Standard

 

R State Standard         £Institutionally Developed          College: N/A

 

 AHS 1015 – Basic Inorganic Chemistry

Course Description

Introduces chemical concept principles, laws, and techniques applicable to the medical laboratory. Topics include: laboratory safety; fundamental principles of chemistry; weight and measures; solutions; and basic laws of chemistry.

 

Competency Areas

Hours

Laboratory Safety        

Class

3

Fundamental Principles of Chemistry

D. Lab

2

Weight and Measures

P. Lab

0

Solutions

Credit

4

Basic Laws of Chemistry

 

 

 

Prerequisite:

MAT 1012

Corequisite:

 

 

Course Guide

 

Competency

After completing this section, the student will be able to:

Hours

Class

D.Lab

P.Lab/

O.B.I.

 

 

 

 

Laboratory Safety           

6

0

0

Facilities and equipment safety

Identify lab safety equipment.

 

 

 

Glassware

Identify the types and uses of glassware.

 

 

 

Chemicals

Identify chemical hazards.

 

 

 

List safety precautions.

 

 

 

Fundamental Principles of Chemistry

6

0

0

Properties and laws

Compare solids, liquids, and gases.

 

 

 

Discuss the laws of conservation of energy and mass.

 

 

 

Radioactivity

Interpret the periodic table of the elements.

 

 

 

Atoms and atomic structure

Draw a Bohr model of an atom and label its parts.

 

 

 

Light

Discuss emission properties and uses of excited atoms.

 

 

 

Weight and Measures

6

10

0

English, Metric, S.I.

Convert among English, Metric, and S.I. units of measurement.

 

 

 

Temperature

Measure temperature and convert readings between Fahrenheit, Celcius and Kelvin scales.

 

 

 

Density and specific gravity

Calculate density and specific gravity from appropriate mass and volume data.

 

 

 

Record measurements with the correct number of significant figures.

 

 

 

Apply significant figures conventions to calculated values.

 

 

 

SOLUTIONS

6

10

0

Percent composition

Calculate percent composition from chemical formulas.

 

 

 

Molecular weight

Determine molecular weight of a compound from its formula.

 

 

 

Avogadro's number and moles

Calculate concentration (including use of  per cent (%), molarity and normality) or volume in dilution and titration problems.

 

 

 

BASIC LAWS OF CHEMISTRY

6

0

0

Ionic and covalent bonds

Differentiate between ionic and covalent bonds.

 

 

 

Molecular formulas

Construct ionic compound formulas from ions.

 

 

 

Balancing equations

Balance chemical equations.

 

 

 

Types of reactions

Identify reactions as single displacement, double displacement, combination or decomposition reactions.

 

 

 

Factors which influence reactions

List factors which affect reactions.

 

 

 

Kinetic molecular theories

Discuss key points of kinetic molecular theory.

 

 

 

Barometric pressure

Explain the measurement of barometric pressure.

 

 

 

Partial pressure

Use Hess’s Law to calculate partial pressure of a gas in a mixture or total pressure of a mixture of gases.

 

 

 

(O2 and CO2)

Apply gas laws to problems involving the respiratory gases oxygen and carbon dioxide.

 

 

 

Types and properties of acids, bases, and salts

Identify and write formulas for common acids, bases, and salts.

 

 

 

Chemical formulas of acids, bases and salts

Calculate pH from [H+] or [H3O+].

 

 

 

Reactions between acids and bases

Describe chemical reactions between acids and bases.

 

 

 

 

Suggested Resources

 

Media
(print/audio/
visual/www/
other)

Author

Year

Title: Subtitle

Edition

Location

Publisher/
Publication

pp.

Print

Baker, F. J. & Silverton, R. E.

1998

Introduction to medical laboratory technology

7th ed.

 

A. Hodder Arnold

448

Bennington, J. L.

1984

Saunders’ dictionary and encyclopedia of laboratory medicine & technology

1st ed.

Philadelphia

Saunders

1700

Bettelheim, B., et.al.

2006

Introduction to general, organic, and biochemistry.

8th ed.

Belmont, CA

Brooks/Cole

928

Bishop, M. L., et. al.

2004

Clinical chemistry: Principles, procedures, correlations.

2nd ed.

Philadelphia

Lippincott, Williams, & Wilkins

704

Block, T. & McKelvy, G.

2005

Lab experiments for general chemistry.

5th ed.

Belmont, CA

Brooks/Cole

400

Campbell, J. M. & Campbell, J. B.

1997

Laboratory mathematics: Medical & biological applications.

5th ed.

Philadelphia

Elsevier: Mosby

496

Estridge, Barbara

2002

Basic medical laboratory techniques.

4th ed.

Philadelphia

Prentice Hall

640

Lide, David

2007

CRC handbook of chemistry and physics.

88th ed.

Boca Raton

CRC Press

2640

Sackheim, G. & Lehman, D.

1997

Chemistry for the health science

8th ed.

Philadelphia

Prentice Hall

643

Walters, N.J, et al.

1999

Basic medical laboratory techniques.

4th ed.

Clifton Park, NY

Centage  Delmar

412

 

Posted: 09/24/08