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MISSISSIPPI GULF COAST COMMUNITY COLLEGE
Course of Study Fall 2003 Date Revised COURSE TITLE: GENERAL CHEMISTRY I COURSE NUMBER: CHE 1214 SCIENCE DEPARTMENT: Jefferson Davis Campus Stephen Roberts, Chair SEMESTER CREDIT HOURS: Four Semester Credit Hours CONTACT HOURS: LECTURE: Three Hours LABORATORY: Two Hours PREREQUISITE COURSES: The student must meet one or more of the following requirements: CHE 1314, or one year of high school chemistry and one year of algebra, ACT composite of 19 and math score of 21, or satisfactory score on challenge exam. COURSE DESCRIPTION: A mathematical approach to the basis of Chemistry. Measurement stoichiometry, solution stoichiometry, gas laws, thermochemistry, periodic table and bonding are studied.
CONTENT : This course emphasizes fundamental treatments of concepts such as structure, energy relationships, and reaction mechanisms. Atomic theory, orbitals, and chemical bonding are stressed. The history of chemistry and methods of scientific discovery are presented. The unfolding of theories of atomic structure, the determination of atomic weight, the discovery of nuclear fission, and the chemical evidence for isomers follow the case history approach. TEXTBOOKS: General Chemistry - with Qualitative Analysis , 5th Addition, Whitten, Davis, Peck. 1996, Saunders College Publishing LAB MANUAL: Laboratory Manual for College Chemistry, Sixth Edition, W. E. Bull, et al. 1980, Harper and Row, Inc. PURPOSE: The purpose of the science programs at Mississippi Gulf Coast Community College is to provide the scientific literacy our students will need to function in a technological society. This purpose is achieved by offering quality lectures and laboratory activities to the community we serve. Our mission if to offer students an educational experience which will foster intellectual development and a lifelong pursuit of knowledge. Services are provided for college transfer credit curricula requiring science courses, science training for two-year technical programs, and science education for the general public. In addition, our responsibilities to the community are met by a personal commitment by faculty members to participate in science fairs, speaking engagements, tours of our science facilities by local school children and consultation with individuals who have needs relating to our discipline.
planned to contribute to the achievement of the following overall goals.
- To provide a firm foundation in a selection of college chemistry topics considered essential to the basic understanding of chemistry necessary for students majoring in science.
- To adequately prepare students to continue their study of chemical principles and concepts in General College Chemistry II (second semester course).
- To develop quantitative problem solving skills providing students with opportunity to apply college level mathematical abilities to chemical calculations.
- To develop an analytical approach to the observation and investigation of natural chemical phenomena.
- To give students a chance to better understand the patterns of organization of matter in the universe. COURSE OBJECTIVES: After completing this course the student should be able to: I. Foundation of Chemistry A. Use the basic vocabulary of matter and energy B. Distinguish between chemical and physical properties and between physical and chemical changes C. Recognize various forms of matter: homogeneous and heterogeneous mixtures, substances, compounds, and elements D. Recognize some common methods of separation used in chemistry E. Apply the concept of significant figures F. Apply the appropriate units to describe the results of measurement G. Use the unit factor method to carry out conversions among units H. Describe temperature measurements on various common scales and convert between themselves I. Carry out calculations relating temperature change to heat absorbed or liberated II. Chemical Formulas and Composition Stoichiometry A. Understand an early concept of atoms B. Use chemical formulas to solve various kinds of chemical problems C. Relate names to formulas and charges of simple ions D. Combine simple ions to write formulas and names of ionic compounds E. Recognize and use formula weights and more relationships F. Interconvert masses, moles, and formulas in problems G. Determine percent compositions in compounds H. Determine formulas from composition
I. Perform calculations about purity of substances III.Chemical Equations and Reaction Stoichiometry A. Write a balanced chemical equation to describe a chemical reaction B. Interpret a balanced chemical equation to calculate the moles of reactants and products involved in the reaction C. Interpret a balanced chemical equation to calculate the masses of reactants and products involved in the reaction D. Determine which is the limiting reactant E. Use the limiting reactant concept in calculations with chemical equations F. Compare the amount of substances actually formed in a reaction (actual yield) with the predicted amount (theoretical yield) and determine the percent yield G. Understand sequential reactions H. Use the terminology of solutions solute, solvent, and concentration I. Calculate concentrations of solutions when they are diluted J. Understand the concept of and calculations for titrations IV. Some Types of Chemical Reactions A. About the periodic table and the classifications of elements B. About reactions of solutes in aqueous solutions C. To recognize nonelectrolytes, strong electrolytes, and weak electrolytes D. The classification of acids, bases, and salts