CHEM V20
COURSE OBJECTIVES:
1. The student will be able to apply the fundamental laws of chemistry to the solution of written problems and questions.
2. The student will be able to solve problems involving the conversion of units between various systems by means of the unit factor method.
3. The student will demonstrate his or her knowledge of the application of chemistry laws and their application to his or her environment through his or her written assignments and exams.
4. The student will develop the ability to intelligently discuss current events and problems involving chemistry with his or her peers and instruction.
5. The minimum level of acceptable performance of the above objectives is 60%.
Representative Text:
Hein, "Foundations of College Chemistry", 10th ed., 2000, International V Thompson Publisher
PREREQUISITE SKILLS REQUIRED
Before entering Chem 20, the student should be able to:
1. add, subtract, multiply and divide real numbers;
2. understand the properties of real numbers;
3. understand the properties of equality and inequality;
4. solve elementary linear and quadratic equations;
5. translate elementary word problems into linear equations and find their solutions;
6. combine exponentials using the properties of exponents;
7. convert numbers into scientific notation;
8. factor elementary polynomials;
9. add, subtract multiply, and divide elementary polynomials and rational expressions;
10. solve elementary equations containing radicals and rational expressions;
11. simplify elementary complex fractions;
12. graph elementary linear and quadratic equations;
13. solve elementary systems of two linear equations;
14. add, subtract, multiply, divide and simplify radicals.
EXIT SKILLS
Upon completion of Chem 20, the student will be able to:
1. use significant figures and scientific notation;
2. use the metric system and do metric/English conversion;
3. give the symbols of the common elements, and the structure of simple molecules;
4. write formulas and give names for cannon salts, acids, and molecular compounds;
5. perform mole calculations up to and including limiting reactant stoichiometry problems;
6. use mass, volume, and length measuring devices and know their relative precision;
7. use chemicals, including strong acids and bases, safely;
8. use common laboratory equipment like beakers, flasks, funnels, etc. properly;
9. handle various glassware correctly;
10 perform acid-base testing with litmus paper or by other means;
11 safely perform a variety of laboratory procedures.
COURSE CONTENT
A. Introduction to chemistry (1/4 week)
1. The scientific method
2. History of chemistry
3. Branches of chemistry
4. Interrelationship of the sciences
B. Mathematical review (1/2 week)
1. Elementary algebra
2. Use of exponentials
3. Significant numbers
4. Precision of measurements
5. Calculations of errors
C. Measurements (1/2 week)
1. The metric system
2. Temperature conversions, calories
3. Density, specific gravity
D. Matter (1/2 week)
1. Physical states
2. Substances and mixtures
3. Physical and chemical changes
4. Conservation of energy
5. Energy in ordinary and nuclear chemical reactions
E. Compositions of matter (3/4 week)
1. Elements and compounds
2. Symbols and formulas
3. Simple equations
4. Law of definite compositions
5. Law of multiple proportions
F. The atom (1 week)
1. Dalton's atomic theory
2. Development of the structure of the atom
3. Modern concept of structure of the atom
4. Isotopes
G. Mass and the atom (1 week)
1. Atomic, molecular weights
2. The mole
H. The Periodic Table (1 week)
1. History
2. Periods and groups
3. Relationship of electronic structure to chemical and physical properties of the elements
I. Chemical bonding (1 week)
1. Ionic and covalent bonding
2. Polarity of bonds and molecules
3. Oxidation numbers
J. Nomenclature (2 weeks)
1. Inorganic compounds - binary and tertiary compounds
2. Organic compounds - alkanes, alkenes, alkynes, simple aromatic compounds,
alcohols, carboxylic acids, aldehydes, Ketones, alkythalides, ethers, amines, amides,
nitrites, amino acids
3. Structural formulas and isomerism
K. Quantitative composition of compounds (1 week)
1. Percentage composition
2. Empirical formula
3. Molecular formula
L. Chemical equations (2 weeks)
1. Balancing simple equations by inspections
2. Balancing oxidation - reducing equations by use of oxidation numbers
3. Mass and mole relationships in chemical equations
4. Types of chemical reactions
5. Reasons a chemical reaction occurs
6. Heat involved in chemical reactions
M. Stoichiometry (2 weeks)
1. Mole and weight relationship
2. Theoretical yield 3. Percentage yield
4. Calculation of amount of reactants
5. Limiting reagents
N. Gases (1 week)
1. Kinetic molecular theory
2. Graham's Law of Diffusion
3. Dalton's Law of Partial Pressure
4. Avogodno's Hypothesis
5. Boyle's Law
6. Charles' Law
7. Quantitative relationship between moles, pressure, volume,and temperature of gases
in the chemical equation
O. Liquids (1/2 week)
1.The hydrogen bond
2. Vanderwaal's forces
3. The chemistry of water
4. Freezing, boiling, evaporation, vapor pressure
P. Solutions (1/2 week)
1. Solids, liquids and gases
2. Factor affecting solubility
3. Expressing concentration of solutions
4. Colligative properties
Q. Ionization (1/2 week)
1. Acids, bases and salts
2. pH
3. Neutralization
4. Ionic equations
5. Titration
R. Carbon and organic chemistry (1 week)
1. Inorganic compounds
2. Carbon to carbon bonds - single, double, triple
3. Formation and a few typical reactions of the alkanes, alkenes, alkynes aromatic series, alcohols, carboxylic acids, aldehypes
ketones, alkylhalides, ethers, amines, amides, nitrides, and amino acids
4. Principal sources and uses
S. Biochemistry (1/2 week)
1. Carbohydrates,
2. Nucleic acids,
3. Enzymes
4. Vitamins
5. Hormones
6. Photosynthesis