Instructional Objectives
Chapter 1. Chemistry: Methods and Measurement
1. Describe the interrelationship of chemistry with other fields of science and medicine.
2. Discuss the approach to science, the scientific method.
3. Distinguish among the terms hypothesis, theory, and scientific law.
4. Describe the properties of the solid, liquid, and gaseous states.
5. Classify properties as chemical or physical.
6. Classify observed changes in matter as chemical or physical.
7. Provide specific examples of physical and chemical properties.
8. Distinguish between intensive and extensive properties.
9. Classify matter as element, compound, or mixture.
10. Distinguish between data and results.
11. Learn the major units of measure in the English and metric systems, and be able to convert from one system to another.
12. Report data and results using scientific notation and the proper number of significant figures.
13. Use appropriate experimental quantities in problem solving.
14. Calculate the density of an object from mass and volume data and calculate the specific gravity of an object from its density.
Chapter 2. The Composition and Structure of the Atom
1. Recognize the interrelationship of the structure of matter and its physical and chemical properties.
2. Describe the important properties of protons, neutrons, and electrons.
3. Calculate the number of protons, neutrons, and electrons in any atom.
4. Distinguish among atoms, ions, and isotopes.
5. Trace the history of the development of atomic theory, beginning with Dalton.
6. Summarize the experimental basis for the discovery of charged particles and the nucleus.
7. Explain the critical role of spectroscopy in the development of atomic theory and in our everyday lives.
8. State the basic postulates of Bohr's theory.
9. Compare and contrast Bohr's theory and the more sophisticated "wave-mechanical" approach.
Chapter 3. Elements, Atoms, Ions, and the Periodic Table
1. Recognize the important subdivisions of the periodic table: periods, groups (families), metals, and nonmetals.
2. Use the periodic table to obtain information about an element.
3. Describe the relationship between the electronic structure of an element and its position in the periodic table.
4. Write electron configurations for atoms of the most commonly occurring elements.
5. Know the meaning of the octet rule and its predictive usefulness.
6. Use the octet rule to predict the charge of common cations and anions.
7. Utilize the periodic table and its predictive power to estimate the relative sizes of atoms and ions, as well as relative magnitudes of ionization energy and electron affinity.
8. Use values of ionization energies and electron affinities to predict ion formation.
Chapter 4. Structure and Properties of Ionic and Covalent Compounds
1. Classify compounds as having ionic, covalent, or polar covalent bonds.
2. Write the formulas of compounds when provided with the name of the compound.
3. Name common inorganic compounds using standard conventions and recognize the common names of frequently used substances.
4. Predict the differences in physical state, melting and boiling points, solid-state structure, and solution chemistry that result from differences in bonding.
5. Draw Lewis structures for covalent compounds and polyatomic ions.
6. Describe the relationship between stability and bond energy.
7. Predict the geometry of molecules and ions using the octet rule and Lewis structure.
8. Understand the role that molecular geometry plays in determining the solubility and melting and boiling points of compounds.
9. Use the principles of VSEPR theory and molecular geometry to predict relative melting points, boiling points, and solubilities of compounds.
Chapter 5. Calculations and the Chemical Equation
1. Know the relationship between the mole and Avogadro's number, and the usefulness of these quantities.
2. Perform calculations using Avogadro's number and the mole.
3. Write chemical formulas for common inorganic substances.
4. Calculate the formula weight and molar mass of a compound.
5. Know the major function served by the chemical equation, the basis for chemical calculations.
6. Balance chemical equations given the identity of products and reactants.
7. Calculate the number of moles of product resulting from a given number of moles of reactants or the number of moles of reactant needed to produce a certain number of moles of product.
8. Calculate theoretical and percent yield.
Chapter 6. States of Matter: Gases, Liquids, and Solids
1. Describe the behavior of gases expressed by the gas laws: Boyle's law, Charles's law, combined gas law, Avogadro's law, the ideal gas law, and Dalton's law.
