Honors Chemistry – Final Exam Review

Chapter 3: Atoms: The Building Blocks of Matter

Define the following terms:

atom, atomic number, isotopes, mass number, atomic mass unit, average atomic mass, mole, molar mass

Essential questions and content:

  • State Dalton’s Atomic Theory
  • Explain the relationship between Dalton’s Theory and the Laws of Conservation of Mass, Definite Proportion, and Multiple Proportions.
  • Describe the properties of cathode rays that led to the discovery of the electron.
  • Describe the contributions that Thomson made to atomic theory.
  • Describe Rutherford’s gold foil experiment and its contribution to atomic theory.
  • Determine the number of protons, neutrons, and electrons in an atom.
  • Identify an isotope.
  • Distinguish between atomic mass and atomic number.
  • Explain how counting can be done my weighing.
  • Identify a mole in terms of Avogadro’s number of particles
  • Determine the molar mass of an element or a compound.
  • Calculate the number of moles, mass, or the number of particles of a sample given appropriate data.

Chapter 22: Nuclear Chemistry

Define the following terms:

Nucleons, nuclide, mass defect, nuclear binding energy, transmutation, band of stability, radioactive decay, alpha particle, beta particle, positron, gamma rays, half-life, decay series, chain reaction

Essential questions and content:

  • Identify a nuclide by atomic number and atomic mass.
  • Relate nuclear stability to the ratio of neutrons to protons.
  • Describe the forms of radioactive decay.
  • Balance Decay Equations
  • Determine the half-life of an isotope or the fraction of the isotope that remains given appropriate data
  • Explain the source of energy in nuclear reactions.
  • Differentiate between nuclear fission and fusion.

Chapter 4: Arrangement of Electrons in Atoms

Define the following terms:

wavelength, frequency, amplitude, electromagnetic spectrum, photoelectric effect, photon, ground state, excited state, Heisenberg uncertainty principle, atomic orbital, quantum number, principle quantum number, angular momemtum quantum number, magnetic quantum number, spin quantum number, Aufbau Principle

Essential questions and content:

  • Identify the major regions of the electromagnetic spectrum
  • Explain the mathematical relationship between wavelength, frequency, and energy of light
  • Discuss the dual wave-particle nature of light
  • Distinguish between a continuous spectrum and line spectrum.
  • Explain how atoms emit light energy.
  • Describe the Bohr model of the hydrogen atom
  • Explain how bright line spectra demonstrates the quantized nature of light energy and provide evidence for the Bohr model.
  • List the four quantum designations in the modern model of the atom and describe their significance.
  • Use quantum designations to determine the distance away from the nucleus, the shape of the orbital, the orientation, and the spin of the electron.
  • Determine the number of electrons that can be located in each energy level and sublevel.
  • Define the Pauli Exclusion Principle.
  • Write the electron configuration of an atom in the ground state.
  • Using Hund’s Rule, construct an orbital diagram for an atom.
  • Distinguish between valence and core electrons in the configuration of an atom.
  • Write the electron configuration using the noble gas notation.
  • Relate the configuration of an element to its position on the periodic table.

Chapter 5: Periodic Law

Define the following terms:

periodicity, atomic number, periodic law, main group elements, atomic radius, ionization energy, electron affinity, valence electrons, Electronegativity, lanthanides, actinides, alkali metals, alkaline-earth metals, transition elements, halogens

Essential questions and content:

  • Explain the role of Mendeleev in the development of the periodic table.
  • Describe the organization of the modern periodic table.
  • Describe how elements belonging to a group or period are related in terms of the number of valence electrons or energy level that is being filled.
  • Locate and describe the general properties of the alkali metals, the alkaline earth metals, the transition metals, the halogens, and noble gases.
  • Define ionization energy, electron affinity, and electronegativity.
  • Describe and explain the trend in atomic radii, ionization energy, metallic character, and electronegativity within a group or period on the periodic table.
  • Describe the differences in chemical behavior of elements as one proceeds across a period or down a group.
  • List and compare the properties of metals, metalloids, and nonmetals.
  • Predict the charges on ions from the location on the periodic table.

Chapter 2: Measurements and Calculations

Define the following terms:

hypothesis, model, theory, accuracy, precision

Essential questions and content:

  • Know the safety rules for the chemical laboratory
  • Know the location and use of the safety equipment in the laboratory
  • Describe the difference between observation, hypothesis, and theory
  • Use the scientific method to solve a problem.
  • Identify both SI base and derived units of measurement.
  • Use scientific notation
  • Explain the cause of uncertainty in measurements.
  • Use the proper technique for measuring.
  • Use significant figures in all calculations.
  • Convert between metric units.
  • Use dimensional analysis in calculations.
  • Distinguish between accuracy and precision
  • Calculate percent error

