Standard

R State Standard £ Institutionally Developed College: N/A

CHM 1213 – Survey of Inorganic Chemistry
Course Description Provides an introduction to basic chemical principles and concepts which explain the behavior of matter. Topics include: measurements and units; structure of matter; chemical bonding; chemical reactions; gas laws; liquid mixtures; acids and bases; salts and buffers; nuclear chemistry; basic laboratory skills and safety procedures.
Competency Areas	Hours
Measurements and Units	Class	4
Structure of Matter	D. Lab	0
Chemical Bonding	P. Lab/O.B.I.	3
Chemical Reactions	Credit	5
Gas Laws
Liquid Mixtures
Acids and Bases
Salts and Buffers
Nuclear Chemistry
Basic Laboratory Skills and Safety Procedures

Prerequisite:	MAT 1111
Corequisite:

Course Guide

Competency	After completing this section, the student will be able to:	Hours
		Class	D.Lab	P.Lab/ O.B.I.
Measurements and Units		2	0	2
Metric, S.I., and English systems	Convert among metric, English, and S.I. units using dimensional analysis (unit-factor analysis).
	Be able to use scientific notation.
Density and specific gravity	Measure and solve problems of density and specific gravity.
Temperature scales	Measure temperature, understand and convert between Fahrenheit, Celsius, and Kelvin scales.
Structure of Matter		5	0	3
Atomic structure	Identify the three subatomic particles, their properties, and relationships.
Atomic mass and atomic number	Determine and explain significance of atomic number and mass number.
Electron configurations	Describe atomic structure relating to energy level, sublevels, orbitals, and electrons.
Periodic table	Relate atomic structure to the arrangement of the periodic table.
Composition of matter	Compare the composition of elements, compounds, and mixtures.
States of matter	Describe the physical basis of the solid, liquid, and gaseous states of matter.
	Determine melting point and boiling point. Describe the energy considerations of phase changes.
Chemical Bonding		5	0	3
Types of bonds Molecular formulas and compounds	Describe ionic, polar, and non-polar covalent bonds. Describe van der Waals interactions.
	Describe the formation of stable (unstable) ions.
	Determine electron-dot structure for atoms, ions, radicals, and covalent compounds.
	Name ionic and covalent compounds using IUPAC inorganic nomenclature.
	Calculate ionic charges from a chemical formula. Define basic rules of oxidation numbers.
Molecular weight	Calculate the molecular weight of a compound from chemical formula.
Empirical Formulae	Determine the empirical formula from percent composition data.
Chemical Reactions		8	0	5
Types of reactions	Identify the basic types of chemical reactions.
Oxidation-reduction reactions (RE-DOX)	Describe oxidation and reduction. Identify oxidizing and reducing agents.
Equations	Describe reactions with balanced equations.
Mole Concept	Describe Avogadro’s number as it relates to the mole concept.
Stoichiometry	Use stoichiometry to balance molar relationships and masses of species in a chemical reaction.
Equilibrium	Describe reaction theory and collision theory. Explain activation energy and catalysts.
	Identify factors that affect an equilibrium reaction.
	Interpret the meaning of equilibrium constant.
	Calculate the equilibrium constant for a given reaction.
	Explain Le Chatelier’s Principle.
Reaction rates	Define reaction kinetics and the meaning of forward and reverse rates. Describe factors which affect the rate of reaction.
	Describe the difference between rate and equilibrium.
GAS LAWS		4	0	3
Properties of gases	Describe the kinetic molecular theory as it relates to the properties of gases.
Gas laws	Interpret and compare Boyle’s Law, Charles’ Law, and Gay Lusaac’s Law.
	Interpret Dalton’s Law and Graham’s Law.
	Demonstrate calculations using the combined gas law and ideal gas law.
Liquid Mixtures		4	0	3
Solutions	Describe properties of a solution.
	Describe methods of expressing concentration, including percent w/w, percent w/v, and molarity.
	Solve problems calculating concentrations and converting concentrations to different units.
Suspensions	Identify properties of a suspension.
Colloidal dispersions	Identify properties of a colloidal dispersion.
Water	Describe the properties and physical constants of water.
Acids and Bases		7	0	5
Acids and bases	Identify the properties, uses, and reactions of acids and bases.
Ionization	Describe ionization as it relates to acid or base strength.
	Briefly describe the Arrhenius and Bronsted-Lowry models of acids and bases.
pH	Explain pH scale. Calculate pH from [H3O^+] or [OH^-].
Salts and Buffers		2	0	3
Reactions of acids and bases	Describe the formation of salts in a neutralization reaction.
Buffer solutions	Explain how buffers maintain pH. Relate this to Le Chatelier’s Principle.
Nuclear Chemistry		2	0	2
Radioactive decays	Explain alpha, beta, and gamma decay.
BASIC LABORATORY SKILLS AND SAFETY PROCEDURES		1	0	1
Skills and 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, & March	2006	Introduction to general, organic and biochemistry.	8^th ed.	Belmont, CA	Brookes/Cole
	Block & McKelvy	2006	Lab experiments for general chemistry.	5^th ed.		Thomson
	Brady, James E. & Senese, Fred	2007	Chemistry: The study of matter and Its changes.	5^th ed.		Wiley, Johns, & Sons	1144
	Brown, LeMay & Bursten	2006	Chemistry: The central science.	10^th ed.		Prentice Hall
	Burns, Ralph	2004	Fundamentals of chemistry.	4^th ed.		Prentice Hall
	Chang, R.	2005	Chemistry.	8^th ed.		McGraw-Hill
	Denniston, Katherine J. & et. al,	2006	General, organic, and biochemistry.	5^th ed.		McGraw-Hill
	Kelter, Mosher, & Scott	2008	Chemistry: The practical approach.		Boston	Houghton Mifflin
	Kotz, Treichel & Weaver	2006	Chemistry and chemical reactivity	6^th ed.		Brooks Cole
	Masterton & Hurley	2008	Chemistry: Principles and reactions	6^th ed.		Brooks Cole
	Moore, Stanitski & Jurs	2007	Chemistry: The molecular science.	3^rd ed.		Delmar
	Olmsted & Williams	2004	Chemistry.	4^th ed.		Wiley, Johns, & Sons
	Sackheim & Lehman.	1998	Chemistry for the health sciences.	8^th ed.		Prentice Hall
	Stanton, Zhu & Atwood	2005	Experiments in general chemistry.	1^st ed.		Brooks/Cole
	Tro, Nivaldo J.	2006	Introductory chemistry.	2^nd ed.		Prentice Hall,
	Whitten, Davis, Peck & Stanley	2006	General chemistry.	8^th ed.		Brooks/Cole
	Zumdahl, Steven	2007	Basic chemistry.	6^th ed.	Boston	Houghton Mifflin

Posted: 10/01/08