Course Descriptions

CHM 100W - World of Chemistry

1. Demonstrate and understanding of fundamental chemical vocabulary and classify matter into categories based on an understanding of chemical and physical properties.
   1. Classify matter by physical state
   2. State the shape and volume characteristics of the three physical states
      1. Classify common samples of matter according to physical state
      2. Identify the processes by which matter changes physical state
      3. Classify materials by physical state at a given temperature through use of reference data
   3. Recognize the application of the scientific method
   4. Based on experimental data, differentiate between elements and compounds
   5. Classify common substances as a mixture or a pure substance
      1. For a pure substance classify as an element or compound
      2. For a mixture classify as homogeneous or heterogeneous
   6. Distinguish between physical and chemical properties and classify examples
   7. Differentiate between metals and nonmetals
      1. Recognize the placement of metals and nonmetals on the Periodic Table
      2. Give typical physical properties of each
      3. Use properties to classify materials as metal or nonmetal
   8. Differentiate between the symbol for an element and a compound
   9. Use Avogadro's Number to convert between number of molecules, formula units, ions,  atomic mass
   10. Perform calculations using scientific notation
   11. Use a reference source on properties of substances to classify a sample substance
2. Explain the importance of units in measurements and perform relevant calculations
   1. Learn metric base units: gram, liter, meter
   2. Recognize the difference between mass and weight
   3. Learn metric prefixes: kilo, centi, milli, micro
   4. Convert between metric units
   5. Convert temperatures between Fahrenheit and Celsius
   6. Interpret data from graphs, charts, and tables
   7. Distinguish between measured numbers and exact numbers
   8. Convert measurements between English and metric units
   9. Calculate density from mass and volume
   10. Experimentally determine the volume of a solid both by direct and indirect methods
   11. Given the parts of one component in a given amount of the total, calculate the per cent of that component
   12. Express and convert between per cent  and decimal values
   13. Learn rules for rounding
3. Demonstrate the relationship between energy changes and changes of state as well as perform appropriate calculations.
   1. Apply the Law of Conservation of Energy
   2. Discuss energy transformation between chemical, mechanical, electrical
   3. Convert between units of energy: calorie, Calorie, and Joule
   4. Use specific heat, temperature and mass in calculations
   5. Differentiate between endothermic and exothermic reactions.
4. Describe the structure of the atom and formation of ions.
   1. Distinguish between elements, compounds, and mixtures in terms of their atomic makeup
   2. State the names, symbols, charges and relative mass for the three subatomic particles
   3. Given the atomic number, state the number of protons and electrons in an atom and use the Periodic Table to identify the element
   4. Describe how anions and cations are formed
   5. Given the number of protons, neutrons and electrons in an ion, write the correct symbol for the ion, including the mass number, atomic number and charge
   6. Using the Periodic Table, identify the following: group, period, metalloid, alkali metal, alkaline  earth metal, halogen, noble gas, inert gas
   7. Describe the trend of nonmetallic or metallic character among elements
   8. List the elements that exist as diatomic molecules
   9. Observe physical properties of some elements and compounds
   10. Use reference data to report physical properties of some elements and compounds.
5. Describe the configuration of electrons within an atom and the resultant availability for chemical reaction.
   1. Recognize significance of electrons in chemical reactions
   2. Recognize the relationship between minimum energy and maximum stability
   3. Describe the nature of attraction and repulsion between subatomic particles
   4. Describe the relationship between the ground state, excited state, and energy being absorbed and released.
   5. Recognize that the light spectrum emitted from an excited atom is unique for a given element
   6. Use the Periodic Table to identify the number of valence electrons for any main group element
   7. Write the Lewis dot structure for any element given the number of valence electrons.
   8. Use trends from the Periodic table to make predictions about properties.
   9. Observe flame tests on several metallic ions and relate to excited state vs. ground state.
   10. Recognize the transition metals on the Periodic Table
6. Describe the role of electrons in chemical bonds and general properties of ionic and molecular compounds.
   1. Differentiate between ionic and molecular compounds
   2. Observe and categorize physical properties of ionic and molecular compounds.
   3. Describe the octet rule and how both ionic or covalent bonding can follow this rule
   4. Recognize the duet rule that applies only to hydrogen
   5. Determine the number of electrons a metal atom will lose to become a cation
   6. Determine the number of electrons a nonmetal atom will gain to become an anion
   7. Using the Periodic Table, predict the charge on an ion
   8. Write formulas for ionic compounds given the charges on the ions
   9. Distinguish between a monatomic ion and polyatomic ion
   10. Recognize the formulas for common polyatomic ions.
   11. Distinguish between single, double and triple covalent bonds and bond strength
   12. Write the Lewis electron dot structures for molecular compounds
   13. Write the Lewis electron dot structures for polyatomic ions
   14. Describe the trends in electronegativity across a period and down a group
   15. Differentiate between ionic, polar and nonpolar bonds based on electronegativity.
   16. Use symbolism to indicate the dipole in a polar covalent bond.
   17. Recognize the shape of a compound based on its Lewis structure and 3-dimensional arrangement.
   18. Determine the relative polarity of a compound based the polarity of its bonds, its Lewis structure and its shape
   19. Determine if a compound will be water soluble or not based on its polarity
   20. Predict the physical property differences between polar and non-polar compounds in terms of attractive forces between molecules
   21. Compare the properties of ionic and molecular compounds
   22. Predict the weight ratio of elements in a compound from the combining ratio of atoms or ions in the compound.
7. Constrict a formula from the name of a compound, and generate a name from a chemical formula.
   1. Name metal ions using both the Stock and Latin root method
   2. Name monatomic anions
   3. Recognize acids
   4. Associate name and formula for binary molecular compounds
   5. Recognize the chemical names for a number of household compounds
   6. Calculate the formula mass for a compound
   7. Calculate percent composition for elements of a compound
8. Represent chemical reactions using balanced equations
   1. Represent reactants and products with appropriate chemical formula
   2. Write and balance equations so that there are equal numbers of atoms of each element on each side of the equation
   3. Develop an activity series and understand its use to predict reactivity
   4. Use double replacement reactions and recognize the significance of the insolubility of some products as a driving force for the reaction
   5. Distinguish between physical change and chemical change and classify examples
9. Perform calculations relating the quantities of chemical reactants and products.  
   1. Interpret a balanced equation to represent the ratio of reactants and products
   2. Use chemical equations and mass balance to predict
      1. Quantities of products from a known quantity of reactant
      2. Quantities of reactants needed to produce a given quantity of product
      3. Given quantities of two reactants, determine the limiting reactant and the excess  reactant
10. Describe the effects of temperature and pressure on the volume of a gas and the relationship for moles of any gas at standard temperature and     
    1. Recognize units of pressure.
    2. Recognize and be able to use the relationship between gas volume, temperature, and pressure
    3. Recognize and use Avogadro’s Law to explain the relationship between the number of particles and gas volume
    4. Recognize the relationship of the Kinetic Molecular Theory to gas behavior
11. Express concentration of solution by various methods and use units of concentration to calculate quantities of solute.
    1. Define solute and solvent
    2. Express and be able to convert concentration of a solution as a % (m/m), parts per million, parts per billion and other appropriate units
    3. Given a %(m/m) concentration, calculate the mass of solute in a given volume or total mass of a solution
    4. Calculate the mass or volume of solute from concentration values
12. Develop laboratory skills, including proper technique for recording measurements with quantity and units consistent with the device. Students will practice safety procedures in a chemical laboratory.
    1. Recognize measuring devices and the significance of a standard reference
    2. Utilize safe laboratory procedures
    3. Recognize common laboratory hazards
    4. Recognize the significance of a Material Safety Data Sheet
    5. Demonstrate the proper use of basic laboratory equipment
    6. Demonstrate the ability to make measurements accurately
    7. Practice basic laboratory techniques such as filtration, distillation, dilution, and others
13. Perform writing tasks to promote learning.
14. Apply chemical principles to everyday/real world examples
15. Demonstrate the learning of concepts through writing.

