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Official Course
Description: MCCCD Approval: 6-28-2011 |
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CHM130AA
2011 Fall – 2012 Spring |
L+L 4.0 Credit(s) 6.0 Period(s) 5.4 Load Acad |
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Fundamental Chemistry with Lab |
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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. Course Notes: Student may receive credit for only one of the following: CHM130 and CHM130LL, or CHM130AA. Course
Attribute(s): General Education Designation: Natural Sciences (Quantitative) - [SQ] |
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Go to Competencies Go to Outline
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MCCCD Official Course Competencies: |
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CHM130AA 2011 Fall – 2012 Spring |
Fundamental Chemistry
with Lab |
1. Define
"chemistry" and describe its main branches. (I)
2. Describe
the relationships between matter and energy. (II)
3. Distinguish
between physical and chemical properties and changes. (II)
4. Interpret
symbols and formulas in terms of numbers and kinds of atoms. (II)
5. Describe
the physical states of matter with the aid of the Kinetic Molecular theory.
(II, IX)
6. Classify
matter as elements, compounds, or mixtures. (II)
7. Describe
the properties of metallic and non-metallic elements. (II)
8. Use
the Unit-Factor Method in solving chemistry-related problems. (III)
9. Name
and write formulas for simple inorganic compounds. (IV, VII)
10. Describe
the relationship between the outer electronic structure of atoms and their
chemical properties. (V)
11. Use the
Periodic Table to estimate the properties of elements and compounds. (V)
12. Characterize
the fundamental particles comprising the atom with respect to charge and mass.
(V)
13. State the
number of protons, electrons, and neutrons in any given isotope, neutral or charged.
(V)
14. Use the
Periodic Table in predicting the number of electrons, formula for a compound,
and metallic or nonmetallic characteristics. (V)
15. Draw a
Lewis structure (electron dot) for a given ion or compound. (VI)
16. State the
type of intermolecular force that exists for a given substance. (VI)
17. Describe
the properties of ionic and covalent compounds. (VI)
18. Describe
the shape and polarity of simple molecules. (VI)
19. Complete
and balance simple chemical equations. (VIII)
20. Solve elementary
stoichoimetry problems. (VIII)
21. Classify a
reaction as endothermic or exothermic. (VIII)
22. List the
factors affecting the rate of a reaction. (VIII)
23. Describe
the chemical and physical properties of water. (IX)
24. Describe
the properties of solutions. (X)
25. Identify
substances as electrolytes or nonelectrolytes. (X)
26. Classify
substances as acids, bases, or salts. (XI)
27. Explain the
behavior of buffer systems. (XI)
28. Define the
pH scale of measuring the relative acidity of solutions. (XI)
29. Define and
identify redox reaction as exemplified by single
replacement and combustion reactions. (XII)
30. Identify
and evaluate chemical hazards and hazard warning signs (such as the 4-bar
Hazardous Material Information System, the 4- diamond National Fire Protection
Association System, and Material Safety Data Sheets). (I)
31. Record
observations accurately, using appropriate chemical terminology. (III)
32. Prepare
written reports, present data in a logical format, analyze data, and report conclusions.
(III)
33. Use
scientific measuring devices to obtain chemical data and report these
measurements with the proper number of digits. (III)
34. Apply
principles, concepts, and procedures of chemistry to lab experiments. (II-XII)
35. Use the
scientific method in interpreting chemical data to arrive at rational
conclusions. (II-XII)
36. Use lab
equipment properly and safely to perform a variety of chemical procedures and
techniques. (II-XII)
37. Cite the
location and operation of common laboratory safety equipment. (I)
Go to Description Go to top of Competencies
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MCCCD Official Course Outline: |
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CHM130AA 2011 Fall – 2012 Spring |
Fundamental Chemistry
with Lab |
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