Content Outline and Competencies:

I. Scientific Method of Learning

   A. Investigate natural phenomena using scientific methodology,

including:

      1. Make observation

      2. Construct hypotheses

      3. State laws

      4. Articulate theories

      5. Develop models

   B. Summarize information about risks and benefits relative to a

scientific issue and compare risks and benefits.

   C. Use the characteristics of critical thinking to analyze scientific

claims, including:

      1. Falsifiability

      2. Logic

      3. Replicability

      4. Sufficiency

II. Atomic Theories of Matter

   A. Describe the atomic theories of:

      1. Democritus

      2. Lavoisier

      3. Proust

      4. Dalton

   B. List the four postulates of Dalton's atomic theory.

   C. Explain the laws of:

      1. Conservation of mass

      2. Definite proportions

      3. Multiple proportions

   D. Locate the fundamental parts of an atom.

   E. Describe the scientific process leading to the modern understanding

of the atom, including experiments and/or theories of:

      1. John Dalton

      2. J. J. Thomson

      3. Eugene Goldstein

      4. Robert Millikan

      5. Ernest Rutherford

      6. Niels Bohr

   F. Use the periodic table to determine the number of protons and

electrons in an atom of any element.

   G. Describe similarities and differences between the Bohr model of the

atom and the quantum mechanical model.

   H. Identify the charge and relative masses of the proton, the neutron

and the electron.

   I. List similarities or differences between elements in families and

periods in the modern periodic table.

III. Atomic Nuclei and Nuclear Reactions

   A. Calculate the number of neutrons, the number of protons or the

nucleon number in an atom, given any two of these.

   B. Supply the missing nuclide in any nuclear reaction.

   C. Give the symbols and general characteristics (penetration and body

damaging powers) for:

      1. Alpha radiation

      2. Beta radiation

      3. Gamma radiation

   D. Identify nuclides that are isotopes.

   E. Describe the relative mass and charge of subatomic particles,

including:

      1. Protons

      2. Neutrons

      3. Electrons

      4. Alpha particles

      5. Beta particles

      6. Gamma rays

   F. Distinguish between nuclear fission and fusion

   G. Given the fraction decrease in activity and the half-life of the

isotope undergoing radioactive decay, calculate the age of an artifact.

   H. List the principal sources of radiation.

   I. Describe the use of radioisotopes in medicine.

      1. List commonly used radioisotopes.

      2. Match the isotopes with procedures in which they are used.

   J. Explain what is meant by "nuclear winter."

IV. Chemical Bonds

   A. Distinguish between compounds with different types of chemical

bonds.

      1. Ionic bonds

      2. Polar covalent bonds

      3. Nonpolar covalent bonds

   B. Calculate simple combining ratios of atoms.

   C. Draw electrons dot symbols for the first 20 elements in the periodic

table.

   D. Given the molecular formula, construct structural formulas for

simple covalent compounds.

   E. Using the periodic table, determine the number of bonds a nonmetal

element will form.

   F. Predict the shape of simple molecules using the VSEPR theory.

   G. Describe transfer of electrons between atoms, which forms ions

bonds.

   H. Describe the sharing of electrons between atoms, which forms

covalent bonds.

   I. Explain the polarity of covalent bonds using electronegativity

differences.

   J. Explain the relationship between valence electrons and molecular

shape using VSEPR theory.

   K. Describe situations where dipole forces, hydrogen bonds and

dispersion forces are important.

V. Chemical Compounds, Formulas and Reactions

   A. Given positive and negative ions, write formulas and names for ionic

compounds.

   B. Given the name of a covalent compound, write the name.

   C. Given a formula, convert between mass and number of moles of the

substance.

   D. Balance simple chemical equations.

E. Calculate mole ratios of reactants and products in a balanced chemical

equation.

VI. Acids and Bases

   A. Describe the properties of acids and bases.

   B. Match pH values and acid or base character.

   C. Describe acid-base chemistry as it applies to situations such as:

      1. Acid rain

      2. Antacids

VII. Oxidation and Reduction Reactions

   A. Identify substances that are oxidized or reduced.

   B. List applications of:

      1. Reducing agents

      2. Oxidizing agents

   C. Describe oxidation and reduction in:

      1. Electrochemical cells

      2. Batteries

      3. Corrosion

   D. Describe the role of oxidation and reduction in biological

processes.

Optional Content Outline and Competencies

VIII. Polymers

   A. Match a given monomer with the polymer produced from it.

   B. Describe the general types of polymers, including:

      1. Addition

      2. Condensation

      3. Cross linked

   C. List advantages and problems associated with use of plastics.

IX. Air

   A. Describe the layers of the atmosphere and their chemical

composition.

   B. Describe the nitrogen and oxygen cycles.

X. Water

   A. Describe the properties of water.

   B. Sketch the water cycle.

   C. Describe the sources and types of water contamination.

XI. Energy

   A. Identify and use the units and terms of energy.

   B. State the first and second laws of thermodynamics.

   C. Give examples of effects of the laws of thermodynamics.

   D. List sources of energy, including:

      1. Fossil fuels

      2. Nuclear

      3. Solar

      4. Hydroelectric

   E. Describe the advantages and disadvantages of each energy source.

LAB:

I. Safety and Measurements

   A. Work safely and effectively in performing laboratory experiments.

   B. Follow written directions accurately.

   C. Perform techniques used in laboratory experiments.

   D. Acquire data using balances and volumetric equipment.

   E. Estimate and verify the mass of an object.

   F. Estimate and verify the length of an object.

   G. Calculate the average of a series of data to the correct number of

significant figures.

   H. Write data and measurements to the correct number of significant

figures.

II. Periodic Table

   A. Group elements that have similar chemical properties.

   B. Separate groups of elements by observing variations in chemical

behavior.

   C. Using experimental data and values from reference sources, verify

the organization of the modern periodic table.

III. Separation of a Mixture

   A. Using physical properties, separate chemicals from a mixture.

   B. Write a laboratory report explaining procedures.

IV. Density

   A. Calculate the density of a regular shaped object.

   B. Calculate the density of an irregular shaped object.

V. Radioactivity

   A. Test the shielding effect of a variety of materials against alpha

and beta radiation.

   B. Test the effect of distance from a radioactive source.

   C. Determine the half life of a radioactive isotope.

VI. Models

   A. Use model kits to construct various shapes of molecules and ions.

VII. The Nitrogen Cycle in an Aquarium

   A. Determine the concentration of ammonia in a sample of aquarium

water.

   B. Determine the concentration of nitrite in a sample of aquarium

water.

   C. Determine the concentration of nitrate in a sample of aquarium

water.

   D. Graph the concentrations of ammonia, nitrite and nitrate over time.

VIII. Water Hardness

   A. Analyze the hardness of water samples using qualitative procedures.

   B. Soften hard water using the following processes:

      1. Heating

      2. Neutralization

      3. Ion exchanges

      4. Washing soda

      5. Chelating agents

IX. Chemical Reactions

   A. Perform chemical reactions.

   B. Observe and record changes that occur in chemical reactions.

   C. Write balanced equations for chemical reactions.

   D. Carry out chemical reactions ot test consumer products for certain

ions.

   E. Identify an unknown substance using chemical tests.

X. Antacids

   A. Quantitatively titrate acid with base.

   B. Neutralize a commercial antacid.

   C. Determine the efficacy of antacids.

XI. Redox/Stain Removal

   A. Carry out a number of chemical reactions that involve the transfer

of electrons.

      1. Write accurate observations of the reactions.

      2. List oxidizing agents in order of strength.

   B. Investigate use of household cleansers as oxidizing agents.

      1. Test a variety of stains with several oxidizing agents.

      2. Evaluate the stain-removing efficiency of the oxidizing agents.

XII. Polymers

   A. Identify different characteristics of polymers.

   B. Match common products with the polymers from which they are made.

   C. Synthesize a polymer.

XIII. Absorption of Ultra Violet Light by Caffeine

   A. Determine the concentration of a solution.

   B. Measure the absorbance of a caffeine solution using a UV-Vis

Spectrophotometer.

   C. Determine the concentration of an unknown caffeine solution using

absorbance and Beer's Law.

Content Outline and Competencies:

LECTURE

I. Conversion Problems and Atomic/Nuclear Structure

   A. Measurements

      1. Write the names and abbreviations for the metric (SI) units used

in measurements of length, volume and mass.

      2. Determine the number of significant figures in measured numbers.

      3. Adjust calculated answers to the correct number of significant

figures.

      4. Use the numerical values of prefixes to write a metric equality.

      5. Use a conversion factor to change from one unit to another.

      6. Calculate the density or specific gravity of a substance and use

the density or specific gravity to calculate the mass or volume of a

substance.

      7. Use units from mega to nano in conversion problems.

      8. Define terms associated with measurement.

      9. Compare and contrast related chemical terms.

   B. Atoms and elements

      1. Given the name of an element, write its correct symbol or vice

versa.

      2. Use the periodic table to identify the group and the period of an

element and whether it is a metal or a nonmetal.

      3. Describe the electrical charge, mass (amu) and location in an

atom for a proton, neutron and electron.

      4. Give the atomic number and mass number of an atom, state the

number of protons, neutrons and electrons.

      5. Give the number of protons, electrons and neutrons in the

isotopes of an element.

      6. Given the name or symbol of one of the first 20 elements in the

periodic table, write the electron arrangement and use it to explain the

periodic law.

      7. Indicate on the periodic table the appropriate families, groups,

periods or sections which are referred to by the following names: alkali

metals, alkaline earth metals, halogens, rare gases, transition metals,

rare gases, transition metals, rare earth metals, semiconductors and

representative elements.  Given an element, indicate which term is

appropriate for the element.

      8. Describe the electromagnetic spectrum, including relationships

between wavelength, frequency and energy.

      9. Define terms associated with atomic structure and the periodic

table.

      10.   Distinguish between related chemical terms.

   C. Nuclear radiation

      1. Describe alpha, beta and gamma radiation.

      2. Write an equation showing mass numbers and atomic numbers for

radioactive decay.

      3. Write an equation for the formation of a radioactive isotope.

      4. Given a half-life, calculate the amount of radioisotope remaining

after one or more half-lives.

