Chemistry Final Exam Study Guide
Your chemistry final will cover chapter 7-16 and 20. Since we just took a test over chapter 20, I
am not going to reprint the chapter 20 study guide. There were some chapters and sections
that we skipped and others that we spent a great deal of time on, so I have tried to set up a
study guide to help you focus your efforts to the concepts I feel are most important. Your final
will be 200pts (probably 80-100 questions) and will be taken on a scan-tron.
Any vocab term that we have discussed, mentioned, looked at, written in notes, etc is fair game
for this test; however do not focus all of you time on studying vocab because there will be
several calculations to solve as well as problem-solving such as balancing equations, writing
chemical reactions, and naming compounds
You can use a 3x5 (inches) notecard filled with whatever notes you want!
Chapter 7-1 (Sample and practice problems pgs 223-228; 230-233)
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Use prefixes to name a binary molecular compound from its formula.
Ex., CO2 is carbon dioxide
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Write the formula of a binary molecular compound given its name
Ex., zinc iodide is ZnI2
Determine the formula of an ionic compound formed between two given.
Ex., Cobalt (IV) oxide is CoO2
Know common monatomic and polyatomic ions and their charges. (table 7-1 pg 205 and
Table 7-2 pg 210)
Know the names and formulas of common binary acids and oxyacids (table 7-5 pg 214)
Also covered in chapters 15-16
Chapter 7-2
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Assign oxidation numbers of each element in the formula of a chemical compound.
(Rules for assigning oxidation numbers are on pg 216 and sample problems on pg 217)
Chapter 7-3
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Be able to calculate the number of molecules, formula units or ions in a given molar
amount of a chemical compound and be able to calculate the percent composition of a
given chemical compound (sample problems 7-9 to 7-11 pgs 225- 228 should be good
practice.)
Chapter 7-4
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Determine and empirical formula from either a percentage or a mass composition.
(Sample problems 7-12 and 7-13 pgs 230-231)
Determine a molecular formula from an empirical formula (Sample problem 7-14 pg
232)
Chapter 8-1
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Be able to write a word and formula equation for a given chemical reaction
Be able to balance chemical formulas
Chapter 8-2
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Be able to classify reactions as synthesis, decomposition, single replacement, double
replacement, or combustion. Based on the type of reaction, be able to predict the
products of a reaction when given only the reactants.
Chapter 8-3
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Be able to determine if a reaction will occur and what the products will be based on an
activity series.
I would strongly suggest completing all practice and sample problems throughout chapter
9!!!!!!
Chapter 9-1
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Be able to write a mole ratio of two substances in a chemical equation. ( Must be able to
correctly balance the chemical equation.)
Chapter 9-2

Be able to calculate the amount in moles or the mass in grams of a reactant or product
based on the amount in moles or mass in grams of a different reactant or product.
(sample problem 9-1 - 9-5)
Chapter 9-3
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Be able to calculate the amount in moles or mass in grams of a product, when one of
the two reactants is in excess and one limits the reaction.(Sample problems 9-6 and 9-7)
Be able to calculate percent yield when given the actual yield and quantity of a reactant.
(sample problems 9-8)
Chapter 10-1
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Be able to explain the behavior of the different states of matter based on the
assumptions of the kinetic molecular theory.
Describe the characteristic properties of gases
Distinguish an ideal gas from a real gas.
Chapter 10-2
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Be able to apply convert units of pressure.
Chapter 10-3
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Know that the temperature and pressure at STP
Be able to use Boyle’s law to calculate volume-pressure changes
Be able to use Charles’ Law to calculate volume temperature changes (remember to
convert temperature to Kelvin.)
Be able to Gay- Lussac’s Law to calculate pressure and temperature changes at a
constant volume.
Be able to use the combined gas law to calculate volume- temperature- pressure
changes.
Chapter 11-1

