Standard

R State Standard £Institutionally Developed College: N/A

CHM 1111 – Chemistry I
Course Description Provides an introduction to basic chemical principles and concepts which explain the behavior of matter. Topics include: measurement; physical and chemical properties of matter; atomic structure; chemical bonding; nomenclature; chemical reactions; stoichiometry and gas laws; basic laboratory skills and lab safety procedures.
Competency Areas	Hours
Measurement	D. Lab	4
Physical and Chemical Properties of Matter	P. Lab	0
Atomic Structure	Credit	3
Chemical Bonding		5
Nomenclature
Chemical Reactions
Stoichiometry
Gas Laws
Basic Laboratory Skills and Safety Procedures

Prerequisite:	Program admission
Corequisite:	MAT 1101 or MAT 1111

Course Guide

Competency	After completing this section, the student will be able to:	Hours
		Class	D.Lab	P.Lab/ O.B.I.
Measurement		5	0	3
Measurement	Use basic metric measurement prefixes and factor multipliers to convert units within the metric system. Describe justifications for S.I. convention.
Calculations	Perform calculations involving density, specific gravity, mass, and volume measurements.
	Apply the conventions of exponential notation and significant figures to mathematical operations.
	Convert between the Fahrenheit, Celsius and Kelvin temperature scales.
Analysis	Use dimensional analysis (unit-factor analysis) in calculations involving conversions from one set of units to another.
	Perform gravimetric analysis and volumetric analysis.
Physical and Chemical Properties of Matter		5	0	3
Properties of matter	Describe and distinguish the general properties of gases, liquids, and solids.
	Explain changes of state (phase changes) in matter and relate to heat.
	Define physical and chemical changes of matter.
	Classify an element as a metal, non-metal or metalloid and relate this to its position on the periodic table.
	Identify diatomic elements.
	Determine the relative electron negativity, atomic radius and other characteristics of an atom by its position on the periodic chart.
	Describe pure substances and mixtures. Introduce mixture separation strategies.
Atomic Structure		5	0	3
Theory	Describe Dalton’s model, Bohr’s model and the modern quantum mechanical theory of atomic structure.
	Describe the electron configuration of any element and how its electron configuration relates to its properties and its position on the periodic table.
Periodic table	Relate the electronic configuration of an element to its position on the periodic table.
	Describe the electronic configuration of any element on the periodic table and how it relates to an element’s properties.
Chemical Bonding		5	0	4
Chemical bonding	Describe and identify ionic and covalent bonding and van der Waals forces.
Theory	Draw Lewis dot structures for molecules.
	Determine the charge of monoatomic ions and simple inorganic radicals. Explain oxidation numbers of elements and compounds.
	Assign electronic geometry and molecular geometry from Lewis dot structure of a molecule.
Nomenclature		5	0	3
IUPAC nomenclature	Name inorganic compounds by the IUPAC system based on their formulas.
	Write formulas of common inorganic compounds based on their IUPAC names.
	Determine if a compound is an acid, base, salt, or covalent compound.
Chemical Reactions		5	0	3
Mole Concept	Calculate molar mass and percent composition of compounds.
	Convert between mass, moles, and number of atoms using formula, formula weight, and Avogadro’s number.
	Calculate empirical formulae and molecular formulae of compounds.
Chemical Equations	Write and balance chemical equations.
Stoichiometry		5	0	5
Calculations	Perform calculations involving composition stoichiometry and reaction stoichiometry.
Classification	Classify chemical reactions as to type of reaction. Write examples of each type of chemical reaction.
Gas Laws
Gases	Summarize the general properties of gases and relate them to the kinetic molecular theory of gases.
	Describe factors that affect the pressure, volume, and temperature of a gas.
	Solve problems associated with gas laws including: Boyle’s Law, Charles’s Law, Gay-Lussac’s Law, Combined Gas Law, Dalton’s Law of Partial Pressures, and Ideal Gas Law.	4	0	5
Basic Laboratory Skills and safety procedures		1	0	1
Safety	Describe safety rules used in the chemistry lab including the use of MSDS, safety shower, eye wash station, storage of chemicals, use of acids, use of Bunsen burner and other items related to safety.

Suggested Resources

Media (print/audio/ visual/www/ other)	Author	Year	Title: Subtitle	Edition	Location	Publisher/ Publication	pp.
Print	Bettelheim, Brown, and March	2006	Introduction to General, Organic and Biochemistry.	8^th ed.	Clifton Park, NY	Centage
	Block and McKelvy	2006	Lab Experiments for General Chemistry.	5^th ed.	Clifton Park, NY	Centage
	Brady and Senese	2007	The Study of Matter and Its Changes.	5^th ed.	New York	John Wiley and suns
	Brown, LeMay and Bursten.	2005	The Central Science, 10th Ed		Philadelphia	Prentice Hall

Posted: 10/01/08