Download Honors Review for Semester 1 Final 2014

This review outlines all the major topics that we have covered thus far and will cover before the final. There are sample
problems, questions, and also some problems given from the text book. The answers to the even numbered problems
are found in the back of the book. I will post the answers to the odd numbered problems before the final. A very
important piece of your preparation for the final exam should be taking time to review your old multiple choice and free
response exams.
CHAPTER 2:
Major Concepts/vocabulary:
1. Define and give an example of a quantitative observation and a qualitative observation.
2. Review scientific notation
3. Metric system:
4. Explain in your own words why there is uncertainty in measurement.
5. Conversions (including cubic measurements)
6. Define the term density. Can it be determined from a single measurement?
Questions from the Text: 35-37, 44, 56, 83, 85, 90, 92, 100
Other problems:
a) What is the length of a crystal of copper sulfate in meters that is 1.25 mm long?
b) DNA is approximately 2.5 nm in length. If an average man is 1.8m tall, how many DNA molecules could be
stacked end to end in an average man?
c) A liquid has a volume in 3.70 liters. What is its volume in ml? in cm3?
d) If an object weighs 0.092g, what is its mass in mg?
e) What is the density of an object with a mass of 1.663 g and a volume of 0.2009 mL?
f) What is the mass in kilograms of 750 mL of a substance that has a density of 0.930 g/ml?
g) An object weighs exactly 5 g on an analytical balance that has an accuracy of 0.1mg. To how many significant
figures should this measurement be recorded?
CHAPTER 3:
Major concepts/vocabulary:
1. Define and illustrate the three states of matter.
2. Define a physical change and give 3 examples.
3. Define a chemical change and give three examples.
4. Differentiate between chemical and physical properties.
5. Define atom, element, compound
6. What is a mixture?
7. What is a pure substance? Give examples.
8. What is the difference between a homogeneous mixture and a heterogeneous mixture?
9. See figure3.6- 3.8 for filtration techniques.
Questions from the text: 5, 8, 13, 14, 18, 21-24, 30, 32-35, 54,
CHAPTER 4:
Major concepts/Vocabulary
1. The story of the Atom: know the major atomic scientists and their contributions towards atomic theory:
Democritus (ancient Greeks), Dalton, Thomson, Rutherford
2. You should also be able to illustrate the above scientists’ models of the atoms, labeling subatomic particles.
3. Define atom, nucleus, proton, neutrons, and electron.
4. From the atomic number and the mass number, you should be able to give the name of the element, number of
protons, neutrons, and electrons.
5. Define Isotope.
6. Calculate average atomic mass from information about the isotopes (see beanium lab from Ch 8)
7. Define ion, and how they are produced.
8. What is a cation? Where are they found on the periodic table?
9. What is an anion? Where are they found on the periodic table?
10. Be able to write ionic compounds from ions.
11. Natural states of the elements: which elements are commonly found in the diatomic state?
12. Where are the metals located on the periodic table? The metalloids? The nonmetals?
Questions from the text: 4, 16, 18, 21, 22, 38, 40, 42, 82, 84
CHAPTER 5:
Major concepts, vocabulary:
1. What are the rules for naming Type I, Type II, Type III, and Type IV molecules?
2. What is an oxyanion?
3. Know prefixes 1-8 ( see Table 5-3)
4. How do you name acids?
5. LEARN POLYATOMIC IONS!
Questions from the text: 10, 14, 18, 20, 36, 40, 50, 58, 60
CH 8: The Mole
Major Concepts/Vocabulary:
1. The mole & Avogadro’s Number
2. Counting by Mass
3. Atoms, Molecules and Formula Units
4. Conversions between Moles, Mass and Particles
5. Average Atomic Mass and Molar Mass
6. Percent Abundance (of an element’s isotopes)
7. Percent Composition
8. Hydrates
9. Calculating Empirical Formulas
10. Calculating Molecular Formulas
Questions from the Text: 4,8,10, 12,18,24,26,28,40,46,52,56,68,70,76,77,80,82,
CH 13: Gases
Major Concepts/Vocabulary:
11. What causes pressure? Pressure conversions
12. How does a barometer work?
13. Gas Laws (PV=nRT, Boyle’s, Charles’, Gay-Lussac’s, Avogadro’s, Combined)
14. Absolute zero
15. STP definition
16. Standard Molar Volume @ STP (22.4 L = 1 mol of any gas!)
17. Only if at STP then you may use the conversion 22.4L = 1mol, if not at STP then you use PV=nRT to find V
18. Dalton’s Law of Partial Pressures (gas collected over water…)
19. Kinetic-Molecular Theory (Ideal vs. Real gasses, PVT changes through motion of molecules)
Questions from the Text: 12, 24, 30, 42, 52, 68, 74
OTHER IMPORTANT STUFF…
 Study your ions & review your old exams during tutoring.
 Review the sample problems in the text to help you remember what type of
calculations you’ll need to know how to do
 Class website has all our powerpoints available - trinechemistry.wikispaces.com
 Start studying now…do a little each night 
 Try hard! This exam is 15% of your final grade (1 ½ letter grades).