Name Date Period __

Chemistry Unit 2 Review-Matter and Energy

I. Vocabulary

_________________________ 1. Anything that has mass and takes up space is called

_________________________ 2. The law that states that matter cannot be created or destroyed in an ordinary chemical reaction.

_________________________ 3. Characteristics of matter that can be described without changing the chemical composition.

_________________________ 4. A physical property of matter that is not dependent upon the particular sample of that type of matter.

_________________________ 5. A physical property of matter that changes with different samples of that matter.

_________________________ 6. Characteristics of matter that describes how a substance reacts or doesn’t react to other substances.

_________________________ 7. Theory that states all matter is made of tiny particles in constant motion.

_________________________ 8. Energy based on the position or condition of the matter.

_________________________ 9. Energy due to the motion of matter.

_________________________ 10. State of matter made of electrically charged atoms with large amounts of energy.

_________________________ 11. Classification of matter that consist of elements and compounds.

_________________________ 12. Atoms of two or more elements, chemically bound in a definite ratio.

_________________________ 13. Atoms of two or more elements, physically combined in no definite ratio.

_________________________ 14. Matter made of only one type of atom.

_________________________ 15. A mixture that is the same throughout. (A solution.)

_________________________ 16. A mixture that is different throughout.

_________________________ 17. A solute dissolved in a solvent.

_________________________ 18. A solution that conducts electricity.

_________________________ 19. A solution that contains all the solute that it can hold at a given temperature.

_________________________ 20. A solution that temporarily holds more solute than it should be able to at a given temperature.

II. Types of Mixtures – Identify each as a Solution, a Suspension or a Colloid.

_____ 1. Particles are large enough to be seen with the naked eye.

_____ 2. Particles dissolve.

_____ 3. Particles are too small to be seen, but can scatter light.

_____ 4. Particles are too small to scatter light.

_____ 5. Particles will separate out of the mixture by filtering.

Name Date Period __

III. Potential or Kinetic Energy – Label each as PE or KE.

_____ 1. Determined by space between particles.

_____ 2. Determined by the speed (motion) of the particles.

_____ 3. An increase in this energy causes temperature to rise.

_____ 4. An increase in this energy causes phase changes.

IV. Phases of Matter

PhaseParticle diagram

Particle Movemen

t

Amount of PE & KE

Keep Volume?

Keep Shape?

Solid

Liquid

Gas

V. Short Answer

1. At the particle level, what happens when a substance dissolves?

2. Why is boiling point an intensive property?

3. Will salt dissolve in oil? Why or why not?

4. Why doesn’t temperature change during a phase change?

5. What factors influence the rate that a solute will dissolve in a solvent?

VI. Classification of Matter – Write E for element, C for compound, HE for heterogeneous mixture or HO for homogeneous mixture.

_____ 1. Sodium chloride _____ 7. Oxygen

_____ 2. Whole milk _____ 8. Air

_____ 3. Beach sand _____ 9. Helium

_____ 4. Apple _____ 10. Salt water

_____ 5. Sugar _____ 11. Liquid mercury

_____ 6. Uranium _____ 12. Asphalt

VII. Identify each of the following as a physical (P) or a chemical (C) property or change.

1. Grinding something into a powder. 2. Boiling water.

Name Date Period __

3. Burning when exposed to oxygen.

4. Insoluble in water.

5. Dissolving salt.

6. Acid and base react to form salt and water.

7. Size.

8. Sublimating dry ice.

9. Magnetizing iron.

10. Painting a fence.

VIII. Phase Changes – Name each of the following phase changes.

_________________________ 1. A solid changing into a liquid.

_________________________ 2. A solid changing directly into a gas.

_________________________ 3. A liquid changing into a gas at room temperature on the surface.

_________________________ 4. A liquid changing into a solid.

_________________________ 5. A liquid changing into a gas within the liquid with the addition of heat.

_________________________ 6. A gas changing into a liquid.

_________________________ 7. A gas changing directly into a solid.

*** Label each of the phase changes as endothermic or exothermic. ***

IX. Phase Change Graphs

I

_____ 1. Which line segments show heat changing into kinetic energy?

_____ 2. Which line segments show heat changing into potential energy?

Tem

pera

ture

oC

90

80

70

60

50

40

30

20

10

0

-10

Time (min)

Temperature vs time

F

G

H

J

Name Date Period __

_____ 3. Which line segment shows matter in all solid phase? Which line segment shows matter in all liquid phase? _____

Which line segment shows matter in all gas phase?

_____ 4. Which line segments show phase changes?

_____ 5. Which line segments represent the particles of matter gaining speed?

_____ 6. Which line segments represent the particles of matter moving farther apart?

_____ 7. What is the boiling point temperature of this substance? What is the melting point temperature? _____ What would be the freezing point temperature?

_____ 8. Which line segment represents matter with the maximum amount of kinetic energy? Which line segment represents matter with the maximum amount of potential energy?

XI. Solubility- use the table below to answer the questions.

1 a. At 90C, 10 g of potassium chlorate is dissolved in 100. g

of water. Is this solution saturated, unsaturated, or

supersaturated?

b. How do you know?

2. A saturated solution of potassium chlorate is dissolved in 100. g of water. If the saturated solution is cooled from 90C to 60C, how many grams of precipitate will be formed?