      5. Describe the processes of nuclear fission and fusion.

      6. Define terms associated with nuclear radiation.

      7. Distinguish between related chemical terms.

II. Compounds, Reactions and Energy

   A. Compounds and their bonds

      1. Using the periodic table, write the electron dot structure for a

representative element.

      2. Using the octet rule, write the symbols of the simple ions for

the representative elements.

      3. Using charge balance, write the correct formula for an ionic

compound.

      4. Given the formula of an ionic compound, write the IUPAC name;

given the IUPAC or common (older) name, write the correct formula.

      5. Diagram the electron-dot structure for a covalent molecule.

      6. Given the formula of a covalent compound, write its correct name;

given the name of a covalent compound, write its formula.

      7. Using electronegativity values, classify a bond as nonpolar

covalent, polar covalent or ionic.

      8. Write a formula of a compound containing a polyatomic ion; given

the formula of a compound containing a polyatomic ion, write the correct

name.

      9. Define terms associated with chemical compounds and bonding.

      10.   Distinguish between related chemical terms.

   B. Chemical quantities and reactions

      1. State a chemical equation in words and determine the number of

atoms in the reactants and products.

      2. Write a balanced chemical equation from the formulas of the

reactants and products for a reaction.

      3. Define oxidation and reduction as it occurs in inorganic

compounds (Loss or gain of electrons) and give an example.

      4. Given the chemical formula of a substance, calculate its molar

mass.

      5. Given the number of moles of a substance, calculate the mass in

grams; given the mass, calculate the number of moles.

      6. Define terms associated with chemical quantities and reactions.

      7. Distinguish between related chemical terms.

   C. Energy and matter

      1. Describe some forms of energy.

      2. Identify the physical state of a substance as a solid, liquid or

gas.

      3. Describe the change of state between solid and liquid and also

between solid and gas.

      4. Describe the change of state between gas and liquid.

      5. Describe the energy in exothermic and endothermic reactions;

describe the function of a catalyst.

      6. Describe energy changes in chemical reactions in terms of energy

diagrams for endothermic, exothermic, catalyzed and uncatalyzed

processes.

      7. Define terms associated with energy changes.

      8. Distinguish between related chemical terms.

   D. Gases

      1. Describe the kinetic theory of gases.

      2. Describe the units of measurement used for pressure and change

from one unit to another.

      3. Define terms associated with gases and pressure.

      4. Distinguish between related chemical terms.

III. Introduction to Organic Chemistry

   A. Alkanes and aromatic hydrocarbons

      1. From its properties, classify a compound as organic or

inorganic.

      2. Draw the complete and the condensed structural formula for an

alkane.

      3. Write the names and condensed and structural formulas of the

first ten unbranched alkanes.

      4. Write balanced chemical equations for the combustion of

hydrocarbons.

      5. Use the IUPAC system to write the names of branched-chained

alkanes.

      6. Write the structural formulas of alkanes and their isomers.

      7. Give the name for a cycloalkane and draw the condensed structural

and geometric formulas.

      8. Describe the bonding in benzene, name aromatic compounds and

write their structural formulas.

   B. Haloalkanes, alkene and alkynes

      1. Classify alkanes, alkenes, alkynes and aromatics according to

their functional groups.

      2. Give the name for a haloalkane or draw the structural formula

from the name.

      3. Write the IUPAC names for the structural formulas of alkenes,

cycloalkenes and alkynes or write their structural formulas from their

names.

      4. Write the names and structural formulas of alkenes that have

cis-trans isomers.

      5. Write the structural formulas and names for the products of the

addition reactions of alkenes.

      6. Given the name of common substituents, write the structure and

vice versa.

      7. Distinguish between complete and incomplete combustion and write

balanced equations for each.

      8. Define terms associated with hydrocarbons.

      9. Distinguish between related chemical terms.

IV. Organic Functional Groups and Reactions

   A. Alcohols, phenols, ethers, aldehydes and ketones

      1. Name simple alcohols, phenols and thiols, draw their condensed

structural formulas and describe their solubility in water.

      2. Give the name of an ether and write the condensed structural

formula from the name.

      3. Name aldehydes and ketones and draw the condensed structural

formula from the name.

      4. Write the reactions and/or products for the oxidation and

reduction of alcohols, aldehydes and ketones.  Classify an alcohol as

primary, secondary or tertiary.

      5. Identify and name compounds containing difunctional groups (diol,

dial, dione).

   B. Carboxylic acids, esters, amines and amides

      1. Give the common names, IUPAC names and condensed structural

formulas of carboxylic acids.

      2. Give the common names, IUPAC names and condensed structural

formulas of esters.

      3. Write equations for the formation of an ester (esterification).

      4. Classify amines and give their names and condensed structural

formulas.

      5. Write equations for the formation of an amide (amidation).

      6. Write the common names, IUPAC names and condensed structural

formulas of amides.

      7. Identify and name compounds containing difunctional groups (Dioic

acid, diamine).

      8. Define terms associated with organic functional groups.

      9. Distinguish between related chemical terms.

V. Solutions, Acids and Bases

   A. Solutions

      1. Describe hydrogen bonding in water.

      2. Define solute and solvent and describe the formation of a

solution.

      3. Describe the solution process for electrolytes and

nonelectrolytes in water.

      4. Convert between grams, moles and equivalents.

      5. Define solubility and distinguish between an unsaturated and a

saturated solution.

      6. Identify an insoluble salt.

      7. Calculate the percent concentration of a solute in a solution and

use percent concentration to calculate the amount of solute or solution.

      8. From its properties, identify a mixture as a solution, a colloid

or a suspension.

      9. Calculate the molarity of a solution and use molarity as a

conversion factor to calculate the moles of solute or the volume needed to

prepare a solution.

     10. Complete and balance precipitation reactions.

     11. Write a balanced equation to show the deionization or

dissociation of electrolytes (salts) in water.

     12. Define terms associated with solutions.

     13. Distinguish between related chemical terms.

   B. Acids and bases

      1. Describe acids and bases using the Arrhenius and Bronsted-Lowry

concepts.

      2. Use the ion product of water to calculate the [H3O+] and [OH-] in

a solution.

      3. Calculate pH from [H3O+] and given the pH, calculate [H3O+] and

[OH-] of a solution.

      4. Write an equation for the ionization of strong and weak acids.

      5. Given the molarity or percent concentration of the solution

describe the preparation

of a dilute solution.

      6. Write a balanced equation for the neutralization reaction between

an acid and a base.

      7. Describe the role of buffers in maintaining the pH of a

solution.

      8. Define terms associated with acids and bases.

      9. Distinguish between related chemical terms.

   C. Carboxylic acids, amines

      1. Write equations for the ionization and neutralization of

carboxylic acids.

      2. Write equations for the ionization of an amine in water and

neutralization of an amine.

VI. Introduction to Biochemistry

   A. Carbohydrates

      1. Classify carbohydrates as monosaccharides, disaccharides and

polysaccharides.

      2. Classify a monosaccharide as an aldose or ketose and indicate the

number of carbon atoms.

      3. Given a Fischer Projection of a monosaccharide, draw the

corresponding mirror image and indicate whether it is a D or L isomer.

      4. Draw the open chain structures for D-glucose, D-ribose and

D-fructose.

      5. Identify alpha and beta structures of Haworth projections for

monosaccharides.

      6. Given the Haworth structure of a disaccharide, identify the type

of glycosidic bond.  For the disaccharides maltose, lactose and sucrose,

identify the monosaccharides

and type of glycosidic bonds.

      7. Describe polysaccharides, alpha and beta bonds and the

monosaccharide units in polysaccharides.

      8. Define terms associated with carbohydrates.

      9. Distinguish between related chemical terms.

   B. Lipids

      1. Identify a fatty acid as saturated or unsaturated.

      2. Describe the structure and functional groups of waxes, fats and

oils.

      3. Draw the structure of the product from the reaction of a

triglyceride with hydrogen, an acid or a base or an oxidizing agent.

Write the products of the saponification reaction.

   C. Amino acids, proteins and enzymes

      1. Write the general structural formula of an amino acid and given

the structural formula of the R group; be able to classify as nonpolar,

polar, acidic or basic based upon their R group side chains.

      2. Given the structure of two amino acids, write the structure of

the resulting dipeptide.

      3. Distinguish between the primary and secondary structures of a

protein.

      4. Distinguish between the tertiary and quaternary structures of a

protein.

      5. Describe denaturation of proteins.

      6. Describe the function of an enzyme as a catalyst.

      7. Define terms associated with proteins.

      8. Distinguish between related chemical terms.

LAB

I. Safety, Measurement, Conversions

   A. Safety

      1. State the safety rules for working in a chemistry lab.

      2. Know the location of safety equipment in the lab and state when

and how it is to be used.

      3. Learn the appropriate names of equipment and glassware in the

lab.

   B. Measurement

      1. Measure length of an object, estimating between the lines of the

measuring device.

      2. Measure volume of a liquid using a graduated cylinder, estimating

between the lines.

      3. Measure mass to the nearest milligram using a laboratory

balance.

      4. Determine the volume of a solid by direct measurement or volume

displacement.

      5. Read the specific gravity from a hydrometer.

      6. Given a table with two sets of data, plot the points on a graph.

   C. Conversions

      1. Use significant figures properly in all calculations.

      2. Convert between different units of length, volume or mass.

      3. Using two measured volumes or two measured masses, calculate the

conversion factor.

      4. Given items in a mixture, calculate percent of each.

      5. Calculate the density of an object.

      6. Use density or specific gravity to calculate the mass or volume

of a substance.

      7. From density values, identify an unknown solid or liquid.

      8. Calculate percent error from an experimental value and an

accepted value.

      9. Given percent and component(s), calculate total amount or

individual items in a mixture.

II. Atoms, Chemical Formulas and Chemical Reactions

   A. Atomic Structure

      1. Given the atomic number and mass number of an atom, state the

number of protons, neutrons and electrons.

      2. Light a Bunsen burner and adjust the flame to get a "noisy" light

blue cone indicating a hot flame.

      3. Identify an unknown cation from flame tests.

      4. Give the electron arrangement for the first 20 elements.

      5. Using the octet rule, write electron configurations of ions.

   B. Chemical Formulas

      1. Write the formula and name of representative ions, transition

metal ions and polyatomic ions.

