PERFORMANCE OBJECTIVES
1. The learner will collect and interpret data utilizing various sources and techniques.
2. The learner will relate the impact of historical scientific discoveries in chemistry to the issues confronting contemporary society using a persuasive presentation of a fully developed position.
3. The learner will use standard laboratory equipment and record measurements in appropriate units.
4. Given a set of learner collected data concerning transformations of matter and energy, the learner will construct a model which adequately represents the transformation.
5. The learner will test a physical and mathematical model of how matter is classified and the changes it undergoes.
6. The learner will access primary and secondary data to gain understanding of atomic theory and structure.
7. The learner will construct a model of the atom from the atomic theory.
8. The learner will use the periodic table to gather necessary information for problem solving.
9. The learner will construct models to determine resulting structures form covalently and ionically joined compound.
10. The learner will use appropriate nomenclature, symbols and formulas for ionic and covalent compounds.
11. The learner will express a chemical reaction in the form of a balanced chemical equation.
12. The learner will construct a model of the behavior of gases applying the gas laws.
13. The learner will identify and discuss the structure and functions of the relationships between solids and liquids.
14. The learner will analyze the properties of water and recognize its uniqueness.
15. The learner will dissolve substances and determine solubility and concentration.
16. The learner will prepare and present an evaluation and limitations between acids, bases and salts.
17. The learner will assign oxidation numbers to elements to determine reactants and products in a redox reaction.
INSTRUCTIONAL OBJECTIVES
The learner will:
A. SCIENCE PROCESSES AND SKILLS
1. Develop skills in observing, classifying, predicting, making inferences, measuring, communicating findings to others, and collecting, interpreting and recording data.
2. Demonstrate skills in using space/time relationships.
3. Engage in scientific experimentation including formulation of hypotheses.
4. Distinguish necessary science skills that will be useful in the world of work.
B. HISTORICAL PERSPECTIVES AND CHEMISTRY CAREERS
1. Become familiar with significant discoveries or work of past scientists and their methods and attributes.
2. Use scientific models and analyze how these models can be modified by the use of current data.
3. Explore various careers related to the field of chemistry and identify the necessary educational training to become involved in the career.
4. Recognize that many aspects of chemistry affects everyday work and life.
C. MEASUREMENT AND MATHEMATICAL EXPRESSION
1. Express measurements in the International System of Units (version of the metric system) throughout the course.
2. Distinguish between fundamental and derived units.
3. Become familiar with the use of unit analysis in problem solving.
4. Recognize and express uncertainty in measurements.
5. Differentiate accuracy expressed in terms of deviation.
6. Demonstrate the ability to do operations with significant figures and exponential notations.
D. MATTER AND ENERGY RELATIONSHIPS
1. Demonstrate a knowledge of the concept of inertia.
2. Compare mass and weight and extend the use of these concepts in investigating and calculating the density of various forms of matter.
3. Identify the different states of matter.
4. Engage in describing both the physical chemical properties of matter.
5. Be able to define energy and differentiate between kinetic and potential forms of energy.
6. Explain the laws of conservation of matter and energy.
E. CLASSIFICATION OF MATTER AND ITS CHANGES
1. Compare and contrast elements, mixtures, and compounds.
2. Compare and contrast physical and chemical changes.
3. Describe energy and entropy changes.
4. Investigate nuclear changes and describe the processes.
F. ATOMIC THEORY AND STRUCTURE
1. Trace the historical development of various atomic theories.
2. Develop a model for atomic structure including the description of the characteristics of the protons and neutrons comprising the nucleus as well as the electrons surrounding the nucleus.
3. Demonstrate an understanding of atomic number and atomic mass (mass number).
4. Define and give examples of isotopes.
5. Demonstrate a working knowledge of the concept of the mole in terms of number of particles, mass and volume as well as being able to state and interpret Avogadro's Number.
6. Define atomic weight and be able to use it to determine gram-atomic and gram-molecular weight.
G. ELECTRON CONFIGURATION
1. Formulate an idea that associates electrons being found in a cloud around the nucleus of an atom.
2. Investigate electrostatic attraction.
3. Describe the wave-mechanical model.
4. Differentiate among the principal, orbital, magnetic and spin quantum numbers.
5. Describe orbital patterns and electron notations.
6. Use orbital notation, electron configuration notation and electron dot notation.
H. PERIODIC TABLE AND PERIODIC LAW
1. Become familiar with the history of the development of the Periodic Table and its historical importance as a predictive tool.
2. Explain the structure of the Periodic Table and note the trends related to the position of elements in periods and groups.
3. Classify elements as metals, nonmetals, or metalloids by their properties.
4. Identify transition elements and rare earth elements and compare their properties.
5. Define and use the periodic properties of atomic radius, ionization energy and electron affinity.
I. CHEMICAL BONDING
1. Explain the significance of valence electrons in bonding.
2. Recognize that ionic bonding is the result of electrostatic attraction between oppositely charged ions.
3. Explain the formation of cations and anions during electron transfer.
4. Demonstrate and understanding of empirical formulas.
5. Compare and contrast the relative sizes of atoms vs. ions.
6. Describe energy changes during ionic bond formation.
7. Become familiar with assigning oxidation numbers.
8. Recognize that covalent bonding results from the simultaneous attraction of two or more nuclei for the same electrons.
