Honors Chemistry
Matter and Change
Chapter 1
Measurement
Chapter 2
Objectives:
Matter and Change:

Describe the difference between a physical change and a chemical change and give several examples of each.

Describe different characteristics of the three states matter.

Classify a mixture as homogeneous or heterogeneous.

Classify a pure substance as an element or a compound.

Identify methods of separations of mixtures.

State the laws of conservation of mass and energy.
Measurement:

Describe the difference between a qualitative and a quantitative measurement.

Describe the difference between accuracy and precision.

Write a number in scientific notation.

State the appropriate units for measuring length, volume, mass, density, temperature and time in the metric system.

Determine the number of significant figures in a measurement or calculation.

Calculate the percent error in a measurement.

Calculate density given the mass and volume, the mass given the density and volume, and the volume given the density and mass.

Honors Chemistry
The Mole
Chapter 3, pages 65-67 and 81-85
Chapter 7, pages 221-233
Chapter 11, pages 335-337
Chapter 13, pages 412-415
Objectives:
 State the postulates of Dalton’s atomic theory.

Define the terms atomic mass and molar mass.
 Define the terms mole and Avogadro’s number.

Write the name for common elements, given the symbol, or the symbol, given the name.

Calculate the molar mass of an element or compound, given its formula.

Identify the seven diatomic elements.

Calculate the mass of an element or compound given the number of moles, or the number of moles of a given mass of an element or compound.

Calculate the number of atoms or molecules of an element or compound given the number of moles, or the number of moles given the number of atoms or molecules.

Calculate the volume of a gas at STP (standard temperature and pressure), or the number of moles of a given volume of an element or compound.

Calculate the volume of a solid or liquid, or the number of moles of a given volume of an element or compound.
 Define a solution’s concentration in terms of molarity.

Calculate the concentration of a solution, given the mass of solute and volume of solution, or the mass of solute needed to prepare a solution of a given concentration.

Calculate the percent composition of each element in a molecular formula.

Calculate the volume of water required to dilute a solution to a given concentration, or the concentration of a solution after a given amount of water is added.

Determine the empirical formula of a substance, given its elemental analysis.

Determine the molecular formula of a substance, given it empirical formula and molar mass.

Calculate the percent water in a hydrate, given its formula.

Determine the formula of a hydrate, given its percent water.

Honors Chemistry
Atomic Structure
Chapter 3 http://en.wikipedia.org/wiki/JJ_Thomson http://en.wikipedia.org/wiki/Oil-drop_experiment http://en.wikipedia.org/wiki/Geiger-Marsden_experiment
Radioactivity
Chapter 22
Objectives:

Describe the experiments of Thomson, Millikan, Rutherford and Chadwick and explain how they contributed to our present understanding of atomic structure.

Describe the mass and charge differences among electrons, protons and neutrons.

Define atomic number, mass number and isotopes in terms of the number of electrons, protons and neutrons.

Determine the atomic mass of an element from the percent abundance of its isotopes, or the abundance from its atomic mass.

Identify the optimum neutron-proton ratios from the elements’ atomic mass.

Identify the products of the most common nuclear decay processes.

Calculate the rate of decay of a radioactive isotope, given its half-life, or its half-life, given its rate of decay.

Calculate the mass defect and binding energy of a nuclide.

Describe nuclear fission and fusion, and calculate the energy released in terms of the mass defect.

Honors Chemistry
The Electron
Periodic Table
Chapter 4 (Skip Quantum Numbers)
Chapter 5
Objectives:

State the mathematical relationship between frequency (or wavelength) of light and its energy.

Describe the photoelectric effect and Einstein’s explanation of it.

Describe the observed emission spectra of atoms in terms of the particle nature of light.

Describe the Bohr model of the atom.

List the atomic orbitals of an atom.

Define the Aufbau Rule for filling atomic orbitals.

Define the Pauli Exclusion Principle.
 Define Hund’s Rule.

Write the electron configuration for any element.

State the significance of an atom or ion possessing the noble gas configuration.

Correlate the electron configuration for an element with its position on the periodic table.

Describe the accomplishments of Dobereiner and Newlands in the identification of patterns of properties among the elements.

Describe the periodic tables of Meyer and Mendeleev.

Identify the various families of elements and define them based on the ions that they form.

State the trends in atomic radius, ionization energy, electron affinity and ion size within a group or period on the periodic table.

Identify the relationship between these trends and the structure of the atom (nuclear charge, filled energy level).

Honors Chemistry
Ionic Bonding
Chapter 6, Sections 1, 3
Metal Bonding
Chapter 6, Section 4
Covalent Bonding
Chapter 6, Sections 2, 5 (Skip Hybridization)
Nomenclature
Chapter 7, Section 1 (Skip Acids)
Objectives:
Ionic/Metal Bonding:

Write the electron configuration of ions of representative elements.

Define ionic bonds in terms of the difference in electronegativity of the atoms.

Write the Lewis electron dot structures of atoms, ions and ionic compounds.

Write the name of an ionic compound (binary, polyatomic and transition metal) given its formula, or its formula given its name.

Describe the properties of ionic, metallic, network covalent and molecular crystals and identify the forces holding them together.
Covalent Bonding:

Describe a covalent bond in terms of the difference in electronegativity of the atoms and the energy changes in bond formation.

