Name Date Period __ Chemistry Unit 2 Review-Matter and EnergyI. 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 Particle Particle Amount of Keep Keep Phase diagram Movement PE & KE Volume? Shape? Solid Liquid GasV. Short Answer1. 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. AsphaltVII. Identify each of the following as a physical (P) or a chemical (C) property or change. 1. Grinding something into a powder. 3. Burning when exposed to oxygen. 2. Boiling water. 4. Insoluble in water.
Name Date Period __ 5. Dissolving salt. 8. Sublimating dry ice. 6. Acid and base react to form salt and water. 9. Magnetizing iron. 7. Size. 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 Temperature vs time 90 80 I 70 J 60Temperature oC 50 H 40 30 20 G 10 F 0 -10 Time (min) _____ 1. Which line segments show heat changing into kinetic energy? _____ 2. Which line segments show heat changing into potential energy?
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 90°C, 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 90°C to 60°C, how many grams of precipitate will be formed?