are not the same

c)

symmetrical shape

d)

dipole moment ,  μ\mu   ≠\ne   0

43.

The formal charges on sulphur, chlorine and oxygen are

a)

S=0, Cl=0, O=0

b)

S= -1, Cl=+2, O=-1

c)

S= +2, Cl= -1, O=-1

d)

S= +2, Cl=-2, O=0

44.

The electronic configurations of element S and R are as follows:

S: 1s2 2s2 2p6 3s2

R: 1s2 2s2 2p5

S and R combine to form ________compound with formula______. Choose the appropriate answer to fill in the blanks.

a)

covalent, SR2

b)

covalent, S2R

c)

ionic, SR2

d)

ionic, S3R2

45.

AsF5 has what shape?

a)
square planar
b)
square pyramidal
c)
tetrahedral
d)

see saw

e)

linear

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