Maricopa Community Colleges  CHM151   19912-19955 
Official Course Description: MCCCD Approval: 12/11/90
CHM151 19912-19955 LEC 3 Credit(s) 3 Period(s)
General Chemistry I
A detailed study of the principles of chemistry. Designed for science majors and students in pre-professional curricula. Prerequisites: A grade of "C" or better required for the following: CHM100 and CHM100LL, or CHM130 and CHM130LL, or one year of high school chemistry and completion of Intermediate Algebra or the equivalent.
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MCCCD Official Course Competencies:
CHM151   19912-19955 General Chemistry I
1. Define "chemistry" and describe its main branches. (I)
2. Use the Factor-Label (dimensional analysis) Method in solving chemistry-related problems. (II)
3. Use metric and SI systems of units. (II)
4. Define the relationships between matter and energy. (III)
5. Describe the physical states of matter with the aid of the Kinetic Molecular Theory. (III)
6. Classify matter as elements, compounds, or mixtures. (III)
7. Describe the properties of metallic and nonmetallic elements. (III)
8. Write formulas for and give names of simple inorganic compounds. (III)
9. Classify a property or change as physical or chemical. (III)
10. Complete and balance chemical equations. (IV)
11. Write a net ionic equation from a given reaction. (IV)
12. Determine the empirical and molecular formula from percentage composition or mass data. (V)
13. Perform calculations usingthe mole concept of mass and number. (V)
14. Solve problems involving the Ideal Gas Laws. (VI)
15. Solve problems involving energy changes that result from physical state changes and from chemical reactions. (VII)
16. Apply Hess's Law to given set of equations. (VII)
17. Calculate heats of reaction from calorimeter data and/or bond energies. (VII)
18. Solve stoichiometry problems, including problems involving solutions and heats of reactions. (VII)
19. Deduce the electronic structure of atoms and show the relationship between electronic structure and the chemical properties of atoms. (VIII)
20. Identify substances as electrolytes or nonelectrolytes. (XI)
21. Use the Periodic Table to estimate the properties of elements and compounds. (VIII)
22. Describe the properties of ionic and covalent compounds. (IX)
23. Describe chemical bonding in terms of Valence Bond Theory and Molecular Orbital Theory. (IX)
24. Use the concepts of electonegativity and bond polarity in conjunction with VSEPR Theory to predict the shapes and polarities of simple ions and molecules. (IX)
25. Write the electron dot structure for an atom, ion, ionic formula, or a covalently bonded specie. (IX)
26. Classify intermolecular forces in a given substance as ionic, covalent, London, dipoole-dipole, hydrogen bonding, or metallic. (X)
27. Classify a crystal as molecular, ionic covalent, or metallic. (X)
28. Describe the properties of solutions. (XI)
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MCCCD Official Course Outline:
CHM151   19912-19955 General Chemistry I
    I. Definition of "chemistry"
        A. History
        B. Scientific method
      II. Measurement
          A. Metric system
          B. Significant figures
          C. Exponential notation
          D. Dimensional analysis
          E. Density/specific gravity
        III. Matter
            A. States of matter
            B. Classification of matter
            C. Properties of matter
            D. Physical and chemical changes
            E. Atomic theory
            F. Formulas and nomenclature of substances
            G. Nomenclature
              1. Ionic binary and ternary - stock system
              2. Covalent binary - classical
          IV. Chemical reactions: an introduction
              A. Balancing equations
              B. Types of reactions
              C. Net ionic equations
            V. Mole calculations with formulas and equations
                A. Atomic and molecular weights
                B. Mass-mole conversions
                C. Percentage composition
                D. Empirical and molecular formula
                E. Stoichoimetry
                F. Limiting reagents and percentage yields
                G. Percent purity
                E. Solution stoichiometry
              VI. Gases
                  A. Gas laws
                  B. Ideal gas law
                  C. Stoichiometry with gases
                  D. Kinetic molecular theory
                VII. Thermochemistry
                    A. Temperature/heat
                    B. Energy and units
                    C. Heats of reaction
                      1. Measuring
                      2. Stoichiometry
                    D. Enthalpy and enthalpy changes
                    E. Hess's Law
                  VIII. Atomic Theory and Periodic Table
                      A. Fundamental particles
                      B. Isotopes
                      C. Binding energy
                      D. Quantum theory
                        1. Quantum numbers
                        2. Energy levels, orbitals
                        3. Electron configuration
                        4. Valence electrons
                      E. Periodic Table and trends
                    IX. Chemical bonding
                        A. Ionic and covalent bonds
                        B. Electron dot structures
                        C. Electronegativity
                        D. Shapes and polarities of molecules - VSEPR
                        E. Molecular orbitals
                      X. Solids and liquids
                          A. General properties
                          C. Changes of state and dynamic equilibrium
                          D. Intermolecular attractions
                          E. Types of substances
                          F. Phase diagrams
                        XI. Solutions
                            A. Definitions
                            B. Terminology
                            C. Concentration calculations
                            D. Colligative properties
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