      2. Write the formula and name of ionic compounds.

      3. Write the formula and name of covalent compounds.

      4. Using electron dot structures, diagram the bonds in covalent

compounds.

      5. Identify a compound as ionic or covalent.

      6. Calculate the molar mass of a substance from the chemical

formula.

      7. Work conversion problems between grams and moles.

      8. Given the mole: mole ratio of elements in a compound, determine

the formula.

   C. Chemical Changes

      1. Distinguish between a chemical and a physical change.

      2. Carry out a reaction according to directions and note evidence of

a chemical change.

      3. Balance a chemical reaction.

      4. Determine if a reaction is endothermic or exothermic using a

thermometer.

III. Organic Chemistry

   A. Simple Hydrocarbons

      1. Given a model of an organic compound, write the complete formula,

condensed formula and name.

      2. Compare the properties of organic and inorganic compounds.

      3. Use the CRC handbook to look up the properties of a compound.

      4. Given the molecular formula of an organic compound, write and

name all the isomers.

      5. Write and balance a combustion reaction for a hydrocarbon.

   B. Oxidation Reactions

      1. Know which alcohols are soluble in water.

      2. Classify an alcohol as primary, secondary or tertiary.

      3. Determine which aldehydes and ketones are soluble in water.

      4. Demonstrate the proper technique of smelling a chemical in lab.

      5. Draw the organic product of an oxidation reaction.

   C. Dehydration Reactions

      1. Given an alcohol and an acid, make a model of the resulting ester

and give the name.

      2. Write the structure of the sodium salt obtained by adding NaOH to

a carboxylic acid.

      3. Complete and balance a neutralization reaction involving a

carboxylic acid.

IV. Properties of Solutions

   A. Solution Concentrations

      1. Define saturated, unsaturated or supersaturated solutions.

      2. Given solubility, determine whether a solution is saturated or

not.

      3. Given a graph of solubility versus temperature, determine the

solubility for a given temperature or vice versa.

      4. Given volume and mass data for a solution and solute, calculate

the concentration as mass/mass percent, mass/volume percent and molarity.

   B. Qualitative Analysis

      1. Test an unknown solution for the presence or absence of the

following cations: Na+, K+, Ca+2, NH4+, Fe+3.

      2. Test an unknown solution for the presence or absence of the

following anions: Cl-, Br-, I-, PO4-3, CO3-2, SO4-2.

      3. Given a cation and anion in an unknown, write the formula and

name of the compound.

   C. Electrolytes and pH

      1. Given a solution and a conductivity meter, decide whether the

solution is a strong, weak or non-electrolyte.

      2. Write the equation for the dissociation of a strong, weak or

non-electrolyte.

      3. Use the pH meter to determine the pH of an unknown solution.

      4. Given [H+] and/or [OH-], calculate the other and determine the

pH.

      5. Decide whether an unknown solution is a buffer by adding small

amounts of acid or base and observing the pH change.

      6. Read a buret.

      7. Write a balance equation for an acid - base neutralization

reaction.

Content Outline and Competencies:

I. Describe Matter and Its Measurement, Including Calculations Done on Measurements

   A. Distinguish among the three states of matter (solid, liquids and gases).

   B. Distinguish among elements, compounds and mixtures.

   C. Distinguish between physical and chemical properties and physical and chemical changes.

   D. State the basic units of measurement for length, mass, volume and temperature in the SI system.

   E. Give the numerical equivalent of selected SI prefixes.

   F. Convert temperatures between Fahrenheit, Celsius and Kelvin scales.

   G. Express numerical answers to the correct number of significant figures.

   H. Solve problems using dimensional analysis, including conversion of units.

   I. Solve problems involving density.

II. Demonstrate an Understanding of Basic Chemical Nomenclature

   A. Write the name and symbol for selected elements.

   B. Write the name and symbol for selected polyatomic ions.

   C. Compare and contrast molecular compounds and ionic compounds.

   D. Write names and formulas for the following types of compounds: ionic compounds, binary molecular compounds and acids.

III. Explain Concepts of Basic Atomic Theory and Relate the Theory to the Periodic Table

   A. Recall the basic ideas in Dalton's atomic theory.

   B. Summarize the experiments of J.J. Thomson, Robert Millikan and Ernest Rutherford that characterized the structure of the atom.

   C. Describe atoms in terms of electrons, protons and neutrons.

   D. Given the isotopic masses and fractional abundances for a naturally occurring element, calculate its atomic weight.

   E. Identify the following areas of the periodic table: metals, nonmetals and metalloids; main groups, transition metals, inner transition metals; alkali metals, alkaline earth metals, halogens and noble gases.

   F. Describe the formation of cations and anions and use the periodic table to predict the charges of monoatomic ions.

IV. Write Chemical Reactions and Solve Problems Involving Chemical Stoichiometry

   A. Calculate the molecular mass of a compound from its formula.

   B. Solve problems relating the mass of a compound to the number of moles of a compound.

   C. Solve problems relating the mass of a compound to the number of molecules.

   D. Calculate the percent composition of a compound from its formula.

   E. Determine the empirical formula of a compound from its percent composition.

   F. Determine the molecular formula of a compound from its empirical formula and molecular mass.

   G. Write a balanced chemical equation given the reactants and products.

   H. Predict the product of the combustion reactions of hydrocarbons and simple compounds having C, H and O.

   I. Identify chemical reactions by type: combination, decomposition, combustion.

   J. Solve problems relating grams and moles of substances in balanced chemical equations.

   K. Calculate theoretical yield and percent yield when actual yield is given.

   L. Recognize the limiting reagent in a reaction and do calculations with limiting reagent.

V. Describe the Nature of Aqueous Solutions and Reactions Occurring in Aqueous Solution

   A. Explain how to make solutions of given concentration.

   B. Explain how to dilute solutions to a specified volume or concentration.

   C. Solve solution stoichiometry problems.

   D. Distinguish among strong, weak and nonelectrolytes in solution.

   E. Write balanced complete and net ionic equations.

   F. List the common acids and bases and classify each as a strong or weak electrolyte.

   G. Assign oxidation numbers to atoms in molecules and ions.

   H. Recognize oxidation-reduction reactions and identify oxidizing and reducing agents.

   I. Balance simple oxidation-reduction reactions by the half-reaction method.

VI. Apply Concepts of Thermochemistry to Physical and Chemical Changes

   A. Recognize and illustrate the law of conservation of energy.

   B. Distinguish between a system and its surroundings and describe the energy changes in a system and its surroundings during a given reaction.

   C. State the first law of thermodynamics.

   D. Solve problems involving enthalpies for physical and chemical changes.

   E. Solve calorimetry and heat capacity problems.

   F. Calculate enthalpy changes using Hess' law and measured enthalpies of reaction.

   G. Calculate standard enthalpies of reaction from standard enthalpies of formation.

   H. Determine the enthalpy of reaction using bond energies.

VII. Describe the Electronic Structure of Atoms and Relate the Electronic Structure to Atomic Properties

   A. Solve problems relating frequency, wavelength and energy of electromagnetic radiation.

   B. Explain the essential feature of Planck's quantum theory.

   C. Discuss how line spectra give evidence of energy quantization.

   D. Describe the wave mechanical model of the atom.

   E. Describe s and p orbitals and recognize d orbitals.

   F. Write a set of quantum numbers for any particular electron.

   G. Write the electron configuration of elements up to atomic number 57.

   H. Write electron configurations for ions of main group and transition elements.

   I. Relate position on the periodic table to electron configuration and quantum numbers.

   J. Describe the scientific contributions of Planck, Einstein, de Broglie, Bohr, Schrodinger, Heisenberg, Pauli and Mendeleyev.

   K. Apply Periodic Trends in atomic radii to predict relative size of an atom.

   L. Predict relative first ionization energies from periodic trends.

   M. Explain the observed changes in value of the successive ionization energies for a given atom.

   N. Describe the periodic trends in metallic and nonmetallic behavior.

   O. Describe the general differences in chemical reactivity between metals and nonmetals.

VIII. Demonstrate an Understanding of Chemical Bonding and its Application to Molecular Structure

   A. Determine the number of valence electrons for an atom and write its Lewis symbol.

   B. Recognize when the octet rules applies to the arrangement of electrons in the valence shell.

   C. Predict the relative size of anions and cations formed from an atom.

   D. Use electronegativity differences between bonding atoms to classify bonds as non-polar, polar covalent or ionic.

   E. Draw Lewis structures for atoms, ions and covalent compounds, recognizing when multiple bonds, resonance structures, expanded valence shells, incomplete valence shells and odd electrons are needed.

   F. Relate the number of electron pairs in the valence shell of an atom in a molecule to the geometrical arrangement around that atom.

   G. Predict molecular geometry using the VSEPR model.

   H. Predict whether a molecule can have a net dipole moment from the molecular shape and the electronegativity of the atoms involved.

   I. Describe covalent bonding using valance bond theory.

   J. Describe sp, sp2 and sp3 hybrid orbitals.

   K. Describe the bonding in a double and triple bond.

   L.  Describe the MO theory description of bonding and antibonding orbitals.

   M.  Relate MO theory to concepts such as the structural, energetic, spectroscopic and magnetic properties of molecules.

IX. Describe the Properties of Solids, Liquids and Gases and Relate Those Properties to Intermolecular Forces

   A. Compare and contrast gases, liquids and solids.

   B. Convert between torr, mm Hg, standard atmosphere and Pascal.

   C. Demonstrate an understanding of the gas laws (Charles', Boyle's ideal, etc.) by working problems with them.

   D. List the points of the kinetic molecular theory and describe how this theory explains the common gas laws.

   E. Work stoichiometry problems involving gases and the gas laws.

   F. Describe how the relative rates of diffusion and effusion of two gases depend on their molar masses (Graham's law).

   G. Describe how a real gas differs from an ideal gas.

   H. Employ the kinetic molecular model to explain the differences between the gas, liquid and solid states.

   I. Recognize where dipole-dipole forces, hydrogen bonding and London dispersion forces are important.

   J. Qualitatively explain the relationship between intermolecular forces and properties of liquids and solids.

   K. Draw a phase diagram of a substance given proper data and use a phase diagram to predict the phases present at a given temperature and pressure.