CHM 101W - Introductory Chemistry

1. Demonstrate understanding of the particulate nature of matter.
   1. Identify the discrete particles in a sample
   2. Differentiate between metallic, ionic, and covalent bonding
   3. Draw or build or describe models of atoms showing nuclear structure
   4. Draw or build or describe models of atoms and ions showing electronic structure
   5. Draw or build or describe Lewis Structure models to convey arrangements of atoms and valence electrons in molecules
   6. Apply VSEPR theory to determine the shapes of molecules (linear through tetrahedral)
   7. Differentiate between atoms, ions, isotopes, molecules, and network solids
   8. Apply naming conventions to write names and formulas for compounds. (ionic, binary covalent compounds, acids, and simple hydrocarbons)
2. Explain the properties and behaviors of matter.
   1. Describe physical states and changes
   2. Describe the concept of density
   3. Explain attractive forces between particles
   4. Describe bonding within a sample of matter
   5. Describe how solutions are formed.
   6. Describe the Kinetic Molecular Theory
   7. Explain nuclear decay and the concept of half-life
   8. Explain electron arrangements/transitions and periodic trends
3. Demonstrate understanding of chemical reactions.
   1. Recognize and use reaction patterns to predict products.
   2. Differentiate between endothermic and exothermic reactions
   3. Construct balanced chemical equations
   4. Explain the significance of a Limiting Reactant
   5. Identify or explain factors that influence reaction rates
4. Explain observations or draw conclusions using quantitative information.
   1. Use scientific notation and significant digits.
   2. Use the metric system and perform unit conversions
   3. Solve quantitative problems involving:
      1. Density
      2. Gas Laws
      3. Stoichiometry
      4. Mole calculations
      5. Solution concentration
      6. Energy
      7. Nuclear half-life
5. Demonstrate laboratory skills.
   1. Use appropriate safety protocols
   2. Use technology associated with a science laboratory
   3. Choose proper equipment for a specific task
   4. Perform measurements with appropriate devices
   5. Record data or observations
   6. Analyze data or results of an experiment
   7. Use evidence to form conclusions
   8. Make decisions using the scientific method 

CHM 105W - Technical Chemistry I

1. Identify the scope of chemical study and implications of industrial and environmental studies    
   1. Identify the major groups of chemicals manufactured in the US.
   2. Classify matter by physical state and identify the processes by which matter changes physical state.
   3. Use a reference source on properties of substances to classify sample substances as to state at a given temperature.
   4. Discuss typical processes for separation of mixtures: sieves, filtration, distillation.
   5. Demonstrate knowledge of chemical language:
      1. use a chemical symbol to determine an element’s name.
      2. understand use of brackets in chemical formula and be able to count atoms.
      3. classify common materials based on formula as element or compound
   6. Distinguish between physical change and chemical properties and changes and classify examples.
   7. Define the following physical properties: density, viscosity, specific gravity, solubility.
   8. Classify top 50 chemicals produced as elements or compounds, inorganic or organic.
   9. Demonstrate safe laboratory procedures; recognize common laboratory hazards.
   10. Explain terms used on a Material Safety Data Sheet including oxidizer, corrosive, reactivity, hygroscopic, sensitizer.
   11. Define and use the terms: atom, atomic (elemental) symbol, boiling point, chemical equation, chemical formula, chemical properties, chemistry, compound, condensation, crystalline solid, element, endothermic reaction, evaporation, exothermic reaction, freezing, fusing, gas, kinetic energy, melting, Law of Conservation of Energy, Law of Conservation of Mass, liquid, matter, mixture, particulate, phase, physical properties, potential energy, precipitate, product, pure substance, reactant, solid, sublimation, vaporization.
   12. Develop computer skills necessary to open files, read Word files, and cut and paste between files.
2. Demonstrate knowledge of measuring techniques and conversion of units in and between SI and English systems of measurement.
   1. Use a calculator for addition, subtraction, multiplication, division, including use of exponents.
   2. Differentiate between accuracy and precision and read measuring devices with linear or dial analog scale (ruler, refractometer), volume (graduate, burette), and digital scale.
   3. Discuss the usefulness of scientific notation and demonstrate the correct use of scientific notation.
   4. Discuss the need for significant figures.
   5. Apply rounding conventions to measured numbers.
   6. Read temperatures on Fahrenheit and Celsius scales and convert between °F and °C.
   7. Use unit conversion method (dimensional analysis) to convert between measurement units.
   8. Use metric base units and prefixes.
   9. Locate sources of conversion information.
   10. Use density to convert between mass and volume.
   11. Calculate specific gravities for liquids and gases.
   12. Calculate volumes of solids with regular dimensions.a. rectangular solid (storage bin, tote); cylindrical solid (tank, pipe, drum); b. sphere (tank)
   13. Discuss the use of tare weights; describe the difference between contained and delivered mass.
   14. Calculate volumes of pipes and tanks from dimensions and convert to gallons, liters.
   15. Manually graph linear data on x and y axis and read data from the graph.
   16. Enter linear data on an Excel spreadsheet, graph data and read data from graph.
   17. Define and use the terms: base unit, conversion factor, density, dimensional analysis, exact number, exponent, mass, scientific notation, significant figure (digit), uncertainty, weight.
3. Demonstrate knowledge of the basic concepts of atomic structure, and relate them to the Periodic Table, electron configuration, formation of ions, and use and relevance of radioactive isotopes.
   1. Discuss the historical development of subatomic particles.
   2. Distinguish between and determine atomic number, atomic mass, mass number.
   3. Calculate average atomic mass of an element from the isotope distribution.
   4. For the following categories of elements: alkali metals, alkaline earth metals, oxygen group, halogens, noble gases, transition metals, metalloids, rare earth metals:
      1. Recognize their placement on the Periodic Table
      2. Discuss general properties of the category
   5. Identify types of radioactive decay (alpha, beta, gamma) and write equations to express alpha and beta decay.
   6. Discuss the difference between fission and fusion.
   7. Describe the relationship between the electromagnetic spectrum and electron energy level changes.
   8. Write electron configurations and discuss their relevance to periodic table.
   9. Determine valence electrons and write appropriate Lewis Dot structures for elements.
   10. Predict trends in properties from the periodic table.
   11. Define and apply the terms: anion, cation, chemical family, electron configuration, excited state, ground state, ion, ionization energy, isoelectronic, Lewis dot symbols, metal, nonmetal, octet rule, orbital, Pauli exclusion principle, photon, principal energy level, quantized energy levels, semimetal, spectrum, sublevels s, p, d, f, valence electrons
4. Demonstrate an understanding of the similarities and differences between ionic and covalent bonds as well as polarity within bonds and molecules.
   1. Predict ionic charge for monatomic ions.
   2. Write formulas for ionic compounds.
   3. Describe the transfer of electrons to form ions when a metal and a nonmetal react.
   4. Describe the concept of sharing of electrons to form a covalent bond when two nonmetals react.
   5. Use electronegativities to distinguish between polar and nonpolar covalent bonds.
   6. Describe ionic attraction and lattice structure characteristics.
   7. Describe the difference between polar bonds and polar molecules, and show how polarity of bonds affects solubility.
   8. Use Periodic Table to predict bond character: ionic, polar covalent, nonpolar.
   9. Describe the difference between single, double and triple bonds (multiple bonds).
