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Lewis Dot and IMFs

Total questions: 48

Worksheet time: 2hrs 36mins

Name
Class
Date
1.

When electrons are completely transferred from one atom to another, the bond between the ions is called

a)

polar covalent

b)

ionic

c)

polar ionic

d)

nonpolar covalent

e)

covalent

2.

How many electrons are in the Lewis structure of lithium nitride?

a)

0

b)

3

c)

4

d)

5

e)

8

3.

How many electrons must a phosphorus atom gain in order to have a full valence shell?

a)

0

b)

1

c)

2

d)

3

e)

5

4.

How many bonding pairs of electrons are in one molecule of ammonia (NH3)?

a)

1

b)

2

c)

3

d)

4

e)

0

5.

How many valence electrons are in one molecule of carbon dioxide?

a)

0

b)

4

c)

6

d)

8

e)

16

6.

Which of the following contains a triple bond?

a)

F2

b)

O2

c)

CN-

d)

CO2

e)

SiCl4

7.

Which of the following contains a double bond?

a)

C2H4

b)

H2

c)

OF2

d)

CF4

e)

OH-

8.

A force that occurs between molecules is called

a)

intramolecular

b)

intermolecular

c)

molecular

d)

covalent

e)

ionic

9.

Of those listed, which type of intermolecular force is the strongest?

a)

covalent

b)

dipole-dipole

c)

hydrogen bonding

d)

molecular

e)

dispersion

10.

This is a correct dot diagram for neon (Ne)

a)

True

b)

False

11.

By replacing the element symbol, this could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

12.

What is the correct formula for this molecule?

a)

NH

b)

N3H

c)

NH3

d)

NH4

13.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
14.
What does an atom's group number help us determine?
a)
Number of protons
b)
Number of electrons
c)
Number of valence electrons
d)
Number of shells
15.

When an atom loses an electron, it becomes a:

a)

Positive ion

b)

Negative ion

c)

Neutral ion

d)

Neutral atom

16.

Ionic compounds are formed when one or more valence electrons are transferred from _____

a)

A nonmetal atom to a metal atom

b)

A nonmetal atom to a nonmetal atom

c)

A metal atom to a nonmetal atom

d)

A metal atom to a metal atom

17.
How are covalent bonds explained?
a)
When one atom takes the other atom's electron
b)
When the atom shares an electron with an another atom
c)
When the two nucleus merge
d)
When the neutrons leave the nucleus
18.

What is the ONLY part of the atom that makes a chemical bond

a)

Nucleus

b)

Electrons

c)

Valence Electrons

d)

Protons

19.

How many lone pairs of electrons (the ones not in bonds) in the molecule pictured above?

a)

2

b)

3

c)

6

d)

8

20.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
21.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
22.
When chlorine reacts it wants to ______________ electron.
a)
gain 1
b)
lose 1
c)
gain 2
d)
lose 2
23.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
24.

Which is the correct Lewis Dot Structure for NH3?

a)
b)
c)
25.

Which is the correct Lewis Dot Structure for H2S?

a)
b)
c)
26.

What is the goal of the Lewis Dot Structure?

a)

To determine the electron position.

b)

To show the element's valence electrons & bonding capabilities.

c)

To find the atomic mass of an element.

d)

To search for the number of electrons in an individual atom.

27.

Hydrogen needs _____ electrons in its valence shell to be stable.

a)

4

b)

6

c)

8

d)

2

28.

According to the octet rule most elements need _______ valence electrons.

a)

2

b)

8

c)

6

d)

18

29.

Which of these is incorrect?

a)
b)
30.
Which of the following is the correct LD Diagram for Hydrogen Cyanide? HCN?
a)
A
b)
B
c)
C
d)
D
31.
In the correct Lewis Structure for methane (CH4), how many unpaired electrons can be found around Carbon?
a)
0
b)
2
c)
4
d)
8
32.
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)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
33.
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
34.
In general, substances with stronger intermolecular forces have ___________  boiling points than those with weaker intermolecular forces
a)
higher
b)
lower
35.
Which noble gas has the highest boiling point?
a)
Xe
b)
Kr
c)
Ar
d)
He
36.
Which of the following will take the longest to evaporate?
a)
CH3CH2OH
b)
CH3OH
c)
CH3CH3
37.
Does H2O have hydrogen bonding?
a)
yes
b)
no
38.

Water, H2O, is classified as what type of molecule?

a)

a polar molecule

b)

a nonpolar molecule

c)

a coordinate covalent compound

d)

an ionic compound

39.

A little lowercase delta plus (δ+) or delta minus (δ–) by the individual atoms signify ___

a)

partial charges

b)

the magnetic poles

c)

a difference in electronegativities

d)

nonpolar molecules

40.

The oxygen sides of water are always doing their best to orient themselves toward ___

a)

magnetic north

b)

the hydrogen sides of other molecules

c)

negative ions

d)

the surface of a liquid

41.

Which of the following forces are found between two NONPOLAR molecules?

a)

Dispersion force

b)

Dipole-dipole

c)

Hydrogen bond

d)

Dipole-induced dipole

42.

What type of intermolecular force requires BOTH molecules to have an H-N, H-O, or H-F connection within them?

a)

Hydrogen bond

b)

Dispersion

c)

Dipole-dipole

d)

Dipole-induced dipole

43.

What type of intermolecular force occurs between two POLAR molecules?

a)

Dispersion

b)

Dipole-dipole

c)

Hydrogen

d)

Dipole-induced dipole

44.

Rank these in order of strength (from strongest to weakest):

Dispersion forces

hydrogen bond

dipole-dipole attraction

a)

dipole-dipole>hydrogen bond>dispersion

b)

Dispersion>dipole-dipole>hydrogen bond

c)

hydrogen bond>dipole-dipole>Dispersion

d)

Dispersion>hydrogen bond>dipole-dipole

45.
In general, substances with stronger intermolecular forces have ________ boiling points than those with weaker forces
a)
Higher
b)
Lower
c)
Forces and boiling point are not related
46.

A diatomic molecule like O2 is always _____ because electrons are shared _____

a)

nonpolar; unequally

b)

polar; equally

c)

nonpolar; equally

d)

polar; unequally

47.
Which formula represents a nonpolar molecule?
a)
HBr
b)
H2S
c)
CBr4
d)
PCl3
48.

Very soluble (able to dissolve) in water:

a)

Ionic Bonds

b)

Covalent Bonds

c)

Both bonds

d)

Neither bond

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