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CPE Science Semester 2 Final Exam Review 2014-15 Instructions for using this review sheet: This review sheet is divided into chapters with the pages covered in each chapter listed because we did not cover all parts of all chapters. The important vocabulary is listed for each chapter. You should make flash cards of the vocabulary to help you study. A set of questions follows the vocabulary in each chapter. Look for the answers to these questions in your book and in your notes. These questions do not necessarily cover everything in the chapter. They just give you an idea of some of the important topics. This sheet is designed so you can then continue to use this as a question/answer review. Study with friends or family by having other people quiz you. Simply answering these questions will not prepare you for your exam. You must study the information, memorize vocabulary, and seek to understand how to do the problems. Chapter 2- Matter Vocabularychemistry matter compound molecule mixture density chemical property Pages covered- 38-42, 45-58 element physical change chemical change reactivity chemical formula pure substance melting point flammability freezing point atom boiling point physical property heterogeneous mixture homogeneous mixture 1. What is the difference between physical and chemical properties? Give an example of each. 2. Should a material have a higher or lower density in order to float in another substance? 3. Which phase of matter generally has the greatest density? 4. What is the difference between a physical change and a chemical change? Give an example of each. 5. Density problems: solve the following problems showing formula, math w/units and circle answer a. If the density of gold is 19.3 g/mL, what is the mass of 5mL of gold? b. A 4mL sample of lead has a mass of 45.2 g/mL. What is its density? c. An irregularly shaped solid object is placed into a graduated cylinder with 100mL of water. It raises the level of the water to 243 mL. If its mass is 12g, what is its density? d. Object X has a mass of 10g and a volume of 10mL. Object Y has a mass of 2g and a volume of 2mL. How do the densities of the two objects compare. Pages covered- only section 1 – 70-78 Chapter 3-States of Matter Vocabularyplasma condensation energy liquid gas thermal energy evaporation law of conservation of mass sublimation solid law of conservation of energy 6. Describe what happens to the molecules of a substance when it is heated. 7. Explain the shape and volume characteristics of solids, liquids, and gases. 8. Explain the motion of particles in solids, liquids, and gases. 9. What is the relationship between temperature and motion of particles? 10. Analyze the phase change diagram for water and answer the following questions. (pg 77) a. At what point(s) (letters A-E) is there no temperature change despite the addition of heat energy? b. What letter represents a gas? c. What letter represents freezing? d. Why is there a constant temperature when a substance is changing phase? (pg 76) Chapter 7- Solutions Vocabulary- solution solvent solute solubility concentration 11. What is the difference between a heterogeneous and homogeneous mixture? Give example of each. 12. List 3 examples of solutions that are not liquids. 13. Identify the solvent and solute Solvent Solute a. dissolving a small quantity of baking soda in water b. water and juice crystals mixed to make fruit drink c. Kim swished some saltwater in her mouth after she lost her tooth in a soccer game. d. Rosanna added a little sugar to her tea because it tasted bitter e. The tea colored the cup of water as it brewed 14. Why is water the universal solvent? 15. Explain the statement “like dissolves like”. 16. Explain why large crystals of coarse sea salt take longer to dissolve in water than crystals of fine table salt. 17. Describe three methods you could use to make a spoonful of salt dissolve faster in water. Chapter 13- Heat and Temperature Vocabulary- temperature thermometer absolute zero convection convection current radiation heat Pages covered- 420-431 thermal conduction 18. Compare conduction, convection, and radiation 19. Relate absolute zero to the kinetic energy of particles 20. What temperature is 45F on the Celsius and Kelvin scale? 