   10. Identify exceptions to the octet rule.
   11. Describe metallic bonds.
   12. Recognize common alloys.
   13. Define and use the terms: alloy, anion, bond, bond dissociation energy, bonding pair of electrons, cation, chemical bond, covalent bond, covalent compound, dipole, double bond, electronegativity, ionic bond, lattice structure, lone pair of electrons, molecular compound, molecule, monatomic ion, multiple bond, nonbonding pair of electrons, nonpolar covalent bond, octet rule, polar covalent bond, polar bond, polyatomic ion, single bond, triple bond.
5. Cross-reference chemicals by name, formula, common name, trade name and CAS number.
   1. Discuss the need for learning chemical nomenclature.
   2. Use appropriate molecular formula for elements that occur as diatomic molecules.
   3. Correctly name and write formulas for compounds made from two nonmetals.
   4. Correctly name and write symbols for monatomic ions with single or multiple charges including use of Stock naming convention to indicate charge on transition metal ions.
   5. Correctly name and write symbols for acid compounds including: nitric acid, chloric acid, bromic acid, iodic acid, manganic acid, carbonic acid, sulfuric acid, chromic acid, and phosphoric acid.
   6. Write formulas for compounds containing the ions: ammonium ion, hydroxide ion, cyanide ion, acetate ion, oxalate ion, chromate ion, dichromate ion
   7. Correctly name and write symbols for ternary salts and hydrates.
   8. Discuss use of common names.
   9. Use a hard-copy reference as well as the Internet to cross-reference compounds by:
      1. chemical name
      2. CAS number
      3. chemical formula
      4. common name
      5. trade-name
   10. Define and use the terms: acid, anhydrous compound, anion, binary ionic compound, binary molecular compound, cation, diatomic molecule, hydrate, hydrated, ion, ionize, monatomic ion, oxyacid, oxyanion.
6. Recognize the types of chemical reactions, and write and interpretchemical equations.
   1. Write and balance simple chemical equations.
   2. Given a balanced chemical equation, describe its meaning on the particular, molar, and macroscopic level.
   3. Classify chemical reactions as one or more of the following: combination or synthesis, combustion, decomposition, single or double replacement, neutralization.
   4. Predict solubility of compounds in a reaction from a table.
   5. Define and use the terms: aqueous solution, balanced equation, combination reaction, combustion reaction, decomposition reaction, double replacement reaction, neutralization reaction, precipitation reaction, single replacement reaction, synthesis reaction.
7. Distinguish between the types of chemical processes, using material balancing, a factors affecting a reaction.
   1. Determine the number of atoms of each element in a formula.
   2. Calculate the molecular mass and formula mass in atomic mass units (amu).
   3. Describe the concept of the mole and calculate molar mass in grams.
   4. Convert between mass, moles, and number of particles.
   5. Calculate percent composition for the elements in a compound.
   6. Use molar mass and the coefficients of balanced equations to predict quantities of reactants and products.
   7. Use molecular weights and stoichiometric relationships to perform calculations to predict quantities of chemicals to be reacted/produced.
   8. Given the expected (calculated, theoretical) yield, calculate the percent yield for a reaction.
   9. Identify limiting reactant situations and predict the theoretical amount of product, and amount of remaining excess reactant.
   10. Convert between the following units of energy: calorie, joule, kilocalorie, kilojoules.
   11. Calculate heat energy as a reactant or product.
   12. Discuss factors that may limit the reactions (mass of reactant, product, vessel size, time, mixing capability).
   13. Discuss factors that may influence and how they influence the reaction rate: temperature, pressure, concentration, surface area.
   14. Discuss the role of catalysts in affecting the rate of reaction.
   15. Discuss the characteristics of a chemical system in an equilibrium state.
   16. Identify conditions that affect the rate of a chemical reaction: temperature, catalyst, concentration.
   17. Apply Le Chatelier’s Principle: concentration, volume, and temperature effects.
   18. Identify examples of catalysts used in industrial processes, and describe the implications of poisoning the catalyst.
   19. Describe the role of equilibrium in controlling a chemical process.
   20. Discuss shifting equilibrium by removing product from the reaction mix
   21. Discuss water treatment reactions: ion-exchange resins / demineralizers.
   22. Define and use the terms: adsorption, balanced equation, catalyst, chemical equation, chemical reaction, distillation, endothermic reaction, equilibrium, equilibrium point, equilibrium reaction, exothermic reaction, limiting factor, material balancing, poisoned catalyst, process, process variable, product, raw material, reactants, reaction rate, reactor.
8. Explain the expressions for concentration of solutions and the physical and chemical properties of common acids and bases.
   1. Define the properties of a solution.
   2. Use the terminology associated with solutions.
   3. Discuss factors that affect solubility.
   4. Calculate and use percent by mass concentration as a conversion factor.
   5. Calculate and use parts per million (and billion) as a conversion factor.
   6. Express solution concentration in molarity and use molarity as a conversion factor.
   7. Calculate the desired quantity of a concentrated solution to use to make known quantity of a dilute solution.
   8. Perform the calculations associated with a titration.
   9. Review structure of acids, bases, salts.
   10. Discuss the concept of a pH scale and interpret a pH as being acidic or basic.
   11. Calculate pH or pOH from molarity of an acid or base and molarity of an acid or base from pH of pOH.
   12. Identify physical properties, uses and hazards of common acids and bases.
   13. Describe the formations of acids from nonmetal oxides and the formation of bases from metal oxides.
   14. Describe the industrial purification of salts by crystallization.
   15. Use an acid/base indicator to indicate pH.
   16. Use pH meter to measure common substances.
   17. Perform an acid/base neutralization reaction using an indicator.
   18. Perform the same neutralization reaction using a pH meter and graph the pH vs. milliliters of titrant.
   19. Define and use the terms: concentrated, dilute, immiscible, indicator, miscible, pH, pOH, saturated, solute, solubility, solvent, supersaturated, titrant, titration, unsaturated.
9. Describe implications of intermolecular forces on physical properties as well as the utilization of physical methods for process optimization.   
   1. Explain the meaning of: calorie, Calorie (large calorie), BTU, bar, mm Hg, atm
   2. Describe the separation concepts for the following purification techniques:
      1. Distillation
      2. Liquid/ liquid extraction
      3. Filtration
   3.  Identify states of matter.
   4. Discuss properties of solids.
   5. Define crystalline vs. amorphous.
   6. Distinguish between metals and nonmetals
   7. Discuss properties of liquids.
      1. Solubility
      2. Define terms: concentration, saturated, supersaturated, solute, solvent
      3. Discuss effects of polarity, temperature, mixing, solubility, filtration, and distillation
   8. Define and use the terms: latent heat, sensible heat, absorption, adsorption, leaching, extracting solvent, carrier solvent, vapor pressure, upper cut point, lower cut point, refluxing,reboiling.
10. Practice general education abilities within the context of course.
    1. Write accurate lab reports reflecting data collected
    2. Analyze data and draw appropriate conclusions
    3. Report results of work to class orally
    4. Evaluate validity of internet source materials
    5. Demonstrate teamwork skills both in small class groups and while working in lab groups.
    6. Use computers effectively to retrieve information from files, create word-processed documents, create basic spreadsheets including graphs, retrieve information from the Internet, and utilize email including attachments.
11. Perform writing tasks to promote learning.
12. Write effectively for a specific audience and purpose.
13. Demonstrate the learning of concepts through writing.

