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WorksheetsIntermolecular Forces Dipole-Dipole Hydrogen Bonding Dispersion Ion Dipole Interaction
Total questions: 27
Worksheet time: 16mins
Name
Class
Date
1.
What intermolecular force present in a sample of pure HCl?
a)
dipole-dipole attraction
b)
London dispersion forces
c)
H-bonds
d)
molecule-ion attraction
2.
What intermolecular force is present in a sample of pure Cl2?
a)
dipole-dipole attraction
b)
H-bonds
c)
London dispersion forces
d)
molecule-ion attraction
3.
Intermolecular forces are the forces that exist
a)
within molecules
b)
between molecules
4.
Which of these is not an intermolecular force?
a)
covalent bonding
b)
hydrogen bonding
c)
London dispersion forces
d)
dipole-dipole forces
5.
What type of intermolecular forces increase with increasing molecular mass?
a)
hydrogen bonding
b)
dipole-dipole forces
c)
London dispersion forces
d)
ion-dipole forces
6.
Which are the strongest intermolecular forces?
a)
hydrogen bonds
b)
dipole-dipole forces
c)
London dispersion forces
d)
molecule-ion attractions
7.
What are the most important intermolecular forces found between water molecules?
a)
hydrogen bonding
b)
dipole-dipole forces
c)
London dispersion forces
d)
ion-dipole forces
8.
Hydrogen bonding is a special type of what force?
a)
London dispersion forces
b)
dipole-dipole forces
c)
ion-dipole forces
d)
covalent force
9.
What type of intermolecular force is present in all substances, regardless of polarity?
a)
London dispersion forces
b)
dipole-dipole forces
c)
ion-dipole forces
d)
hydrogen bonding
10.
Which of these molecules exhibits hydrogen bonding as its major intermolecular force of attraction when dissolved in water?
a)
HBr
b)
HCl
c)
HF
d)
all of these
11.
What explains the very high melting and boiling point of water?
a)
Dipole-dipole forces between water molecules
b)
Hydrogen bonds between water molecules
c)
London dispersion forces between water molecules
d)
Molecule-ion attractions between water molecules
12.
What force explains the ability for water molecules to dissolve ionic compounds?
a)
Dipole-dipole attraction
b)
Hydrogen bonds
c)
Molecule-ion attraction
d)
London Dispersion forces
13.
Which of these typically increases when intermolecular forces increase?
a)
Boiling Point
b)
Melting Point
c)
Viscosity
d)
All of these
14.
In general, substances with stronger intermolecular forces have ________ boiling points than those with weaker forces
a)
Higher
b)
Lower
c)
The same
15.
Which of these has the strongest London dispersion forces?
a)
F2
b)
Br2
c)
Cl2
d)
I2
16.
Hydrogen bonding occurs when hydrogen is bonded to N, O, or F. Which of the following would have hydrogen bonding with water molecules?
a)
CBr4
b)
NO2
c)
H2S
d)
NH3
17.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
18.
Does NH3 have hydrogen bonding?
a)
yes
b)
no
19.
Which is the second strongest intermolecular force, after hydrogen bonding?
a)
dipole-dipole attraction
b)
London forces
20.
A substance capable of hydrogen bonding has a ___________ boiling point than a similar substance that doesn't hydrogen bond.
a)
higher
b)
lower
21.
What are intermolecular forces?
a)
forces of attraction or repulsion which act between neighboring particles
b)
forces which keep a molecule together.
22.
Is intermolecular bonding generally stronger or weaker than intramolecular bonding?
a)
Stronger
b)
Weaker
23.
Which type of force is this?
a)
Intramolecular
b)
Intermolecular
24.
Which of the following would have the highest boiling point?
a)
H2
b)
HCl
c)
H2S
d)
H2O
25.
What is a dipole?
a)
A polar molecule
b)
A nonpolar molecule
c)
A diatomic element
26.
What type of intermolecular force is the result of temporary uneven distribution of electrons around molecules that result in momentary dipoles?
a)
dipole-dipole
b)
molecule-ion
c)
London dispersion
d)
hydrogen bonds
27.
Which of the following would have molecule-ion attractions?
a)
Cl2(aq)
b)
H2O(s)
c)
NaCl(aq)
d)
CaBr2(s)
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