   L. Given heating/cooling curves, calculate the heat associated when a given substance changes from one condition to another.

   M. Compare and contrast crystalline and amorphous solids.

   N. Categorize crystalline solids as ionic, molecular, covalent network and metallic solids.

All exams will be taken in class (no take home exams will be given).
 60% of grade     3-6 Unit exams         
 20% of grade     Final exam            
 20% of grade     Quizzes and homework    
100%
Final grades will be determined with the following percentage scores:
   A = 90% - 100% 
   B = 80% -  89% 
   C = 70% -  79% 
   D = 60% -  69% 
   F =  0% -  59%

Content Outline and Competencies:

I. Work in the Laboratory in Accordance with Good Laboratory
Practices
   A. Dress in an appropriate manner as to promote safety in the
laboratory, wearing a lab coat and goggles when anyone is working with
chemicals in the laboratory.
   B. Follow written directions accurately.
   C. Work safely and effectively, using equipment and chemicals carefully
and correctly.
   D. Demonstrate use of required techniques.
   E. Dispose of waste products in a proper manner.

II. Gather and Record Qualitative and Quantitative Data Accurately
   A. Acquire data using balances and volumetric glassware.
   B. Make and record visual observations.
   C. Use computers, when appropriate, as data acquisition tools.
   D. List or describe experimental assumptions made and any deviations
from the written  experimental procedures.

III. Handle and Evaluate Data in Logical, Productive and Meaningful Way
   A. Create notebooks and laboratory reports that are clear,
understandable and accurate.
   B. Display computer data in a spreadsheet or graphically, as
appropriate.
   C. Correlate observations with chemical or physical processes.
   D. Carry out suitable calculations with quantitative data, recognizing
when data and calculations are within a reasonable range.
   E. Use observations of experimental data to present relevant
conclusions pertaining to the experimental procedure.

IV. Correlate Laboratory Work with Principal Topics in Chemistry I,
Lecture
   A. Measurements
   B. Chemical reactions and stoichiometry
   C. Thermochemistry
   D. Gas laws

   Written laboratory reports    40-60% of grade
   Quizzes (minimum of 8)        20-30% of grade
   Exam(s)                       20-30% of grade  
      Total                        100%

Final grades will be determined with the following percentage scores:
   A = 90% - 100%
   B = 80% -  89%
   C = 70% -  79%
   D = 60% -  69%
   F =  0% -  59%

Content Outline and Competencies:

I. Mixtures and Their Characteristics
   A. Describe the processes by which solutes and solvents interact in
forming solutions. Include terms about the nature of particles, the
various forces and energy involved.
   B. Solve concentration problems with molarity, mass percent, mole
fraction, molality and ppm.
   C. Solve problems with Henry's law.
   D. Describe temperature effects on solubility.
   E. Explain qualitatively the colligative properties, vapor pressure
lowering, boiling point elevation and freezing point depression, and work
quantitative problems.
   F. Describe the process of osmosis and some applications and solve
quantitative problems.
   G. Describe how the colligative properties of solutions of electrolytes
differ from those of solutions of non-electrolytes.
   H. Describe the characteristics of colloids and give examples.

II. Chemical Kinetics and Interpretation of Chemical Reactions
   A. Discuss the effect of concentration, temperature, catalysis and
physical state upon rate of reaction.
   B. Distinguish between average rate and instantaneous rate.
   C. Describe the two types of rate laws (differential and integrated).
   D. Distinguish between first and second order reactions.
   E. Explain why a rate law must be determined experimentally.
   F. Discuss and apply the method of initial rates.
   G. Discuss the relationship between half-life equations and reaction
order.
   H. Use graphs and equations to determine the order of a reaction.
   I. Draw a reaction profile to explain the progress of a reaction.
   J. Describe the collision model and discuss the temperature dependence
of reaction rates.
   K. Define and calculate activation energy.
   L. Discuss reaction mechanisms and explain the rate-determining step.
   M. Explain the effect of a catalyst on a chemical reaction.

III. Chemical Equilibria and Applications
   A. Explain how the terms reversible reaction and dynamic equilibrium
are related.
   B. Write the general equilibrium constant expression and explain its
significance.
   C. Explain why the concentrations of pure liquids and solids are never
used in equilibrium constant expressions.
   D. Show how the numerical value of the equilibrium constant changes
when the stoichiometric coefficients are changed or the reaction is
reversed.
   E. Explain the differences between the terms Kc and Kp and the relation
of either to Qc.
   F. Explain the difference between an equilibrium position and
equilibrium constant.
   G. Given Keq and initial concentration of reactants and/or products,
calculate the final concentrations of reactants and/or products.
   H. List the external factors that can affect equilibria.
   I. Explain how changes in temperature, pressure, volume or
concentration affect the equilibrium position for a chemical reaction.
   J. Describe the effect of a catalyst on a system as it approaches
equilibrium.

IV. Chemical Equilibria in Aqueous Solutions
   A. Explain the similarities and differences between terms such as: Ka
and Kb, pH and pOH, and pKa and pKb.
   B. Apply Brønsted-Lowry acid-base concepts to determine the relative
strength of acids and their conjugate bases.
   C. Name and list the common strong acids (HCl, HBr, HI, HNO3, H2SO4 and
HClO4) and strong bases (i.e., any hydroxide base).
   D. Relate [H+] and [OH-], pH and pOH.  Calculate the pH for solutions
of strong acids and bases.
   E. Identify a weak acid or base and write a chemical equation to
represent its ionization. Set up an equation for determining its
ionization constant expression (Ka and Kb).
   F. Calculate from appropriate data, ionization constants (Ka or Kb),
concentration of the non-ionized acid or base, the concentration of ions
in aqueous solution, the pH and the percent dissociation.
   G. Relate acid strength to Ka and base strength to Kb.
   H. Explain why certain salts give acidic, basic or neutral solutions
and show how to calculate the pH of these solutions.
   I. Describe the ionization of a polyprotic acid in aqueous solution.
   J. Explain how bond strength and polarity affect acid-base properties.
   K. Identify the Lewis acid and base in a chemical reaction.
   L. Describe the effect of common ions on the ionization of weak acids
or bases and calculate the concentration of species present in solutions
of weak acids or bases with their common ion.
   M. Explain why pure water cannot resist changes in pH as well as a
buffered solution.
   N. Use the Henderson-Hasselbach equation to determine the pH of a
buffered solution.
   O. Calculate the pH of a buffer solution from concentrations of the
buffer components and a value of Ka and Kb, and describe how to prepare a
buffer having a specific pH.
   P. Determine the changes in pH of a buffer solution that result from
addition of acids or bases.
   Q. Determine the volume of a solution of known concentration required
to titrate another solution of known volume and concentration.
   R. Determine the concentration of a solute in a solution by titrating
it against a known amount of another substance.
   S. Sketch a titration curve for the titration of:
      1.  Strong acid with a strong base 
      2.  Weak acid with a strong base
      3.  Weak base with a strong acid
      4.  Polyprotic acid or base
   T. Write an equation to express the relationship between a solid solute
and its constituent ions in a saturated solution.
   U. Calculate the Ksp from molar solubility and molar solubility from
Ksp.
   V. Calculate the effect of a common ion on the molar solubility of a
salt.
   W. Predict whether precipitation will occur when salt solutions are
mixed and determine
the concentration of ions remaining in solution after precipitation.
   X. Solve chemical equilibrium problems involving complex ions.

V. Thermodynamics in Chemical and Physical Processes
   A. Explain the similarities and differences between such terms as
enthalpy, entropy and free energy.
   B. Apply the first, second and third law of thermodynamics to the
analysis of chemical and physical processes.
   C. Predict whether the entropy change in a given process is positive,
negative or near zero.
   D. Use data tables to determine enthalpy, entropy and free energy
changes.
      1. Use enthalpies of formation to calculate ∆H for a reaction
(Hess’s Law).
      2. Use standard molar entropies to calculate ∆S for a
reaction.
      3. Use Gibbs free energies of formation to calculate ∆G for a
reaction.
   E. Explain how ∆H, ∆S and ∆G are related to reaction
spontaneity.
   F. Explain how a knowledge of ∆H, ∆S and ∆G allows
one to predict the conditions under which a reaction will occur.
   G. Describe the relationship between the standard free energy of
reaction and the equilibrium constant. Calculate Keq for a chemical
reaction from ∆H°f and S° or ∆G°f.
   H. Calculate ∆G for a chemical reaction that occurs under
nonstandard conditions.

VI. Electrochemical Reactions and Applications
   A. Describe oxidation-reduction reactions as electron loss and electron
gain.
   B. Using the half-reaction method, balance half-reactions in acidic
and/or basic solutions to complete an oxidation-reduction equation.
   C. Describe the components and operation of voltaic and electrolytic
cells.
   D. Using standard half-cell potentials, calculate cell potentials for
both voltaic and electrolytic cells and make predictions about reaction
spontaneity.
   E. Using a table of standard reduction potentials, predict whether a
selected reaction will occur (e.g., Will copper replace silver ion in
solution?).
   F. Explain the similarities and differences between terms such as anode
and cathode, voltaic cell and electrolytic cell, electromotive force and
voltage.
   G. Relate cell potential, free energy change and equilibrium constant.
   H. Using the Nernst equation, calculate the cell potential for
reactions occurring under nonstandard conditions.
   I. Solve stoichiometry problems involving electrolytic cells.
   J. Describe practical applications for voltaic and electrolytic cells
(batteries, corrosion and commercial electrolytic cells).

VII. Nuclear Reaction Processes
   A. Explain the similarities and differences between such terms as
alpha, beta and gamma radiation; binding energy and mass defect; fission
and fusion.
   B. Review and describe the composition of the nucleus.
   C. Name the different types of radioactive decay (e.g., alpha decay)
and describe the characteristics of each.
   D. Write balanced equations for radioactive decay processes.
   E. Calculate the rate of radioactive decay, the half-life or the number
of atoms or moles in a sample of a radioactive nuclide if two of the three
terms are known.
   F. Write equations for nuclear transformation reactions.
   G. Describe some of the practical and beneficial uses of
radioisotopes.
   H. Describe the processes of nuclear fission and fusion and discuss the
problems with using either process as a source of energy.
   I. Describe the difference between commonly used units of radiation
(i.e., curie, rad, rem).