CHM 106W - Technical Chemistry II

1. Regain familiarity with general chemistry concepts needed for understanding of introductory organic chemistry.
   1. Understand atomic structure including subatomic particles and electron configuration
   2. Use electronegativity to predict the nature of bonds as either covalent or ionic and be able to represent with appropriate Lewis Dot structures
   3. Recognize the common notations for isotopes
   4. Understand atomic mass and the relationship to molar mass
   5. Recognize the relationship between empirical and molecular formulas
   6. Differentiate between acids and bases in accordance with the Arrhenius, Bronsted-Lowry and Lewis theories
   7. Understand oxidation, reduction, oxidizing agent, reducing agent
   8. Understand occurrence and significance of hydrogen bonding
2. Understand the structure, nomenclature and some reactions of saturated hydrocarbons.  
   1. Describe the tetrahedral nature of the carbon atom
   2. Explain the role of hybridization in formation of single bonds around the carbon atom
   3. Express alkanes and halogenated alkanes as Lewis structures
   4. Know the IUPAC names and formulas for the C1-C10 alkanes
   5. Become familiar with both natural sources and commercial uses of alkanes
   6. Understand isomerization
   7. Recognize the utility of structural formulas, condensed formulas, Lewis structures, ball and stick models and space-filling models
   8. Write structural formulas and IUPAC names for the isomers of an alkane or halogenated alkane
   9. Learn common names for short chain branched alkanes
   10. Give the IUPAC name of a hydrocarbon or a halogenated hydrocarbon when given the structural formula
   11. Give the structural formula of a hydrocarbon or a halogenated hydrocarbon when given the IUPAC name
   12. Write equation for the halogenation of an alkane including all possible mono-substituted  product isomers
   13. Write structure formulas and names for cycloalkanes C3-C6.
   14. Understand the two conformations for cyclohexane.
   15. Understand the derivation and utility of the octane number system
   16. Understand and be able to use the following terms: acyclic, alkane, alkyl group, axial position, CFCs, catalytic cracking, conformational isomer, cycloalkane, equatorial, functional group, halide, halogenated, homologous series, hydrocarbon, isomer, isomerism, monosubstitution, paraffin, petrochemical, saturated, sigma bond, unsaturated
3. Understand the structure, nomenclature and some reactions of unsaturated hydrocarbons.    
   1. Explain the sp2 and sp hybridization of carbon atoms and the formation of a pi bond, double and triple bonds
   2. Distinguish, by formulas, the difference between saturated and unsaturated hydrocarbons
   3. Name and write structural formulas of alkenes, alkynes, cycloalkenes, and aromatic compounds
   4.  Determine from structural formulas whether a compound can exist as geometric isomers
   5. Correctly use the terms “cis” and “trans” to describe isomers
   6. Write equations representing addition reactions of alkenes and alkynes
   7. Explain the formation of carbocations and their role in chemical reactions
   8. Understand Markovnikov’s rule for addition of HCl, HBr, HI, and H+/H2O to alkenes and alkynes
   9. Recognize the results of the Baeyer test for unsaturation
   10. Explain simple chemical tests that can be used to differentiate between alkanes, alkenes, and alkynes
   11. Compare benzene structure and properties to cyclohexane
   12. Relate IUPAC names for substituted benzene compounds to structural formulas
   13. Write equations for the following reactions of benzene compounds
   14. Halogenation with chlorine or bromine
   15. Nitration
   16. Friedel-Crafts Alkylation
   17. Oxidation of side chains
   18. Understand and be able to use the following terms: alkene, alkyne, aromatic compound, geometric isomer, cycloalkene, cracking, pyrolysis, dehydration, addition reaction, carbocation, Markovnikov’s rule
4. Have an understanding of the structure, nomenclature and some reactions of alcohols, ethers, phenols and thiols.
   1. Name alcohols, ethers, phenols and thiols by common and IUPAC methods
   2. Write the structural formula for the above when given the name
   3. Recognize and identify primary, secondary and tertiary alcohols.
   4. Understand the common sources, means of preparation, uses and hazards for common alcohols, ethers, phenols and thiols
5. Have an understanding of the structure, nomenclature and some reactions of aldehydes and ketones.   
   1. Recognize the aldehyde and ketone functional groups within a molecule
   2. Name aldehydes and ketones by common and IUPAC methods
   3. Write formulas of aldehydes and ketones when given their names
   4. Write equations showing the oxidation of alcohols to aldehydes and ketones
6. Understand the structure, nomenclature and some reactions of carboxylic acids and esters
   1. Give the common and IUPAC names of selected carboxylic acids
   2. Write the structural formulas for saturated, unsaturated, aromatic and dicarboxylic carboxylic acids
   3. Understand correlation between molecular mass and the properties of solubility in water and boiling point
   4. Write equations for the preparation of carboxylic acids by:
   5. Oxidation of alcohols and aldehydes
   6. Hydrolysis of esters
   7. Saponification of fats
   8. Oxidation of aromatic hydrocarbons
   9. Write equations for the reactions of carboxylic acids to form salts and esters
   10. Write common names, IUPAC names and formulas of esters
   11. Identify the portion of an ester that is derived from a carboxylic acid and the portion derived from an alcohol
   12. Compare and contrast the cleansing action of a soap and synthetic detergent
   13. Recognize differences in the composition of natural fats and oils and the effect on the properties of the triacylglycerols (triglycerides, fats).
   14. Differentiate between: fat and oil; salt of a carboxylic acid and a soap; hydrogenation, hydrogenolysis, hydrolysis and saponification; cationic, anionic and nonionic surfactants,
7. Have an appreciation for the utility of polymers and an understanding of the relationship between structure and function.
   1. Recognize naturally occurring polymers including fibers
   2. Be able to represent polymers in terms of their repeating units
   3. Write formulas for condensation polymers, given the monomer
   4. Identify polymers from their tradenames using standard reference materials
   5. Recognize characteristics of common polymeric materials and thereby classify the polymer into major categories such as polyethylene, polystyrene, polyurethane, silicone polymer, PET, etc.
   6. Demonstrate understanding of the functional characteristics of common polymers
   7. Understand the difference between addition and condensation polymers
   8. Understand thermoset vs. thermoplastic resins
   9. Differentiate between a polymeric fiber, resin and film.
   10. Understand the role of polymer additives
   11. Recognize the role of polymer properties in determining recycling capability
8. Understand of the relationship between structure and function of amide and amine compounds.
   1. Recognize the amide functional group
   2. Use IUPAC nomenclature system for amides
   3. Predict hydrolysis products of amides in acid and base solutions
   4. Recognize the amine functional group
   5. Recognize heterocyclic compounds and be able to name using reference information
   6. Appreciate the uses of urea and the alkaloid group of pharmaceuticals.
9. Understand of the relationship between structure and function of carbohydrates and lipids.  
   1. Recognize optical isomers
   2. Classify carbohydrates as monosaccharide, disaccharide, oligosaccharide and polysaccharide
   3. Differentiate between glucose and fructose
   4. Describe hydrolysis of disaccharides
   5. Recognize the significance of sugars and sugar substitutes
   6. Discuss the utility of polysaccharides (polymers) starch and cellulose
   7. Recognize the classification of lipids as being simple lipids, compound lipids, steroids or fat-soluble vitamins
10. Understanding of the relationship between structure and function of amino acids, polypeptides and proteins.
    1. Recognize foods that are major sources of protein
    2. List the elements usually contained in protein molecules
    3. Recognize the names of the amino acids and be able to use a reference to determine their structure; identify the functional groups present
    4. Predict the structure of a peptide linkage between two amino acids
    5. Differentiate between primary and secondary structure of a protein
    6. Discuss the role of enzymes in biodegradation
11. Work independently to locate chemical information and analyze data effectively.    
    1. Use reference books to locate physical and chemical properties as well as safety information.
    2. Use internet search engines to locate chemical information above and also vendor information, career opportunities, and opinions on social issues regarding chemicals.
    3. Evaluate the credibility of information retrieved from the internet
    4. Understand the implementation of risk assessment
    5. Determine the information required to make a chemical decision
    6. Make decisions based on data and observations
    7. Pay close attention to detail and observe trends
    8. Have a general understanding of the considerations in choosing a chemical container  (sampling size or industrial)
    9. Utilize appropriate sampling techniques
    10. Understand the concept of calibrating an instrument against a standard
    11. Use chemical principles to explain observed phenomena
    12. Follow a standard operating procedure
12. Perform writing tasks to promote learning.
13. Write effectively for a specific audience and purpose.
14. Demonstrate the learning of concepts through writing.

