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Official Course
Description: MCCCD Approval:
4-27-2010 |
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CHM130 2010 Fall – 2011 Summer II |
LEC 3.0 Credit(s) 3.0 Period(s) 3.0 Load Acad |
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Fundamental
Chemistry |
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A survey of the fundamentals of general chemistry. Emphasis on essential concepts and
problem solving techniques. Basic
principles of measurement, chemical bonding, structure and reactions,
nomenclature, and the chemistry of acids and bases. Preparation for students taking more
advanced courses in chemistry.
Designed to meet needs of students in such diverse areas as
agriculture, nursing, home economics, physical education and water
technology. Prerequisites: Grade of "C" or
better in CHM090, or MAT090, or MAT091, or MAT092, or MAT093, or MAT102, or
(MAT103AA and MAT103AB), or satisfactory score on math placement exam. |
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Go to Competencies Go to Outline
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MCCCD
Official Course Competencies: |
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CHM130 2010
Fall – 2011 Summer II |
Fundamental Chemistry |
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1.
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Define "chemistry" and describe its main
branches. (I) |
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2.
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Describe the relationships between matter and energy. (II)
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3.
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Distinguish between physical and chemical properties and
changes. (II) |
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4.
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Interpret symbols and formulas in terms of numbers and
kinds of atoms. (II) |
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5.
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Describe the physical states of matter with the aid of the
Kinetic Molecular theory. (II, IX) |
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6.
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Classify matter as elements, compounds, or mixtures. (II) |
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7.
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Describe the properties of metallic and non-metallic
elements. (II) |
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8.
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Use the Unit-Factor Method in solving chemistry-related
problems. (III) |
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9.
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Name and write formulas for simple inorganic compounds.
(IV, VII) |
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10.
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Describe the relationship between the outer electronic
structure of atoms and their chemical properties. (V) |
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11.
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Use the Periodic Table to estimate the properties of
elements and compounds. (V) |
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12.
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Characterize the fundamental particles comprising the atom
with respect to charge and mass. (V) |
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13.
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State the number of protons, electrons, and neutrons in
any given isotope, neutral or charged. (V) |
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14.
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Use the
Periodic Table in predicting the number of electrons, formula for a compound,
and metallic or nonmetallic characteristics. (V) |
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15.
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Draw a Lewis structure (electron dot) for a given ion or
compound. (VI) |
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16.
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State the type of intermolecular force that exists for a
given substance. (VI) |
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17.
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Describe the properties of ionic and covalent compounds.
(VI) |
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18.
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Describe the shape and polarity of simple molecules. (VI) |
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19.
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Complete and balance simple chemical equations. (VIII) |
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20.
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Solve elementary stoichoimetry problems.
(VIII) |
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21.
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Classify a reaction as endothermic or exothermic. (VIII) |
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22.
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List the factors affecting the rate of a reaction. (VIII) |
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23.
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Describe the chemical and physical properties of water.
(IX) |
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24.
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Describe the properties of solutions. (X) |
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25.
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Identify substances as electrolytes or nonelectrolytes.
(X) |
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26.
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Classify substances as acids, bases, or salts. (XI) |
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27.
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Explain the behavior of buffer systems. (XI) |
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28.
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Define the pH scale of measuring the relative acidity of
solutions. (XI) |
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29.
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Define and identify redox
reaction as exemplified by single replacement and combustion reactions. (XII)
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Go to Description Go to top of
Competencies
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MCCCD
Official Course Outline: |
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CHM130 2010
Fall – 2011 Summer II |
Fundamental Chemistry |
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I. Definition of chemistry II. Properties of matter A. State of matter B. Classification of matter
C. Physical vs chemical changes D. Energy III. Measurement A. Metric system B. Unit-factor method of
solving problems C. Density D. Temperature scales IV. Mole concept A. Atomic and molecular
weights B. Mass-mole conversions C. Percentage composition V. Atomic theory and
periodic table A. Fundamental particles B. Isotopes C. Quantum theory 1. Energy levels 2. Orbitals
3. Electron configuration 4. Valence electrons D. Periodic Table and
trends E. Electronegativity
VI. Chemical bonding A. Ionic and covalent bonds
B. Electron dot structures C. Shape and polarity of
molecules VII. Nomenclature A. Binary and ternary B. Ionic-Stock C. Covalent-classical VIII. Chemical equations A. Balancing equations B. Types of chemical
reactions C. Stoichiometry
D. Heats of reaction E. Rates of reactions F. Driving forces G. Equilibrium IX. Properties of solids,
liquids, and gases A. Kinetic molecular theory
B. Changes of state
(terminology involved) C. Properties of states D. Inter-molecular forces
and changes of state E. Water, hydrogen, and
oxygen X. Solutions A. Definition B. Properties C. Weight percent
concentration D. Molarity
E. Terminology XI. Acids-bases A. Arrhenius definitions B. Bronsted/Lowry
definition C. pH scale D. Buffers XII. Electrochemistry A. Oxidation/reduction B. Redox
reactions |
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Go to Description Go to top of
Competencies Go to top of Outline