StudyGuide

Chem 127 - Final Exam Study Guide

You should know how to do each of the following, and be familiar with each of the listed terms:

Chapter 1: The Foundations of Chemistry

Report an answer to a calculation with the proper number of significant figures
Perform calculations using dimensional analysis (factor-label method)
Use SI/metric prefixes
Perform calculations involving densities and percentages
Recognize the postulates of Dalton’s atomic theory
TERMS: atom, atomic number, chemical change, compound, conversion factor, density, element, energy, mass, matter, molecule, physical change, significant figures, SI units, SI derived units, temperature

Chapter 2: Chemical Formulas and Composition Stoichiometry

Identify molecular compounds and ionic compounds
Calculate formula mass and molecular mass
Perform conversions between mass, moles, and number of atoms/molecules
Perform calculations with percent composition, empirical formulas, and combustion analysis
TERMS: anion, amu, cation, empirical formula, formula weight, ion, ionic compound, molar mass, mole, molecular formula, molecular weight, polyatomic ion

Chapter 3: Chemical Equations and Reaction Stoichiometry

Balance chemical equations
Use stoichiometry to calculate the mass of reactant needed or the mass of product produced in a reaction
Recognize a limiting reactant and how it determines the amount of product that can be made
Calculate a theoretical yield and a percent yield from a reaction
Calculate concentrations (molarity) of species in solution
Perform stoichiometric calculations using concentrations of reactants and products
Determine the concentration of a chemical species in a solution prepared from the dilution of a more concentrated solution
TERMS: actual yield, aqueous solution, concentration, dilution, limiting reactant, molarity, percent yield, products, reactants, solute, solution, solvent, theoretical yield

Chapter 4: Some Types of Chemical Reactions

Classify an element according to its position on the periodic table
Name molecular and ionic compounds
Identify an ionic compound as soluble or insoluble
Identify and predict the products of a precipitation reaction
Write the net ionic equation and identify the spectator ions for a reaction in aqueous solution
Identify a chemical compound as a strong, weak, or non-electrolyte
Identify a chemical compound as a strong acid, weak acid, strong base, or weak base
Identify and predict the products of an acid/base reaction
Assign an oxidation number to an element in a compound
Identify a redox reaction, as well as the oxidizing and reducing agents in the reaction
TERMS: acid, alkali metals, alkaline earth metals, base, binary compound, dissociation, electrolyte, group (family), halogens, ionization, metal, metalloids, metathesis reaction, net ionic equation, neutralization reaction, noble gases, nonmetals, oxidation, oxidation number, oxidizing agent, period, periodic table, precipitate, precipitation reaction, redox reaction, reducing agent, reduction, salt, semiconductor, spectator ions, strong acid, strong base, total ionic equation, weak acid, weak base

Chapter 5: The Structure of Atoms

Give the number of protons, neutrons, and electrons in an atom of an isotope
Calculate atomic weight given the percent natural abundance of the isotopes of an element
Calculate frequencies and wavelengths of light waves
Calculate energies of photons
Calculate wavelengths of emitted photons from the hydrogen atom in the Bohr model of the atom
Draw shapes of s, p, and d orbitals
Describe an orbital with an acceptable combination of three quantum numbers
Determine whether an atom is diamagnetic or paramagnetic
Assign a reasonable set of four quantum numbers to any electron in an atom
Write electron configurations of atoms
TERMS: angular momentum quantum number, canal ray, cathode ray, continuous spectrum, diamagnetism, electromagnetic radiation, electron, electron configuration, excited state, frequency, ground state, Heisenberg Uncertainty Principle, isotopes, line spectrum, magnetic quantum number, neutron, nucleus, nuclide symbol, orbital, paramagnetism, period, photoelectric effect, photon, principal quantum number, proton, quantum, quantum numbers, spin quantum number, wavelength

Chapter 6: Chemical Periodicity

Predict trends in atomic and ionic size, ionization energies, electronegativities, and electron affinities
TERMS: effective nuclear charge, electron affinity, electronegativity, ionization energy, isoelectronic, noble gas configuration, shielding

Chapter 7: Chemical Bonding

Determine how electrons are transferred to make ionic bonds
Determine how electrons are shared to make covalent bonds
Draw Lewis structures of molecules
Calculate formal charges for each atom in a Lewis structure and use formal charges to determine the favored Lewis structure
Draw all important resonance structures for a molecule
Determine bond order
Determine whether or not a bond is polar
TERMS: bond dissociation energy, bonding pair, covalent bond, dipole moment, double bond, formal charge, Lewis formula, lone pair, nonpolar bond, octet rule, polar bond, resonance, single bond, triple bond, valence electrons

Chapter 8: Molecular Structure and Covalent Bonding Theories

Use VSEPR theory to predict the shapes of molecules
Determine whether or not a molecule is polar
Use valence bond theory to determine the hybridization of atoms in molecules
Use valence bond theory to determine which orbitals are overlapping to make covalent bonds in molecules
Use valence bond theory to explain how double and triple bonds form
TERMS: hybridization, pi bond, sigma bond, valence bond theory, valence shell electron pair repulsion (VSEPR) theory

Chapter 13: Liquids and Solids

Identify the types of intermolecular forces present in a given liquid
Describe how intermolecular forces affect viscosity, surface tension, capillary action, evaporation, vapor pressure, and boiling point of a liquid
Correctly interpret phase diagrams
TERMS: critical point, critical pressure, critical temperature, dipole-dipole interactions, dipole-induced dipole interactions, dispersion forces, dynamic equilibrium, hydrogen bond, LeChatelier’s Principle, London forces, phase diagram, polarizability, supercritical fluid, triple point, volatility

Chapter 10: Reactions in Aqueous Solution I: Acids, Bases, and Salts

Classify acids and bases according to the Arrhenius, Bronsted-Lowry, and Lewis definitions
Identify conjugate acid/base pairs
Determine relative acid strength based on Lewis structure
Write balanced acid-base reactions
TERMS: acid, amphiprotism, autoionization, base, leveling effect

Chapter 11: Reactions in Aqueous Solution II: Calculations

Correctly balance a redox reaction in acid or base solution
Perform calculations based on acid-base and redox titrations
TERMS: buret, equivalence point, half-reaction, indicator,

Chapter 12: Gases and the Kinetic-Molecular Theory

Use the ideal gas law to calculate pressure, volume, temperature, and moles of ideal gases
Calculate partial pressures of each gas in a mixture of gases
Use the ideal gas law in reaction stoichiometry problems
Identify the basis assumptions of the kinetic molecular theory
Understand the factors that affect the rates of diffusion and effusion
Understand the differences between ideal gases and real gases
TERMS: atm, bar, barometer, diffusion, effusion, ideal gas, manometer, mole fraction, partial pressure, pressure, root-mean-square speed, STP, torr, van der Waals equation

Chapter 14: Solutions

Express solute concentration in molarity, molality, and mole fraction
Understand the factors that affect miscibility and solubility
Understand how solution concentration affects each of the following colligative properties: vapor pressure, boiling point, freezing point, and osmotic pressure
Calculate molecular weights by freezing point depression and boiling point elevation
Understand how temperature affects the solubility of a solid, liquid, or gas
TERMS: colligative properties, ideal solution, miscibility, molality, osmosis, osmotic pressure, Raoult’s Law, reverse osmosis, saturated solution, supersaturated solution