CHM 107 - Chemistry For Engineering Technology

1. Relate the effects of temperature and pressure on the volume of a gas and the moles of any gas at standard temperature and pressure.    
   1. Convert between temperatures expressed in Celsius and Kelvin
   2. Convert between pressure expressed in atmospheres, torr, mm Hg
   3. Observe the relationship between volume and pressure for a gas
   4. State Boyle’s Law and express mathematically
   5. Given a change of pressure, calculate the change of volume and the reverse
   6. Recognize the significance of the partial pressure of water vapor in measuring the pressure of a gas collected by displacement of water
   7. Observe the relationship between temperature and volume for a gas
   8. State Charles’ Law and express mathematically
   9. Given a change of temperature, calculate the change of volume and the reverse
   10. Combine application of Boyle’s Law and Charles’ Law; use Combined Gas Law
   11. Use the Ideal Gas Law to solve for pressure, volume, number of moles, or temperature
   12. Recognize Avogadro’s Law and understand that at any given temperature and pressure, there are an equal number of moles of any gas in an equal volume
   13. Recognize that at standard temperature and pressure (273 Kelvin, 760 mm Hg), 1 mole of a gas has a volume of 22.4 L
   14. Use the density relationship to calculate molar mass (g/mole) using the Ideal Gas Law
   15. Use molar mass and the Ideal Gas Law to calculate density of a gas at a given temperature and pressure
   16. Given a balanced chemical equation, the mass of one reactant or product, and the T and P of a gaseous reactant or product, calculate the volume of the gaseous reactant or product.
   17. Given a balanced chemical equation, the volume of a gaseous reactant or product and a given T and P, calculate the mass of another reactant or product
   18. Understand the applications of Kinetic Molecular Theory to gases
   19. Recognize the relationship of the Kinetic Molecular Theory to Boyle’s Law, Charles’ Law, and Dalton’s Law of Partial Pressures
   20. Define and be able to use the following terms: atmosphere, torr, partial pressure, standard temperature, standard pressure, molar gas volume, universal gas constant, ideal gases
   21. Recognize the difference between an Ideal Gas and a real gas.
2. Express concentration of solution by various methods and use units of concentration to calculate quantities of solute.
   1. Define solute and solvent
   2. Define and be able to use the following terms: soluble, insoluble, solubility, saturated, unsaturated, dilute, concentrated, miscible, immiscible, concentration, molarity
   3. Express concentration of a solution as a % (m/m)
   4. Given a %(m/m) concentration, calculate the mass of solute in a given volume
   5. Calculate the mass of solute and solvent to prepare a given % (m/m) solution.
   6. Calculate the mass of solute and volume of solvent to prepare a given % (m/v) solution
   7. Calculate the volume of solute and solvent to prepare a given % (v/v) solution
   8. Convert between % and ppm
   9. For a given molarity solution, calculate the mass of solute required / L
   10. For a given molarity and volume, calculate the number of moles of solute
   11. Calculate the volume of a solution with a specified molarity to deliver a given amount of solute
   12. Given the molarity and volume of a concentrated solution, calculate the volume required to prepare a dilute solution of a specified molarity
   13. For a given molality solution, calculate the mass of solute required/ 1000 g of solvent
3. Explain the structure, nomenclature and some reactions of carboxylic acids and esters.
   1. Give the common and IUPAC names of selected carboxylic acids
   2. Write the structural formulas for saturated, unsaturated, aromatic and dicarboxylic carboxylic acids
   3. Understand correlation between molecular mass and the properties of solubility in water and boiling point
   4. Write equations for the preparation of carboxylic acids by:
      1. Oxidation of alcohols and aldehydes
      2. Hydrolysis of esters
      3. Saponification of fats
   5. Oxidation of aromatic hydrocarbons
   6. Write equations for the reactions of carboxylic acids to form salts and esters
   7. Write common names, IUPAC names and formulas of esters
   8. Identify the portion of an ester that is derived from a carboxylic acid and the portion derived from an alcohol
   9. Compare and contrast the cleansing action of a soap and synthetic detergent
   10. Recognize differences in the composition of natural fats and oils and the effect on the properties of the triacylglycerols (triglycerides, fats).
   11. Differentiate between: fat and oil; salt of a carboxylic acid and a soap; hydrogenation, hydrogenolysis, hydrolysis and saponification; cationic, anionic and nonionic surfactants,
4. Differentiate characteristics of the atomic structure and molecular arrangement of common engineering materials.
   1. Identify characteristics of the following lattice structures of metals and why they form from a molten state:
      1. Face-center-cubic (FCC)
      2. Body-center-cubic (BCC)
      3. Hexagonal close packed (HCP)
   2. List at least 3 common metals within each group (FCC, BCC, HCP).
   3. Compare the formation of a pure metal from a molten state with that of an alloy.
   4. Identify characteristics of the amorphous structure of glass and ceramics.
5. Explain the utility of polymers and of the relationship between structure and function.
   1. Recognize naturally occurring polymers including fibers
   2. Represent polymers in terms of their repeating units
   3. Write formulas for condensation polymers, given the monomer
   4. Identify polymers from their tradenames using standard reference materials
   5. Recognize characteristics of common polymeric materials and thereby classify the polymer into major categories such as polyethylene, polystyrene, polyurethane, silicone polymer, PET, etc.
   6. Demonstrate understanding of the functional characteristics of common polymers
   7. Understand the difference between addition and condensation polymers
   8. Understand thermoset vs. thermoplastic resins
   9. Differentiate between a polymeric fiber, resin and film.
   10. Understand the role of polymer additives
   11. Recognize the role of polymer properties in determining recycling capability
6. Identify the relative importance of chemical bonding in engineering materials.
   1. Differentiate between the 4 types of bonds-Covalent, Ionic, Metallic, Vanderwaal.
   2. Identify how each of the 4 bonds can be most easily broken.
   3. Explain how slip planes and lattice structure defects in metals can be used to break bonds and reshape metals.
7. Explain how engineering materials degrade over time.
   1. Explain what happens when you place 2 dissimilar metals in contact with each other.
   2. Explain the process involved in the rusting of ferrous metals.
   3. Explain the process of oxidation of aluminum.
   4. Explain the process of degradation of plastics due to chemicals and heat.
8. Explain the relationship between structure and function of carbohydrates and lipids.
   1. Recognize optical isomers
   2. Classify carbohydrates as monosaccharide, disaccharide, oligosaccharide and polysaccharide
   3. Differentiate between glucose and fructose
   4. Describe hydrolysis of disaccharides
   5. Recognize the significance of sugars and sugar substitutes
   6. Discuss the utility of polysaccharides (polymers) starch and cellulose
   7. Recognize the classification of lipids as being simple lipids, compound lipids, steroids or fat-soluble vitamins
9. Explain the operation of commonly-used batteries.
   1. Identify the role of the anode, cathode, and electrolyte.
   2. Explain how a common flashlight battery works.
   3. Compare lead-acid storage battery operation with more recently-developed battery types.
10. Explain the process of chemical etching in manufacture.
    1. Explain how chemical etching is done on flat surfaces.
    2. Explain how chemical etching is used in building printed circuit boards for microchips in the semiconductor industry.
11. Identify the characteristics of liquid engineering materials.    
    1. Compare the chemical formulations of the following hydraulic fluids:
       1. petroleum oils
       2. phosphate esters
       3. chlorinated hydrocarbons
       4. alcohol
    2. Identify whether the fluids in (1) above are chemically compatible with the following seal materials:
       1. rubber
       2. thermoplastic
       3. thermoset
       4. cork
       5. wood
       6. cast iron

CHM 111 - General Chemistry I

1. Demonstrate understanding of the particulate nature of matter.
   1. Identify the discrete particles in a sample
   2. Differentiate between metallic, ionic, and covalent bonding
   3. Draw or build or describe models of atoms showing nuclear structure
   4. Draw or build or describe models of atoms and ions showing electronic structure
   5. Apply VSEPR theory to determine the shapes of molecules (linear through octahedral)
   6. Draw or build or describe Lewis and line structure models to convey arrangements of atoms and valence electrons in molecules
   7. Differentiate between atoms, ions, isotopes, molecules, network solids
   8. Apply naming conventions to write names and formulas for compounds. (ionic, binary covalent compounds, acids, and organic compounds)
   9. Identify common organic functional groups
2. Explain the properties and behaviors of matter.
   1. Describe phase changes
   2. Explain the concept of density
   3. Explain attractive forces between particles
   4. Describe bonding within a sample of matter
   5. Describe how solutions are formed.
   6. Describe the Kinetic Molecular Theory
   7. Explain nuclear decay and the concept of half-life
   8. Explain electron arrangements and periodic trends
3. Demonstrate understanding of chemical reactions.
   1. Recognize and use reaction patterns to predict products.
   2. Describe the significance of entropy, enthalpy, and Gibbs free energy
   3. Construct balanced chemical equations
   4. Explain the significance of a Limiting Reactant
   5. Identify or explain factors that influence reaction rates
   6. Write equilibrium equation and mass action expressions
   7. Describe the relationship between K and the position of the equilibrium
   8. Use Le Chatelier’s principle to predict the effects of a disturbance in an equilibrium
   9. Write ionization/dissociation equations for acids, bases, and ionic compounds
   10. Classify reactions as an oxidation-reduction reaction
   11. Assign oxidation numbers to atoms in reactions
   12. Describe the function of a buffer
4. Explain observations or draw conclusions using quantitative information.
   1. Use significant digits.
   2. Use the metric system and perform unit conversions
   3. Solve quantitative problems involving:
      1. Gas Laws
      2. Stoichiometry
      3. Mole calculations
      4. Solution concentration
      5. Energy
      6. Density
      7. pH and pOH, K_w, pK_a
      8. Electromagnetic energy
5. Demonstrate laboratory skills.
   1. Use appropriate safety protocols
   2. Use technology associated with a science laboratory
   3. Choose proper equipment for a specific task
   4. Perform measurements with appropriate devices
   5. Record data or observations
   6. Analyze data or results of an experiment
   7. Use evidence to form conclusions
   8. Make decisions using the scientific method 

CHM 111H - General Chemistry I - Honors

1. Demonstrate understanding of the particulate nature of matter.
   1. Identify the discrete particles in a sample
   2. Differentiate between metallic, ionic, and covalent bonding
   3. Draw or build or describe models of atoms showing nuclear structure
   4. Draw or build or describe models of atoms and ions showing electronic structure
   5. Apply VSEPR theory to determine the shapes of molecules (linear through octahedral)
   6. Draw or build or describe Lewis and line structure models to convey arrangements of atoms and valence electrons in molecules
   7. Differentiate between atoms, ions, isotopes, molecules, network solids
   8. Apply naming conventions to write names and formulas for compounds. (ionic, binary covalent compounds, acids, and organic compounds)
   9. Identify common organic functional groups
2. Explain the properties and behaviors of matter.
   1. Describe phase changes
   2. Explain the concept of density
   3. Explain attractive forces between particles
   4. Describe bonding within a sample of matter
   5. Describe how solutions are formed.
   6. Describe the Kinetic Molecular Theory
   7. Explain nuclear decay and the concept of half-life
   8. Explain electron arrangements and periodic trends
3. Demonstrate understanding of chemical reactions.
   1. Recognize and use reaction patterns to predict products.
   2. Describe the significance of entropy, enthalpy, and Gibbs free energy
   3. Construct balanced chemical equations
   4. Explain the significance of a Limiting Reactant
   5. Identify or explain factors that influence reaction rates
   6. Write equilibrium equation and mass action expressions
   7. Describe the relationship between K and the position of the equilibrium
   8. Use Le Chatelier’s principle to predict the effects of a disturbance in an equilibrium
   9. Write ionization/dissociation equations for acids, bases, and ionic compounds
   10. Classify reactions as an oxidation-reduction reaction
   11. Assign oxidation numbers to atoms in reactions
   12. Describe the function of a buffer
4. Explain observations or draw conclusions using quantitative information.
   1. Use significant digits.
   2. Use the metric system and perform unit conversions
   3. Solve quantitative problems involving:
      1. Gas Laws
      2. Stoichiometry
      3. Mole calculations
      4. Solution concentration
      5. Energy
      6. Density
      7. pH and pOH, Kw, pKa
      8. Electromagnetic energy
5. Demonstrate laboratory skills.
   1. Use appropriate safety protocols
   2. Use technology associated with a science laboratory
   3. Choose proper equipment for a specific task
   4. Perform measurements with appropriate devices
   5. Record data or observations
   6. Analyze data or results of an experiment
   7. Use evidence to form conclusions
   8. Make decisions using the scientific method 
6. Practice independent, intellectual curiosity.
   1. Complete at least one significant project which demonstrates higher level, academic rigor.
7. Apply higher level, critical thinking skills to deepen understanding of course material.
   1.  Actively engage with peers in discussions, seminars, or other formats to enhance the depth of knowledge of the relevant material.