VIII. Critical Thinking Skills
   A. Solve algebraic problems given new data.
   B. Apply appropriate chemical theories in new situations to explain and
predict.
   C. Recognize and explain chemical phenomena in everyday occurrences.

A comprehensive final exam is required. The semester grade will be
determined as follows:

All exams will be taken in class (no take home exams will be given).
 60% of grade      3-6 Unit exams                        
 20% of grade      Final exam                      
 20% of grade      Quizzes and homework    
100%

   Grading Scale:
         A  =  90  - 100%
         B  =  80  -  89%
         C  =  70  -  79%
         D  =  60  -  69%
         F   =  0  -  59%

Content Outline and Competencies:

I. Students Will Work in the Laboratory in Accordance with Good
Laboratory Practices
   A. Dress appropriately on lab days, wearing long pants and shoes will
enclosed toes.  Wear a lab coat and goggles when anyone in the laboratory
is using chemicals.
   B. Follow written directions accurately.
   C. Work safely and effectively, using equipment and chemicals carefully
and correctly.
   D. Demonstrate use of required techniques.
   E. Obtain samples from stock reagents that are correct substance,
concentration and sample size.
   F. Dispose of waste products appropriately.

II. Students Will Gather and Record Qualitative and Quantitative Data
Accurately

III. Students Will Handle and Evaluate Data in Meaningful Ways
   A. Keep notebooks and worksheets that are neat, clean, understandable
and accurately represent work done.
   B. Display computer data in a spreadsheet or graphically, as is
relevant.
   C. Correlate observations with chemical reactions.
   D. Carry out suitable calculations with quantitative data, recognizing
when data and calculations are within a reasonable range.
   E. Use applicable theories to draw experimental conclusions and explain
observations.

IV. Students Will Correlate Laboratory Work with Principal Topics in
Chemistry II, Lecture, Including:
   A. Chemical kinetics
   B. Chemical equilibria
   C. Acid-base chemistry
   D. Electrochemical reactions

  Written laboratory reports    40% - 50% of grade
  Quizzes (minimum 8)           20% - 30% of grade
  Exam(s)                       20% - 30% of grade
      Total                         100%

Grading Scale:
      A = 90% - 100%
      B = 80% -  89%
      C = 70% -  79%
      D = 60% -  69%
      F =  0% -  59%

Content Outline and Competencies:

I. Classify Compounds as to Bond Structures, Shape and Functional
Groups
   A. Describe the structure of the atom and write the electronic
structure of the atoms.
   B. Compare and contrast related terms such as ionic and covalent
bonding, sp, sp2 and sp3 hybrid orbitals.
   C. Use VSEPR theory to describe the molecular geometry and shape.
   D. Use electronegativity and molecular shape to describe polar and
nonpolar molecules.
   E. Draw Lewis structures of selected compounds.
   F. Recognize and draw all of the common functional groups of organic
compounds.
   G. Solve problems and recognize the type of hybrid orbital of the C or
N atom of each functional group.
   H. Correctly define, explain and use the terms and concepts related to
bonding and geometry.

II. Alkanes and Cycloalkanes
   A. Name and draw structures for alkanes and cycloalkanes by the IUPAC
system.
   B. Predict and explain the general trends in the physical properties of
alkanes.
   C. Draw and name the structural isomers for alkanes.
   D. Show the conformation of small alkanes and the cis-trans isomerism
of cycloalkanes.
   E. Correctly define, explain and use the terms and concepts related to
alkanes and cycloalkanes.

III. Alkenes and Alkynes
   A. Use the IUPAC system to name and draw selected alkenes and alkynes.
   B. Discuss the bonding and electronic structure of alkene.
   C. Apply the sequence rules to classify alkenes as E or Z isomers.
   D. Determine the degree of unsaturation for organic compounds using
their molecular formula.
   E. Predict the outcome of symmetrical and unsymmetrical addition
reactions of alkenes.
   F. Correctly define, explain and use the terms and concepts related to
alkenes and alkynes.

IV. Alcohols and Ethers
   A. Predict trends in physical properties of alcohols, phenols, ethers
and thiols based on structure and bond.
   B. Name alcohols and ethers using the IUPAC system of naming.
   C. Classify alcohols as primary, secondary and tertiary.
   D. Describe the condition and the product of oxidation of alcohols.
   E. Correctly define, explain and use the terms and concepts related to
alcohols and ethers.

V. Aldehydes and Ketones
   A. Describe the structure and properties of aldehydes and ketones.
   B. Name aldehydes and ketones using the IUPAC system of nomenclature.
   C. Propose methods for the preparation of aldehydes and ketones.
   D. Predict reactions of aldehydes and ketones.
   E. Correctly define, explain and use the terms and concepts related to
aldehydes and ketones.

VI. Carboxylic Acids and Esters
   A. Name (by IUPAC) and draw structures for both carboxylic acids and
esters.
   B. Discuss the physical properties of carboxylic acids and esters.
   C. Propose synthetic methods for the preparation of carboxylic acids
and esters.
   D. Predict chemical reactions of esters.
   E. Predict polymerization reactions to form polyesters.
   F. Correctly define, explain and use the terms and concepts related to
carboxylic acids and esters.

VII. Amines and Amides
   A. Describe the structure of amines and amides including hybrid orbital
overlap and approximate bond angles.
   B. Use common or IUPAC prefixes and suffixes to name amines and
amides.
   C. Classify amines as primary, secondary and tertiary.
   D. Predict trends in physical properties of amines based on structure,
bond polarity and hydrogen bonding.
   E. Describe conditions and predict products of reaction of amines with
acids.
   F. Predict polymerization reactions to form polyamides.
   G. Describe the conditions and predict products for the formation of
amides, also the hydrolysis of amides.
   H. Correctly define, explain and use the terms and concepts related to
amines and amides.

VIII. Carbohydrates
   A. Name the monosaccharides having 3 to 6 carbons.
   B. Recognize chiral compounds and differentiate between enantiomers and
diastereomers.
   C. Describe the D and L sugars.
   D. Draw the Fischer and Haworth projection for monosaccharides.
   E. Describe the process and the results of mutarotation.
   F. Describe the oxidation, reduction and formation of glycosides from
monosaccharides.
   G. Describe the use of Benedict and Tollen's reagents in determining
whether a sugar is a reducing or nonreducing sugar.
   H. Correctly define, explain and use the terms and concepts related to
sugars.

IX. Lipids
   A. Describe the common properties of all lipids.
   B. Describe the different classes of lipids and list examples of the
common classes.
   C. Describe the structure, properties and chemical reactions of
saturated and unsaturated fatty acids.
   D. Describe and draw the formulas for the triglycerides (fats and oils)
and phosphoglycerides.
   E. Predict trends in physical properties of triglycerides on structure,
bond polarity and isomerism.
   F. Describe the hydrogenation of oils and the hydrolysis and
saponification of triglycerides.
   G. Describe the structure and draw formulas for sphingolipids, steroids
and waxes.
   H. Describe the general structure and the function of lipoproteins.
   I. Correctly define, explain and use the terms and concepts related to
lipids.

X. Amino Acids, Proteins and Enzymes
   A. Describe in detail the general structure of alpha amino acids,
including the chirality of the alpha carbon and the zwitterion, types of
amino acids based on the side chain change.
   B. Describe the relative acidity and basicity of amino acids for
different side groups.
   C. Describe in detail the peptide bond (amide bond).
   D. Describe in detail the primary, secondary, tertiary and quaternary
structure of proteins.
   E. Describe the effect of change in pH, temperature change and adding
specific reagents on protein structure.
   F. Use the enzyme classification and naming of enzymes.
   G. Discuss the mechanism of enzyme catalysis including the enzyme and
substrate complexes, active sites and the rate of reaction.
   H. Discuss how the concentration of enzyme or substrate, pH and
temperature affects the function of enzyme.
   I. Recognize the function of vitamins in enzyme activity.
   J. Identify the importance of enzyme activity in metabolic processes.
   K. Correctly define, explain and use the terms and concepts related to
proteins and enzymes.

XI. Nucleic Acids
   A. Identify the different types of nucleotides.
   B. Recognize nucleic acid structure.
   C. Identify the base pair interactions present in DNA.
   D. Outline the steps in replication, transcription, and translation.
   E. Describe mechanisms that cause mutations.
   F. Identify the methods utilized in genetic engineering
   G. Correctly define, explain and use the terms and concepts related to
nucleic acids, DNA, and RNA.

XII. Attitudes and Work Habits
   A. Identify and develop positive attitudes toward tasks and fellow
students appropriate for the laboratory, including giving and accepting
criticism and praise.
   B. Identify and develop productive work habits, including attending to
detail, completing tasks, maintaining the work setting and recording
data.
   C. Identify and develop collaborative/teamwork skills, including
solving problems in groups, building consensus and responding to
supervision.

Three to five unit exams will be given along with a comprehensive
final.
There will be 10-12 quizzes given during the semester.
Homework will be assigned and may be graded.

Laboratory: A written lab report is required for each experiment and the
report grade is based on completeness, organization, quality and writing
style.

The semester grade will be determined as shown below:

Exams                           50 – 70%
Quizzes/Homework                 5 – 10%
Laboratory (Reports & lab test) 10 – 20%
  Total:                          100%

Grading Scale:
   A = 90% - 100% 
   B = 80% -  89%
   C = 70% -  79% 
   D = 60% -  69% 
   F =  0% -  59%

Content Outline and Competencies:

I. Teaching as a Career

A. Determine suitability/interest in teaching as a career through thoughtful self-reflection.

B. Explore pathways to a career in teaching.

C. Identify personal learning styles and discuss their implications for classroom interactions.

II. Strategies for Practical Lesson Design

A. Design and deliver inquiry-based hands-on lessons.

B. Write performance objectives for each lesson, including mathematics and/or science connections, and appropriate assessments for those objectives.