9. Describe electron sharing.
10. Develop a model for diatomic and polyatomic molecules.
11. Determine molecular formulas.
12. Explain energy changes and bond energies in relation to covalent bonding.
13. Describe resonance and the resonance hybrid.
14. Explain hybridization.
15. Demonstrate and understanding of electronegativities to determine the nature of the bond and predict the degree of covalency of a bond.
16. Identify compounds with ionic bonding.
17. Distinguish between the polar covalent bond and the non-polar covalent bond.
18. Explain that molecules may be held together by hydrogen bonds.
J. CONCEPTS OF CHEMICAL COMPOSITION
1. Write formulas of compounds from their names.
2. Name binary compounds and compounds having polyatomic ions given their formulas.
3. Analyze the significance of the chemical formula.
4. Relate the composition of compounds to their formulas.
5. Determine formula/molecular weight.
6. Engage in percent composition problems.
7. Determine empirical/molecular formulas.
8. Demonstrate a knowledge of the Law of Definite Composition and the Law of Multiple Proportions.
9. Relate the concept of atomic and molecular masses to the mole.
K. CHEMICAL EQUATIONS
1. Explain the uses of a balanced equation and the various meanings of the coefficients.
2. Express coefficients as mole proportions (molar volumes).
3. Determine mass proportions.
4. Explain equation writing procedures.
5. Predict the products of a reaction knowing the reactants.
6. Relate equations to reactions involving precipitates an/or gases.
7. Recognize the role of catalysts in equation writing.
8. Compare and contrast composition, decomposition, and replacement reactions.
9. Explain ionic reactions and recognize "spectator" ions.
10. Describe a reversible reaction.
11. Solve problems involving stoichiometric relationships.
L. BEHAVIOR OF GASES
1. Describe the Kinetic Molecular Theory.
2. Explain the properties of gases.
3. Investigate the conditions for expansion of gases and pressure changes.
4. Recognize how low density affects gas behavior.
5. Become familiar with the basis for Grahm's Law of Diffusion.
6. Describe the behavior of an ideal gas.
7. Describe the attractive forces between gas molecules.
8. Explain that molecules may be held together by Van der Waals' forces.
9. Explain that polar molecules may exist due to dipole forces (dipole moment).
10. Analyze, define and use the gas laws including Charles' Law, Boyle's Law, Gay-Lussac's Law and the combined gas law.
11. Develop and use the Ideal Gas Equation.
12. Interpret the behavior of a mixture of gases using Dalton's Law of combining volumes of gases.
13. Define and explain Avogadro's Principle and relate the mole concept to volumes of gases.
14. Define and give examples of specific gravity.
15. Compute the density of a gas.
16. Determine experimentally the molecular weight of gases.
17. Solve gas volume problems and problems involving masses of gases.
M. BEHAVIOR OF LIQUIDS AND SOLIDS
1. Interpret the general characteristics of liquids based upon the type of bonding present.
2. Explain specific gravity as it applies to liquids.
3. Investigate the role of physical equilibrium in explaining the behavior of liquids.
4. Define equilibrium vapor pressure.
5. Explain La Chatelier's Principle.
6. Explain that phase is determined by the kinetic energy content.
7. Define boiling and liquefaction of gases.
8. Calculate molar heat of vaporization from experimental data.
9. Interpret the general properties of solids based upon the type of bonding.
10. Define freezing and melting point in relation to changes of state.
11. Calculate molar heat of fusion from experimental data.
12. Define sublimation.
13. Compare and contrast amorphous solids and crystalline solids.
14. Describe six crystal systems.
15. Describe types of lattice structure; ionic, covalent, metallic, molecular, and liquid crystals.
N. THE NATURE OF WATER
1. Investigate the physical and chemical properties of water.
2. Explain the molecular structure of water.
3. Become familiar with the importance of hydrogen bonding.
4. Describe the behavior of water with metals, metallic and nonmetallic oxides.
5. Distinguish between hydrous and anhydrous compounds.
6. Define efflorescence and deliquescence.
O. THE SOLUTION PROCESS
1. Develop the idea that the solution process is a sum of reactions between solute and solvent.
2. Explain how concentrations of solutions are expressed by defining molarity, normality and molality.
3. Calculate molecular masses, freezing points, and boiling points from molal concentrations.
4. Distinguish between electrolytes and nonelectrolytes.
5. Predict solubilities from information about types of chemical bonds present in both solute and solvent.
6. Describe the fundamentals of solution equilibrium.
7. Identify characteristics of saturated and supersaturated solutions.
8. Investigate the effects of pressure and temperature on solubility.
9. Explain solution rates.
P. ACIDS, BASES AND SALTS
1. Explain the development of the present acid-base theories.
2. Describe neutralization.
3. Determine relative strengths of acids and bases.
4. Perform calculations involving hydrogen-ion concentration.
5. Explain the importance of indicators in experimentation.
6. Define hydrolysis and interpret the results of hydrolysis.
7. Explain the action of buffers.
8. Demonstrate laboratory skills by performing titration.
Q. OXIDATION-REDUCTION REACTIONS
1. Explain oxidation state.
2. Assign oxidation state.
3. Distinguish between oxidizing agent and reducing agent.
4. Balance redox equations.
5. Relate redox reactions to the field of electrochemistry and demonstrate a variety of practical examples.