CHM 112 - General Chemistry II

1. Explain the properties and behaviors of matter.
   1. Describe bonding within a sample of matter
   2. Describe how solutions form
   3. Explain nuclear decay and the concept of half-life
2. Demonstrate understanding of chemical reactions.
   1. Recognize and write an autoionization reaction
   2. Explain the significance of a limiting reactant
   3. Identify or explain factors that influence reaction rates
   4. Write equilibrium, constant expressions, and equilibrium constants
   5. Use Le Chatelier’s principle to determine the effects of equilibrium on a reaction
   6. Identify and write acid/base conjugate pairs
   7. Balance aqueous redox reactions in acidic and basic solutions
   8. Explain concepts of reaction mechanisms, molecularity, and rate-determining steps
3. Explain observations or draw conclusions using quantitative information.
   1. Solution concentration
   2. Energy
   3. Colligative Properties
   4. Acid-Base Calculations
   5. Nuclear half-life
   6. Solubility
   7. Quantum chemistry
   8. Kinetics
   9. Equilibrium
   10. Electrochemistry
4. Demonstrate laboratory skills.
   1. Use appropriate safety protocols
   2. Use technology associated with a science laboratory
   3. Choose proper equipment for a specific task
   4. Perform measurements with appropriate devices
   5. Record data or observations
   6. Analyze data or results of an experiment
   7. Use evidence to form conclusions
   8. Make decisions using the scientific method 

CHM 112H - General Chemistry II - Honors

1. Explain the properties and behaviors of matter.
   1. Describe bonding within a sample of matter
   2. Describe how solutions form.
2. Demonstrate understanding of chemical reactions.
   1. Recognize and write an autoionization reaction
   2. Explain the significance of a limiting reactant
   3. Identify or explain factors that influence reaction rates
   4. Write equilibrium, constant expressions, and equilibrium constants
   5. Use Le Chatelier’s principle to determine the effects of equilibrium on a reaction
   6. Identify and write acid/base conjugate pairs
   7. Balance aqueous redox reactions in acidic and basic solutions
   8. Explain concepts of reaction mechanisms, molecularity, and rate-determining steps
3. Explain observations or draw conclusions using quantitative information.
   1. Solution concentration
   2. Energy
   3. Colligative Properties
   4. Acid-Base Calculations
   5. Nuclear half-life
   6. Solubility
   7. Quantum chemistry
   8. Kinetics
   9. Equilibrium
   10. Electrochemistry
4. Demonstrate laboratory skills.
   1. Use appropriate safety protocols
   2. Use technology associated with a science laboratory
   3. Choose proper equipment for a specific task
   4. Perform measurements with appropriate devices
   5. Record data or observations
   6. Analyze data or results of an experiment
   7. Use evidence to form conclusions
   8. Make decisions using the scientific method 
5.  Practice independent, intellectual curiosity.
   1. Complete at least one significant project which demonstrates higher level, academic rigor.
6. Apply higher level, critical thinking skills to deepen understanding of course material.
   1. Actively engage with peers in discussions, seminars, or other formats to enhance the depth of knowledge of the relevant material.

CHM 210 - Organic Chemistry I

1. Communicate effectively.
   1. Demonstrate understanding by reading, speaking, and writing.
   2. Employ critical writing and active listening to obtain or convey information.
   3. Collect and analyze data.
   4. Identify trends, solve problems, and conclude logically by integrating concepts.lusions.
2. Demonstrate understanding of fundamental concepts of bonding and molecular structure
   1. Describe atoms in terms of atomic structure, orbital electrons configurations and chemical bonding theory.
   2. Explain the basic principles of ionic and covalent bonding.
   3. Describe the relationship of acids, bases, electrophiles and nucleophiles to the reactivity of organic molecules.
   4. Draw and explain resonance structures and formal changeof organic molecules and dipole moments of covalent bonds.
   5. Predict the formation of polar bonds and polar molecules based on electronegativity.
   6. Use the concept of orbital hybridization to describe bonding in organic molecules.
3. Demonstrate the understanding of basic structures and properties of organic molecules.
   1. Recognize and identify the common organic functional groups and their elemental components.
   2. Use line bonds diagrams to explain chemical structures.
   3. Determine the degrees of unsaturation of a molecule.
   4. Describe the stability, bonding structure and physical properties of alkane, alkene, alkyne, alkyl halides and organometallic compounds.
   5. Explain the stability of aromatic systems using resonance, the importance of aromaticity, and anti-aromatic and non-aromatic compounds
4. Apply the fundamental rules of nomenclature.
   1. Name and draw the homologous series of alkanes and alkyl groups for the first twelve carbons in the series (C1 through to C12).
   2. Use the rules to name and draw cycloalkanes, alkenes, alkynes, alkyl halides, substituted benzenes, aromatic and organometallic compounds.
5. Demonstrate an understanding of alkane and cycloalkane conformers.
   1. Draw staggered and eclipsed conformers of various alkanes to illustrate their stability
   2. Explain steric and torsional strain of different alkane and cycloalkane conformations.
   3. Draw and identify the axial and equatorial bonds in various cycloalkanes.
   4. Explain the conformational mobility of cyclohexane and its substituted derivatives that produces chair conformers from ring flipping
6. Demonstrate an understanding of the important concepts of stereochemistry.
   1. Explain chiral and achiral molecules, enantiomers and racemates.
   2. Explain optical activity dextrorotatory, levorotatory, specific rotation and plane polarized light.
   3. Draw and name isomers from a given chemical formula.
   4. Classify and draw E and Z stereoisomers of alkenes.
   5. Classify and draw cis and trans stereoisomers of cycloalkanes.
   6. Classify and draw the configuration of enantiomers either in line-bond structures or Fischer projections.
   7. Explain diastereomers, constitutional isomers, stereoisomers and meso-compounds.
7. Demonstrate and understanding of the major organic reactions and recognize their characteristics.
   1. Describe and identify the major reactions: rearrangement, addition, substitution and elimination reactions.
   2. Describe a chemical reaction in terms of energy diagrams, transition states, bond dissociation energies, rates and equilibria, homogenic and heterogenic reactions, bond breaking and bond making processes.
   3. Use mechanisms to explain the electrophilic addition reactions and syntheses of alkenes and identify the reagents used in these transformations. Explain Markovnikov’s rule and the stability of carbocation intermediates in these reactions.
   4. Use mechanisms to explain the major reactions and syntheses of alkynes and identify the reagents used in these transformations.
   5. Use the SN1, SN2, E1 and E2 mechanisms to explain the major reactions and syntheses of alkyl halides. Identify the nucleophiles and bases reagents used in these reactions.

CHM 210LW - Organic Chemistry I Laboratory

1. Demonstrate understanding of the importance of laboratory safety and maintenance.
   1. Complete the agreement provided after reading the safety protocols and regulations of the science laboratory.
   2. Conduct safe lab procedures and recognize common laboratory hazards.
   3. Identify and locate all safety features within the laboratory (eye wash fountains, fire extinguishers, fire alarms fire blankets, etc.).
   4. Complete the agreement provided after reading the procedures of safe and ethical use of equipment and instrumentation used in the laboratory.
   5. Dispose of all waste materials properly (chemicals, sharps, broken glassware), if necessary review Safety Data Sheets.
   6. Use personal protection (e.g. goggles, gloves, lab coat) properly.
   7. Clean up all work areas and return all equipment to designated areas before leaving the laboratory.
   8. Report any accidents, incidents or breakages immediately.
2. Record experimental work to promote learning of good laboratory practices.
   1. Locate Safety Data Sheets, as needed.
   2. Use a laboratory notebook to communicate experimental concepts and results.
   3. Record and analyze the data and results of an experiment.
   4. Produce reports to inform others of your progress in the laboratory.
3. Demonstrate understanding of how to perform fundamental organic chemistry experiments.
   1. Recognize and name all the glassware items used in the laboratory.
   2. Use standard laboratory equipment and classical techniques to carry out macroscale and microscale experiments.
   3. Describe the objectives of performing organic experiments.
   4. Conduct a broad range of organic transformations which illustrate topics drawn from the organic chemistry lecture sequence.
   5. Follow directions as presented, but troubleshoot and explain deviations from expected procedures and results.
   6. Design experiments with proper safety features.
4. Demonstrate understanding of core lab concepts and effectively complete experiments and analysis in organic chemistry.
   1. Perform stoichiometric calculations for reactions (limiting reagent, theoretical yield).
   2. Perform fundamental methods of laboratory separations and purifications: thin layer chromatography, recrystallization, simple and fractional distillation.
   3. Perform basic methods of preparative chemistry: refluxing reaction mixtures, extractions and controlled chemical transformations.
   4. Identify and assess the purity of organic compounds using melting point, thin layer chromatography, and gas chromatography.
   5. Characterize and identify organic compounds by physical and spectroscopic methods including but not limited to: Infra-Red (IR), proton NMR spectrophotometry (and other methods as presented).