21. Draw the convection currents that would be seen in a pot on the stove. Show where different temperature zones are in the pot. 22. If two objects that have different temperatures come into contact with each other, what will happen? What can you say about their temperatures after several minutes of contact? 23. Temperature is proportional to the average kinetic energy of particles in an object. Thus an increase in temperature results in a(n) a. increase in mass c. increase in average kinetic energy b. decrease in average kinetic energy d. decrease in mass Chapter 4- Atoms and the Periodic Table Vocabularynucleus proton neutron electron valence electron periodic law period group Pages covered- 104-108,110-128- skip section 4 ion metalloid nonmetal atomic number metal mass number isotope 24. What is the atomic mass of oxygen? 25. List the names and location of all the chemical families on the periodic table. 26. What is the atomic number of lead? 27. Where are metals located on the periodic table? 28. How many electrons are in one atom of xenon? 29. How many protons are in one sulfur atom? 30. How many neutrons are in one fluorine atom? 31. Which groups contain the most reactive elements? The least reactive? 32. Where are protons, neutrons, and electrons located in the atom? 33. What is Dalton’s atomic theory? 34. Draw Bohr’s atomic model. inert 35. Define modern atomic theory. 36. Noble gases have how many valence electrons? 37. Where is the nucleus located? 38. Chemical bonding involves what part of an atom? 39. What is a Lewis dot diagram used for? 40. What is the difference between atomic number and atomic mass? 41. Why are Noble gases inert? Chapter 5- The Structure of Matter Pages covered-144-145, 151-155, 159-161- Skip section 4 Vocabulary- ionic bond metallic bond covalent bond oxidation number polyatomic ion 42. What is the oxidation number of all atoms in group 18 of the periodic table? 43. Between which types of atoms do ionic bonds, covalent bonds, and metallic bonds occur? 44. Do metal atoms tend to gain or lose electrons? 45. What makes an atom stable? 46. Show the correct ionic bonding for the following compounds: a. NaCl b. CaCl2 c. Mg3P2 47. Determine the type of bond holding the atoms together in the following compounds: a. KCl b. NH3 c. CH4 d. CO2 48. First, write the correct formula needed for these elements to combine, then name the resulting compound. Formula Name a. Sodium and Iodine b. Sodium and Oxygen c. Magnesium and Bromine d. Phosphorus and Fluorine Chapter 6-Chemical Reactions Vocabularyreactant product chemical energy Pages covered-184-189, 198-201 skip sections 2 and 4 exothermic reaction endothermic reaction chemical equation 49. What is the difference between an endothermic and an exothermic reaction? 50. Where are reactants and products located in a chemical equation? 51. One molecule of C6H12O6 consists of how many atoms of C, H, and O? 52. What is changed or added to balance a chemical equation? 53. In the formula NH3, what does the 3 refer to? 54. Balance the following equations a. KClO3 KCl + O2 b. Zn + HCl ZnCl2 + H2 c. Ba(NO3)2 + NaCl BaCl2 + NaNO3 d. H2O + O2 H2O2 55. How many atoms of each element are present in the following formulas? a. Ca(NO3)2 b. NH4CO3 c. 2Mg(C2H3O2)2 d. P2(SO4)3 Chapter 9- Nuclear Changes Pages covered- 284-288, 293-298 skip section 3 Vocabularyradioactivity nuclear radiation alpha particle beta particle gamma ray fission nuclear chain reaction fusion critical mass 56. Explain the similarities and differences between fission and fusion. 57. Explain the similarities and differences between alpha particles, beta particles, and gamma rays 58. What is half-life? 59. Nuclear changes refer to what part of the atom changing? 60. What is nuclear decay? Chapter 19- The Solar System Vocabularyplanet solar system satellite Pages covered- 630-636, 646-649 skip section 2 phase eclispse nebula nebular model accretion 59.Explain the solar nebular theory of how the solar system formed. 60. What is the difference between the theories of Ptolemy and Copernicus? 61. What did Aristotle do? 62. What is the approximate age of the solar system? 63. What did Kepler do? Chapter 20- The Universe Vocabularystar light-year red giant white dwarf red shift big bang theory Pages covered-666-673, 680-686 skip section 2 supernova 64. Explain the Big Bang theory 65. Explain how the surface temperature of a star is measured. 66. What happens when a star forms? 67. What are the 3 possible fates of the Universe? 68. What is the approximate age of the Universe? black hole universe