Review for Semester #1 Honors Chemistry Final
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.
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
6. Define the term density. Can it be determined from a single measurement?
Questions from the Text: 31-33, 40, 52, 79, 81, 86, 88, 96
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
Questions from the text: 13,14, 18, 21-24,54,
CHAPTER 4:
Major concepts/Vocabulary
1. The story of the Atom: know the major atomic scientists and their contributions towards atomic theory: Democritus,
Dalton, Thomson, Rutherford, Bohr
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)
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? Which are liquids at room
temperature?
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 1-10 ( 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
CHAPTER 6:
Major concepts/vocabulary:
1. List the 5 visual clues that may indicate a chemical reaction
2. Label the reactants and products in a sample chemical equation.
3. Is a reaction a chemical or physical change? What is happening to the atoms in the molecules?
4. What is conservation of mass? How does this apply to writing chemical equations?
5. Be able to write and balance equations from word equations and vice versa.
6. What does (aq) mean?
Questions from the text: 9, 13, 20, 22, 38, 40, 54, 64, 68, 76
CHAPTER 7:
Major concepts/vocabulary:
1. What are the 4 driving forces of reactions?
2. Give examples of the 5 major types of reactions (know single replacement, but acid/base will be later).
3. What does it mean if an ionic compound is soluble in water? What property does this give the solution? Where can we look
to find this information?
4. Review notes on predicting products for each of the major types of reactions.
5. Be able to write molecular, complete ionic, and net ionic equations for double replacement reactions.
6. What are spectator ions?
7. How do you use the Activity series? What does it describe?
8. Will the following reactions take place? Predict the products.
a. Ag + CuNO3
b. KBr + F2 
c. Zn + MgCl2
d. Li + AuNO2 
Questions from the text: 61-66, 70, 74, 86, 92
*We will also cover Ch 8 before the final, you will be on your own to review this material.
HINTS: Review Notes, old Tests, go to tutoring, READ THE BOOK, Learn your IONS!
CH 11: Modern Atomic Theory
Major Concepts/Vocabulary
 Electromagnetic radiation
 Wavelength vs. Frequency-and the Greek symbols
 c = λν & E = hν
 Niels Bohr Model of the Atom: electrons move from the ground to the excited state and release photons of energy when
they return to the ground state.
 Wave-Mechanical Model (Orbitals): Defines energy levels as orbitals, where electrons have a 90% probability of being.
 Be able to write electron configuration in longhand and shorthand notation. (Electron Hotel)
 Valence electrons
 Ionization Energy & Atomic Size, definition and periodic trend.
Questions from the Text: 5,6,10, 24, 50, 54, 62, 73, 74, 80, 82, 90, 108