Chemistry Final Exam Study Guide 2014
Semester 2 topics: Chapter 10 Mole Relationships, chapter 11 Chemical Rxns (skip 11.3), chapter
12 Stoich, 13.1 and 14 on Gases, 15 on Thermochemistry, parts of chapter 19 on Acids and
Bases, and parts of chapter 16 on dilutions.
All of the math rules that we’ve used all year will be applied in the final exam. All other semester 1
material will be tested to a total of 30% of the exam. You can locate and download the semester
exam chemistry review guide from the website if you want to review semester 1 topics.
The exam will be in the typical format: multiple choice with a calculations and problem solving
segment.
Section 10.1 – The Mole: A Measurement of Matter
 Know how to use Avogadro’s Number** (6.02 x 1023) and know how it relates to a mole of
any substance
 Know that the mole can be used to determine the number of particles, the mass, or the
volume of an element or compound.
 Understand the meaning of a representative particle and be able to determine what the
representative particle would be for a particular substance (moles, atoms, molecules…)
 Be able to convert between representative particles and moles. Know what conversion
factor to use!
Section 10.2 – Mole-Mass and Mole-Volume Relationships
 Know the definition of molar mass, and be able to determine the molar mass of an atom or
compound using the periodic table.
 Be able to use molar mass to convert between the mass in grams of a substance and
moles of a substance
 Know the conditions for STP (Standard Temperature and Pressure)
 Know the relationship between moles of a gas and volume of a gas at STP
o 1 mol gas at STP** = 22.4 L of gas
 Be able to convert between density of a gas and molar mass of a gas at STP
 Know how to convert between representative particles, mass, and volume of a gas at STP
using the Mole Map. Know how to set up these conversion factors and perform
calculations (ex. Find the mass in grams of a certain volume of a gas at STP)
Section 10.3 – Percent Composition and Chemical Formulas
 Know the definition of percent composition
 Be able to calculate the percent composition for each element in a compound given the
masses of each element in the compound
 Be able to calculate the percent composition for each element in a compound based on the
molar mass of that compound (given the name or the formula)
 Be able to use percent composition as a conversion factor for calculating the mass of a
particular element present in a given mass of a compound.
o Remember: 76.8% C is the same as saying 76.8 g of C / 100.0 g of Compound
 Know the definition of an empirical formula
 Know that the empirical formula may or may not be the same as the molecular formula
 Be able to identify a formula as the empirical or molecular formula of a compound.



Be able to determine the empirical formula of a compound from the percent compositions of
each element (percent to mass, mass to mole, divide by small, multiply ‘til whole)
Be able to find the molecular formula given the empirical formula and the molar mass of a
compound.
Know the meaning of “efm”
** you will be given Avogadro’s number and the volume of gas at STP value (22.4 L/mol) on the
test
Chapter 11 Vocabulary
Word Equation
Skeleton Equation
Balanced Equation
Aqueous solution
Catalyst
Coefficient
Soluble
Insoluble
Precipitate
Complete Ionic Equation
Spectator Ions
Net Ionic Equation
11.1 – Describing Chemical Change
 Know the general structure of a chemical reaction (reactants  products)
 Know what takes place during a chemical reaction (bonds broken, formed, atoms rearranged)
 Be able to write word equations, skeleton equations, and balanced equations
 Know how to distinguish the state of the reaction materials in an equation (s) (l) (g) (aq)
 Know the meaning of an aqueous (aq) solution
 Know the purpose of a catalyst and how you would represent a catalyst in a chemical equation
 Be able to represent the addition of heat in a chemical equation
 Be able to write the equation for a reversible reaction
 Be able to balance equations using coefficients (remember that we don’t write the coefficient 1)
 Be able to write and balance a chemical equation from a written description of a reaction.
11.2 – Types of Chemical Reactions
 Know the difference between the 5 different types of chemical reactions discussed in class
(combination, decomposition, single replacement, double replacement, combustion)
 Be able to determine the products of a reaction given the reactants (this requires determining
which type of reaction will most likely take place)
 Be able to determine the reactants of a reaction given the products
 Be able to determine the products of a single-replacement reaction given the Activity Series of
Metals (also be able to determine when no reaction would take place)
 Know the three most likely types of products of a double-replacement reaction (also known as
the driving forces of a double-replacement reaction)
 Be able to write and balance the equation for the combustion of a given hydrocarbon.
