COMPETENCY 1. Demonstrate awareness, and proper use, of laboratory safety techniques.
ENABLING OBJECTIVES
1-1. Differentiate between safe and unsafe procedures, applications, and methods of disposal of chemicals.
1-2. Chose the appropriate safety equipment for specific laboratory situations.
1-3. Decide which safety and emergency procedures to follow in case of particular accidents including fires and hazardous material spills.
1-4. Demonstrate proper methods for carrying and moving chemicals and equipment.
1-5. Demonstrate the ability to understand and follow the safety codes on chemical containers.COMPETENCY 2. Apply System Internationale, "SI", units as used in chemistry.
ENABLING OBJECTIVES
2-1. Identify the base units of the SI system and describe the standards for each.
2-2. Describe the concept of a derived quantity and its units, and identify the dimension (combination of base units) for any derived quantity, initially including area, volume and density.
2-3. Using dimensional analysis, determine whether an equation is dimensionally valid, and establish the dimensions of a quantity.
2-4. Explain and give examples of the system of subdivision used in the SI system, including the use of prefixes to represent powers of ten.
2-5. Use conversion factors to convert quantities from one metric unit to another, and also between metric and English units.
2-6. Experimentally determine density for a variety of substances.COMPETENCY 3. Integrate computer use into the laboratory environment.
ENABLING OBJECTIVES
3-1. Acquire experimental data from computer interfaced hard and software.
3-2. Create spreadsheets, databases, and reports using relevant utility software
3-3. Produce tables and graphs of data using available graphing software programs.
3-4. Conduct statistical analysis of data using relevant utility software.
3-5. Utilize computer laboratory interface to record measurements.COMPETENCY 4. Apply appropriate experimental and measurement skills and techniques to laboratory experiences, and organize laboratory data using proper report and logbook format.
ENABLING OBJECTIVES
4-1. Select appropriate systems of measurement, using proper units, metric prefixes and number of significant digits.
4-2. Report the degree of uncertainty of a measurement, and carry out mathematical operations with measurements containing stated uncertainties.
4-3. Determine the significant digits in a recorded measurement, and carry out mathematical operations using these measurements with answers rounded off to the correct number of significant digits.
4-4. Determine the limit (decimal place) to which a measurement can be made for any measuring instrument. 4-5. Differentiate between precision and accuracy and calculate each.
4-6. Make linear and volume measurements and determine masses of materials using various pieces of equipment.
4-7Use the TI-83 to analyze experimental data, using standard deviation and statistical tests to evaluate significance.
4-8 Maintain a current, organized, and accurate laboratory logbook.
4-9 Write a laboratory report that includes title, introduction, procedure, data/observations, results, and conclusion.COMPETENCY 5. Categorize matter and its properties.
ENABLING OBJECTIVES
5-1. Describe the general properties of matter.
5-2. Identify common elements by chemical symbols.
5-3. Classify matter according to whether it is an element, a compound, or a mixture.
5-4. Distinguish between physical and chemical properties of matter.
5-5. Carry out physical and chemical changes to determine chemical and physical properties of substances 5-6. Use physical methods to separate the components of a mixture.
5-7. Introduction to Material Science: Compare and contrast the various classifications of solid materials (ceramics, composites, polymers, metals).
5-8. Material Science: Compare properties of modern commercial solid materials and determine the classification and structure of these materials.
5-9. Describe the events leading to the modern day arrangement of the periodic table.
5-10. Observe periodic trends of the general characteristics of metals, nonmetals, and metalloids.COMPETENCY 6. Integrate the main features of atomic theory and the atomic mass scale.
ENABLING OBJECTIVES
6-1. Describe the postulates of the modern atomic theory.
6-2. Relate the Laws of Conservation of Mass, Definite Composition, and Multiple Proportions to atomic theory.
6-3. Locate and describe the main components of the atom as used in chemistry.
6-4. Define isotope, and relate atomic number, mass number, and number of atomic particles to each other, and interpret and write isotope symbols.
6-5. Calculate atomic mass from isotope abundances.
6-6. Define Avogadro's number and its relationship to the atomic mass scale.
6-7. Experimentally verify the Law of Conservation of Mass.COMPETENCY 7. Characterize the electronic structure of the atom.
ENABLING OBJECTIVES
7-1. State and interpret the postulates of the Quantum Theory.
7-2. Relate energy differences, wavelength, and frequencies of EMR.
7-3. Describe the atomic spectrum of hydrogen in terms of the Bohr model.
7-4. Identify the four quantum numbers and relate each in terms of energy differences and mathematical interpretation.
7-5. Write electron configurations for elements.
7-6. Use Hund's rule to draw orbital diagrams for electrons in an atom.
7-7. Experimentally determine the wavelengths and frequencies line spectrum of selected elements using the Spec-20.
COMPETENCY 8. Relate ionic and covalent bonding to the electronic structure of atoms and the ionic and/or molecular compounds they form.
ENABLING OBJECTIVES
8-1. Identify basic differences between atoms, molecules, and ions and classify compounds as being ionic or molecular.
8-2. Describe the formation of cations and anions, and relate it to electronegativity and position on the periodic table.
8-3. Write Lewis structures to show the covalent bonding in molecules and polyatomic ions.
8-4. Determine the polarity of covalent bonds from electronegativities.
8-5. Experimentally determine the number of ionizable hydrogens in a compound using pH probes and Vernier interfaces and software.
8-6. Explain the theory of atomic bonding in solids including covalent, Van der Waals, and metallic bonding.
8-7. Material Science: Using atomic structure and bonding theories, provide a model to illustrate various crystalline structures including body centered cubic (BCC), face centered cubic (FCC) and closed packed hexagonal (CPH).