Chapter 6: Chemical Bonding

Define the following terms:

chemical bond, ionic bonding, covalent bonding, nonpolar and polar covalent bonds, bond length, bond energy, lattice energy, ionic compound, formula unit, crystal lattice, delocalized electrons, metallic bonding, hybridization, intermolecular forces, molecule, molecular compound, octet rule, unshared pair, single bond, double bond, triple bond, resonance, malleability, ductility, VSEPR theory, dipole, dipole-dipole forces, hydrogen bonding, London dispersion forces

Essential questions and content:

  • Explain why bonds form
  • Describe the nature of ionic and covalent bonds.
  • Predict bond type using relative positions on the periodic table.
  • Describe a polar covalent bond.
  • Differentiate between ionic and covalent using the chemical formulas.
  • Describe the arrangement of ions in a crystal lattice.
  • List and explain the physical properties of ionic compounds.
  • Draw Lewis diagrams for molecular substances.
  • Differentiate between single, double, and triple covalent bonds.
  • Define resonance and explain how it contributes to bond theory.
  • Explain VSEPR theory.
  • Use VSEPR theory to predict the shapes of molecules.
  • Explain how hybridization relates the shape of molecules to the orbitals occupied by the electrons.
  • Predict the polarity of molecules
  • Describe the types of intermolecular forces of attraction: London dispersion, dipole-dipole forces, and hydrogen bonds.
  • Predict the type of intermolecular force given the formula of the molecule.
  • Describe the electron-sea model of metallic bonding.
  • Give the characteristic properties of a metallic crystal.
  • Describe a covalent network solid and give the characteristic properties.
  • Classify the substance by bond type given the structure, formula, or physical properties.
  • Predict and explain the physical properties of a substance given the bond type.

Chapter 7: Chemical Formulas and Chemical Compounds

Define the following terms:

oxidation number, oxidation state, formula mass, molar mass, percentage composition, empirical formula, molecular formula

Essential Questions and Content:

  • Interpret a chemical formula in terms of the number of atoms or ions it contains.
  • Differentiate between ionic and molecular compounds
  • Name an ionic compound given its formula
  • Using prefixes, name a binary molecular compound from its formula
  • Write the formula of a binary molecular compound from its name.
  • Assign oxidation state numbers to elements in compounds.
  • Name common acids and give their formulas.
  • Use molar mass to convert between the mass and number of moles of a compound.
  • Calculate the number of particles in a given mass of compound.
  • Calculate the percent composition of a compound given its formula.
  • Determine the empirical formula from the percentage composition or mass composition.
  • Differentiate between an empirical and molecular formula of a compound.
  • Determine the molecular formula from the empirical formula and molecular mass.

Chapter 8: Chemical Equations and Reactions

Define the following terms:

chemical equation, precipitate, synthesis, decomposition, single replacement, double replacement, combustion, activity series

Essential questions and content:

  • Describe the clues that indicate a chemical reaction has occurred.
  • Define the symbols used in chemical equations.
  • Write a chemical equation from a sentence description.
  • Balance a chemical equation.
  • Describe the relationship between balancing a chemical equation and the Law of Conservation of Mass.
  • Give general equations for synthesis, decomposition, combustion, single replacement, and double replacement reactions.
  • Classify a reaction according to type.
  • Predict the products of a reaction given the reactants.
  • Explain the significance of the activity series.
  • Use an activity series to predict if a given reaction will occur.

Chapter 9: Stoichiometry

Define the following terms:

stoichiometry, mole ratio, limiting reactant, excess reactant, theoretical yield, actual yield, percent yield

Essential questions and content:

  • Interpret a balanced equation in terms of the mole ratios between reactants and products.
  • Convert between mass, moles, number of particles, and gas volume of reactants and products in chemical reaction.
  • Identify the limiting reactant in a chemical reaction.
  • Use the limiting reactant to calculate the maximum amount of product formed or the amount of excess reactant in a reaction.
  • Distinguish between theoretical yield, actual yield, and percent yield.
  • Calculate the percent yield, given the actual yield.

Chapter 10: Physical Characteristics of Gases

Define the following terms:

ideal gas, elastic collisions, temperature, diffusion, effusion, real gas, pressure, barometer, manometer, STP, partial pressure, kinetic molecular theory, absolute zero

Essential Question and Content:

  • List the physical properties of a gas.
  • Use the KMT to explain the physical properties of a gas.
  • Explain what gas pressure is and how it is measured.
  • State the standard conditions for temperature and pressure.
  • Use Boyle’s Law to calculate volume and pressure changes at constant temperature.
  • Use Charles’ Law to calculate volume and temperature changes at constant pressure.
  • Use the Law of Gay-Lussac to calculate pressure and temperature changes at constant volume.
  • Use the combined gas law to correct the volume of a gas for a new pressure and temperature.
  • Apply Dalton’s Law of Partial Pressure to determine the pressure of a mixture of gases or the partial pressure of a gas in a mixture.