C. Use technology and the Internet to enhance classroom lessons, collaborate, and communicate.

III. Concepts and Components of Teaching Theory

A. Identify instructional strategies that meet the needs of diverse learners.

B. Distinguish between learner-centered and teacher-centered instructional strategies.

C. Discuss state and national science and mathematics standards and their implications for curriculum decisions.

D. Identify current issues in the theory and practice of teaching.

IV. Components of a Field Experience

A. Observe a math-science lesson taught by a cooperating teacher.

B. Interact with a population of diverse student learners in a school setting while teaching a lesson in an elementary school classroom.

C. Receive and synthesize feedback from a cooperating teacher as a peer and mentoring colleague in order to improve techniques.

Content Outline and Competencies:

I. Molecular Structure and Chemical Bonding Theories
   A. Draw Lewis electron dot structures for molecules.
   B. Draw resonance forms for a molecule having delocalized bonding.
   C. Determine the relative stability of resonance forms using formal
charges.
   D. Apply the VSEPR model to describe molecular geometry and shape.
   E. Draw a three-dimensional representation of a given molecule.
   F. Discuss the formation of a covalent bond.
   G. Identify bonds as covalent or ionic. 
   H. Describe the electronic structure of molecules using valence bond
theory.
   I. Predict the hybridization state of atoms in a molecule.
   J. Apply the theory of resonance to show the unusual stability of the
allyl radical and other conjugated pi-bonded species.
   K. Explain the unusual stability of the allyl radical and other
conjugated pi-bonded species in terms of molecular orbital theory.

II. Structure and Properties of Organic Molecules
   A. Predict whether a molecule has a net dipole moment.
   B. Identify the type(s) of intermolecular forces which operate between
molecules.
   C. Predict general trends in boiling points and solubilities based on
intermolecular forces.
   D. Predict relative acidities and basicities based on structure,
bonding and resonance forms of conjugate acid-base pairs.
   E. Predict the direction of Brönsted-Lowry acid-base reactions.
   F. Identify Lewis acids and bases.
   G. Identify by name the following type of compounds (given a condensed
structural formula): alkanes, alkenes, alkynes, aromatic hydrocarbons,
alkyl halides, alcohols, ethers, aldehydes, ketones, carboxylic acids,
esters, amides, amines and phenols.
   H. Draw condensed structural formulas for the following types of
compounds: alkanes, alkenes, alkynes, aromatic hydrocarbons, alkyl
halides, alcohols, ethers, aldehydes, ketones, carboxylic acids, esters,
amides, amines and phenols.

III. Analysis of Organic Reactions
   A. Classify organic reactions as addition, elimination, substitution or
rearrangement.
   B. Distinguish between polar and radical mechanisms.
   C. Identify reagents as electrophiles and nucleophiles.
   D. Apply thermodynamic concepts to the analysis of organic chemical
reactions.
   E. Calculate the enthalpy change for a reaction from a table of bond
energies.
   F. Relate the equilibrium constant for a chemical reaction to the
standard free energy change for that reaction.
   G. Apply qualitative ideas from transition state theory to the analysis
of organic chemical reactions.
   H. Draw and interpret an energy diagram for a chemical reaction.
   I. Discuss the meaning of the term activation energy.

IV. Nomenclature
   A. Given the structure, provide correct IUPAC names for alkanes,
cycloalkanes, alkenes,   alkynes, dienes and alkyl halides.
   B. Given the name, draw correct condensed structural formulas for
alkanes,
cycloalkanes, alkenes, alkynes, dienes and alkyl halides.
   C. Draw and use common names for all 3- and 4-carbon alkyl groups.

V. Alkanes and Cycloalkanes
   A. Name and draw structures for alkanes and cycloalkanes by the IUPAC
system.
   B. Identify carbon and hydrogen as being primary, secondary or
tertiary.
   C. Draw all possible isomers given the molecular formula.
   D. Draw Newman projections of different conformations of molecules and
predict their relative stability.
   E. Discuss the applicability of Bayer strain theory to the stabilities
of cycloalkanes.
   F. Compare and contrast the terms ring and angle strain.
   G. Draw structures for both boat and chair cyclohexane.
   H. Distinguish (by drawing) the difference between axial and equatorial
positions in
cyclohexane.
   I. Recognize cis and trans isomers of disubstituted cyclohexanes.
   J. Predict the stability of substituted cyclohexanes by estimating
steric interactions.

VI. Alkenes, Alkynes and Conjugated Dienes
   A. Name and draw structures for alkenes and alkynes by the IUPAC
system.
   B. Determine the degrees of unsaturation of an organic compound from
its molecular formula.
   C. Discuss the bonding and electronic structure of alkenes.
   D. Draw and name cis-trans isomers of alkenes.
   E. Apply the sequence rules to classify alkenes as E or Z isomers.
   F. Use heats of hydrogenation to determine the relative stability of
alkenes.
   G. Show by reaction the preparation of alkenes, alkynes and conjugated
dienes.
   H. Predict the products of reactions of alkenes, alkynes and conjugated
dienes.
   I. Discuss the bonding and electronic structure of alkynes.
   J. Compare and contrast the reactions of alkenes and alkynes.
   K. Explain why the terminal hydrogen in terminal alkynes is acidic.
   L. Explain the unusual stability of conjugated dienes.

VII. Alkyl Halides
   A. Name and draw structures for alkyl halides by the IUPAC system.
   B. Show by reaction the preparation of  alkyl halides.
   C. Predict the products of reactions of alkyl halides.

VIII. Stereochemistry
   A. Recognize the difference between constitutional isomers and
stereoisomers.
   B. Determine if an object or molecule is chiral.
   C. Apply the RS system of nomenclature to stereoisomers.
   D. Compare and contrast, using examples if necessary, the following
terms: enantiomers,
diasteromers and meso compounds.
   E. Draw Fischer projections of chiral compounds.
   F. Explain the difference between relative and absolute
configurations.
   G. Predict the theoretical number of stereoisomers.
   H. Predict the stereochemical outcome of selected reactions.

IX. Substitution and Elimination Reactions
   A. Discuss the kinetics involved with nucleophilic substitution
reactions.
   B. Classify reactions as SN1, SN2, E1 or E2.
   C. List a set of ideal conditions for SN1, SN2, E1 or E2 reactions.
   D. Discuss the factors that can influence the rates of SN1, SN2, E1 or
E2 reactions.
   E. Predict the products of  SN1, SN2, E1 or E2 reactions.
   F. Explain the limitations placed upon elimination reactions that
involve the cyclohexane ring.

X. Mechanisms
   A. Draw and explain the radical mechanism for the halogenation of
alkanes.
   B. Explain the relationship of the structure of free radicals to
stability.
   C. Draw and discuss each step of the mechanism of an alkene addition
reaction.
   D. Explain the relationship of carbocation structure to stability.
   E. Recognize when carbocation rearrangement is likely to occur.
   F. Apply the Hammond postulate to the analysis of a reaction
mechanism.
   G. Draw and explain the mechanism for a SN1, SN2, E1 or E2 reaction.
   H. Compare and contrast kinetic and thermodynamic control of 1,2- and
1,4-addition reactions of conjugated dienes.

XI. Spectral Interpretation
   A. Identify functional groups by their infrared absorptions.
   B. Correlate the infrared spectrum of a known organic compound to its
structure.
   C. Propose a structure for an unknown consistent with its infrared
spectrum and other data such as the molecular formula.

XII. Critical Thinking
   A. Devise a reasonable synthetic pathway for producing a desired
compound from a specific starting material.
   B. Propose a reaction mechanism to explain the outcome of a reaction
you have never seen before.
   C. Determine the structure of an unsaturated compound from its
molecular formula and its cleavage and/or hydrogenation products.

XIII. Students Will Work in the Laboratory in Accordance with Good
Laboratory Practices
   A. Dress appropriately on lab days, wearing long pants and shoes with
enclosed toes, and wear a lab coat and goggles when anyone in the
laboratory is using chemicals.
   B. Follow written directions accurately.
   C. Work safely, using equipment and chemicals carefully and correctly.
   D. Obtain samples from stock reagents that are the correct substance,
concentration and sample size.
   E. Dispose of waste products appropriately.

XIV. Students Will Gather and Record Qualitative and Quantitative Data
   A. Record data in a concise and accurate fashion, reporting visual
observations, such as color, state and speed of reaction.
   B. Demonstrate required techniques, which include:
      1. Assembly of microscale glassware
      2. Use of milligram balance
      3. Use of automatic pipet
      4. Monitoring and controlling the temperature of a reaction vessel
      5. Filtration
      6. Crystallization
      7. Determination of melting point and boiling point
      8. Extraction
      9. Use of drying agents
     10. Reflux
     11. Simple and fractional distillation
     12. Thin-layer chromatography
     13. Column chromatography
     14. Gas chromatography
     15. Refractometry
     16. Infrared sample preparation
     17. Operation of infrared spectrometer
   C. List or describe experimental assumptions made.

XV. Students Will Handle and Evaluate Data in Meaningful Ways
   A. Create notebooks and laboratory reports that are clear,
understandable and accurately represent the work done.
   B. Correlate observations with appropriate chemical and/or physical
processes.
   C. Carry out suitable calculations with quantitative data, recognizing
when data and calculations are within a reasonable range.
   D. Use applicable theories to draw experimental conclusions and explain
observations.

All exams will be taken in class (no take home exams will be given)
 
 40% of grade         3-6 Unit Exams                  
 20% of grade         Final Exam             
 10% of grade         Quizzes and/or Homework      
 30% of grade         Laboratory    
100%

Grading Scale:
   90% - 100% = A
   80% -  89% = B
   70% -  79% = C
   60% -  69% = D
    0% -  59% = F

Content Outline and Competencies:

I. Structure Determination by Spectroscopy
   A. Mass spectroscopy
      1. Use mass spectroscopy data to interpret molecular structure.
      2. Interpret mass spectral fragmentation patterns.
      3. Use mass spectra to determine molecular weights and base peaks
and to distinguish between hydrocarbons.
      4. Write molecular formulas corresponding to a given molecular ion.
   B. Infrared spectroscopy
      1. Identify the regions of the electromagnetic spectrum used for
infrared spectroscopy.
      2. Relate energy, frequency and wavelength for electromagnetic
radiation to infrared spectroscopy.
      3. Interpret infrared spectra relating to functional groups in
organic molecules.
      4. Interpret infrared spectra for hydrocarbons.
   C. Nuclear magnetic resonance spectroscopy
      1. Describe how NMR signals are obtained.
      2. Interpret chemical shift patterns relating to chemical
structure.
      3. Interpret 1H NMR peak areas using integration techniques in
relationship to proton counting.
      4. Use spin-spin splitting of 1H NMR signals to interpret molecular
structure in organic molecules.
      5. Relate and use the number of 1H NMR absorptions to proton
equivalency in a molecule.
      6. Relate and use chemical shifts in 1H NMR spectroscopy to
determine chemical structure in organic molecules.
      7. Use 1H NMR spectra to determine the chemical structure of a
compound.
      8. Interpret 13C NMR spectroscopy relating to functional groups in
organic molecules.
      9. State the uses of 1H NMR spectra.   