Correlate bond energy and bond length for single, double and triple bonds.

State the octet rule and families of elements involved in exceptions to it.

Write the Lewis electron dot structures of compounds and ions containing covalent single, double and triple bonds.

Explain resonance and apply it to determine the bond orders of relevant compounds.

Describe the shapes of molecules using Valence Shell Electron Pair Repulsion (VSEPR)
Theory.

Identify appropriate molecular shapes (linear, trigonal planar, tetrahedral, pyramidal and angular/bent) and specify the corresponding bond angles.

Describe the effect of unshared electron pairs on bond angles.

Describe the formation of σ (sigma) and π (pi) bonds and identify them in molecules.

List the types of intermolecular forces and rank them by strength.

Determine whether a bond is polar or non-polar.

Determine whether a molecule is polar or non-polar.

Write the name of a binary covalent compound given its formula, or its formula given its name.

Honors Chemistry
Chemical Reactions
Chapter 8, Skip Balancing Equations
Chapter 14, Pages 425-430
Objectives:

Identify a reaction as a combination/synthesis, decomposition, single-replacement, double-replacement, or combustion reaction.

Predict the products of a chemical reaction.

Use the activity series of metals to determine which reactions are product-favored.

Predict the formation of a precipitate in an aqueous reaction, by applying the solubility rules for ionic compounds.

Decide whether or not a reaction is a redox reaction.

Write the half reactions for a redox reaction.

Write the net ionic reaction for aqueous reactions.

Honors Chemistry
Stoichiometry
Chapter 8, Balancing Equations
Chapter 9
Objectives:

Balance a chemical reaction.

Using the balanced chemical equation, determine the number of moles of reactant needed or product formed, given the number of moles of another reactant or product.

Calculate the theoretical mass yield of a reaction, given the balanced equation and reagent masses, reagent volume, or volume of solutions of known concentration.

Calculate the theoretical volume yield of a reaction (if a gas, at STP), given the balanced equation and reagent masses.

Calculate the concentration of solution of a product of a reaction, given the balanced equation and reagent masses.

Identify the limiting reagent in a chemical reaction and the maximum amount of product that can be formed, given the amount of each reagent.

Calculate the percent yield in a chemical reaction, given the amount of product formed.

Calculate the percent composition of an impure mixture.

Honors Chemistry
Gases
Chapter 10
Chapter 11 (Sections 1-2)
Objectives:

Explain the relationship between the temperature of a sample of gas and the kinetic energy of the particles of that gas.

Describe how pressure is measured with a barometer and manometer.

Convert values of pressure among the common units.
 Determine the relationship between pressure and volume of a gas (Boyle’s Law).
 Determine the relationship between temperature and volume of a gas (Charles’ Law).

Determine the relationship between temperature and pressure of a gas (Gay-Lussac’s Law).
 State Avogadro’s hypothesis relating particles of a gas to volume.
 State Dalton’s Law of partial pressure and its relationship to Avogadro’s hypothesis.

Describe an ideal gas.

Calculate the amount of gas at any specified conditions of pressure, volume and temperature.

Determine the molar mass of a gas from its density.

Honors Chemistry
Solutions
Chap. 13, Pages 401-410, 416-418
Chap. 14, Pages 436-444
Solutions:

Calculate the molality of a solution.

Calculate the mole fraction of a solution component.

Describe the relationship of temperature and vapor pressure of a pure liquid.

Define the boiling point of a pure liquid.

State the mathematical relationship between the vapor pressure of a solution and its concentration (Raoult’s Law).
 State the mathematical relationship between solubility and pressure of a gas (Henry’s Law).

Describe a solvation as exothermic or endothermic based on the change in maximum solubility as a function of temperature.

State the mathematical relationship on the dependence of freezing point or boiling point on the concentration of the solution.

Calculate the freezing/boiling point of a solution given the solution concentration, or the concentration given the freezing/boiling point.

Calculate the molar mass of a solute from its freezing point depression/boiling point elevation.

Calculate the osmotic pressure of a solution.

Predict the flow of solvent when two different solutions are in contact with a semipermeable membrane.

Honors Chemistry
Electron Transfer
Chapter 19.3-19.4
Objectives:

Describe the components of a galvanic/voltaic cell.

Define the chemical reactions occurring at the cathode and anode of an electrochemical cell.
 Calculate E° for an oxidation-reduction reaction.

Describe the difference between a galvanic cell and an electrolytic cell.

Define batteries, fuel cells and corrosion in terms of electrochemical reactions.

Honors Chemistry
Acids and Bases
Chapters 15 and 16
Objectives:
Acids/Bases:

Describe the physical properties of acids and bases.

Define acids and bases in terms of the ionization of water. o Arrhenius o Bronsted-Lowry o Lewis

Write the chemical formula for an acid given the name, or the name given the formula.

Determine the products of a reaction of an acid and a base.

Identify the conjugate acid-base pairs of a reaction.

Define pH and pOH in terms of the ionization of water.

Calculate the pH of a solution of a strong acid or base.

Describe the difference between strong and weak acids and bases.

Define the terms polyprotic and amphiprotic/amphoteric.

Determine whether an oxide is acidic or basic.

Calculate the concentration of an acid or base by titration.

Describe how an indicator performs in a titration.