2014-2015 CHEMISTRY FINAL REVIEW: Organize your NOTEBOOK to refresh your memory. Identify areas on which you need
to spend more study time. For those areas go back to your homework assignments, text, study guides, and notes. The questions
on the test will be similar to those on the chapter tests. The test includes multiple choice questions. You will be given a periodic
table and you may use a calculator. You may use ONE HANDWRITTEN NOTE CARD. In class, you may refer to the scrapbooks for
inspiration.
I have referenced problems in the text with answers in the appendix that relate to the different subjects. You do NOT need
to do these, but they are helpful for you to look at to see if you remember the material. Your notes, handouts, and
worksheets are the BEST references. If you read a question in the book and don’t recall it, review that material in your notes
and consider using your notecard for it.
Include information that you need on the following topics on your notecard (info in italics will not be on the test):
Chemical Formulas and Chemical Compounds
o Calculate molar mass p 221 #20c #21c
o Convert between moles, grams, # of particles, or volume of a gas p 221 #22c #24c
o Calculate the % composition of a compound #29c
o Define and calculate empirical and molecular formulas from either % composition or mass composition p222 #38 #49
Chemical Equations and Reactions
o List observations that indicate that a chemical reaction may have occurred p248 #2 and #4
o Write word and formula equations using symbols to include information about the reaction p248 #17 and #19
o Balance chemical equations p 249 #35c, #36c, #37c
o Define and give general equations for 5 types of chemical reactions See star chart notes
o Classify reactions See star chart notes
o Given the reactants, predict products of single-displacement, double-displacement, combustion, and simple synthesis
and decomposition reactions
o Use the activity series for single-displacement reactions See notes and chart
o Use the solubility chart/guidelines for double-displacement reactions See #9a and c and e
Stoichiometry
o Define stoichiometry See notes
o Explain the importance of the mole ratio p 328 # 2
o Determine the mole ratio of substances from the chemical equation p 328 # 7
o Use the mole map to perform stoichiometric calculations from moles, grams, volume, or # of particles to grams to
moles, grams, volume, or # of particles p 329 #22
o Differentiate theoretical yield and actual yield See notes and p 331 #43
o Determine limiting reactant, theoretical yield, percentage yield, and excess reactant p 330 # 30, 34, 37c, p 331 #40
and # 48
States of Matter and Graham’s Law
o State and explain the kinetic molecular theory of matter (KMT) and use it to explain properties of matter See notes
and p 510 #1p545 #4,6
o Define ideal gas and describe the conditions under which real gases deviate from ideal gas behavior p 511 #22
o Describe these properties of gases: expansion, density, fluidity, compressibility, diffusion, effusion See notes
o Use KMT to describe properties of gases, liquids and solids p 545 #17
o Define vaporization, boiling, condensation, melting, freezing, sublimation, deposition See notes
o Distinguish crystalline and amorphous solids p 546 #36
o Describe changes of state in terms of KMT p545#15
o Recognize and describe conditions of dynamic equilibrium See notes
o Interpret phase diagrams and heating curves See notes
o Describe equilibrium vapor pressure p 546 #25
o Describe the structure of water and use it to explain its physical properties p 545 #13
o Calculate the amount of heat energy released or absorbed when a quantity of water freezes or melts p 525 ex 14.1
o Describe the processes of diffusion and effusion See notes
o Use Graham’s Law to calculate the ratio of effusion/diffusion of two gases based on their molar masses See notes
Gases
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Define pressure and convert between various pressure units p 510 #4c and #5c
State STP See notes
State and use Dalton’s Law, Charles’ Law, Boyle’s Law, Gay-Lussac’s Law, Avogadro’s Law, combined Gas Law, Ideal
Gas Law p 510 # 7a, #10, #13, #14, #25a
Explain Gas Laws using KMT See notes and p 512, # 53
Understand standard molar volume of a gas = 22.4 L at STP
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Solutions
o Define solution and list different solute-solvent combinations and give examples p 587 #1
o Contrast solutions with suspensions and colloids See notes
o Distinguish electrolytes and non-electrolytes See notes
o Describe the solution process and explain using KMT See notes
o List and explain factors that affect the rate of dissolution in solid/liquid solutions and gas/liquid solutions p 587 #9
o Compare the effect of temperature on solubility See notes on solubility curves
o Interpret solubility curves See notes on solubility curves
o Define %solution, molarity, and molality and perform concentration calculations p588#25
o Describe how to prepare a solution See notes p588 #25, again
o Calculate dilutions p 588 #31c
Ions in Aqueous Solutions and Colligative Properties Your notes are the best resource on this subject
o Write equations for dissolution of ionic compounds in water
o Use solubility chart to predict if precipitate will form when soluble ionic compounds are formed
o Write the total ionic equations and the net ionic equation for precipitation reactions
o Draw and explain the formation of the hydronium ion
o Distinguish strong and weak electrolytes
o List 4 colligative properties and explain
o Calculate boiling point elevation, freezing point depression and solution molality of non-electrolytes and electrolytes
Acids and Bases
o List general properties of acids and bases and give examples
o Name common acids
o Define acid and base according to Bronstead-Lowry, Arrhenius, and Lewis definitions…intro level info only
o Explain difference between strong and weak acids and bases….intro level info only
o Describe a conjugate acid and a conjugate base
o Explain acid rain
Acid-Base Titration and pH
o Describe the self-ionization of water
o Define pH and explain and use the pH scale
o Find pH given hydronium ion concentration or hydroxide concentration…easy problems
o Find hydronium ion concentration or hydroxide concentration given pH….easy problems
o Describe indicators
o Explain titration procedures
o Calculate molarity from concentration data