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Lewis Dot Structures

Total questions: 70

Worksheet time: 2hrs 30mins

Name
Class
Date
1.
How many electrons should Lithium have around its Lewis dot model?
a)
1
b)
2
c)
3
d)
4
2.
How many electrons should Carbon have around its Lewis dot model?
a)
1
b)
3
c)
4
d)
5
3.
How many electrons should Chlorine have around its Lewis dot model?
a)
5
b)
6
c)
7
d)
8
4.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
5.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
6.
This could be the dot diagram of
a)
Mg
b)
Cl
c)
C
d)
O
7.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
8.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
9.

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

a)

8

b)

4

c)

2

d)

3

10.

CO2 has how many lone pairs on the central atom?

a)

0

b)

1

c)

2

d)

3

e)

4

11.

NH3 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

12.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

13.

Carbonate (CO32-) has how many double bonds?

a)

0

b)

1

c)

2

d)

3

14.

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

a)

Single

b)

Double

c)

Triple

15.

CH2O has which of the following?

a)

Multiple double bonds

b)

Multiple single bonds

c)

One double bond

d)

One single bond

e)

A lone pair

16.

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

a)

H

b)

Li

c)

Be

d)

B

e)

C

17.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
18.
A covalent bond is
a)
a bond that shares electrons metallicaly
b)
A bond that shares electrons with non metals
c)
Metalloids bonding
d)
metals and nonmetals bonding
19.
How many electrons does each line indicate are shared?
a)
1
b)
2
c)
3
d)
4
20.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
21.

What is this element?

1s22s22p63s23p6

4s23d104p6

a)

Argon

b)

Krypton

c)

Selenium

d)

Bromide

22.

Choose the correct shortcut configuration for iodine.

a)

[Ar]4s24d104p5

b)

[Kr]5s24d105p5

c)

[Xe]5s25d105p5

d)

none of the above

23.

What are valence electrons?

a)

All the electrons an atom has.

b)

Only the electrons in the 1st energy level.

c)

Only the electrons in the outer energy level.

d)

Total number of protons and neutrons.

24.

Which version of carbon is the anion?

a)
b)
c)
25.

When a bond forms between hydrogen (H) and oxygen (O), the electrons are shared. Which diagram correctly shows the bond between hydrogen and oxygen?

a)
b)
26.

Covalent bonds form between which 2 types of elements?

a)

metals and non-metals

b)

2 metals

c)

2 non-metals

27.

How many electrons can the first shell hold?

a)

2

b)

4

c)

6

d)

8

28.
What happens when the sodium atom loses an electron?
a)
It become negatively charged 
b)
It become positively charged
c)
none
29.
If an atom loses two electrons what charge will it have?
a)
+ 2
b)
 - 2
c)
+1
d)
-1
30.
According to the diagram below, how many bonds will this atom need to make to be stable?
a)
1
b)
2
c)
3
d)
4
31.
How many more valence electrons does Oxygen need to be stable?
a)
6
b)
2
c)
4
d)
It's already stable with 8
32.
Most elements will gain or lose electrons so that they end up with _______ valence electrons.
a)
2
b)
6
c)
8
d)
10
33.
If electrons are shared unequally then the bond is....
a)
Non-polar covalent
b)
Ionic
c)
Non-polar ionic
d)
Polar covalent
34.
If electrons are shared equally then the bond is....
a)
Non-polar covalent
b)
Ionic
c)
Non-polar ionic
d)
Polar covalent
35.
Metals and nonmetals form which kind of bond?
a)
Polar covalent
b)
Ionic
c)
Non-polar covalent
d)
Metallic
36.
How strongly an atom attracts electrons is called....................
a)
Ionization energy
b)
Electronegativity
c)
Electricity
d)
Nuclear force
37.

What is a Lewis Dot Structure?

a)

It shows all of the particles in the atom.

b)

Contains protons and neutrons

c)

Only shows the element symbol and it's outer most electron shell

d)

Contains protons and electrons

38.

What is the atom called when there is adding or removing electrons creates atoms with (+) or (-) charges?

a)

isotopes

b)

ions

c)

neutral

d)

stable

39.

