Chemistry I Accelerated
Study Guideline - Chapter 13: States of Matter
__________________________________________________________________
By the end of this chapter the skills you should be able to demonstrate
are:
1. Explain the properties of the different phases of matter in terms of
the Kinetic Molecular Theory.
2. Relate temperature and energy transfer to molecular motion.
3. Describe characteristics of substances in each of the three common
states of matter in terms of kinetic theory and bonding in the
substances.
4. Explain the relationship of melting point to bonding type and to
crystal type.
5. Describe the structure and properties of crystals, liquid crystals and
amorphous solids.
6. Describe at the molecular level the changes occurring at the melting
and boiling point.
7. Name the six different phase changes.
8. Interpret heating and melting curves and phase diagrams.
9. Explain and calculate heat of fusion and vaporization.
Suggested Problems:
p.409
#63, 65, 66, 69, 70, 71, 76
p.411
#7-11
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Dr. Corell - Chemistry I Accelerated
Phases of Matter - Kinetic Molecular Theory
Word List
attraction
between
greater/less
greater/smaller
addition/removal
boiling/freezing/melting
motion
solid(s)/liquid(s)/gas(es)
kinetic/potential
close together/far apart
shape
translational motion
solidification
force
temperature
volume
Matter exists in three phases called ______________, ______________ and ______________. Each
sample of a substance in the solid phase has a definite ______________ and definite ______________. In
the liquid phase, each sample has a definite ______________ but takes the ______________ of its
container. In the gas phase, the sample has both the ______________ and the ______________ of its
container.
A sample of matter can change from one phase to another by the addition or removal of energy. When
a sample changes from solid to liquid, the phase change is called ______________. At standard
atmospheric pressure, the temperature at which this change occurs is called the normal ______________
point. Other terms often applied to phase changes are: freezing, the changing from ______________ to
______________ at the normal ______________ point (_________________is a synonym for freezing);
condensation, the changing from _________________ to ________________; and sublimation, the change
directly from the ______________ phase to the ______________ phase without an intermediate
______________ phase.
Change in phase is caused by the ______________ or ______________ of energy and can take place
with no changes in temperature. If no change in ______________ occurs when energy is added to a sample,
the ______________ energy of the substance increases. Particles in the ______________ phase, with rigid
structure and fixed volume, have the lowest state of ______________ energy. When sufficient energy is
added to change to the liquid phase, the particles are moved into positions of increased ______________
energy. If enough energy is added to a liquid at its boiling point, conversion to the ______________ phase
takes place and the particles move into positions of even greater ______________ energy as they become
separated by even greater distances.
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There are three main differences between the phases ______________, ______________ and
______________. One of these differences is in the distances ______________ the particles making up the
material. In gases under ordinary pressure, the gas particles are relatively _____ _________ compared to
the separation between particles in the _____________ and _____________ phase. The particles making up
liquids are slightly farther apart than those making up ______________.
A second main difference between phases is the ______________ of attraction between particles. In
gases there is essentially no force of ______________ between particles. In liquids and solids there are
relatively large forces of ______________between particles.
The third main difference is based upon the ______________ of the particles. A major difference
between the phases is the amount of translational motion, the movement from one point to another. Gases by
far have the greatest ________________ _____________, as anyone who has been near a dead skunk can
tell you. The translational motion associated with liquids is small, but is considerably ______________than
that of solids.
page 3
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A Heating Curve
Use the table at the bottom of the page to describe the following heating curve for
different intervals of time. Fill in the blanks in the last two column of the table with either
no change or increasing.
Time Interval on
Heating Curve
Phases present
Temperature (ave. kinetic
energy of particles)
Interval I
Interval II
Interval III
Interval IV
Interval V
page 4
Potential Energy
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A Cooling Curve
A sample of naphthalene in the liquid phase was allowed to cool. Temperature reading of the sample
were taken every minute while the cooling was taking place, as shown below.
Time (min.)
Temp.(°C)
Time (min.)
Temp.(°C)
Time (min.)
Temp.(°C)
0
1
2
3
93.4
87.2
82.6
80.6
4
5
6
7
80.6
80.6
80.6
80.6
8
9
10
11
80.6
80.4
74.2
67.8
Using the following grid, graph the data from the table above
1. Based on these data, what is the melting point of naphthalene?
2. Label the time intervals as follows:
I - for the interval where there is a phase change from liquid to a solid
II - for the interval where the liquid cools
III - for the interval where the solid cools
3. In which region(s) is kinetic energy content decreasing? Explain.
4. In which region(s) is potential energy content decreasing? Explain.
page 5
______________
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Energy in changes of phase
Choose words from the word list to fill in the blanks in the following paragraphs relating
to the phases of matter.
absorption/release
heat/temperature
kinetic/potential
boiling/melting
increases/decreases
particles
cooling/heating/warming
increasing/decreasing
phase
energy
Most substances can change in ______________ from solid to liquid by the ______________ of heat.