Chapter 12 Vocabulary:
Stoichiometry
Mole Ratio
Limiting Reagent
Excess Reagent
Actual Yield
Theoretical Yield
Percent Yield
Review:
Law of Conservation of Mass
Balancing Equations
Molar Mass (mass moles, molesmass)
1 mole of gas at STP = 22.4L (moles  volume, volume moles)
1 mol = 6.02 x 1023 representative particles (atoms, molecules, formula units…) (particles
moles, moles
particles)
12.1 – The Arithmetic of equations
 Know the meaning of stoichiometry and how it involves balanced equations
 Be able to interpret a balanced chemical equation in terms of mass, volume, number of moles
and number of particles.
 Know that number of atoms and mass of reactants are conserved in a chemical reaction, but
that moles, volume, and number of representative particles are not necessarily conserved and
be able to explain what this means.
12.2 – Chemical Calculations
 Know how to form a mole ratio using the coefficients of a balanced equation
 Be able to use the mole ratio to convert between moles of one substance and moles of another
substance in a chemical reaction
 Be able to use molar masses and mole ratios to convert between grams of one substance and
grams of another substance in a chemical reaction (mass  moles moles  mass)
 Be able to use the mole ratio to convert between liters of one substance and liters of another
substance in a chemical equation
12.3 – Limiting Reagent and Percent Yield
 Know the meanings of the terms: Limiting Reagent and Excess Reagent
 Be able to determine the limiting and excess reagents based off of calculations from the given
amounts of available reactants.
 Know how to use the amount of limiting reagent available to calculate the theoretical yield of
product produced.
 Be able to calculate the percent yield given the actual yield and the calculated theoretical yield
 Know that the actual yield is determined experimentally, and the theoretical yield is determined
through calculations.
 Important: If you are given the amounts of multiple reactants, you MUST first determine the
limiting reagent and use only that value to determine the amount of product produced.
 Be able to explain what would make the % yield less than 100%, and what would make it more
than 100%.
 Be able to perform limiting reagent and percent yield calculations given lab data similar to what
you did in the Limiting Reagent and Percent Yield lab.
Gases Vocabulary
Kinetic Energy
Temperature
Kinetic Theory
Compressibility
Gas Pressure
Atmospheric Pressure
Ideal Gas
Partial Pressure
Equations to know: You will be given the pressure conversions, temperature conversions, R
values, and Combined Gas Law and Ideal Gas Law
1 atm = 101.3 kPa
K = Co + 273
Ideal Gas Law: PV = nRT
R = 8.31 (L•kPa)/(mol•K)
R = 0.0821 (L•atm)/(mol•K)
Dalton’s Law of Partial Pressure: Ptotal = P1+ P2
+ P3+…
Properties of Gases
Factors Affecting Gas Pressure
 Know the meaning of kinetic energy and how it is related to temperature
 Be able to explain what takes place on a molecular/atomic level at absolute zero
 Know how Kinetic Theory is used to explain the differences between solids, liquids, and gases
 Know the 3 major assumptions of Kinetic Theory
 Be able to explain why gases have a high level of compressibility
 Know the 4 variables used to explain gas behavior (P,V,T,n) and the units for each
 Know how 1 atm is defined and the connection between mmHg and a barometer.