Know the standard molar volume of a gas at STP and be able to use it to calculate gas
masses, volumes, and molar mass of a given gas.
Chapter 11-2
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Be able to solve for amount of moles, temperature, pressure, or volume of a gas by
using the ideal gas law. (Value of R pg 342) (Sample problems 11-3, 11-4, 11-5)Also be
able to use the ideal gas law to calculate the molar mass or density of a gas. (Sample
problem 11-6)
Chapter 12-1
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Describe the motion and properties of liquids according to the kinetic molecular theory.
Chapter 12-2
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Describe the motion and properties of solids according to the kinetic molecular theory.
Distinguish between the two types of solids
Chapter 13-1
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Distinguish between heterogeneous and homogenous mixtures.
List three different solute-solvent combinations
Compare the properties between suspensions, colloids, and solutions.
Distinguish between electrolytes and non-electrolytes.
Chapter 13-2
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Compare the effects of temperature and pressure on solubility
Explain the meaning of like dissolves like in terms of polar and non-polar substances
Explain solution equilibrium and distinguish between saturated, unsaturated, and supersaturated solutions.
List and explain at least three factors that affect the rate at which a solid solute dissolves
in a liquid solvent.
Chapter 13-3
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Be able to calculate the concentration of a solution in either molarity (M) = moles
solute/ L solution or molality(m)= moles solute/ mass(kg) solvent
Be able to calculate the amount of solute in a given amount of solution when given the
concentration
Be able to calculate the amount of solution that contains a given amount of solute.
Chapter 14-1
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Be able to write net ionic equations
Determine if a product will be soluble or insoluble based on solubility rules (these will be
provided for you)
Chapter 14-2
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Be able to calculate freezing point depression, boiling point elevation and solution
molality of non-electrolytic and electrolytic solutions.
Chapter 15-1
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Be able to list general properties of both acids and bases
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Name common binary acids and oxyacids when given their chemical formula. (There is a
list of these in chapter 15 on page 468, as well as rules for naming and a table of
common acids and bases in chapter 7.)
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Define and identify acids and bases according to the Arrhenius theory of ionization, the
Bronsted-Lowry definition and the Lewis definition.
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Define the differences between strong and weak acids and bases
Chapter 15-2
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Be able to identify conjugate acid-base pairs in a chemical reaction
Determine the formula for the conjugate pair of an acid/base.
Be able to write chemical equations, overall ionic equations, and net ionic equations for
acid or base reactions.
Be able to write reactions that represent the multiple stages of ionization. (figure 15-10
gives a good example of this.)
Chapter 15-3
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Be able to explain the process of acid/base neutralization
Be able to write chemical reactions that represent neutralization between an acid and a
base salt + water
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Be able to write the formula of oxyacids/ bases and binary acids/ bases when given the formula.
o Potassium carbonate_________________________________
o Carbonic acid_______________________________________
o Sulfuric acid________________________________________
o HClO4 _____________________________________________
o H2SO3______________________________________________
o Hydrochloric acid_____________________________________
o Bromic Acid_________________________________________
Explain the difference between and Arrhenius Acids/Bases and Bronsted Lowry Acids/ Bases.
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Why are strong acids also strong electrolytes.
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What is the difference between a strong and weak acid?
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Explain the relationship between conjugate acids and bases. (What does a base form from…..A
strong acid or base forms what?)

Label the conjugate acid/base pairs in the following reaction between water and acetic acid:
H2O + CH3COOH

H3O+ + C2H3COO-
Be able to determine the products of an acid base neutralization reaction. (Think of this as a
double displacement reaction)
Ca(OH)2 + HF ____________
+ _______________
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Explain the meaning of both a Lewis acid and a Lewis Base. How is this different from the
Bronsted -Lowry or Arrhenius definition of acids and bases?
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What is meant by the term “ self- ionization of water”?
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How can Kw (1x10-14M2) be used to calculate [H3O+] or [OH-]?
o
Practice problems 1-4 pg 484
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Be able to explain the ph scale (And apply pOH) . Be able to state approximate pH ranges of
some common household materials. (pg 486)

Calulate pH from [H3O+ ] and pOH from [OH-]. From these values determine if the solution is an
acid, a base, or neutral. Ph= -log [H3O+ ] pOH= - log [OH-].
o
Practice problem 1 pg 487

Calculate [H3O+] from pH and [OH-] .
o Practice problems 1-4 pg 490