CHEM 1212 - General Chemistry I

7.5 Credits

This is the first half of the one-year general chemistry program for students who have some knowledge of chemistry as indicated by assessment testing or who have recently completed college chemistry with a grade of C or better. Topics include naming, atomic structure; chemical reactions; essentials of bonding; periodic properties; VSEPR theory; modern bonding theories; stoichiometry; thermochemistry; and the chemistry of solids, liquids, and gases. This course includes both lecture and lab components.

Prerequisites: (3) College-level reading, writing, and math proficiency; CHEM 1010 or strong high school chemistry course and MATH 1425

Lecture Hours: 6.0
Lab Hours: 4.5
Internship Hours: 0.0
Clinical or Practicum Hours: 0.0

Course Objectives

demonstrate a logical sequence in problem solving based on the scientific method;
demonstrate an ability to classify matter in terms of composition and then use physical and chemical properties to characterize and separate matter into the classifications;
demonstrate a knowledge of atomic structure and the relationship between atomic structure and compound formation;
explain the correlation between what is happening in a system as viewed on the macroscopic scale with what is actually happening on the sub-microscopic (atomic or molecular) scale;
demonstrate knowledge and application of the periodic table;
write routine chemical formulas and name chemical compounds;
solve problems involving mathematical processes to explain physical or chemical phenomena;
demonstrate a knowledge of chemical bonding and the ability to distinguish the types of bonding based on chemical formulas;
demonstrate the relationship between the formula, the molecular shape and the properties of a compound;
explain the difference between atomic and molecular orbitals as applied to bonding;
write chemical equations to describe what happens in a chemical transformation and classify the reactions based on the transformation;
demonstrate an understanding of the relationship between energy and chemical transformations;
demonstrate an understanding of the properties of an Ideal gas and be able to use mathematical equations to relate the properties of gases;
explain the correlation between what is happening in a system as viewed on the macroscopic scale with what is actually happening on the submicroscopic (atomic or molecular) scale;
demonstrate the ability to quantitatively relate the amounts of substances involved in a chemical transformation;
demonstrate an understanding of the properties of solids, liquids and gases.

For the laboratory component of this course: Students will demonstrate laboratory proficiency in the following areas:

a. awareness of safety requirements in a general chemistry laboratory setting and the location and operation of safety equipment;

b. safe handling, use and disposal of chemicals in the laboratory setting, particularly flammable solvents and acids and bases;

c. proper use and handling of laboratory equipment;

d. relating classroom concepts to a laboratory setting;

e. carrying out specific laboratory techniques both independently and as utilized in a chemistry laboratory including but not limited to:

1. making basic measurements both accurately and precisely

2. studying colligative properties of solutions

3. a study of chemical equilibria

4. a study of the properties and reactions of acids, bases and buffers

5. a study of reaction rates

6. thermodynamics applied to chemical systems

7. electrochemistry

8. qualitative analysis (identifying unknowns)

f. collect and interpret data in the laboratory including the analysis of data for error factors.

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