CHM 220 - Organic Chemistry II

1. Communicate effectively.
   1. Demonstrate understanding by reading, speaking, and writing.
   2. Employ critical writing and active listening to obtain or convey information.
   3. Collect and analyze data.
   4. Identify trends, solve problems, and conclude logically by integrating concepts.
2. Recognize the importance of the pre-requisite organic chemistry material.
   1. Explain fundamental concepts of bonding and molecular structure.
   2. Describe alkane and cycoalkane conformers.
   3. Explain the important concepts of stereochemistry.
   4. Recognize the major organic reactions of alkenes, alkynes, alkyl halides and aromatic compounds.
3. Demonstrate an understanding of the basic structures and properties of organic molecules.  
   1. Use line bonds diagrams to explain chemical structures.
   2. Describe the stability, bonding, structure and physical properties of amines, alcohols, thiols, sulfides, disulfides, ethers and major carbonyl functional groups.
   3. Discuss the acidity and basicity of these functional groups and the effects of substituents.
   4. Identify these functional groups through analysis of spectroscopic data (NMR, IR and mass spectrometry).
4. Apply the fundamental rules of nomenclature.
   1. Name and draw the homologous series of carbonyl functional groups and sulfur derivatives for the first twelve carbons in the series (C1 through to C12).
   2. Use the rules to name and draw amines, alcohols, thiols, sulfides, disulfides, sulfoxides, sulfones, ethers and major carbonyl functional groups.
5. Demonstrate an understanding of the important  organic reactions.
   1. Explain the important reactions of amines, alcohols, thiols, ethers, sulfides, sulfoxides, and sulfones.
   2. Use mechanisms to explain the major reactions and synthesis of amines, alcohols, thiols, ethers, sulfides, sulfoxides, and sulfones.
   3. Explain the important nucleophilic addition reactions of aldehydes and ketones.
   4. Use mechanisms to explain the major reactions and synthesis of aldehydes and ketones.
   5. Describe the nucleophilic acyl substitution reactions of carboxylic acid and their derivatives.
   6. Use mechanisms to explain the major reactions and  synthesis of carboxylic acid and their derivatives.
6. Demonstrate an understanding of the major α-substitution and carbonyl condensation reactions.   
   1. Discuss enolate ions and the keto-enol tautomerization of carbonyl compounds to undergo chemical reactions.
   2. Describe the mechanisms of α-substitution and carbonyl condensation reactions.
   3. Explain the importance of enolate ions in malonic ester synthesis and acetoacetic ester synthesis.
   4. Explain how aldol and enone products are produced through simple and mixed condensation reactions.
   5. Describe Claisen, mixed Claisen and Dieckmann condensation reactions.
7. Apply organic chemistry principles to biochemical macromolecules.
   1. Carbohydrates:
      1. Draw and identify the major monosaccharides and disaccharides and polysaccharides.
      2. Explain the different epimeric, anomeric centers and mutarotations in reference to Howarth and Fischer projections.
      3. Describe the major reactions of monosaccharides and disaccharides.
   2. Lipids:
      1. Explain the difference between fats and oils, saponifiable and non-saponifiable lipids.
      2. Draw and recognize the  structures of saturated and unsaturated fatty acids, glycerol, phospholipids, sphingolipids, steroids, prostaglandins, leukotrienes and thromboxanes.
      3. Explain the major reactions of fatty acids, lipids and steroids.
   3. Amino Acids, Proteins, Enzymes and Nucleic Acids:
      1. Recognize and draw the amino acid and zwitterionic forms and predict the structure of  peptide linkages between  amino acid.
      2. Identify the primary, secondary and tertiary structures of proteins and the types of bonding involved.
      3. Discuss the simple classification of enzymes by their function and reaction and recognize the terms of selectivity active site, inhibition, denaturation and cofactors.
      4. Discuss and identify the common aromatic heterocycles and nucleic acids found in biological systems.
8. Apply organic principles to polymers.
   1. Recognize naturally occurring polymers including fibers.
   2. Draw and recognize polymers from their monomeric units.
   3. Describe the step-growth synthesis of polyamides and polyesters.
   4. Recognize characteristics of common polymeric materials and classify them, their properties  and recycling uses.
   5. Demonstrate understanding of the functional characteristics of common polymers.
   6. Explain the difference between addition and condensation polymers.
   7. Explain the differences between thermoset and thermoplastic resins, polymeric fiber, films and additives.

CHM 220LW - Organic Chemistry II Laboratory

1. Demonstrate an understanding of the importance of laboratory safety and maintenance.
   1. Complete the agreement provided after reading the safety protocols and regulations of the science laboratory.
   2. Conduct safe lab procedures and recognize common laboratory hazards.
   3. Identify and locate all safety features within the laboratory (eye wash fountains, fire extinguishers, fire alarms fire blankets, etc.).
   4. Complete the agreement provided after reading the procedures of safe and ethical use of equipment and instrumentation used in the laboratory.
   5. Dispose of all waste materials properly (chemicals, sharps, broken glassware), if necessary review Safety Data Sheets.
   6. Use personal protection (e.g. goggles, gloves, lab coat) properly.
   7. Clean up all work areas and return all equipment to designated areas before leaving the laboratory.
   8. Report any accidents, incidents or breakages immediately.
2. Record experimental work to promote learning of good laboratory practices.
   1. Locate Safety Data Sheets as needed.
   2. Use a laboratory notebook to communicate experimental concepts and results.
   3. Record and analyze the data and results of an experiment.
   4. Produce reports to inform others of your progress in the laboratory.
3. Demonstrate an understanding of core lab concepts and effectively complete experiments and analysis in organic chemistry.
   1. Perform stoichiometric calculations for reactions (limiting reagent, theoretical yield).
   2. Perform laboratory methods of separations, purifications, recrystallizations, steam distillations, refluxing reactions, extraction and controlled chemical transformations.
   3. Identify and assess the purity of organic compounds using melting point, thin layer chromatography, and gas chromatography.
   4. Characterize and identify organic compounds by physical and spectroscopic methods including but not limited to: Infra-Red (IR), proton NMR spectrophotometry (and other methods as presented).
4. Demonstrate understanding of how to perform advanced syntheses reactions.
   1. Use standard and non-standard laboratory equipment and classical techniques to carry out macroscale and microscale experiments.
   2. Describe the objectives of performing organic experiments.
   3. Use established techniques for handling air sensitive reagents.
   4. Conduct a broad range of organic transformations of alcohol and carbonyl derivatives drawn from the organic chemistry lecture sequence.
   5. Perform basic qualitative analysis experiments to identify specific unknown samples and reagents.
5. Demonstrate understanding of how to combine the fundamental laboratory techniques to solve a chemical problem.
   1. Design experiments to answer specific chemical questions, outline important strategies using proper safety features.
   2. Troubleshoot through directions from expected procedures and results.
   3. Perform basic qualitative analysis methods to identify samples and reagents.
   4. Analyze and interpret data acquired from experiments and analysis.
   5. Produce a report to explain the results of the experiments, the data obtained and clear rationale for the conclusions derived.

