MOHAWK VALLEY COMMUNITY COLLEGE
UTICA, NEW YORK
COURSE OUTLINE
I. Catalog Description
CH091--Essentials of Chemistry 1
C-2, P-3, Cr-0
Prerequisite: An appropriate Mathematics Placement Test result or
MA045 Basic Math Skills or MA050 Introductory Mathematics.
This course introduces chemistry for those who have had no prior
chemistry study or who need a chemistry review. Topics include matter,
measurement, atomic structure and the periodic table, chemical bonding
and reaction, and the three phases of matter. This course does not fulfill a
laboratory natural science requirement in any degree or certificate
program.
II. Student Learning Outcomes
Many students graduate from high school without high school Chemistry.
Some of these students then apply to College programs that require high
school Chemistry as a pre-requisite. Essentials of Chemistry 1 and 2 are
intended to help students overcome this obstacle.
Upon the completion of Essentials of Chemistry 1, the students will be
able to:
1. Relate the observable properties and characteristics of elements,
compounds, and mixtures to the concept of atoms and molecules.
2. Recognize the states of matter and conditions associated with them.
3. Describe the sub-atomic structures of atoms, ions and isotopes, and
relate this information to chemical activity.
4. Utilize the strategy of dimensional analysis to solve problems.
5. Perform stoichiometric calculations involving chemical reactions.
6. Apply the law of conservation of mass to balance formula equations.
7. Write the names and formulae for inorganic compounds.
8. Predict the physical and chemical properties of compounds.
9. Appreciate the usefulness of chemistry in other areas of study.
10. Demonstrate appropriate safety techniques and proper use of
protective equipment.
11. Demonstrate skills in measuring and recording data.
-2-
III. Main Topics
1. Matter and Measurement
a. Elements - Compounds – Mixtures
(i) Symbols of Elements in Chemical Formulas
b. Measurements in Chemistry
c. Metric system
d. Density
e. Dimensional Analysis
f. Unit Conversions
g. Properties of Matter
h. Changes in Matter
i. Energy
j. Heat
2. Atomic Structure and the Periodic Tables
a.
b.
c.
d.
e.
f.
Dalton's Atomic Theory
Nuclear Atom
Bohr Model
Electron Configuration
Periodic Table
Elements
(i) Isotopes
(ii) Atomic Number
(iii) Mass Number
3. Nomenclature
a. Ionic Compounds
b. Molecular Compounds
4. Chemical Equations
a.
b.
c.
d.
e.
f.
Balancing Chemical Equation (The Law of Conservation of Mass)
Types of Chemical Reactions
The Mole and Avogadro's Law
Molecular and Formula Masses
Molecular formula
Stoichiometry
(i) Mole Ratios
(ii) Mass-Mass Calculations
-35. Chemical Bonds
a. Lewis Structure (Electron Dot)
b. Ionic Bonding
c. Covalent Bonding
(i) electronegativity
(ii) bond polarity
d. Lewis Formulas - Octet Rule
e. Polyatomic Ions
6. Gases
a.
b.
c.
d.
e.
f.
g.
h.
i.
j.
Kinetic Molecular Theory
Boyle's Law
Charles' Law
Molar Volume of a Gas (Avogadro's Law)
Combined Gas Law
Ideal Gas Law
Henry's Law
Dalton's Law of Partial Pressures
Density of Gases
Stoichiometry in the Gas Phase
ESSENTIALS OF CHEMISTRY I PRACTICUM SCHEDULE MAY INCLUDE
BUT NOT BE LIMITED TO THE FOLLOWING TOPICS
Week
1
2
3
4
5
6
7
8
9
10
11
12
13
14
Whole Numbers and Decimals
Signed Numbers
Powers of Ten Logarithms
Measurement Concepts and Dimensional Analysis
Metric System Density and SG
The Division and Properties of Matter
Atomic Structure
Chemical Bonding and Formula Writing
Naming Compounds
Balancing Chemical Equations
Weight Relations in Chemistry
Chemical Equations and Stoichiometry
The Gas Laws
REVIEW
-4ESSENTIALS OF CHEMISTRY I LABORATORY SCHEDULE
Week
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
Feb. 2011
Check-in and Safety
Lab Techniques
Measurements
Preparation and Properties of O2
Freezing Point Graphing
Periodic Table
Calorimetry and Specific Heat
Water in Hydrates
Composition of Potassium Chlorate
Single Displacement Rx
Double Displacement Rx
Quantitative Preparation of Potassium Chloride
Boyle's Law
Charles’ Law
Check-out