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WorksheetsLewis Structures
Total questions: 49
Worksheet time: 1hrs 14mins
Name
Class
Date
1.
This is the correct dot diagram for sodium (Na)
a)
true
b)
false
2.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
3.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
4.
This is the correct dot diagram for nitrogen (N)
a)
true
b)
false
5.
This is a correct dot diagram for magnesium (Mg)
a)
true
b)
false
6.
This is a correct dot diagram for carbon (C)
a)
true
b)
false
7.
This is a correct dot diagram for neon (Ne)
a)
true
b)
false
8.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
9.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
10.
If electrons are shared unequally then the bond is....
a)
Non-polar covalent
b)
Ionic
c)
Non-polar ionic
d)
Polar covalent
11.
If electrons are shared equally then the bond is....
a)
Non-polar covalent
b)
Ionic
c)
Non-polar ionic
d)
Polar covalent
12.
Metals and nonmetals form which kind of bond?
a)
Polar covalent
b)
Ionic
c)
Non-polar covalent
d)
Metallic
13.
How strongly an atom attracts electrons is called....................
a)
Ionization energy
b)
Electronegativity
c)
Electricity
d)
Nuclear force
14.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
15.
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
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.
What is the correct structure for BF3?
a)
Option A.
b)
Option B.
c)
Option C.
d)
Option D.
18.
How many valence electrons are in Phosphorus?
a)
15
b)
4
c)
5
d)
31
19.
How many electrons does each line indicate are shared?
a)
1
b)
2
c)
3
d)
4
20.
When writing Lewis Structures, only __________ electrons are used.
a)
Inner shell
b)
Core
c)
Valence
d)
Stable
21.
Atoms of H only form _________ bonds.
a)
Double
b)
Single
c)
Multiple
d)
Triple
22.
What is the correct Lewis Dot Structure for ammonia NH3
a)
b)
c)
d)
23.
Which is the correct molecular structure for carbon dioxide?
a)
b)
c)
d)
24.
Is this the correct structure for CH2O?
a)
Yes
b)
No
25.
Which of the following is the correct Lewis structure for water?
a)
A
b)
B
c)
C
26.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
27.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
28.
NH3 has how many lone pairs?
a)
0
b)
1
c)
2
d)
3
29.
CCl4 has how many double bonds?
a)
0
b)
1
c)
2
d)
3
30.
In HCN (Carbon is usually the central atom) what kind of bond is between the C and N
a)
Single
b)
Double
c)
Triple
31.
Which of the following factors plays an important role in the identification of specific intermolecular forces in a molecule?
a)
bond type
b)
density
c)
solubility
d)
molecular polarity
32.
Which of the following molecules contains only London dispersion forces?
a)
CF4
b)
HCl
c)
H2O
d)
MgO(aq)
33.
Which of the following molecules predominantly consists of dipole-dipole forces?
a)
HF
b)
Ne
c)
O2
d)
ICl
34.
Which of the following molecules has hydrogen bonding?
a)
HCl
b)
HI
c)
HF
d)
HBr
35.
Which of the following statements correctly explains why hydrogen bonding is such a strong intermolecular force?
a)
There is an attraction between a small, weakly electronegative hydrogen atom and a large, strongly electronegative atom of fluorine, nitrogen, or oxygen
b)
There is an attraction between a small, highly electronegative hydrogen atom and a large, highly electronegative fluorine atom
c)
There is an attraction between the hydrogen and oxygen atoms, only
d)
There is an attraction between the hydrogen and nitrogen atoms, only
36.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
London Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
37.
Hydrogen bonding occurs when hydrogen is bonded to N, O, or F. Which of the following has hydrogen bonding?
a)
CBr4
b)
NO2
c)
H2S
d)
NH3
38.
Does H2O have hydrogen bonding?
a)
yes
b)
no
39.
Does HF have hydrogen bonding?
a)
yes
b)
no
40.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
41.
Which is the second strongest intermolecular force, after hydrogen bonding?
a)
dipole-dipole attraction
b)
London dispersion forces
42.
________________________ have the strongest intermolecular forces of attraction.
a)
Dipole- Dipole
b)
London Dispersion Forces
c)
Hydrogen Bonds
43.
Intermolecular force present in HCl?
a)
dipole dipole
b)
London dispersion forces
c)
H-bond
d)
ionic
44.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons
c)
The transfer of electrons
d)
None Of the above
45.
Type of intermolecular force present in I2, Br2, and Cl2.
a)
dipole dipole
b)
H-bond
c)
London dispersion
d)
metallic
46.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
47.
All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces. Which of these has ONLY London forces?
a)
I2
b)
NH3
c)
OCl2
d)
SH2
48.
Rank these in order of strength:
covalent bond
London forces
hydrogen bond
dipole-dipole attraction
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
49.
Which is the weakest intermolecular force?
a)
dipole-dipole attraction
b)
London dispersion forces
c)
Hydrogen bonds
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