Name: ___________________________________ Date: __________________ Period: _____
Review Chemistry I Honors Unit 11: States of Matter
1.
Kinetic-Molecular Theory (KMT) describes the physical states of matter in terms of the
_________________ of particles and the __________________ between them.
a) Particles in the __________ state are closest together.
b) Particles in the __________ state have the most freedom of motion.
c) Particles in the __________ state have the weakest attractions.
2.
The ____________ ____________ energy of particles in a substance is directly proportional to
the _________________ of the substance.
3.
What happens to the average kinetic energy of a gas as it is heated? _________________
4.
What is temperature? ______________________________________________________
________________________________________________________________________
5.
Which has particles that are moving at 0oC? (circle all that are correct)
A. solid iron
B. liquid iodine
C. ammonia vapor
D. hydrogen gas
Which has the greatest average kinetic energy?
A. nitrogen gas at –50 C
B. neon gas at 20 C
C. CH3CH2OH vapor at 25 C
D. H2O vapor at 100 C
Choice ____ because __________________________________________________
6.
What is the temperature at which there is absolutely NO motion of particles?
It’s called ___________________________ at ______ K or ______ oC.
7.
Why are gases compressible, but liquids and solids are not? _______________________
________________________________________________________________________
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8.
Consider the simple water cycle diagram below. Group the phase changes by heat energy
absorbed or released, by interparticle space, and by intermolecular attractions in the boxes.
absorbs energy
releases energy
more space
between molecules
less space
between molecules
less attraction
between molecules
more attraction
between molecules
condensation
melting
vaporization
freezing
deposition
sublimation
9.
During each of the phase changes listed in #8, the temperature of the water will _______________
because its ________________ energy is changing while its average kinetic energy is constant.
10. List the intermolecular attractions in decreasing order of strength from strongest to weakest:
_____________________ > _____________________ > _____________________
Strongest
Weakest
11. Describe how dispersion forces occur between two atoms or molecules.
___________________________________________________________________
___________________________________________________________________
12. Describe dipole-dipole forces between two molecules.
___________________________________________________________________
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13. Which substance has hydrogen bonding as its main intermolecular force?
A. SO2
B. HCl
C. F2
D. NH3
How do you recognize a molecule that can form hydrogen bonds?
___________________________________________________________________
14. Describe how a hydrogen bond forms between molecules.
__________________________________________________________________
__________________________________________________________________
15. The strong attractions between polar water molecules cause water to have which of the
following properties: (circle all that apply)
A.
B.
C.
D.
E.
F.
G.
H.
greater surface tension
higher density liquid than solid (ice)
greater attraction to nonpolar molecules
higher boiling point
higher temperature
higher specific heat capacity
higher heat of fusion
higher heat of vaporization
S
H2S
H
H2O
H
16. Hydrogen sulfide (H2S) boils at –60oC. Even though water is a smaller molecule that
should become a gas more easily than H2S, water doesn’t boil until it reaches 100oC.
Why are water molecules so difficult to separate from liquid phase to form a gas?
__________________________________________________________________
__________________________________________________________________
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17. Stronger intermolecular attractions cause liquids to have _____________ boiling points and
cause solids to have ______________ melting points.
A.
B.
C.
D.
lower
lower
higher
higher
, lower
, higher
, lower
, higher
18. Identify which of the following changes involves the breaking of intramolecular bonds,
and which involve the breaking of intermolecular attractions? (circle one for each)
A. H2O(s)  H2O(l)
intramolecular bonds or intermolecular attractions
B. Fe2O3(s)  2 Fe(s) + 3 O2(g)
intramolecular bonds or intermolecular attractions
C. F2(g)  2 F(g)
intramolecular bonds or intermolecular attractions
D. NH3(l)  3 H2(g) + N2(g)
intramolecular bonds or intermolecular attractions
19. Warm water vapor from the air condenses onto a glass of cold ice water.
This happens when the water vapor __________ heat to/from the glass
causing the glass to become ___________.
A.
releases/to , warmer
B.
releases/to , cooler
C. absorbs/from , warmer
D. absorbs/from , cooler
20.
Heat is energy that is transferred due to a difference in _____________________.
21.
Describe the direction of heat flow when a hot rock at 105 C is placed into cool water at 18 C.
o
o
Heat flows from _____________________ to _______________________ making the
___________________ cooler and the ____________________ warmer until they both
have the same _________________________________.
22.
o
o
Describe the direction of heat flow when a piece of ice at 0 C is held in your hand at 37 C.
Heat flows from _____________________ to _______________________ making
___________________ cooler and ____________________ warmer until they both
have the same _________________________________.
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For #23-26, refer to the heating curve below for water as heat is added at a constant rate.
E
Temperature ( C)
D
o
C
B
A
Heat added
23. Circle which phase(s) of water exist(s) in each section of the heating curve.
section A.
solid
liquid gas
section B.
solid
liquid gas
section C.
solid
liquid gas
section D.
solid
liquid gas
section E.
solid
liquid gas
24. Circle which type of energy is increasing in the sample during each section as heat is being added.
section A.
kinetic
potential
section B.
kinetic
potential
section C.
kinetic
potential
section D.
kinetic
potential
section E.
kinetic
potential
25. If heat were removed instead of added, the process occurring in section D would be _____.
A.
B.
C.
D.
vaporization
freezing
condensation
NONE of the above
26. Section B is shorter than section D because water has a lower heat of __________________
than heat of _____________________ so it takes more energy to ___________ a sample of water
than it does to ____________ the same sample of water.
5
o
27. A cup of water contains 55 g of water at a temperature of 21.4 C. How much heat must be
o
o
removed from the water to lower its temperature to 2.5 C? (the specific heat of water is 4.18 J/g C)
For #28-33, refer to the phase diagram below for water.
5
A
B
Label each
section on the
diagram
2
1
(A, B, C)
with the
correct phase
(s, l, g)
4
3
C
28. The phase change from A to C is called _______________ and from C to B is ______________.
29. The boiling point of the substance is shown at Point ___ which is the point at which
___________ and ___________ phases coexist in equilibrium.
30. Point 4 represents the ___________ point, which is the point at which…
________________________________________________________________.
31. The critical point is shown at Point ___ which represents the temperature above which a
____________ could not exist and the pressure above which a _____________ could not exist.
32. A sample of the substance is held constant at a temperature of 300 K while the
pressure is decreased from 10 atm to 0.01 atm. The phase change that occurs is ______________.
33. A sample of the substance is held constant at a pressure of 1 atm while the temperature
is increased from 150 K atm to 250 K. The phase change that occurs is ______________.
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