II. Benzene and Aromaticity
   A. State sources of aromatic hydrocarbons.
   B. Name by IUPAC and draw structures for aromatic compounds.
   C. Recognize and be able to use the names and structures for toluene,
phenol, aniline,
acetophenone, benzaldehyde and benzoic acid.
   D. Explain how Kekule accounted for the unusual properties of benzene.
   E. Use thermodynamic data to show that benzene is more stable than the
hypothetical compound 1,3,5-cyclohexatriene.
   F. Compare the reactivity of benzene to cyclohexene.
   G. List the four postulates of resonance theory.
   H. Use molecular orbital (MO) theory to describe the bonding in benzene
and other aromatic compounds.
   I. Relate aromaticity to Huckel's rule and MO theory.
   J. Predict aromaticity of heterocylic compounds.
   K. Predict aromaticity of ions.
   L. Describe the bonding in polycyclic aromatic hydrocarbons.
   M. Identify the spectroscopic regions of the IR for aromatic compounds
for use in structural determination of organic molecules.

III. Chemistry of Benzene:  Electrophilic Aromatic Substitution
   A. Draw and explain the general mechanism for electrophilic aromatic
substitution.
   B. Predict the products and/or write mechanisms for electrophilic
aromatic substitution reactions studied.
   C. Use the above listed reactions in synthesis.
   D. Explain how substituents affect the reactivity of aromatic rings.
   E. Discuss ortho-para and meta directors, giving some characteristics
and examples of each.
   F. Predict the orientation of incoming groups in disubstituted benzene
rings.
   G. Predict the orientation of incoming groups in trisubstituted benzene
rings.
   H. Recognize the conditions necessary for nucleophilic aromatic
substitution to occur.
   I. Draw and explain the addition-elimination mechanism and the
elimination-addition mechanism in nucleophilic aromatic substitution
reactions.
   J. Use oxidation reactions of aromatic compounds.
   K. Use reduction reactions of aromatic compounds.
   L. Identify the difference in reactivity between the aromatic ring and
a substituted side-chain in oxidation and radical bromination reactions.
   M. Use the reactions learned for electrophilic aromatic substitution to
work synthesis problems.

IV. Alcohols and Thiols
   A. Name by IUPAC and draw structures for alcohols.
   B. Identify sources and uses of simple alcohols.
   C. Compare the physical properties of alcohols to alkanes and alkyl
halides.
   D. Show how to use acid-base reactions to prepare alkoxide ions.
   E. Show how alcohols are prepared from alkenes, aldehydes, ketones,
esters and carboxylic acids.   
   F. Prepare alcohols from reduction of carbonyl groups.
   G. Show how the Grignard reaction can be used to make 1o , 2 o or 3 o
alcohols.
   H. Describe the limitations of the use of the Grignard reaction in
synthesis or organic compounds.
   I. Show how alkenes, alkyl halides and tosylates can be prepared from
alcohols.
   J. Show how alcohols may be oxidized to carbonyl compounds.
   K. Use the alcohol reactions studied in synthesis reactions.
   L. Discuss the use of protecting groups in organic synthesis.
   M. Identify the spectroscopic regions of the IR for alcohols for use in
structural determination of organic molecules.
   N. Describe the similarities of thiols to alcohols.

V. Ethers, Epoxides and Sulfides
   A. Name by IUPAC and draw structures for ethers.
   B. Compare the physical properties of ethers to alkanes of comparable
molecular weights.
   C. Describe the industrial preparation of ethers.
   D. Prepare ethers via the Williamson ether synthesis.
   E. Prepare ethers via alkoxymercuration-demercuration of alkenes.
   F. Predict the products formed in an acid-induced cleavage of an
ether.
   G. Name cyclic ethers:  epoxides.
   H. Show by equations how epoxides are produced.
   I. Show the mechanism and predict the product formed (with correct
stereochemistry) in the acid-catalyzed and base-catalyzed ring opening
reactions of epoxides.
   J. Use the ether and epoxide reactions studied in synthesis.
   K. Discuss the use of crown ethers in organic synthesis.
   L. Identify the Spectroscopic regions of the IR for ethers and epoxides
for use in structural determination of organic molecules.
   M. Describe the similarities of Sulfides to ethers.

VI. Aldehydes and Ketones:  Nucleophilic Addition Reactions
   A. Compare the physical properties of aldehydes and ketones to alkanes
and alcohols of comparable molecular weights.
   B. Name by IUPAC and draw structures for aldehydes and ketones.
   C. Recognize and use the following common names: formaldehyde,
acetaldehyde and ketones.
   D. Show the general mechanism for nucleophilic addition at the carbonyl
group.
   E. Show by equations the preparation of aldehydes and ketones.
   F. Show by reactions how aldehydes and ketones react with oxidizing and
reducing agents.
   G. Predict the products of nucleophilic addition reactions with a
variety of reagents studied for aldehydes and ketones.
   H. Use the above listed reactions in synthesis.
   I. Identify the spectroscopic regions of the IR for aldehydes and
ketones for use in structural determination of organic molecules.

VII. Carboxylic Acids
   A. Name by IUPAC and draw structures for both mono and dicarboxylic
acids.
   B. Recognize and use the following common names: formic acid, acetic
acid, benzoic acid and oxalic acid.
   C. Discuss the structure and physical properties of carboxylic acids.
   D. Discuss the acidity of carboxylic acids and the factors that affect
the stability of the carboxylate anion.
   E. Discuss substituent effects on acidity of benzoic acids and
substituted benzoic acids.
   F. Show by equations the preparation of carboxylic acids.
   G. Predict the products of reactions of carboxylic acids.
   H. Predict the products of reduction of carboxylic acids to primary
alcohols.
   I. Use the carboxylic reactions studied in synthesis.
   J. Identify the spectroscopic regions of the IR for carboxylic acids
for use in structural determination of organic molecules.

VIII. Carboxylic Acid Derivatives and Nucleophilic Acyl Substitution
Reactions
   A. Name by IUPAC convention and draw structures for acid halides, acid
anhydrides, amides, esters and nitriles.
   B. Recognize and use the following common names: acetyl chloride,
acetic anhydride, acetamide and acetonitrile.
   C. Show the general mechanism for nucleophilic acyl substitution.
   D. Predict the products of carboxylic acid derivative reactions.
   E. Predict the products of nucleophilic acyl substitution reactions of
carboxylic acid derivatives studied and be able to use those reactions in
synthesis problems.
   F. Use the carboxylic acid derivative reactions studied in synthesis.
   G. Identify the spectroscopic regions of the IR for carboxylic acid
derivatives for use in structural determination of organic molecules.

IX. Carbonyl Alpha-Substitution Reactions
   A. Show keto-enol tautomerism in carbonyl compounds.
   B. Show how tautomerism differs from resonance.
   C. Illustrate the mechanism of alpha-substitution reactions.
   D. Predict the products of carbonyl alpha-substitution reactions
studied and be able to use those reactions in synthesis.     
   E. Describe the acidity of alpha-hydrogen atoms:  enolate ion
formation.
   F. Predict the reactivity of enolate ions.

X. Carbonyl Condensation Reactions
   A. Show the general mechanism of carbonyl condensation reactions.
   B. Predict the products of condensation reactions of aldehydes and
ketones:  the aldol reaction.
   C. Describe the difference of carbonyl condensation reactions versus
alpha-substitution reactions.
   D. Identify aldol products.
   E. Identify mixed aldol products.
   F. Identify intramolecular aldol products.
   G. Predict the products of reactions studied that are similar to the
aldol condensation reaction.
   H. Use the condensation reactions studied in synthesis.
   
XI. Carbohydrates
   A. Classify carbohydrates by the number of carbons, presence and size
of ring, and type of glycoside linkage.
   B. Draw Fischer projections for depicting carbohydrates.
   C. Use the DL sugars nomenclature system.
   D. Draw monosaccharides in the various representations studied and be
able to convert from one representation to another.
   E. Convert from straight chain to the cyclic hemiacetal formation for
monosaccharides.
   F. Explain mutarotation in sugars.
   G. Explain why some sugars are reducing and others are not.
   H. Predict the products of reactions studied of monosaccharides.
   I. Explain the Fischer Proof.
   J. List simple disaccharides.
   K. Discuss the similarities and differences of the polysaccharides
starch and cellulose.

XII. Aliphatic Amines
   A. Name by IUPAC and draw structures for amines.
   B. Discuss structure and bonding in amines.
   C. Relate physical properties of amines to structure.
   D. Discuss basicity of amines in terms of their structure.
   E. Compare the basicity of amines to amides.
   F. State industrial sources and uses of alkylamines.
   G. Show by equations reactions of amines.
   H. Use reactions to synthesize amines.
   I. Identify the spectroscopic regions of the IR for amines for use in
structural determination of organic molecules.

XIII. Arylamines and Phenols
   A. Explain why alkyl amines are more basic than arylamines.
   B. Show how to prepare arylamines.
   C. Predict the products of reactions of arylamines.   
   D. Use the replacement reactions of arenediazonium salts in synthesis.
   E. Show how diazonium salts can be used in coupling reactions.
   F. State industrial uses of phenols.   
   G.  Explain the acidity of phenols in terms of their structure.
   H. Show by reactions the preparation of phenols.
   I. Predict the products of reactions of phenols.
   J. Use reactions of phenols to solve synthesis problems.
   K. Recognize the spectroscopic regions of the IR for arylamines and
phenols for use in structural determination of organic molecules.