Chapter 11: Molecular Composition of Gases

Define the following terms:

Avogadro’s Law, molar volume, ideal gas law, ideal gas constant

Essential Questions and Content:

  • State Avogadro’s Law and explain its significance.
  • Define the standard molar volume of a gas and use it to calculate gas mass and volume.
  • State the ideal gas equation.
  • Derive the ideal gas constant and state its units.
  • Use the ideal gas equation to calculate the amount of gas at any condition of temperature and pressure.
  • Use the ideal gas equation to calculate the molar mass of a gas given its density.
  • Explain how Avogadro’s law applies to the volumes of gases in a chemical reaction.
  • Apply the principles of stoichiometry to determine the volume of any gas that is produced or consumed in a chemical reaction.
  • State graham’s law of effusion.
  • Determine the relative rate of effusion of two gases of known molar masses using Graham’s Law.

Chapter 12: Liquids and Solids

Define the following terms:

surface tension, capillary action, vaporization, evaporation, boiling, freezing, amorphous, unit cell, equilibrium, Le Chatelier’s Principle, equilibrium vapor pressure, volatile liquid, normal boiling point, molar heat of vaporization, molar heat of fusion, triple point, critical temperature, critical pressure, specific heat, crystalline solids, melting point, supercooled liquids, condensation, sublimation, deposition

Essential Questions and Content:

  • List and compare the physical properties of liquids and solids.
  • Explain the properties of liquids and solids according to the KMT.
  • Describe the process by which solids change into liquids and liquids into gases.
  • Distinguish between amorphous and crystalline solids.
  • Define crystal structure and unit cell.
  • Explain the relationship between equilibrium and changes of state.
  • Define Le Chatelier’s Principle.
  • Predict the change in state using Le Chatelier’s principle
  • Describe the energy changes that take place in processes of boiling, melting and sublimation.
  • Define what is meant by the vapor pressure of a liquid or solid.
  • Explain the relationship between vapor pressure, volatility, boiling point, and the strength of the forces holding particles together.
  • Define the molar heat of vaporization and molar heat of fusion.
  • Calculate the amount of heat energy absorbed or released when a given quantity of substance changes state.
  • Interpret a phase diagram.
  • Explain the physical properties of water in terms of the intermolecular forces that exist between molecules.

Chapter 13: Solutions

Define the following terms:

solution, soluble, homogeneous, heterogeneous, solute, solvent, suspension, colloid, solution equilibrium, saturated solution, unsaturated solution, supersaturated solution, solubility, hydration, miscible, immiscible, heat of solution, concentration, molarity, molality, electrolyte, nonelectrolyte

Essential Questions and Content:

  • Identify the types of solutions
  • Describe the solution process in terms of the interaction between solute and solvent.
  • Distinguish between saturated, unsaturated, and supersaturated solutions.
  • Describe the factors that affect solubility and the rate at which the solute dissolves.
  • Define molarity and calculate its value given the amount of solute in a given volume of solution.
  • Define molality and calculate its value given the amount of solute dissolved in a given mass of solvent.

Chapter 14: Ions in Aq. Solutions and Colligative Properties

Define the following terms:

colligative property, freezing point depression, boiling point elevation

Essential Questions and Content:

  • Describe the colligative properties of a solution.
  • Calculate the freezing point depression or boiling point elevation of a solution.

Chapter 17: Reaction Energy and Reaction Kinetics

Define the following terms:

heat, temperature, specific heat, heat of reaction, enthalpy, enthalpy change, molar heat of formation, molar heat of combustion, entropy, free energy, reaction rate, chemical kinetics, rate law, calorimeter, thermochemistry, reaction mechanism, intermediates, collision theory, activation energy, activated complex, catalyst,, rate-determining step

Essential Questions and Content:

  • Distinguish between heat and temperature.
  • Define the units of heat energy.
  • Perform specific heat calculations.
  • Define the change in enthalpy as the heat of reaction at constant pressure.
  • Associate energy changes to the bond making and bond breaking processes that occur in a reaction.
  • Differentiate between exothermic and endothermic reactions.
  • Label and interpret energy diagrams.
  • Use calorimetry data to determine the change in enthalpy.
  • Define the heat of formation and relate it to the stability of a compound.
  • Use Hess’s Law to determine the heat of reaction given appropriate data.
  • Explain the relationship between the enthalpy change and the tendency of a reaction to occur.
  • Define entropy.
  • Calculate the change in entropy given the absolute entropy values.
  • Explain the relationship between entropy change and the tendency of a reaction to occur.
  • Define the change in free energy.
  • Use the Gibbs equation to determine the change in free energy.
  • Relate the sign of ∆G to the spontaneity of a reaction.
  • Define the reaction mechanism
  • Interpret a reaction pathway using collision theory.
  • Define activation energy.
  • Draw and label energy diagrams showing the activation energy and the activated complex.
  • Define the rate of reaction and describe how it can be determined.
  • List and explain factors which affect the rate of reaction.
  • Define a catalyst and describe how it can affect the rate of reaction.
  • Explain the rate law for a chemical reaction.
  • Determine the rate law for a chemical reaction given appropriate kinetics data.
  • Discuss the relationship between the rate law and the reaction mechanism.