CHEM 162 - General Chemistry II

CHEM 162 Diagnostic Quiz Study Guide page 1 of 3

CHEM 162: Diagnostic Quiz Study Guide Chapter 1

• Scientific method

• Significant Figures (Sig Figs)

• Scientific notation

• Problem solving by unit analysis method

• Metric system - Know all prefixes from femto to tera - Carry out metric-metric conversions

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

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 theoretical yield

× 100%

CHEM 162 Diagnostic Quiz Study Guide page 2 of 3

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

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 mole-

to-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, acid-

base indicators, titration, endpoint – Solve problems using titration data. – Carry out error analysis (how different kinds of

experimental error will impact experimental results)

CHEM 162 Diagnostic Quiz Study Guide page 3 of 3

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 2

22

1

11 T VP

T VP

= and

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

T; R= Kmol

atmL 0.08206

⋅

⋅ will be given.

– 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

Mole fraction: XA= mixture in moles of # total A of moles of #

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.