The temperature at which the change from solid to liquid occurs is called the ________________ point. The
temperature at which the change from liquid to gas occurs is the ________________ point.
The graph on page four shows the ________________ of a substance as it is heated over a period of
time. A graph of this kind is called a ________________ curve. Kinetic energy is the energy associated
with the motion of the ________________ within a sample. Temperature is a measure of the average kinetic
energy of the __________________ due to their motion. The energy due to position with respect to each
other is called ________________ energy.
The behavior of a typical substance as it is heated is shown in the graph. The substance is a solid at
time=0. Throughout the entire time the substance is being heated, __________________ is being added as
heat at a constant rate. The changes in temperature show increasing __________________ energy and the
changes in phase show increases in ________________ energy. A __________________ curve shows the
same events in the reverse order. In the case of a cooling curve, changes in temperature show ____________
in kinetic energy and changes in phase show _____________ in potential energy.
page 6
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Vapor Pressure and Boiling
The vapor pressure of a gas above its own liquid depends on temperature. The boiling
point, or temperature at which bubbles of vapor form within a liquid, depends upon
both vapor pressure and atmospheric pressure. The following graph shows the vapor
pressure curves for two substances A and B
Answer the following questions based on the above graph
1. What is the vapor pressure of A at 35°C?
1. __________________
2. What is the vapor pressure of B at 35°C?
2. __________________
3. At what temperature is the vapor pressure of A 106.6 kPa?
3. __________________
4. What is the vapor pressure of B at this temperature?
4. __________________
5. At what temperature is the vapor pressure of B 106.6 kPa?
5. __________________
6. What is the “normal” boiling point of A?
6. __________________
7. What is the “normal” boiling point of B?
7. __________________
8. At what temperature would A boil in Denver where atmospheric
pressure is 93.3 kPa?
9. What would the atmospheric pressure have to be in order for B to
boil at the same temperature as you gave in your answer to #8?
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8. __________________
9. __________________
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The following table shows the vapor pressure of a certain liquid at various temperatures.
Graph the data in the table provided.
Temp °C
Pressure (kPa)
Temp °C
Pressure (kPa)
Temp °C
Pressure (kPa)
0
10
20
30
40
50
1
2
4
7
11
16
60
70
80
90
100
110
22
29
37
46
56
68
120
130
140
150
80
93
107
122
1. What effect does rising temperature have on vapor pressure?
2. Account for this effect in terms of energy, molecular forces, closed container and equilibrium.
3. What must be true at the boiling point of a liquid?
4. If atmospheric pressure was 96 kPa, what would be the boiling point of the substance whose vapor
pressure you graphed?
5. What would happen to the boiling point if the atmospheric pressure would begin to rise?
6. How would the cooking time of an egg that is to be hard boiled be affected by high altitude? Explain.
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Condensed States of Matter
Fill in the following chart comparing solids and liquids
Physical Property
Liquids
1. Compressibility
2. Density
3. Shape
4. Rate of Diffusion
Solids
5. Describe the behavior of the molecules in a liquid. Explain this behavior in terms of intermolecular forces.
6. How do intermolecular forces determine molecular arrangements in solids?
7. List three physical properties that are dependent on both the kind of particles that make up a substance and
the strength of the attractive force between the particles.
8. Why are the bonds within the sodium chloride unit cell stronger than those between sugar molecules?
9. What is the principal feature of a metallic bond?
10. Diamond and graphite are both made of carbon, yet graphite is soft and diamond is one of the hardest
substances known to man. Explain the differences between these two in terms of intermolecular forces.
11. Which of these two would have the higher melting point: a molecular solid held together by dispersion
forces or a molecular solid held together by hydrogen bonds? Why?
12. Movements between atoms or molecules is limited or slow in both the solid and the ____________ state.
13. The smallest repetitive unit in a crystalline structure is called a ______________________.
14. Unlike crystalline solids, amorphous substances may _______________ before melting over a wide
range of temperatures.
