Chemistry 120 Study Guide
These review items are intended to focus your study for examinations.  Whereas the exam will focus mainly on the material listed here, these are not to be construed as exam questions.  Any material presented, whether in class, in your reading, homework or labs should be considered fair game.

Chapter 1

  1. Be able to define: accuracy, atom, boiling point, chemical change, chemistry, compound, data, density, element, energy, exact number, fundamental vs. derived measurement, gas, heat, heterogenous matter, homogenous matter, hypothesis, kinetic energy, law, liquid, mass, matter, measurement, melting point, meniscus, mixture, model, molecule, observation, percent error, physical change, potential energy, precision, pure substance, random error (AKA indeterminant error), science, scientific method, scientific notation, SI unit, significant figure, solid, solution, systematic error (AKA determinant error), temperature, theory, uncertainty, unit cancellation (AKA dimensional analysis), volume, weight
  2. Be able to discuss the components of the scientific method and put them into practice.
  3. Be able to accurately perform quantitative measurements given commonly used measuring devices (and use the units).
  4. Know metric and SI units of measurement for each of the measurements used in class.
  5. Know and be able to use the abbreviations for each of the measurements used in class.
  6. Be able to explain the difference between a fundamental and derived measurement.
  7. Know the prefixes and mathematical meanings commonly used with measurements.  For example, "M" in Mm stands for 'mega' meaning 1,000,000 or 106.
  8. Tell the difference between accuracy and precision, either in words or with a small diagram.
  9. Know the difference between a systematic and random error.
  10. Be able to determine the number of significant figures in a measurement.
  11. Be able to accurately use significant figures accurately in calculations.
  12. Be able to identify when something is an exact number (conversion factors will be used as exact numbers)
  13. Be able to convert between English and metric units using dimensional analysis.
  14. Be able to convert any number to or from scientific notation.
  15. Know the difference between mass and weight. (weight is affected by gravity)
  16. Be able to interconvert °C and K measurements.
  17. Be able to work with density. (calculate a density, determine how many mL required to get specified number of grams, etc.)
  18. Use the units of density correctly (a solid is not g/mL, e.g.)
  19. Know the three states of matter and their characteristics. (Solids have a fiixed shape and a fixed volume, but liquids have an indefinite shape and fixed volume, etc.)
  20. Be able to discuss matter in terms of being homogenous vs. heterogenous, a pure substance vs. a mixture, etc.
  21. Know a number of physical separation methods and how and when to use them.
  22. Know the difference between an atom, a compound and a molecule (and later on ion).
  23. Know that a compound is a combination of two or more elements, and the types of formulas used to describe compounds. (Molecular formula, structural formula, and condensed structural formula).
  24. Begin to learn the names, symbols, and a little information about the common elements.  The common elements would be virtually all the main group elements and "some" of the transition elements.
  25. Know the difference between physical and chemical properties, and chemical and physical changes.  For example, "a white, powdery substance" describes a physical property; "metal turns dark on exposure to oxygen gas" is a chemical property.
  26. Given a description of an event, be able to determine whether a physical or chemical change has taken place.  For example, "water melts" describes a physical change; "a piece of metal exposed to the elements turns rusty" is a chemical change.
Chapter 2
  1. Be able to define:  atom, proton, neutron, electron, nucleus, mass number, atomic number, isotope, atomic weight,  group, period, alkali metal, alkaline earth metal, halogen, noble gas, transition element, metal, nonmetal, metalloid, lanthanide, actinide, oxidation state, ion, anion, cation, polyatomic ion.
  2. Be able to discuss Dalton's atomic theory, as well as be able to give examples of how Dalton was incorrect, based on 21st century knowledge.
  3. Be able to explain the law of conservation of matter, law of definite proportions, and law of multiple proportions.
  4. What are the 3 subatomic particles and their properties? (charge, mass, location in atom)
  5. Be able to diagram and explain experiments used to determine the structure of an atom.
  6. Be able to use atomic number, atomic mass and atomic weight.
  7. Be able to name covalent molecules, ionic compounds, and ionic compounds containing polyatomic ions.
  8. Be able to name compounds containing variable charge elements.
  9. Be able name acids.
  10. Know the names, formulas and charges of the most common polyatomic ions.  Also be able to look at a table of polyatomic ions and be able to find the less common polyatomic ions.
  11. Know two types of bonds (ionic and covalent) and when they form (between what elements: ionic form between metal and nonmetal, covalent between two nonmetals).
  12. Be able to correctly determine the formula unit of an ionic compound.
  13. Diagram in detail an atom. Include the names, locations, properties and numbers of all subatomic particles.
  14. Know what isotopes are and how to determine the number of neutrons in an isotope.
  15. Describe the periodic table. Include periods vs. groups, names of groups, metal vs. nonmetal location and properties, properties of groups, why elements are placed where they are.
