Name _______________________
Mr. Taylor-Waldman
Unit 2 Test Review: States of Matter
→ Fully completed review sheets can be handed in on the day of the test (Monday, Dec. 21) for three
points extra credit. All blanks must be filled in, and all review questions must be answered completely.
Chapter 2, Section 1 – The Four States of Matter (pages 42-47 in CBB textbook, “States of Matter”
powerpoint file on my Weebly)
Terms
Shape
Volume
Particle Arrangement
Solid
_____________
Definite
fixed positions and ___________ in place
Liquid
Indefinite
_____________ close together but free to move around
Gas
_____________
Indefinite
spread very far apart and moving fast
crystalline solids: solids with a patterned arrangement of particles that melt at an _______________
temperature. Examples: _______________________________
amorphous solids: solids with no patterned arrangement of particles that don’t __________ at an exact
temperature but get softer and softer when heated. Examples: glass, rubber, plastic, butter
plasma: a fourth state of matter that occurs when high-energy particles in a gas lose or gain electrons.
surface tension: an increased “pull” among the top surface molecules of a liquid that brings these
molecules ____________ ______________. This causes the surface to act as if it has a thin skin.
viscosity: a liquid’s ________________ to flow. High viscosity ex: ____________ low: ____________
hydrogen bonding: _________ H atoms in one water molecule are pulled toward the negative O atom in
another water molecule.
cohesion: the strong attraction water molecules have for one another.
hydrophilic: water-“loving” end of a soap molecules which dissolves in water.
hydrophobic: water-“fearing” end of a soap molecule that doesn’t dissolve in water and can attach to
fat or oil molecules.
Concepts
1. Each state of matter can be described by its shape and __________ (is it definite or indefinite?).
2. The arrangement, energy, and motion of molecules differs between the four states of matter.
3. Crystalline and amorphous are two different types of solids. Many compounds and elements
are crystalline solids. All crystalline solids have an ____________ melting point and particles
arranged in a regular ____________. Amorphous solids don’t have an exact ____________
____________ and their particles are not in a pattern.
4. Flames are an example of plasma. In the “Firestorm” article in Science World, we learned that
solids, liquids, gases and plasma are all present in a forest fire. We also learned about different
type of technology used to fight forest fires.
5. Two unique properties of liquids are surface tension and viscosity. Know how cohesion and
hydrogen bonding relate to surface tension.
6. In STEM Lab #3, we explored surface tension and viscosity through experiments with floating a
paper clip on water, putting water drops on a quarter, and a viscosity “race.” We also saw how
soap can weaken bonds in a liquid like milk because of its dual hydrophobic and hydrophilic
structure.
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Chapter 2, Section 2 – Changes of State (pages Pages 48-53 in CBB textbook, “Changes of States”
powerpoint file on my Weebly)
Terms
Solid
Liquid
Gas
Exo- or Endothermic?
Melting
Freezing
Vaporization
Condensation
Sublimation
Evaporation: vaporization only on the _____ _________ of a liquid. Ex: a puddle disappearing over
time
Boiling: vaporization at and _________ a liquid’s surface. Ex: heating a pot of water on a stove
Concepts
1. Changes of state occur when a substance loses or gains a sufficient amount of thermal energy.
2. The lower the air pressure, the ______________ a liquid’s boiling point.
3. Given a set volume/mass of water, it takes far more time and energy for water to boil than it
does for water to melt. This is because the difference in energy and particle speed between the
liquid state and the gas state is much greater than the energy/particle speed difference between
the ______________ state and ______________ state.
Chapter 2, Section 3 and 4 – Gas Laws and Graphing Gases (pages Pages 55-65 in CBB textbook,
“The Gas Laws” powerpoint file on my Weebly)
Terms
pressure: the measure of the force of the outward push of a gas on the walls of the container. This
occurs because gas particles are in constant collision with each other and with their container.
Boyle’s Law: at constant temperature, when volume ___ pressure ↑
Charles’s Law: at constant pressure, when volume ↑ temperature ↑
The Third Gas Law: at constant ______________, when temperature ↑ pressure ___
direct relationship: a mathematical relationship where two variables increase or decrease together
indirect relationship: a mathematical relationship where as one variable decreases, the other variable
______________.
Concepts
1. The three measurements used to describe gas: _________, __________ and ____________.
2. In Boyle’s Law, Charles’s Law, and the Third Gas Law there is always one constant and two
variables that affect each other.
3. In STEM Lab #4, we looked at how the gas laws could be used to explain the “can crushing,”
“egg in the flask,” and “balloon in hot and cold water” experiments.
4. Be able to recognize a graph of Charles’s Law, the Third Gas Law, or Boyle’s Law.
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5. Know how to identify a graph that is directly proportional and one that is indirectly proportional.
Review Questions
1.Why are the particles of a solid not actually stationary? What happens to solid particles as a substance melts?
2. What is an amorphous solid? How are its particles arranged? Describe the melting point of amorphous solids.
3. Label each letter in the graph below. Why is the interval between D and E much larger than the interval
between B and C?
4. What is viscosity? Give one example of a liquid with high viscosity, and one with low viscosity.
5. What is the name of the process in which a gas cools and becomes a liquid? What are two examples of this
process?
6. When you see steam, fog, or clouds, are you seeing water in its gas state or liquid state? Can you see water
when it is a gas (water vapor)? Explain.
7. According to Boyle’s Law, what happens as the volume of a gas decreases, and what value is constant?
8. On a cold winter afternoon in January, you and your parents buy 15 helium balloons for your uncle’s birthday
party and then leave them in your parent’s car for three hours. When you come back to your car you see that the
balloons have noticeably deflated and aren’t as nearly as large as when you bought them. Why did this happen,
and which gas law explains the change you have observed? Be specific!
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9. Thinking back to the Surface Tension and Viscosity lab, explain what caused the water on your quarter to form a
curved “dome” shape? Use the terms surface tension, cohesion, and hydrogen bonding in your explanation.
10. State the Third Gas Law, and give an example that illustrates this law. Then, draw a simple graph, with each
axis labeled, to illustrate this law.
11. Describe
what happened in the “can crushing” or “egg in the flask” experiment. Which two gas
laws describe why the can was crushed, or why the eggs was forced into the bottle, and how do they explain it?
12. What does it mean if two variables in a graph are directly proportional? Inversely proportional? Draw a simple
graph that shows an inverse relationship.
13. How does heating a gas in a rigid (inflexible) container change its pressure?
14. What happened to the food coloring when the q-tip was placed in the dish, and why did this happen?
15. Describe the process of sublimation and give one example of this change of state.
16. Why does the evaporation of sweat cool your body on a warm day? (hint: is evaporation exo- or endothermic?)
17. At want point to particles that are losing energy and slowing down start to form regular patterns?
18. Using what you know about the particles in a gas, explain why a gas has no definite shape or volume.
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19. Death Valley, am extremely dry, desert region in Eastern California, is 282 feet below sea level. Predict whether
water will boil at a lower or higher temperature than normal, and explain why this is the case.
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