Standard

R State Standard £ Institutionally Developed College: N/A

AHS 1127 – Health Sciences Chemistry

Course Description

Provides an introduction to basic chemical principles and concepts which explain the behavior of matter. Topics include: measurement and units; atomic structure; chemical bonding; physical states of matter; nomenclature; stoichiometry; liquid mixtures; organic chemistry; and biochemistry.

Competency Areas	Hours
Measurement and Units	Class	4
Atomic Structure	D. Lab	2
Chemical Bonding	P. Lab/O.B.I.	0
Physical States of Matter	Credit	5
Nomenclature
Stoichiometry
Liquid Mixtures
Organic Chemistry
Biochemistry

Prerequisite:	Program admission level math achievement
Corequisite:

Course Guide

Competency	After completing this section, the student will be able to:	Hours
		Class	D.Lab	P.Lab/ O.B.I.

Measurement and Units		2	2	0
Calculations	Perform calculations involving density, specific gravity, mass, and volume measurements.
	Apply the conventions of exponential notation and significant figures to mathematical operations.
Analysis	Use dimensional analysis in calculations involving conversions from one set of units to another.
	Perform gravimetric analysis and volumetric analysis.
Atomic Structure		4	2	0
Theory	Describe modern atomic theory and the three fundamental particles that make up atoms.
	Summarize the basic ideas of quantum mechanics.
Periodic table	Relate the electronic configuration of an atom to its position on the periodic table.
	Predict properties and reactivities of elements.
Chemical Bonding		4	2	0
Chemical bonding	Describe various types of chemical bonding.
Theory	Outline the significance and main ideas of various bonding theories.
Physical States of Matter		4	3	0
Properties of matter	Describe the general properties of gases, liquids, and solids.
	Distinguish among the general properties of gases, liquids, and solids.
	Discuss the types of changes matter undergoes.
Nomenclature		4	0	0
IUPAC nomenclature	Name inorganic compounds by the IUPAC system based on their formulas.
	Write formulas of common inorganic compounds based on their IUPAC names.
Stoichiometry		8	5	0
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.
Acids and bases	Discuss the properties of acids and bases.
Gases	Summarize the general properties of gases.
	Use the gas law equations to describe the behavior of gases.
liquid mixtures		4	2	0
Solutions	Describe properties of a solution.
	Describe methods of expressing concentration.
	Solve problems dealing with concentrations.
Suspensions	Identify properties of a suspension.
Colloidal dispersions	Identify properties of a colloidal dispersion.
Water	Describe its properties and physical constants.
Organic Chemistry		5	2	0
Alkanes	Describe and identify alkanes.
Alkenes and alkynes	Describe and identify alkenes and alkynes.
Aromatic Hydrocarbons	Describe and identify aromatic hydrocarbons.
Hydrocarbon Derivatives	Describe and identify hydrocarbon derivatives.
Organic Polymers	Describe and identify organic polymers.
Biochemistry		5	2	0
Energy requirements of Organisms	Describe energy requirements of organism.
Proteins	Describe and identify proteins.
Enzymes	Describe and identify and enzymes.
Carbohydrates	Describe and identify carbohydrates.
Fats and Oils	Describe and identify fats and oils.
Nucleic Acids	Describe and identify nucleic acids.

Suggested Resources

Media (print/audio/ visual/www/ other)	Author	Year	Title: Subtitle	Edition	Location	Publisher/ Publication	pp.
Print	Adamson, A. W	1986	A textbook of physical chemistry.	3^rd ed,	New York	Elsevier	971
	Bettelheim, B., et.al.	2006	Introduction to general, organic, and biochemistry.	8^th ed.	Belmont, CA	Brooks/Cole	928
	Bettelheim, B., et.al.	2006	Introduction to general, organic, and biochemistry: Student solutions manual.	8	Clifton Park, NY	Centage Delmar	192
	Bretherick, L.	1986	Hazards in the chemical laboratory.	4^th ed.	London	Royal Society of Chemistry	618
	Cotton, F. A., & Wilkinson, G	1999	Advanced inorganic chemistry.	6^th ed.	New York	John Wiley & Sons	1376
	Davis, R. E	1988	Study guide to accompany general chemistry with qualitative analysis	3^rd ed.	Philadelphia	Saunders
	Hein, M., et al.	1988	College chemistry: An introduction to general, organic, and biochemistry	4^th ed.	Pacific Grove	Brooks Cole	903
	Kanare, H. M.	1985	Writing the laboratory notebook.		Washington, DC	Oxford University Press	145
	Lefèvre, M. J.	1990	First aid manual for chemical accidents.	2^nd ed.	New York	Wiley Johns and Son	272
	Loebel, A. B.	1987	Chemical problem solving by dimensional analysis.	3^rd. ed.	Boston	Centage	417
	Mackison, F. W., et al.	1987	NIOSH pocket guide to chemical hazards.	1^st ed.	Washington DC	U.S. Government	424
	Manufacturing Chemists' Association, Inc	1972	Guide for safety in the chemical laboratory.	2^nd ed.	Princeton, N.J.	D. Van Nostrand	505
	Murrell, J. N., et al.	1987	The chemical bond.	2^nd ed.	New York	John Wiley & Sons	346
	Seese, W. S., & Daub, G. W.	1995	Basic chemistry.	7^th ed.	Englewood Cliffs, N.J.	Prentice Hall	232
	Vogel, A. I.	1978	Vogel’s textbook of quantitative inorganic analysis.	4^th ed.	New York	John Wiley & Sons
	Weast, R. C.	1987	Handbook of chemistry and physics.	68^th ed.	Boca Raton, FL	CRC Press	2376
	Weiss. G., et al.	1988	Experiments in general chemistry.		Philadelphia	Saunders
	Whitten, K. W., et al.	1988	General chemistry with qualitative analysis.	3^rd ed.	Philadelphia	Prentice Hall
	Whitten, K. W., et al.	1988	Lecture outline to accompany general chemistry with qualitative analysis.	3^rd. ed.	Philadelphia	Prentice Hall
Audio visuals (film)	Fisher Scientific Company		Safety: Isn’t it worth it?	#229	Pittsburg	Author

Posted: 09/24/08