XIV.  Laboratory 
   A. Record data in a concise and accurate manner, reporting visual
observations such as color, physical states and temperature conditions.
   B. Correctly demonstrate required techniques, which include:
      1. Use of the laboratory balance
      2. Use of an automatic pipette
      3. Use of a heating plate with a heating block or sand bath to
monitor the temperature of a reaction
      4. Use of filtration equipment
      5. Use of equipment for crystallization and recrystallization
techniques
      6. Use of melting point apparatus to determine melting points of
organic compounds
      7. Use of equipment to determine the boiling points of organic
liquids
      8. Use of drying agents
      9. Use of equipment for reflux of reaction mixtures
     10. Use of distillation equipment
     11. Use of chromatography techniques for compound identification
     12. Use of FTIR to prepare samples and obtain spectra of organic
compound
   C. List and/or describe experimental assumptions made.
   D. Dress appropriately on lab days, which includes wearing long pants
or skirts, enclosed toes, lab coat and goggles.
   E. Follow written directions accurately.
   F. Work safely using equipment and chemicals safely and appropriately.
   G. Obtain stock reagents correctly.
   H. Dispose of waste products according to chemical hygiene guidelines.
   I. Create notebooks and laboratory reports according to written
guidelines.
   J. Correlate observations with appropriate chemical and/or physical
processes.
   K. Make calculations with the data collected, recognizing  calculations
that do not fall within reasonable ranges.
   L. Use applicable theories learned in lecture to draw experimental
conclusions and explanations of observations.  

All exams will be taken in class (no take home exams will be given)
 
 40% of grade        3-6 Unit Exams                   
 20% of grade        Final Exam        
 10% of grade        Quizzes and/or Homework       
 30% of grade        Laboratory              
100%

Grading Scale:
   A = 90% - 100%
   B = 80% -  89%
   C = 70% -  79%
   D = 60% -  69%
   F =  0%  - 59%

Content Outline and Competencies:

I. Investigate the Properties of Water and the Application of Aqueous
Solutions to Biochemical Systems
   A. Compare and contrast the different types of intermolecular forces.
   B. Describe the different types of acids and bases.
   C. Cite examples of buffer systems.
   D. Calculate pH and composition of buffers using the
Henderson-Hasselbach equation.
   E. Describe the effects of changes in pH on the uptake and release of
O2 and CO2 in red blood cells.

II. Describe the Structures and Functions of Amino Acids and Small
Peptides
   A. Classify amino acid structures according to ionic properties and
polarity.
   B. Investigate the stereochemistry of amino acids.
   C. Predict the acid-base characteristics of amino aids and peptides.
   D. Investigate the reactions and functions of small peptides and amino
acids.

III. Explain Aspects of Protein Structure
   A. Compare and contrast the four levels of protein structure.
   B. Describe different protein purification techniques.
   C. Determine the most appropriate chromatography method for a given set
of circumstances.
   D. Determine the primary structure of polypeptides from a set of data.
   E. Compare and contrast the different types of secondary structure.
   F. Describe the structure and functions of collagen.
   G. Summarize the tertiary structure of proteins.
   H. Compare and contrast differences in the structure and functions of
Hb and Mb.
   I. Relate the quaternary structure of Hb to cooperative binding of O2.
   J. Describe the effects of bisphosphoglycerate on Hb and Mb.

IV. Examine the Properties of Enzymes
   A. Classify major classes of enzymes.
   B. Correlate the relationship between free energy, catalysts and
kinetics.
   C. Interpret enzyme kinetics according to the Michaelis-Menton scheme.
   D. Determine the effects of inhibitors and activators on Km and Vmax
values.
   E. Describe allosterism and allosteric enzymes.
   F. Compare and contrast the concerted and sequential models for
allosteric enzymes.
   G. Describe zymogen activation.
   H. Explain the different modes of catalytic action in enzymes.
   I. Draw the mechanism for serine proteases.
   J. Classify coenzymes.

V. Describe the Structures and Functions of Lipids and Biological
Membranes
   A. Compare and contrast different classes of lipids.
   B. Describe the structures and properties of fatty acids.
   C. Describe the structures and functions of steroids.
   D. Explain the synthesis of eicosanoids.
   E. List the functions of eicosanoids.
   F. Compare and contrast the functions of the lipid soluble vitamins.
   G. Detail the reactions of the action of vitamin A in the process of
vision.
   H. Describe the composition and structure of membranes.
   I.    Compare and contrast the methods of membrane transport.
   J. Detail the action of the Na+, K+-ATPase.
   K. Describe enzyme receptors and the action of the insulin receptor.

VI. Describe the Structures and Functions of Carbohydrates
   A. Describe the structures of common monosaccharides and
disaccharides.
   B. Compare and contrast the structures and functions of
polysaccharides.

VII. Relate Principles of Thermodynamics to Biological Systems
   A. Relate thermodynamic properties to equilibrium and spontaneity of
chemical reactions.
   B. Calculate the change in free energy for systems not at equilibrium
and not at standard conditions.
   C. Calculate the ?GEN from equilibrium constant data (or an equilibrium
constant from ?GEN data).
   D. Calculate the ?GEN from standard reduction potentials.
   E. List high energy groups utilized in metabolism.
   F. Compare and contrast catabolic and anabolic pathways in metabolism.

VIII. Describe the Pathways Involved with Carbohydrate Metabolism
   A. Write the reactions of glycolysis.
   B. Discuss the energetics involved with glycolysis.
   C. Describe the regulation of glycolysis including activators and
inhibitors of the major regulatory enzymes.
   D. Write the reactions involved with glycogen metabolism.
   E. Describe the control of glycogen metabolism including the effect of
the c-AMP cascade.
   F. Write the reactions involved with gluconeogenesis.
   G. Describe how glucagon can affect the control of the reactions of
glycolysis and
gluconeogenesis in liver cells.
   H. Describe the major products of the pentose phosphate shunt and write
the overall reaction of the pathway.
   I. Detail the steps involved with the reaction of pyruvate in the
pyruvate dehydrogenase complex.
   J. Describe the regulation of the pyruvate dehydrogenase complex
including the   activators and inhibitors of enzymes in the complex.
   K. Write the reactions of the citric acid cycle.
   L. Describe the regulation of the citric acid cycle including
activators and inhibitors of the major regulatory enzymes.
   M. Write the reactions involving the entry and exit of metabolites into
and out of the citric acid cycle.
   N. Describe the major reactions occurring in the compartments of the
mitochondria.
   O. Write the reactions of the electron transport system.
   P. Describe the effects that uncouplers and inhibitors of oxidative
phosphorylation have on the production of ATP.
   Q. Describe the chemiosmotic coupling theory and its relationship to
the generation of ATP.
   R. Describe how a proton gradient can be utilized by the ATPase to
drive the production of ATP.
   S. Write the reactions required to oxidize NADH in the cytoplasm under
aerobic conditions.
   T. Explain how the action of cytochrome P450 is involved with oxidation
reactions occurring in the liver.

IX. Describe the Processes Involved in the Light Reactions of
Photosynthesis
   A. Describe the major reactions occurring in the compartments of the
chloroplast.
   B. Describe the photochemical pigments found in the antenna complex.
   C. Explain the role of carotenoids in photoprotection for
photosynthesis.
   D. Explain the steps involved in the principal photochemical events in
the light reactions of photosynthesis.
   E. Write the products of the Z-scheme of the light reactions of
photosynthesis.

X. Describe the Reactions Involved with Lipid Metabolism
   A. Compare and contrast the types of lipoproteins.
   B. Write the reactions involved in the transport of fatty acids into
the mitochondria.
   C. Write the reactions for the catabolism of saturated fatty acids.
   D. Calculate the number of ATP produced from the complete oxidation of
a fatty acid.
   E. Write the reactions for the formation of ketone bodies.
   F. Write the reactions involved with transporting acetyl-SCoA from the
mitochondria to the cytoplasm.
   G. Write the reactions involved with fatty acid synthesis.
   H. Describe the synthesis of the phospholipids and cholesterol.

XI. Describe Reactions Involved with Amino Acid Metabolism
   A. Describe the nitrogen cycle and the reactions of the nitrogenase
complex.
   B. List the ketogenic and glycogenic amino acids.
   C. Draw the mechanism for transamination reactions.
   D. Write the overall reaction of the urea cycle.

XII. Explain Aspects of the Structure of Nucleic Acids
   A. Compare and contrast the structures of purines and pyrimidines.
   B. Describe the structures of nucleotides and nucleosides.
   C. List Chargaff's rules as they apply to the primary structure of
DNA.
   D. Describe the secondary structure of B form DNA.
   E. Compare and contrast the structures of B form DNA and Z form DNA.
   F. Describe the tertiary structures of DNA.
   G. Determine the linking number associated with a piece of DNA.

XIII. Describe the Processes Associated with the Central Dogma Theory of
Molecular Biology
   A. Diagram the central dogma theory of molecular biology.
   B. Describe the processes required to sequence a piece of DNA.
   C. Discuss the experiments which show that replication is
semiconservative.
   D. Describe the processes and reactions necessary to replicate DNA.
   E. Compare and contrast different types of mutations in DNA.
   F. Describe repair mechanisms for DNA.
   G. List the requirements for transcribing a piece of DNA.
   H. Describe the processes and reactions necessary for transcription.
   I. Discuss post-transcriptional modifications of RNA.
   J. Discuss regulation of transcription and the Lac Operon.
   K. Interpret the universal genetic code.
   L. Describe the structures of t-RNA and r-RNA.
   M. Describe the processes and reactions necessary for translation.
   N. List post-translational modifications of proteins.
 
XIV. Describe the Experimental Basis for Recombinant DNA Technology
   A. Describe the experimental procedures for introducing a recombinant
into a host cell.

Examinations/projects      60-70% of grade
Quizzes                    10-20% of grade
Final exam                    20% of grade
       Total                 100%

Final grades will be determined with the following percentage scores based
upon the total number of points obtained:
   A = 90% - 100%
   B = 80% -  89%
   C = 70% -  79%
   D = 60% -  69%
   F =  0% -  59%