8-8. Distinguish between electrolytes and nonelectrolytes using experimental observations.
8-9. Relate the vapor pressure and phase of substances to the intermolecular attractions present in the substances.
8-10. Use VSEPR model to predict the geometric shape of simple molecules and polyatomic ions.
8-11. Construct models of molecules and polyatomic ions to illustrate their predicted geometric shapes.
8-12. Predict the polarity of molecules by using the VSEPR model for molecules containing polar covalent bonds.
8-13. Experimentally relate solubilities of solutes in solvents to their polarities.
COMPETENCY 9. Apply rules of chemical nomenclature to writing formulas and naming compounds.
ENABLING OBJECTIVES
9-1. Write names of ionic and binary covalent compounds from their formulas using older system of prefixes and suffixes and the newer IUPAC system.
9-2. Use ion-charge method to write formulas for ionic compounds.
9-3. Write formulas for binary covalent compounds.
9-4. Write formulas for the basic acids.COMPETENCY 10. Apply the mole concept to calculations involving masses and/or numbers of atoms, molecules, or formula units.
ENABLING OBJECTIVES
COMPETENCY 11. Apply stoichiometry experimentally and in calculations.
10-1. State the masses of atoms or molecules in terms of molar masses.
10-2. Convert numbers of atoms and molecules to masses by using the mole, and vice versa.
10-3. Calculate, and prepare solutions of known molarity.
10-4. Distinguish between empirical and molecular formulas.
10-5. Experimentally determine the empirical formula of an ionic compound.
10-6. Calculate percentage composition of a compound from its formula, and from experimental data.
10-7. Calculate empirical and molecular formulas from experimental data.
ENABLING OBJECTIVES
11-1. Calculate mass relationships based on balanced chemical equations.
11-2. Determine the limiting reactant, and the theoretical yield for chemical reactions.
11-3. Experimentally determine the mole ratio for a chemical reaction, and use it to determine the equation or the reaction.
11-4.Carry out calculations involving solution concentrations in mole fractions and molarity.COMPETENCY 12. Categorize chemical reactions and write balanced equations for reactions.
ENABLING OBJECTIVES
12-1. Write and balance chemical equations when given reactants and products.
12-2. Classify those equations that come under the heading of synthesis, decomposition, replacement, and ionic reactions.
12-3. Predict the products of chemical reactions when given the reactants.
12-4. Define oxidation and reduction, and identify any species undergoing oxidation or reduction, and identify the oxidizing and reducing agents.
12-5. Use solubility rules to predict the formation of insoluble products, and the activity series to predict the occurrence of replacement reactions.
12-6. Relate complete and incomplete combustion to oxidation.
12-7. Experimentally determine an activity series of metals.
12-8. Carry out examples of each kind of reaction, and write balanced equations for each.
12-9.Study various types of environmentally relevant reactions, such as those relating to acid rain and corrosion, and determine the reactants and conditions that permit these reactions to occur.COMPETENCY 13. Relate the concepts of energy, enthalpy, entropy and Gibbs free energy to chemical reactions.
ENABLING OBJECTIVES
13-1. Classify the various forms of energy.
13-2. Summarize the changes in energy that take place during a chemical reaction.
13-3.Experimentally determine the specific heat capacity or several substances, and relate these quantities to the structures of the substances.
13-4. Distinguish between exothermic and endothermic reactions.
13-5. Distinguish between heat and temperature.
13-6. State the three Laws of Thermochemistry.
13-7. Calculate DH for a reaction using specific heats and heats of formation.
13-8. Experimentally measure heat flow using a calorimeter, and use the measurements to write a thermochemical equation for the reaction.
13-9. Calculate "q" and DE for a system according to the First Law of Thermodynamics.
13-10. Define and calculate DH and DS for a reaction, and relate the signs to characteristics of the reaction.
13-11. Use the Gibbs-Helmholtz equation to calculate the Gibbs energy change for a reaction.
13-12. Compare and contrast various possible sources of energy and the consequences to the environment of using these sources.COMPETENCY 14. Relate the concept of equilibrium to chemical reactions, especially with reference to acids and bases.
ENABLING OBJECTIVES
14-1. Write the expression for Kc from the balanced equation for a reaction involving gases.
14-2. Calculate Kc from equilibrium concentrations of all species, or from original concentrations of all species and the equilibrium concentration of one species.
14-3. Using LeChatelier's Principle, predict the effect of a change in the number of moles, volume, or temperature upon the position of an equilibrium.
14-4. Relate the acidic and basic properties of aqueous solutions to the dissociation of water. 14-5. Carry out calculations involving pH and pOH.
14-6. Compare strong and weak acids and bases.
14-7. Write equations for reactions between acids and bases.
14-8. Carry out acid-base titrations using pH probes and interfacing and write equations for the reactions. 14-9. Compare Arrhenius, Bronsted-Lowry, and Lewis theories of acids.COMPETENCY 15: Describe gases in terms of the kinetic theory of gases and apply the gas laws and the Ideal Gas Equation to problems.
ENABLING OBJECTIVES
15-1. Define pressure and relate to kinetic theory.
15-2. Describe the effect of temperature on pressure and volume of gases.
15-3. Apply mole-volume relationship of gases to gas-phase reactions.
15-4. Describe the relationship between pressure and volume of gases.
15-5. Combine Boyle's, Charles, and Avogadro's laws of gases into the ideal gas law.
15-6. Describe diffusion of gases and relate to Graham's Law.
15-7. Describe mixtures of gases in terms of Dalton's Law of Partial Pressure.
15-8. Relate density of gases to molar volume and molar mass.
15-9. Describe the operation of mercury barometers.
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