|Course||Course Title||Credit Hours|
|CHEM 111||General Chemistry 1||(4-3) 4 Cr. Hrs.|
This course is designed as a first course in a traditional one-year program in general college chemistry and includes fundamental concepts such as chemical formulas, chemical equations, laws of chemical combination and physical, chemical and nuclear properties. Atomic and molecular structure, bonding, stoichiometry, periodicity, gases, solutions, acids, bases, oxidation-reduction and nuclear chemistry are also covered in this course. Laboratory work correlates with lecture and stresses the major concepts in this course.
(A requirement that must be completed before taking this course.)
- CHEM 051 or equivalent with a grade of 2.0 or better.
- MATH 113 or equivalent. Math may be concurrent.
Upon successful completion of the course, the student should be able to:
- Differentiate between the information (measurements, observations) and the explanations (hypotheses, theories, laws) of natural phenomena in application of the Scientific Method.
- Formulate solutions to mathematical problems using the technique of dimensional analysis.
- Apply the rules of significant figures both to reading measurements from scales and to the results of calculations that use measurements.
- Interpret element symbols, chemical formulas and chemical equations.
- Employ the modern model of atomic structure.
- Differentiate between physical, chemical and nuclear properties and changes.
- Predict modes by which unstable nuclei decay.
- Write balanced equations describing nuclear reactions.
- Employ the Bohr and Quantum Mechanical models of electronic structure to describe atoms and formation of chemical bonds.
- Predict the properties and characteristics of elements based on patterns and relationships found within the Periodic Table.
- Employ ionic bonding models.
- Write correct names or formulas of chemical compounds.
- Differentiate between ionic and molecular compounds.
- Apply Electron Dot Structures to ionic and covalent bonding.
- Employ VSEPR theory, valence bond theory and hybridization and the basics of molecular orbital theory to describe covalent bonding and shapes of molecules/polyatomic ions.
- Analyze the bond type and three-dimensional shape of a molecule to determine intermolecular forces and relative physical properties.
- Relate the physical states of matter (solid, liquid, gas) and their characteristic macroscopic properties to the molecular or ionic structure of matter.
- Apply the concepts of solution chemistry.
- Solve a variety of mathematical problems relating to chemical quantities, including basic mole concept, stoichiometric relationships, molarity, solution stoichiometry, density, yield determination, percent composition and formula determination.
- Differentiate between various types of chemical reactions.
- Write balanced molecular and ionic equations for reactions in aqueous solution.
- Apply the concepts of acids and bases to analyze and predict the behavior of various acid-base systems.
- Employ appropriate methods for balancing chemical equations, including the half-reaction method and/or other appropriate methods to balance oxidation-reduction equations.
- Relate the macroscopic behavior of gases to the premises of the Kinetic-Molecular Theory of Gases.
- Use the gas laws to calculate properties and quantities of gases under various conditions.
- Apply a working knowledge of laboratory safety, including proper use of safety equipment (e.g. protective eyewear) and safe work habits.
- Utilize laboratory equipment in the performance of laboratory experiments.
- Organize laboratory data, calculations and analyses in an accurate and detailed fashion.
- Execute appropriate chemical disposal procedures in the laboratory.
- Demonstrate interpersonal communication and group work skills while cooperating with other students to complete laboratory experiments.
Note: This course may not be offered every semester.
Please check the CHEM section of the current course schedule for availability.