Final Exam Review
Although this exam is only over second semester, there are concepts from first semester
that are the basis of concepts for second semester. Some of these are: formula writing,
density, ionic and covalent compounds. (Also, if I have forgotten a topic I reserve the right to update this list)
Chemical Equations
 Name chemicals when given the formula and write correct formulas for chemicals when given
their names (covalent compounds, ionic compounds, acids, bases, etc.)
 Know which elements are diatomic
 Know the state of matter for all elements
 Know the common indications or evidence of a chemical reaction
 Write chemical equations when given the reaction in words
 Know the meaning of different symbols used in a chemical equation (+, , , Δ, s, l, g, aq, etc)
 Balance chemical equations
 Know and be able to identify common characteristics of each of the 6 types of reactions discussed
in class
 Classify chemical equations as 1 of the 6 types discussed in class
 Predict the products of a chemical reaction when given the reactants
 Use the Activity Series to determine whether a single replacement reaction will occur
 Use the Solubility Table to determine if an ionic compound is soluble (aq) or insoluble (s)
 Write complete and net ionic equations for single and double replacement reactions
Stoichiometry
 Understand how to calculate: moles, molar mass,
 how to calculate moles of using the liters of a gas using the conversion 22.4L=1mole
 Use mole ratios to calculate moles, grams of reactants and products in a chemical
reaction
 Limiting reagent
 Empirical formul
 Molecular formula
Solutions:


basic terminology – solute, solvent, dilute, concentrated, saturated, unsaturated
8 methods used in class to measure the concentration of a solution – know how to calculate any of the variables in
each of these :
molarity (M) =
molality (m) =
normality (N) =
parts per million (ppm) =
or
parts per billion (ppb)
mass percent (m/m) =
mass/volume percent (m/v) =
volume percent (v/v) =
mole fraction =
 how proof relates to % v/v in an alcoholic beverage
 where and when certain units of concentration are most frequently used
 how to create a solution with a specific molarity in the lab
 use M1V1 = M2V2 to solve problems and to perform a dilution in the lab
 understand what it means to “dilute” a solution
EQUILIBRIUM AND REACTION RATES REVIEW
EQUILIBRIUM
-
Differentiate between an irreversible rxn () and a reversible rxn (↔)
What is chemical equilibrium?
o What are the conditions necessary for it to be achieved?
o How do the two reaction rates compare at equilibrium?
o What chemicals are present in the reaction? (reactants, products, both?)
o What is the difference between static and dynamic equilibrium?
o How does the Keq of a forward rxn mathematically relate to Keq of the reverse rxn?
- Correctly write chemical reactions, Keq, expressions
- Calculate Keq for a rxn when given concentrations
- Use a given Keq value to find the concentration of a substance at equilibrium
- What does the size of Keq mean? What if Keq >, <, or = 1?
- Explain how the concentrations of chemicals change and when they remain constant from the beginning of a rxn
until it reaches equilibrium
- Explain and apply Le Chatelier’s Principle to a system in equilibrium with respect to various stresses
- Predict equilibrium shifts, changes in reactant/product concentrations, and changes to Keq based on Le Chatelier’s
Principle when stresses are applied
- What is ∆H? What does it mean when it is + or -? Endothermic or exothermic? Is heat considered to be a
reactant or product?
REACTION RATES
-
-
What are chemical kinetics?
What is the rate of a chemical rxn? How is it found?
Use graphs, data, stoichiometry and/or balanced chemical equations to calculate rxn rates of individual
reactants/products
Explain how and why temperature, concentration, pressure (for gas), and surface area affect rxn rates – don’t just
simply know that these are the main factors affecting rates
Know other factors that can affect the rate of a rxn, including catalysts, inhibitors, orientation of molecules,
stirring, etc.
What is activation energy?
What things must occur for a rxn to actually happen?
Interpret an activation energy diagram with respect to Ea, ΔH, a catalyst, PE, exothermic vs. endothermic, starting
energy, etc.
What does a catalyst do?
What is an enzyme? Where are they
ACIDS/BASES












Know general properties/characteristics of acids and base
Explain strong vs. weak acids and bases
Know the difference between strong and concentrated acids/bases
Explain the self-ionization of water – be able to write the equation(s) to show it
Use Kw to calculate [H+] or [OH-]
Know the pH, [H+] and [OH-] of a neutral solution
What does pH stand for? What about pOH?
Explain the pH/pOH scale and use them to classify a substance as acid, base, or neutral
Know how the [H+] and [OH-] compare in acidic, basic, and neutral solutions
Can pH and pOH ever be <0 or >14?
Calculate pH, pOH, [H+], [OH-]
What is an indicator?