Does the following reference Polar, Nonpolar, or both:

"electronegativity values are the same"?

a)

Polar

b)

Nonpolar

c)

Both

40.

CO2 has polar bonds but is a NON POLAR molecule. Why?

a)

it has an asymmetrical shape

b)

bond polarity or dipole moment between C and O atoms cancel

c)

there is net dipole moment between C and O atoms in molecule

d)

bond polarity does not exist between C+ and O- atoms

41.

Is this molecule polar or nonpolar?

a)

polar

b)

nonpolar

42.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
43.
In a polar bond, the more electronegative element will assume a partial ________ charge.
a)
positive
b)
negative
44.

Type of bond between Br & Br

a)

Ionic

b)

Polar Covalent

c)

Nonpolar Covalent

45.
Which molecule contains bonds with a GREATER polarity?
a)
HCl
b)
CCl4
46.

What is the shape? Hint: Draw the Lewis dot structure for NH3.

a)

tetrahedral

b)

trigonal pyramidal

c)

trigonal planar

d)

bent

47.
What is the shape of H2O?
a)
linear
b)
tetrahedral
c)
bent
d)
trigonal pyramidal
48.

SiCl4 has what shape?

a)

trigonal planar

b)

pyramidal

c)

tetrahedral

d)

trigonal pyramidal

49.

3 atoms bonded and 0 lone pairs

a)

linear

b)

trigonal planar

c)

bent

d)

tetrahedral

e)

trigonal pyramidal

50.

3 atoms bonded and 1 lone pairs

a)

true linear

b)

trigonal planar

c)

bent

d)

tetrahedral

e)

trigonal pyramidal

51.

Which of the following compounds has only single bonds?

a)

I only

b)

II only

c)

III only

d)

I and III

e)

III and IV

52.
A molecule of methane has what shape?
a)
Tetrahedral
b)
Triangular
c)
Pyramidal
d)
Octahedral
53.
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
54.
Atoms of H only form _________ bonds.
a)
Double
b)
Single
c)
Multiple
d)
Triple
55.
 Lone electron pairs in a molecule...
a)
Never exist
b)
Are lost in space
c)
Creates an isotope
d)
Push the bonded atoms closer
56.

What is the total number of valence electrons in Ammonium ion (NH4+).

a)

9

b)

8

c)

10

d)

12

57.
Traveling across a period, from left to right, the atomic radii ______________.
a)
Increases
b)
Decreases
c)
Stays the same
58.
Each element wants to gain or lose electrons so that it can have the same electron configuration as......
a)
a Nobel gas
b)
other elements in its family
c)
other elements in its period
d)
it used to have before reacting
59.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
60.
How many total lone pairs would there be in the Lewis structure for the oxygen molecule?
a)
1
b)
2
c)
3
d)
4
61.
How many total lone pairs would be found in the Lewis structure for C2H4
a)
0
b)
2
c)
4
d)
6
62.

What is the oxidation number for elements in the Alkali Earth Metals family?

a)

-1

b)

-2

c)

+1

d)

+2

63.

What is the oxidation number for the Halogens family?

a)

-1

b)

-2

c)

+1

d)

+2

64.

What is the oxidation number for the Carbon family?

a)

4

b)

-4

c)

+4

d)

-/+4

65.
What molecular shape is the structure shown here? (BCl3)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
66.
Boron, an exception when it comes to stability, only needs to be surrounded by ____ valence electrons.
a)
2
b)
4
c)
6
d)
8
67.
What molecular shape is the structure shown here? (BeCl2)
a)
linear
b)
bent
c)
trigonal planar
d)
tetrahedral
68.
True or False: You can use Lewis Dot structures to diagram elements, ions, ionic compounds, molecular compounds, and polyatomic ions.
a)
True
b)
False
69.
True or False: Lewis Dot diagrams (or structures) show ALL electrons for each atom.
a)
True
b)
False
70.
To determine the SHAPE of a molecular compound you assess the number of bonding groups and unshared electron pairs...
a)
on the central atom only
b)
on all elements in the compound
c)
on the cations only
d)
on the anions only

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