15. In a molecular solid, intramolecular covalent bonds are __________ than intermolecular attractive forces.
16. The stronger the intermolecular force in a liquid, the _______________ the boiling point.
17. The state of a substance at room temperature depends on the ____________ of the ________________
________________.
18. Water molecules in an ice cube are held together by __________________ forces or, more specifically.
__________________ bonds.
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Dr. Corell - Chemistry I Accelerated
True/False - If the statement is true, write true. If the statement is false change the
underlined word(s) to make the statement true.
____________________ 19. Intermolecular forces determine metallic properties such as the boiling point
of a substance
____________________ 20. Intermolecular forces are forces of attraction between atoms.
____________________ 21. Covalent bonds are the forces between molecules.
____________________ 22. Covalent bonds result from electrons being shared between atoms in a
molecule.
____________________ 23. Intermolecular forces result from the electron interactions between
neighboring molecules.
____________________ 24. When the electron cloud is not distributed symmetrically, a molecule has
polarity.
____________________ 25. Chemical bonds include ionic bonds, metallic bonds and atomic bonds.
____________________ 26. Intermolecular forces include dispersion forces, dipole-dipole forces, and
helium-bond forces.
On the line at the left, write the letter of the term that matches each description below.
Each choice can be used once, more than once, or not at all.
a. dispersion
b. dipole– dipole
c. hydrogen bonding
_____ 27. the force in-between SO2 molecules.
_____ 28. the force that accounts for HF being a liquid while H2 and F2 are gases
_____ 29. the force that depends on temporary, induced dipoles
_____ 30. the only intermolecular force that exists in noble gases
_____ 31. the attractive force between neighboring molecules with dipoles
_____ 32. the attractive force that arises because of the large difference in electronegativities in the N–H
bonds
33. Check each of the following that could be used to explain why water has an unusually high boiling
point.
_____ a. water molecules have a strong intermolecular force
_____ b. there are no nitrogen atoms in water
_____ c. oxygen is more electronegative than hydrogen
_____ d. water is an angular molecule
_____ e. oxygen atoms are smaller than hydrogen atoms
_____ f. water does not contain metallic bonds
_____ g. there is a large difference in electronegativity between oxygen and hydrogen
page 10
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Dr. Corell - Chemistry I Accelerated
On the line at the left, write the letter(s) of the solids that exhibit the property listed below.
Each choice can be used once, more than once, or not at all.
a. ionic solid
b. metallic solid
_________ 34. high melting point.
c. molecular solid
d. network-covalent solid
__________ 35. poor conductor
_________ 36. malleable
__________ 37. brittle
Changes of State
On the line at the left, write the term from the list that matches the description
condensation
freezing point
sublimation
deposition
melting
vaporization
equilibrium vapor pressure
phase change
volatile
__________________ 38. conversion of a solid directly to a gas.
__________________ 39. opposite of vaporization
__________________ 40. temperature at which solid and liquid forms of a substance exist in equilibrium
__________________ 41. conversion of a substance from one of the three physical states of matter to
another
__________________ 42. pressure exerted by a constant number of gas particles above a liquid or a solid
__________________ 43. change of state from liquid to gas
__________________ 44. description of a liquid that evaporates easily
__________________ 45. transformation of a gas directly into a solid
__________________ 46. phase change from a solid to a liquid
On the line at the left, write “true” if the statement is true. If the statement is false, change
the underlined word(s) to make the statement true.
____________ 47. The average kinetic energy of the particles in a liquid depends on the temperature.
____________ 48. Solids do not flow because the attractive forces between their particles are weaker than
those in liquids or gases.
____________ 49. Dynamic equilibrium is reached when the rate of vaporization exceeds the rate of
condensation.
____________ 50. Condensing liquid water is the opposite of melting solid ice.
____________ 51. All three states of matter can exist in equilibrium at the triple point.
52. Why do ice cubes if they are left sitting in the freezer for a long time become rounded?
53. The heat of fusion for water is 6.00 kJ/mol. Calculate how much energy must be used by your body to
melt 1500 grams of ice.
page 11
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54. At the triple point of ice, liquid water and water vapor all exist at the same time. Compare the kinetic
energy and total energy of the molecules of the ice, liquid water, and water vapor at the triple point.
55. Six transitions are listed in the diagram below. Use arrows to connect each transition to its beginning
state and its ending state. One example is done for you. When completed, each beginning and ending
state will be used twice.
