CHEM 162: Diagnostic Quiz Study Guide
Chapter 1
• Scientific method
• Problem solving by unit analysis method
• Significant Figures (Sig Figs)
• Metric system
- Know all prefixes from femto to tera
- Carry out metric-metric conversions
• Scientific notation
Chapter 2
• Metals, nonmetals, and semimetals:
- Location on Periodic Table and properties
• Know which elements are solids, liquids, gases
at room temperature (25˚C)
• Know which elements exist as diatomic
molecules at 25˚C (H2, N2, O2, F2, Cl2, Br2, I2)
• molecule: compound of 2 or more nonmetals
held together by covalent bonds
• ionic compound: consists of metal + nonmetal(s)
– formula unit indicates ratio of ions present
• Know the names and symbols of the first 18
elements of the Periodic Table, all elements on
Fig. 2.22 on p. 61, Ti, and U. Correct spelling of
element names counts!
KNOW all of names and symbols for the
POLYATOMIC IONS
Nomenclature:
– Identify a compound as ionic or molecular
– Given formula of a compound, determine name.
– Given name of a compound, determine formula.
Molecule or Molecular Compounds: all nonmetals
– Use Greek prefixes when more than one
– Know ammonia, methane, hydrogen peroxide
Ionic Compounds: metal + nonmetal(s) ions
– cation(s) and anion(s) with overall charge of zero
– Determine the charges on Main-Group elements
using the Periodic Table
– Use charges on anions to determine charges on
metals that can multiple charges.
– have high melting points, all solids at 25˚C
Acids: Have H in front, physical state is (aq)
– Be able to name acids given the formula or
determine the formula given the name.
Chapter 3
Balance Chemical Equations
Stoichiometry: Calculations involving amounts of
reactants and products in a chemical reaction
– coefficients in balanced chemical equation give
mole-to-mole ratios of reactants and products
– Solve mass-mass stoichiometry problems
Limiting Reagent Problems
– Calculate the amount of product made given
amount of reactants and chemical equation
– Reactant producing smallest = limiting reagent
– All other reactants = in excess
CHEM 162 Diagnostic Quiz Study Guide
Be able to calculate the amount of reactant in
excess that remains after the reaction
Yields of Reactions
theoretical yield: amount of product predicted by
balanced equation when limiting reagent is used up
actual yield: amount of product one actually gets
Percent yield =
actual yield
× 100%
theoretical yield
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Chapter 4
Aqueous Solutions: liquid or solid solute in H2O
– solution: mixture of 2 or more substances
– solute: substance present in smaller amount
– solvent: substance present in larger amount
Predict products of a reaction given reactants for
• Precipitation Reactions
– precipitate (ppt): solid forming from 2 solutions
• Acid-Base Neutralization Reactions
– HX + MOH → water + salt
– HX + MHCO3 → water + CO2 + salt
– HX + MCO3 → water + CO2 + salt
• Oxidation-Reduction (Redox) Reactions
– Combination reaction
– metal + nonmetal → ionic cmpd (s)
– Single-replacement reactions
– Given Activity Series
– solid metal + metal solution
– solid metal + acid
– active metal + H2O (l)
– Combustion reaction
– CxHy + O2 → CO2 (g) + H2O (g)
– CxHyOz + O2 → CO2 (g) + H2O (g)
Know Arrhenius and Brønsted-Lowry (B-L)
definitions for acids and bases
Electrolyte: substance that dissolves in water to
produce ions that conduct electricity
– strong electrolyte: breaks up completely
→ many ions present to conduct electricity
– e.g. strong acids & bases, aqueous salts
– weak electrolyte: breaks up to small degree
→ only a few ions present to conduct
electricity
– e.g. weak acids & bases, insoluble salts
– nonelectrolyte: a molecular compound that
forms molecules in water (e.g sugar)
→ no ions → does not conduct electricity
Acids and Bases as electrolytes
– Know strong acids and strong bases!
– All other acids and bases are weak
– Recognize strong acids and bases ionize
completely while weak acids and bases don’t
CHEM 162 Diagnostic Quiz Study Guide
Chemical Equations and (Net) Ionic Equations
– Chemical Equation: compounds shown intact
– Complete/Total Ionic Equation:
– shows strong electrolytes as ions
– Spectator Ions: unchanged in reaction
– Net Ionic Equation: Shows substances that
change in a chemical reaction
Guidelines for writing Net Ionic Equations:
1. Complete and balance molecular/chem
equation
2. Leave solids, liquids, gases, weak electrolytes
as compounds; break up strong electrolytes
3. Cancel spectator ions
4. Simplify coefficients if possible
5. If all reactants and products cancel
(all spectator ions) → NR
Oxidation-Reduction (Redox) Reactions
– Be able to determine oxidation numbers for all
the atoms/elements in a chemical equation.
– Use oxidation numbers to determine which
reactant was oxidized (reducing agent) and
which reactant was reduced (oxidizing agent)
– Determine the # of electrons gained or lost.
Molarity, Solution Stoichiometry, Mass Percent
Concentration, and Volumetric Analysis
– Use molarity and volume to solve for moles
– Use chemical equation given to determine moleto-mole ratios needed to solve problems
– Solve a variety of problems combining molarity,
mass percent concentration, and topics covered
from previous chapters.
Acid-Base Titrations
– Know the definitions for standard solution, acidbase indicators, titration, endpoint
– Solve problems using titration data.
– Carry out error analysis (how different kinds of
experimental error will impact experimental
results)
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Chapter 6: Gases
Know the physical properties of gases
Gas pressure and Atmospheric pressure
– Standard atmospheric pressure: 760 torr at 0˚C
– Convert between units of pressure:
1 atm ≡ 760 torr ≡ 760 mmHg
Know how a manometer is used to measure gas
pressure for open systems (p. 2 of lecture notes).
Solve for a variety of problems involving gases
– Given 2 sets of conditions, use
P1V1
P V
= 2 2 and
T1
T2
cancel variables that stay the same to simplify,
and temperature must be in Kelvins
– Use ideal gas law (PV=nRT) to solve for P, V, n, or
0.08206 L ⋅ atm
T; R=
will be given.
mol ⋅ K
– Recognize that STP is standard temperature and
pressure, defined at 0.00˚C and 1.00 atm.
Dalton’s Law of Partial Pressure:
– Use Dalton’s Law (Ptotal = P1 + P2 + P3 + …) to solve
for total pressure or the partial pressure of
one gas in a mixture
# of moles of A
Mole fraction: XA=
total # of moles in mixture
Partial pressure (PA): PA = XA Ptotal
– Solve for mole fraction, total pressure, or
partial pressure given other variables
Kinetic Theory of an Ideal Gas
– Know the kinetic theory of gases regarding
particle volume, particle motion, attraction,
collisions, and the average kinetic energy of each
particle being proportional to the temperature.
YOU WILL BE GIVEN A PERIODIC TABLE WITH ELEMENT SYMBOLS, ATOMIC
NUMBERS, AND ATOMIC MASSES, ALL RELEVANT CONSTANTS, THE SOLUBILITY
RULES, AND THE ACTIVITY SERIES.
YOU WILL NEED A BASIC SCIENTIFIC CALCULATOR TO COMPLETE THE QUIZ.
CHEM 162 Diagnostic Quiz Study Guide
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