2. Use gas law equations to calculate conditions and changes in conditions of gases.
3. Describe the major points of the kinetic molecular theory of gases.
4. Explain the relationship between the kinetic molecular theory and the physical properties of macroscopic quantities of gases.
5. Describe properties of the liquid state in terms of the properties of the individual molecules that comprise the liquid.
6. Describe the processes of melting, boiling, evaporation, and condensation.
7. Describe the dipolar attractions known collectively as van der Waals forces.
8. Describe hydrogen bonding and its relationship to boiling and melting temperatures.
9. Relate the properties of the various classes of solids (ionic, covalent, molecular, and metallic) to the structure of these solids.
Chapter 7. Reactions and Solutions
1. Classify chemical reactions by type: combination, decomposition, or replacement.
2. Recognize the various classes of chemical reactions: precipitation, reactions with oxygen, acid–base, and oxidation–reduction.
3. Distinguish among the terms solution, solute, and solvent.
4. Describe various kinds of solutions, and give examples of each.
5. Describe the relationship between solubility and equilibrium.
6. Calculate solution concentration in weight/volume percent and weight/weight percent.
7. Calculate solution concentration using molarity.
8. Perform dilution calculations.
9. Interconvert molar concentration of ions and milliequivalents/liter.
10. Describe and explain concentration-dependent solution properties.
11. Describe why the chemical and physical properties of water make it a truly unique solvent.
12. Explain the role of electrolytes in blood and their relationship to the process of dialysis.
Chapter 8. Chemical and Physical Change: Energy, Rate, and Equilibrium
1. Correlate the terms endothermic and exothermic with heat flow between a system and its surroundings.
2. State the meaning of the terms enthalpy, entropy, and free energy and know their implications.
3. Describe experiments that yield thermochemical information and calculate fuel values based on experimental data.
4. Describe the concept of reaction rate and the role of kinetics in chemical and physical change.
5. Describe the importance of activation energy and the activated complex in determining reaction rate.
6. Predict the way reactant structure, concentration, temperature, and catalysis affect the rate of a chemical reaction.
7. Write rate equations for elementary processes.
8. Recognize and describe equilibrium situations.
9. Write equilibrium-constant expressions and use these expressions to calculate equilibrium constants.
10. Use LeChatelier's principle to predict changes in equilibrium position.
Chapter 9. Charge-Transfer Reactions: Acids and Bases and Oxidation-Reduction
1. Identify acids and bases and acid-base reactions.
2. Write equations describing acid-base dissociation and label the conjugate acid-base pairs.
3. Describe the role of the solvent in acid-base reactions, and explain the meaning of the term pH.
4. Calculate pH from concentration data.
5. Calculate hydronium and/or hydroxide ion concentration from pH data.
6. Provide examples of the importance of pH in chemical and biochemical systems.
7. Describe the meaning and utility of neutralization reactions.
8. State the meaning of the term buffer and describe the applications of buffers to chemical and biochemical systems, particularly blood chemistry.
9. Describe oxidation and reduction, and describe some practical examples of redox processes.
10. Diagram a voltaic cell and describe its function.
11. Compare and contrast voltaic and electrolytic cells.
Chapter 10. The Nucleus, Radioactivity, and Nuclear Medicine
1. Enumerate the characteristics of alpha, beta, and gamma radiation.
2. Write balanced equations for common nuclear processes.
3. Calculate the amount of radioactive substance remaining after a specified number of half-lives.
4. Describe the various ways in which nuclear energy may be used to generate electricity: fission, fusion, and the breeder reactor.
5. Explain the process of radiocarbon dating.
6. Cite several examples of the use of radioactive isotopes in medicine.
7. Describe the use of ionizing radiation in cancer therapy.
8. Discuss the preparation and use of radioisotopes in diagnostic imaging studies.
9. Explain the difference between natural and artificial radioactivity.
10. Describe the characteristics of radioactive materials that relate to radiation exposure and safety.
11. Be familiar with common techniques for the detection of radioactivity.
12. Know the common units in which radiation intensity is represented: the curie, roentgen, rad, and rem.