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- MatterPages covered- 38-42, 45-58
Vocabulary-
chemistry matterelementphysical changechemical changereactivity
compoundmoleculechemical formulapure substancemelting point flammability
mixturedensityfreezing pointatomboiling pointphysical property
chemical propertyheterogeneous mixturehomogeneous 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
- If the density of gold is 19.3 g/mL, what is the mass of 5mL of gold?
- A 4mL sample of lead has a mass of 45.2 g/mL. What is its density?
- 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?
- 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.
Chapter 3-States of MatterPages covered- only section 1 – 70-78
Vocabulary-
plasmaenergygasthermal energyevaporationsublimationsolid condensation liquid law of conservation of mass 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)
- At what point(s) (letters A-E) is there no temperature change despite the addition of heat
energy? - What letter represents a gas?
- What letter represents freezing?
- Why is there a constant temperature when a substance is changing phase? (pg 76)
Chapter 7- Solutions
Vocabulary- solution solventsolute solubilityconcentration
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 / Solutea. / 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 offine table salt.
17. Describe three methods you could use to make a spoonful of salt dissolve faster in water.
Chapter 13- Heat and TemperaturePages covered- 420-431
Vocabulary- temperature thermometer absolute zero heat thermal conduction
convection convection current radiation
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)
- increase in massc. increase in average kinetic energy
- decrease in average kinetic energyd. decrease in mass
Chapter 4- Atoms and the Periodic TablePages covered- 104-108,110-128- skip section 4
Vocabulary-
nucleusprotonneutronelectronionnonmetalatomic number
valence electronperiodic lawperiod group metalloidmetal mass number isotope inert
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.
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 MatterPages covered-144-145, 151-155, 159-161- Skip section 4
Vocabulary- ionic bondmetallic bondcovalent bond
oxidation numberpolyatomic 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. CaCl2c. Mg3P2
47. Determine the type of bond holding the atoms together in the following compounds:
a. KClb. NH3c. CH4d. CO2
48. First, write the correct formula needed for these elements to combine, then name the resulting compound.
Formula / Namea. Sodium and Iodine
b. Sodium and Oxygen
c. Magnesium and Bromine
d. Phosphorus and Fluorine
Chapter 6-Chemical ReactionsPages covered-184-189, 198-201 skip sections 2 and 4
Vocabulary-
reactant product chemical energy 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
- KClO3 KCl + O2c. Ba(NO3)2 + NaCl BaCl2 + NaNO3
- Zn + HCl ZnCl2 + H2d. H2O + O2 H2O2
55. How many atoms of each element are present in the following formulas?
- Ca(NO3)2b. NH4CO3c. 2Mg(C2H3O2)2d. P2(SO4)3
Chapter 9- Nuclear ChangesPages covered- 284-288, 293-298 skip section 3
Vocabulary-
radioactivitynuclear radiationalpha particlebeta particle
gamma rayfission nuclear chain reactionfusioncritical 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 SystemPages covered- 630-636, 646-649 skip section 2
Vocabulary-
planet solar system satellite phase eclispse nebulanebular 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 UniversePages covered-666-673, 680-686 skip section 2
Vocabulary-
starlight-yearred giantwhite dwarfsupernovablack holeuniverse
red shiftbig bang theory
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?