MOHAWK VALLEY COMMUNITY COLLEGE
UTICA, NEW YORK
COURSE OUTLINE
I.
Catalog Description
CH095--Chemistry Review
C-2, P-3, Cr-0
Prerequisite: High School Math Course A, or a Math Placement Test
Score of 18, or MA050 Introductory Mathematics.
This refresher course is for those with high school chemistry more than
five years ago. Topics include mathematics in chemistry, bonding,
symbols, the periodic table, and atomic structure as well as gas laws,
equilibrium, solutions, concentrations, pH, buffers, and organic functional
groups.
II. Student Objectives
Upon the completion of Chemistry Review, the students will be able to:
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Apply general chemical principles as they pertain to Anatomy and
Physiology.
Relate the observable properties and characteristics of elements,
compounds, and mixtures to the concept of atoms and molecules.
Describe the conditions associated with the solid, liquid and gaseous
states of matter.
Describe the sub-atomic structures of atoms, ions and isotopes, and
relate this information to chemical activity.
Perform stoichiometric calculations involving chemical reactions.
Explain the importance of safety, not only with laboratory chemicals,
but also with chemicals used in the home and job site.
Demonstrate an understanding of the importance of science as a
necessary function for decision making in society.
Generate accurate laboratory records and demonstrate an
appreciation of the importance of record keeping, not only in the
laboratory and class, but also beyond (tax records, nursing charts,
audits, etc.)
-2III. Major Topics
Topics will be chosen from but not limited to the following areas.
1
The Mathematics of Chemistry
Measurements, Metric vs. English
Basic Units of weight, length and volume
Factor Label System for solving problems
Scientific Notation
2
Temperature
Density
Specific Gravity
Physical States of Matter
Energy
Mass and Energy Conservation Laws
3
Atomic Structure
Ionic and Covalent Bonding
Elements
Nomenclature
Chemical Equations
Writing Chemical Equations
Types of Chemical Equations
Exothermic and Endothermic Reactions
Gram Atomic Weight
4
The Mole
Percent Composition
Empirical and Molecular Formulas
Calculations with Empirical and Molecular Formulas
5
Calculations from Chemical Equations
Stoichiometry
Mole-Mole Calculations
Mole-Mass and Mass-Mass Calculations
Limiting Reagent
Yield Calculations
-36
The Gaseous State of Matter
Properties of Gases
Kinetic-Molecular Theory
Boyles'Law
Charles' Law
Standard Temperature and Pressure
Combined Gas Laws
Dalton's Law
Avogadro's Law
Mole-Mass Volume Relationship
Density of gases
Specific Gravity of gases
Ideal Gas Equation
Gaseous Stoichiometry
7
Water and the Properties of Liquids
Evaporation
Vapor Pressure
Surface Tension
Boiling Point
Freezing Point
Changes of State
Structure of the Water Molecule
The Hydrogen Bond
Chemical Properties of Water
8
Solutions
Components of a Solution
General Properties of Solutions
Solubility
Factors of Solubility
Rate of Dissolving Solids
Concentration of Solutions
Colligative Properties
Osmosis and Osmotic Pressure
9
Acids, Bases Salts
Electrolytes
Dissociation and Ionization
pH
Neutralization
Colloids
-410
Equilibrium
Chemical Equilibrium
Factors Effecting Equilibrium
Buffer Solutions
11
Organic Chemistry
Saturated and Unsaturated Hydrocarbons
12
Alcohols, Ethers, Phenols Aldehydes and Ketones
13
Carboxylic Acid, Esters, Amides and Amines
14
Polymers
Carbohydrates
Lipids
Amino Acids
Enzymes
15
Nuclear Chemistry
CHEMISTRY REVIEW CH095 LABORATORY SCHEDULE
Week
Title
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
Safety, Orientation & Check-In
Measurements
Freezing Points --Graphing of Data
Water in Hydrates
Quantitative Precipitation of Carbonate
Double Displacement Reactions
Chemical Equilibrium—Reversible Reactions
Charles’ Law
Properties of Solutions
Ionization--Acids, Bases and Salts
Neutralization - Titration 1 & 2
Models 1 & 2; Hydrocarbons
Alcohols, Esters, Aldehydes and Ketones
Synthesis of Aspirin
Polymers—Macromolecules; Check Out
Feb. 2011