E. Which kinds of compounds are soluble and which kinds are insoluble in water F. How to describe reactions in aqueous solutions by writing formula unit equations as well as total ionic and net ionic equations G. About displacement reactions and the activity series H. About precipitation reactions I. About oxidation numbers J. To balance equations for oxidation reduction reactions V. The Structure of Atoms A. The evidence for the existence and properties of electrons, protons, and neutrons B. The arrangements of these particles and in atoms C. Isotopes and their composition D. The relation between isotopic abundance and observed atomic weights E. The wave view of light and how wavelength, frequency, and speed are related F. The particle description of light and how it is related to the wave description G. Atomic emission and absorption spectra and how these were the basis for an important advance in atomic theory H. The quantum mechanical picture of the atom I. The four quantum numbers and possible combinations of their values J. The shapes of orbitals and the usual order of their relative energies K. Ways to determine electronic configurations of atoms
D. Apply the Aufbau Principle to find the molecular orbitals descriptions for homo- nuclear diatomic molecules and their ions E. Apply the Aufbau Principle to find the molecular orbitals description for hetero- nuclear diatomic molecules and their ions F. Find the bond order in diatomic molecules G. Relate bond order to bond stability H. Use the MO concept of delocalization for molecules in which VB theory would postulate resonance X. Reactions in Aqueous Solutions 1: Acids, Bases, and Salts A. To understand the Arrhenius theory B. About hydrated hydrogen ions C. To understand the Barnsted-Lowry theory D. The properties of aqueous solutions and acids E. The properties of aqueous solutions of bases F. How to predict the strengths of binary acids G. About acid - base reactions H. About acidic and basic salts I. To understand the strengths of ternary acids J. About amphoterism K. How to prepare acids L. To understand the Lewis theory XI. Reactions in Aqueous Solutions II: Calculations A. Review molarity calculations and expand your understanding of molarity B. Learn about standardization and the use of standard solutions of acids and bases and using:
- The mole method and molarity
- Equivalent weights and normality C. Review redox reactions and balancing redox equations D. Learn about redox titrations using:
- The mole method and molarity
- Equivalent weights and normality XII. Gases and the Kinetic Molecular Theory A. About the properties of gases and how they differ from liquids and solids B. How we measure pressure C. To understand the absolute (Kelvin) temperature scale D. About the relationships among pressure, volume, temperature, and amount of gas (Boyle’s, Charles, Avogrado’s, and the combined gas law) and the limitations of each one E. To use Boyle’s, Charles, Avagrado’s, and the combined gas law as appropriate to calculate changes in pressure, volume, temperature, and amount of gas F. To do calculations about gas densities and the standard molar volume
G. About the ideal gas equation, and how to use it to do calculations about a sample of gas H. To determine molecular weights and formulas of gaseous substances from measured properties of gases I. To describe how mixtures of gases behave and to predict their properties J. About the kinetic-molecular theory of gases, and how this theory is consistent with the observed gas laws K. About molecular motion, diffusion and effusion of gases L. What molecular features are responsible for nonideal behavior of real gases and when this nonideal behavior is important M. To carry out calculations about the gases involved in chemical reactions XIII. Liquids and Solids A. About the properties of liquids and solids and how they differ from gases B. To understand the kinetic-molecular description of liquids and solids, and how this description differs from that for gases C. To use the terminology of phase changes D. To understand various kinds of intermolecular attractions and how they are related to physical properties such as vapor pressure, viscosity, melting point, boiling point, and so on E. To describe evaporation, condensation, and boiling in molecular terms F. To do calculations about the heat transfer involved in warming or cooling with- out a change of phase G. To do calculations about the heat transfer involved in phase changes H. To describe melting, solidification, sublimation, and deposition molecular terms I. To interpret P vs. T phase diagrams J. About the regular structure of crystalline solids K. About the various types of solids L. To relate the properties of different types of solids to the bonding or interactions among particles in these solids M. To visualize some common simple arrangements of atoms in solids N. To carry out calculations relating atomic arrangement, density, unit cell size, and ionic or atomic radii in some simple crystalline arrangements O. About the bonding in metals P. Why some substances are conductors, some are insulators, and others are semi-conductors. XIV. Solutions A. To understand the factors that favor the dissolution process B. About the dissolution of solids in liquids, liquids in liquids, and gases in liquids C. How temperature and pressure affect dissolution and rates of saturation D. To express concentrations of solutions in terms of molarity and mole fractions E. About colligative properties of solutions: lowering of vapor pressure (Raoult’s Law), boiling point elevation, and freezing point depression