56. In the phase diagram (three phases of matter), correctly label the x-axis, the triple point, normal melting
and boiling points and the critical temperature. Write in the names of the six phase transitions in the
arows provided.
page 12
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Dr. Corell - Chemistry I Accelerated
Processes Involving Liquids and Solids
boiling
deliquescence
evaporation
condensation
distillation
fusion
crystallization
efflorescence
hydration
decrepitation
equilibrium
sublimation
The change of a liquid to a gas is called _______________. The change of a gas to a liquid is called
______________. A balance in the rates of such opposing processes is called ___________. The change
of a liquid to bubbles of gas of the same substance within the liquid is called _____________. A process for
purifying a liquid by changing it to a gas and then changing it back to a liquid is called ______________.
The quantity of heat needed to change a unit mass of a solid to a liquid is called the heat of ___________
of the substance. The change of a solid directly to a gas is called ______________. The water that is
sometimes chemically combined in the crystals of a compound is called water of ______________. The
spontaneous loss of such water at room temperature is called ______________. The removal, by heat, of
water that is only mechanically enclosed and not chemically bound in a crystal is called ______________.
The spontaneous absorption, by a solid, of enough atmospheric moisture to dissolve the solid is called
______________.
NONMETAL ELEMENTS PUZZLE
In the puzzle below find the full name of every nonmetal element. Each name is in a straight-line
segment. To help you get started, ARGON, NEON and, OXYGEN are in bold. Letters may be used
more than once. The unused letters spell out a message.
N
M
N
S
U
L
F
U
R
L
R
I
O
E
I
M
U
I
L
E
H
E
I
C
N
O
E
N
T
T
A
R
T
U
E
E
M
O
E
K
R
Y
P
T
O
N
S
U
D
N
A
O
R
C
O
R
A
U
I
I
I
C
G
X
O
R
I
T
R
N
N
R
I
A
E
E
Y
S
N
A
O
E
E
O
page 13
T
R
N
P
N
G
E
N
H
L
N
L
A
B
L
O
D
O
E
N
P
E
I
H
T
O
O
O
U
X
F
N
S
S
M
C
S
N
S
R
C
R
A
D
O
N
O
I
A
N
E
G
O
R
D
Y
H
C
R
T
N
A
R
G
O
N
H
D
P
T
B
Y
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Dr. Corell - Chemistry I Accelerated
Challenge Problems – States of Matter
1.
People frequently run dehumidifiers in their homes in the summer and humidifiers in the winter. How
can the action of these devises help keep us comfortable?
2.
Hot molten rock wells up at fissures deep in the oceans. Boiling has sometimes been observed at these
sites. Would the boiling point occur at a higher, lower, or the same temperature at the ocean’s surface.
Give the reason for your answer. No bubbles of steam ever make it to the ocean surface to give
evidence of the boiling far below. How can you account for this fact?
3.
What is the final temperature when 7500.0 J of energy is added to 18.0 g of ice at 0.00°C? Heat of
fusion of ice = 334 J/g.
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4. How much heat energy is kilojoules required to turn 45.0 g of solid cesium at 24.0°C into gaseous
cesium at 1161.0K? Cesium’s melting point = 28.4°C; boiling point = 674.8°C. Specific heat of solid
cesium = 0.2421 J/(g x °C); specific heat of liquid cesium is 0.2349 J/(g x °C); specific heat of gaseous
cesium is 0.1564 J/(g x °C); heat of fusion of cesium = 2087 J/mol; heat of vaporization of cesium is
67 kJ/mol.
page 15
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Condensed Matter - Word Scramble
Use the clues provided to help you unscramble the letter to form words related to the condensed forms of
matter. The letters in the circles spell out, in order, the name of a change.
CLUES
1. Ionic, molecular and network
7. Really more like a liquid
2. Kind of a cell
8. Lattice forming
3. Not malleable
9. Balance
4. Absorbing of and dissolving in water
10. Without water
5. Having high vapor pressure
11. Very hard solid
6. Alloy of mercury
1. S L S I O D
__ __ __ __ __ __
2. T I N U
__ __ __ __
3. L T I R B E T
__ __ __ __ __ __ __
4. E U I E E Q S L T N D C
__ __ __ __ __ __ __ __ __ __ __ __
5. O V I E T L L A
__ __ __ __ __ __ __ __
6. A A G L M M A
__ __ __ __ __ __ __
7. O U H A O S P M R
__ __ __ __ __ __ __ __ __
8. L S C A Y L R T N I E
__ __ __ __ __ __ __ __ __ __ __
9. Q I I R E L M U U B I
__ __ __ __ __ __ __ __ __ __ __
10. R Y N D H A O S U
__ __ __ __ __ __ __ __ __
11. K W T O N R E
__ __ __ __ __ __ __
Word: ___________________________________
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