  16. Be able to predict what oxidation state an atom will develop.
Chapter 3
  1. Be able to define:  stoichiometry, formula weight, molar mass, coefficient, precipitate, supernate, mole, limiting reagent, endothermic reaction, exothermic reaction, heat of reaction, Avagadro's number, percent composition, mole ratio.
  2. Be able to determine the molar mass or formula weight of a compound, given its formula or systematic name.
  3. Be able to calculate an empirical formula from experimental data.
  4. Be able to determine a molecular formula, given empirical formula and experimental data.
  5. Given a chemical equation, be able to describe the reaction in words, and understand what superscripted and subscripted numbers mean.
  6. Be able to develop a chemical equation, given a description of the reaction.
  7. Be able to balance a chemical equation.
  8. Given a chemical equation, determine the limiting reagent.
  9. Given a chemical equation, determine the theoretical yield.
  10. Be able to correctly calculate the percent yield of a reaction if given an actual yield.
Chapter 4
  1. Be able to define:  acid (strong, weak and polyprotic), aqueous, base (strong and weak), dilution, dissociation, electrolyte (strong, weak and non), equivalence point, half-reaction, hydration, indicator, ionization constant, molarity, molecular equation, net ionic equation, neutralization, oxidation, oxidation state, oxidizing agent, precipitate, redox reaction, reducing agent, reduction, solubility, solute, solution, solvent, spectator ion, standard solution, stock solution, titration, total ionic equation.
  2. Be able to explain how to make up a solution, either from solid or liquid components.
  3. Be able to determine whether a chemical species is a solute or a solvent.
  4. Be able to predict whether a compound is soluble in water.
  5. Be able to indicate the ions resulting if a compound dissociates.
  6. Know that if an ionic compound is soluble in water, that it is an electrolyte.
  7. Be able to tell if a compound is a strong-, weak-, or non-electrolyte.
  8. Know the three strong acids (sulfuric, nitric and hydrochloric) and one weak base (ammonia).
  9. Be able to accurately convert names and formulas of acids and bases.
  10. Be able to accurately perform calculations involving molarity of a solution.
  11. Given a description of a chemical reaction, be able to write a molecular equation.
  12. Be able to convert a molecular equation to a total or a net ionic equation.
  13. Be able to accurately perform stochiometric calculations involving molarity.
  14. Be able to balance redox reactions in acidic solution and, to a lesser comfort level, in basic solution.
  15. Be able to determine the oxidation state of atoms in compounds.
  16. Be able to indicate the common oxidation state of predictable elements.
Chapter 5
  1. Be able to define:  absolute zero, Avagadro's law, combined gas law, Dalton's law of partial pressure, diffusion, effusion, gas, ideal gas, ideal gas law, kinetic molecular theory (KMT), molar volume, pressure, real gas, root mean square (velocity), STP, temperature, torr, universal gas constant, and volume.
  2. Be able to interconvert units of pressure (mm Hg, torr, Pa).  Remember 760 mm Hg=760 torr=1 atm.
  3. Know the combined gas law and the ideal gas law.
  4. Be able to utilize Avagadro's law and Dalton's law of partial pressure.
  5. Be able to discuss and explain the postulates of the kinetic molecular theory (KMT).
  6. Be able to discuss why a gas might behave as "real" instead of "ideal."
  7. Be able to calculate the root mean square velocity of a gas.
  8. Be able to calculate and compare rates of diffusion (and effusion) of gases.
Chapter 6
  1. Be able to define:  endothermic, extensive property, exothermic, heat, intensive property, kinetic energy, potential energy, state function, surroundings, systen, temperature, and work
  2. Be able to accurately calculate the kinetic energy of a particle.
  3. Be able to distinguish whether a reaction is exothermic or endothermic.
  4. Be able to accurately perform calculations involving calorimetry.
  5. Be able to accurately calculate enthalpies using Hess's law.
  6. Be able to accurately calculate standard enthalpy of formation.
Chapter 7 and 8
  1. Be able to define:  continuous vs. discontinuous spectrum, electromagnetic radiation, electronegativity, excited state, frequency, ionization energy, ground state, group vs. period, orbital, valence electron, and wavelength
  2. Be able to interconvert wavelength, frequency, and speed.
  3. Be able to calculate the amount of energy involved in electron transitions.
  4. Be able to determine quantum numbers for elements.
  5. List the electron configuration of commonly encountered elements.
  6. Be able to describe periodic trends for electron affinity, ionization energy, electronegativity, size, melting point, boiling point; and be able to rank elements according to those properties.