 Be able to convert between atm and kPa
 Be able to explain how changes in the amount of gas, temperature, and volume will affect gas
pressure
 Know that gas always moves from regions of higher pressure to lower pressure
The Gas Laws
 Be able to explain the Pressure-Volume Relationship using Boyle’s Law and be able to
perform calculations involving pressure and volume with constant temperature
 Be able to explain the Temperature-Volume Relationship using Charles’ Law and be able to
perform calculations involving temperature and volume with constant pressure
 Be able to explain the Temperature-Pressure Relationship using Gay-Lussac’s Law and be
able to perform calculations involving temperature and pressure with constant volume
 Know how to use the combined gas law to perform calculations
 Remember that all equations involving temperature MUST have record in units of Kelvin (not
oC)
Ideal Gases
Gas Molecules: Mixtures and Movement
 Know how and when to use the ideal gas law
 Know under what conditions gases tend NOT to act as an ideal gas
 Be able to perform calculations involving the relationship between number of gas particles at
STP and volume
 Be able to convert between volume, number of moles, mass, and molecules (involves molar
mass and Avogadro’s number)
 Know the meaning of partial pressure and how to use Dalton’s Law of Partial Pressure to
calculate the total pressure, or the partial pressure of one of the component gases
Thermochemistry Chapter 17
I. Vocabulary
Be familiar with the following terms so that you can recognize and use them when they appear in
questions or directions for solving problems.
State/phase (of matter)
Potential energy (in chemistry)
Kinetic energy (in chemistry)
Energy
Heat
Temperature
System/Surroundings/Universe
Endothermic reaction
Exothermic reaction
calorie (lowercase “c”)
Joule
Heat capacity
Specific heat
Calorimetry
Calorimeter
Enthalpy
Thermochemical equations
Heat of reaction
Heat of combustion (simply the heat of reaction for a combustion reaction)
Heat of reaction (Hrxn)
Hess’s Law
II. Formulas
You do not have to memorize these formulas, just know how to use them. They will be part of a data
bank on the assessment.
H = q = mCT (m is grams)
H = nHfus (for solidliquid) and H = nHvap (for liquid  gas) where n = moles
qsystem = -qsurroundings and vice-versa
III. Major concepts
17.1 Thermochemistry: The Flow of Energy (Intro to Thermochem)
 Vocabulary
 What is potential and kinetic energy in terms of chemical bonds and temperature?
 Heat vs. Temperature
 Identifying thermochemical “points of view” ex) is a reaction or flow of heat endo or exothermic
if you define the system as x?
 Heat capacity vs. specific heat
 Know that specific heats are available in reference charts and are not meant to be memorized
 Heat capacity depends on mass and chemical composition
 What does it mean about a substance if it has a high specific heat? A low specific heat?

Be able to calculate heat change (enthalpy change) in a substance that does NOT change
states using the q = mCT formula. Be able to solve for any of the variables if given the other
three.
17.2 Measuring and Expressing Enthalpy Changes
 Vocabulary
 Know how a calorimeter works (the kind we used in our lab; the system is the chemical
reaction between the chemicals and the surroundings for which you are measuring H are
equal and opposite (signs) to the system H)
 Sign of H if reaction is endothermic and sign of H if reaction is exothermic
 Use thermochemical equations to calculate the H for the formation or decomposition of
particular substances.
17.4 Hess’s Law and Standard Heat of Formation
 Vocabulary
 Be able to use Hess’s Law and various thermochemical equations to determine the Hrxn for
any reaction
Acid/Base and Solutions (parts of chapters 16-19)
Vocabulary
Neutralization Reaction: When you combine and acid and a base, you neutralize them. This
makes the pH neutral. Your products are water and a SALT. A salt for example would be NaCl, or
KI, or CaBr2, etc. These reactions are DRs and are always exothermic.










Know the Arrenius and Bronsted-Lowry definitions of acids and bases
Be able to name the conjugate acid of a base, and the conjugate base of an acid.
Be able to identify conjugate pairs in a reaction.
Be able to distinguish acids and bases from one another in a reaction.
Know where acids, bases, and neutral solutions lie on the pH scale.
o Acids are < 7
o Bases are > 7
o Neutral solutions are 7.
Know what happens when a strong acid and strong base are combined
o They NEUTRALIZE each other. See above.
Know the definition of a salt and be able to recognize the salt produced in a neutralization
reaction. See above.
o Example) HCl + NaOH  H2O + NaCl
Be able to calculate dilutions from stock solutions using M1V1 = M2V2
Be able to identify an acid as monoprotic, diprotic, or triprotic, and be able to tell what that
means about the acid.
Be able to calculate the concentration of an unknown acid from acid/base titration data for a
monoprotic acid (MacidVacid = MbaseVbase)