CHM 221 - Organic Biochemistry

1. Communicate effectively
   1. Demonstrate understanding by reading, speaking, and writing.
   2. Employ critical writing and active listening to obtain or convey information.
   3. Collect and analyze data.
   4. Identify trends, solve problems, and conclude logically by integrating concepts.
2. Apply chemical principles to biochemical systems
   1. Explain the basic principles of ionic and covalent bonding.
   2. Describe the importance of pH and its relationship to the reactivity and stability of molecules.
   3. Explain the significance of hydrogen bonding to biochemical molecules.
   4. Explain the first and second laws of thermodynamics, coupling of reactions, catabolic, anabolic, exergonic and endergonic reactions.
3. Apply organic chemistry principles to biochemical systems
   1. Draw and name functional groups and use their chemical properties to predict the reactivity and physical characteristics of molecules.
   2. Recognize how functional groups in biochemically relevant macromolecules are inter-converted.
   3. Explain the molecular structures of functional groups in terms of enantiomers, chiral and achiral centers, stereoisomers, isomers and conformers.
4. Apply principles of enzyme kinetics to biochemical systems
   1. Explain how enzymes are specific and selective catalysts with reference to the chemical properties of amino acids and prosthetic groups.
   2. Define activation energy and describe how it is related to reaction rates, free energy and bonding energy.
   3. Describe the Michaelis-Menton and allosteric model for enzyme kinetics to calculate Km and Vmax.
   4. Recognize the importance of pH, temperature, salt concentration, enzyme concentration, substrate concentration and inhibitors in regulating enzymatic activity.
   5. Explain the differences between competitive, non-competitive and uncompetitive inhibitors and how these can be identified using enzyme kinetics and Lineweaver-Burke plots.
   6. Describe the simple classification of enzymes by their function.
5. Describe cellular process in a biochemical system
   1. Carbohydrate metabolism:
      1. Describe the major points of regulation and interconnections between glycolysis, the pentose pathway, anaerobic degradation and the Krebs cycle.
      2. Identify and explain the importance of ATP, NADH, and FADH2 in glycolysis, the Kreb cycle, the pentose pathway and the electron transport chain.
      3. Explain the physiological relevance of these pathways and strategies for driving endothermic reactions.
      4. Explain the significance of the pentose pathway and anaerobic respiration and their regulation points.
   2. Fat metabolism:
      1. Explain the major molecules involved in fatty acid metabolism and ?-oxidation.
      2. Describe the methods of regulation, the interconnections of these metabolic pathways and recycling of the metabolites.
      3. Compare the overall energy efficiency of the aerobic respiration, anaerobic degradation of glucose and lipid metabolism.
   3. Nitrogen metabolism:
      1. Explain the major molecules involved in deamination and the carbon chain breakdown from the available amino acid pool.
      2. Describe the methods of regulation and interconnections of protein metabolism.
      3. Describe the methods of regulation and interconnections of nucleic acid metabolism.
   4. Cell signaling / communication:
      1. Identify the major molecules and the reactions involved in cell signaling.
      2. Describe how cell signaling regulates the various metabolic processes within a cell.

CHM 222LW - Organic Biochemistry Laboratory

1. Communicate effectively.
   1. Demonstrate understanding by reading, speaking, and writing.
   2. Employ critical writing and active listening to obtain or convey information.
   3. Collect and analyze data.
   4. Identify trends, solve problems, and conclude logically by integrating concepts.
2. Demonstrate an understanding of the importance of laboratory safety and maintenance.
   1. Complete the agreement provided after reading the safety protocols and regulations of the science laboratory.
   2. Conduct safe lab procedures and recognize common laboratory hazards.
   3. Identify and locate all safety features within the laboratory (eye wash fountains, fire extinguishers, fire alarms fire blankets, etc.).
   4. Complete the agreement provided after reading the procedures of safe and ethical use of equipment and instrumentation used in the laboratory.
   5. Dispose of all waste materials properly (chemicals, sharps, broken glassware), if necessary review Safety Data Sheets.
   6. Use personal protection (e.g. goggles, gloves, lab coat) properly.
   7. Clean up all work areas and return all equipment to designated areas before leaving the laboratory.
   8. Report any accidents, incidents or breakages immediately.
3. Record experimental work to promote learning of good laboratory practices
   1. Locate Safety Data Sheets as needed.
   2. Use a laboratory notebook to communicate experimental concepts and results.
   3. Record and analyze the results and data of an experiment.
   4. Produce reports to inform others of your progress in the laboratory.
4. Apply chemical methods to biochemical systems
   1. Use basic chemistry skills to make reagents in a laboratory setting including the concept of moles and molar solutions, percent solutions, normality, and dilutions.
   2. Perform and demonstrate an understanding of the principles of extraction, chromatography, serial dilutions, buffers and pH.
   3. Use chemical methods to explain colorimetric assays, enzyme catalysis and protein concentrations.
   4. Use chemical tests and indicators to determine the presence of specific organic functional groups found in biological macromolecules.
   5. Use various tests and reactivity’s to compare and identify specific functional groups found in biochemical systems.
5. Demonstrate the competent use of laboratory instrumentation and equipment
   1. Accurately use critical pieces of equipment like micropipetors, balances, spectrophotometers, hot plates and water baths etc.
   2. Exhibit proper handling of enzymes, solutions, solids and glassware used in biochemical experiments and analysis.
   3. Design and conduct experiments with proper safety features.
   4. Conduct controlled experiments without wasting reagents and time.
   5. Explain the use of UV-visible spectrometers, IR spectrometers for quantitative and qualitative analysis.
   6. Use structural drawing programs to draw major macromolecules.
6. Demonstrate use of equipment to study enzyme kinetics
   1. Explain how enzymes are specific and selective catalysts with reference to the chemical properties of amino acids and prosthetic groups.
   2. Define activation energy and describe how it is related to reaction rates, free energy and bonding energy.
   3. Conduct enzyme kinetics to calculate Km and Vmax.
   4. Conduct enzyme kinetics to identify competitive, non-competitive and uncompetitive inhibitors using Lineweaver-Burke plots.
   5. Explain the reactivity of enzymes with variables such as pH, substrate concentration, temperature and enzyme concentration.

CHM 230 - Chemical Analysis/Instrumentation

1. Demonstrate or describe sample collection, storage, and packaging methods
   1. Use or describe appropriate procedures and equipment to preserve sample integrity
   2. Record information to establish or maintain chain of custody for samples
2. Formulate conclusions from calculations associated with analytic methods.
   1. Calculate quantities of reagents needed for preparation of solutions using various concentration units.
   2. Perform statistical calculations including determination of average, deviation, and standard deviation
   3. Apply statistical tests to data and identify outliers
   4. Prepare calibration curves or tables for internal standard, external standard, or standard addition methods
   5. Use calibration curves to determine sample concentration or quantity of active ingredient
   6. Use results of an experiment to support a conclusion
3. Demonstrate laboratory skills
   1. Maintain a laboratory notebook following good laboratory practices
   2. Use technology associated with a science laboratory
   3. Make decisions using the scientific method
   4. Record data accurately with the appropriate number of significant digits as dictated by the precision of the equipment or glassware
   5. Demonstrate or describe “wet” analytical techniques and sample preparation methods
      1. Prepare and use apparatus to:
         1. Standardize solutions,
         2. Conduct titrations
         3. Perform gravimetric analysis
         4. Perform serial dilutions
         5. Prepare solutions of a specified concentration
         6. Determine sample mass by difference
   6. Demonstrate or describe proper use and maintenance of laboratory equipment and instrumentation
      1. Use standards to verify calibration of electronic balances
      2. Choose appropriate equipment for a specific task (volumetric pipette, graduated cylinder burette, analytical balance, etc.)
      3. Operate or explain the operation of various instruments including sample preparation
         1. UV-Visible Spectrometer
         2. Gas Chromatograph
         3. High Performance Liquid Chromatograph
         4. Nuclear Magnetic Resonance Spectrometer
         5. Infrared Spectrometer
         6. Mass Spectrometer
         7. Electrophoresis Unit
         8. Atomic Absorption Spectrometer
4. Explain chemical principles or theory associated with analytical instruments.
   1. UV-Visible Spectrometry
   2. Gas Chromatography
   3. High Performance Liquid Chromatography
   4. Nuclear Magnetic Resonance Spectroscopy
   5. Infrared Spectroscopy
   6. Mass Spectrometry
   7. Electrophoresis
   8. Atomic Absorption Spectroscopy
5. Troubleshoot laboratory instrumentation
   1. Perform checks or tests to isolate components and determine sources of a malfunction
   2. Evaluate instrumental output and determine whether results are consistent with expectations
   3. Make recommendations for correcting unacceptable or erroneous outputs
6. Demonstrate understanding of the importance of laboratory safety and maintenance
   1. Recognize common laboratory hazards and conduct lab procedures safely
   2. Identify and locate all safety features within the laboratory (eye wash fountains, fire extinguishers, fire alarms fire blankets, etc.)
   3. Demonstrate safe and ethical use of equipment and instrumentation used in the laboratory
   4. Dispose of all waste materials properly (chemicals, sharps, and broken glassware), if necessary review Safety Data Sheets
   5. Use personal protection (e.g. goggles, gloves, lab coat) properly
   6. Clean up all work areas and return all equipment to designated areas before leaving the laboratory
   7. Report any accidents, incidents or breakages immediately
   8. Locate the Safety Data Sheets, as needed

CHM 290-299 - Special Projects in Chemistry