  7. Be able to name groups of the periodic table (including metal, nonmetal, metalloid, transition elements, etc.)
  8. Be able to predict, based on periodic table placement, things such as valence electrons, oxidation state, bonds formed, etc.
Chapter 9
  1. Be able to define:  bond energy, coordinate covalent bond, covalent bond, dipole moment, double bond, formula unit, ionic bond, isoelectronic ion, nonpolar covalent bond, polar covalent bond, resonance structure, and VSEPR
  2. Be able to determine the type of bond formed between elements.
  3. Be able to determine the formula unit of ionic compounds.
  4. Be able to rank ions by size.
  5. Be able to determine dipole moments, given elements and table of electronegativities.
  6. Be able to draw Lewis dot structures of simple compounds and polyatomic ions and use them to determine shape.
  7. Know that there are exceptions to the octet rule and be able to list and explain several of them.
  8. Be able to draw resonance structures of molecules and discuss how they relate to actual molecular structure.
  9. Be able to accurately calculate formal charge of molecules.
  10. Be able to accurately calculate energy changes in a reaction using bond enthalpies.
  11. Be able to state whether molecules are polar, given elements and table of electronegativities.
Chapter 10
  1. Be able to define:  antibonding MO, atomic orbital, bonding MO, delocalized electron, diamagnetic, heteronuclear molecule, hybrid atomic orbital, localized electron model, molecular orbital, paramagnetic, pi bond, and sigma bond.
  2. Be able to distinguish between, sp3, sp2, sp, sp3d, and sp3d2 hybridized atomic orbitals
  3. Understand and be able to explain why hybridization is required to explain properties of molecules such as bond length.
  4. Be able to distinguish between a sigma and a pi bond and explain electron locations in each.
  5. Be able to explain what orbitals have to be hybridized to get correct molecular shape and number of bonds (four equivalent bonds = sp3, e.g.)
  6. Understand bonding orbital (sigma) represents addition of wave function, and antibonding (sigma*) represents subtraction of wave function.
  7. Be able to predict the location of electrons in orbitals of simple compounds or ions using the "localized electron model"
  8. Be able to draw Lewis dot structures of simple compounds and polyatomic ions and use them to determine shape.
  9. Be able to calculate bond order and predict the likelyhood of molecule formation.
  10. Comprehend the concept of electron delocalization (remember that pi electrons must be teated as delocalized).
  11. Be able to predict whether an atom will be paramagnetic or diamagnetic.
Chapter 11
  1. Be able to define:  alloy, amorphous vs. crystalline solid, condensation, critical point, critical pressure, critical temperature, dipole-dipole interaction, enthalpy of fusion, enthalpy of vaporization, hydrogen bond, intermolecular force, lattice, London force, normal boiling point, specific heat, sublimation, superheated, unit cell, vapor pressure, vaporization.
  2. Be able to determine which intermolecular forces are expected for a chemical species.
  3. Be able to explain the three intermolecular forces:  what causes them, how strong are they, what type of species exhibit them, etc.
  4. Be able to rank compounds according to their melting point, etc.
  5. Be able to diagram a temperature-energy diagram, given experimental data.
  6. Be able to label a temperature-energy diagram.
  7. Be able to relate properties of matter (vapor pressure, e.g.) to intermolecular forces.
  8. Be able to explain why some liquids exhibit properties such as surface tension.
  9. Be able to use a phase diagram to determine, under some set of conditions, whether a substance is gas, liquid or solid.  Be able to identify points (critical temperature, e.g.) on the phase diagram.
  10. Be familiar with the types of crystals discussed in class.  For example, given a picture of a unit cell, you should be able to say whether it is simple cubic, face-centered cubic, or body-centered cubic.
  11. Be able to calculate the number of atoms present in a unit cell..
  12. Be able to calculate density based on crystal size and type of packing (or vice versa).
Chapter 12
  1. Be able to define:  colligative properties, colloid, enthalpy of solution, hydrophilic, hydrophobic, isotonic, molarity, osmosis, osmotic pressure, semipermeable membrane, solubility, solute, solution, solvent, suspension, and Tyndall effect
  2. Be able to accurately calculate the concentration of solutions using molarity, normality, molality, percent solution or mol fraction.
  3. Be able to predict whether or not a solute will be soluble in a solvent.
  4. Be able to list several factors affecting solubiltiy and relate the observations to the KMT.
  5. Be able to perform calculations using Raoult's law (P° as a constant would be given).
  6. Be able to perform calculations involving colligative properties to determine actual melting point and boiling point, molar mass of compounds,  dissociation, and so on.
  7. Be able to explain processes like dialysis.
  8. Know what a colloidal solution is, why it scatters light, and be able to give several examples.

Please send your comments and suggestions to: twiese@fhsu.edu