Course Outline for Chemistry 30A
Introductory and Applied Chemistry I

Effective: Fall 2017
SLO Rev: 10/03/2016
Catalog Description:

CHEM 30A - Introductory and Applied Chemistry I

4.00 Units

Chemistry of inorganic compounds, atomic theory, bonding, equations, gas laws, solutions, acid-base theory and oxidation-reduction. Designed to meet the requirements of certain programs in allied health and technological fields and for general education.
Prerequisite: MTH 65, MTH 65B or MTH 65L or MTH 53 or MTH 53B.
1905.00 - Chemistry, General
Letter Grade Only
Type Units Inside of Class Hours Outside of Class Hours Total Student Learning Hours
Lecture 3.00 54.00 108.00 162.00
Laboratory 1.00 54.00 0.00 54.00
Total 4.00 108.00 108.00 216.00
Measurable Objectives:
Upon completion of this course, the student should be able to:
  1. make unit conversions in the metric system using the prefixes kilo, deci, centi, milli, and micro;
  2. describe the structure of the atom in terms of protons, neutrons and electrons;
  3. write electron configurations using the periodic table;
  4. perform calculations using the mole concept to relate grams to moles for given chemical formulas and for simple stoichiometry problems;
  5. identify properties of states of matter;
  6. perform simple calculations involving heat, including specific heat problems and nutritional problems;
  7. use standard nomenclature for ionic compounds, binary molecular compounds and acids;
  8. write balanced equations for chemical reactions including those in aqueous solution and those involving elementary oxidation-reduction;
  9. describe ideal gas laws qualitatively and quantitatively;
  10. define concentration units of solutions and use these definitions in problem solving;
  11. describe properties of solutions such as surface tension, osmosis and dialysis and their application to biological systems;
  12. identify and describe effects of intermolecular forces;
  13. describe buffer solutions in terms of their composition and function, especially ones in biological systems;
  14. interpret reactions according to acid-base theory;
  15. use the pH scale to compare acidity;
  16. write balanced net and total ionic equations;
  17. use Le Chateller’s principle to predict the qualitative effects of changes in concentration, temperature and pH on an equilibrium;
  18. describe factors affecting the rates of reactions;
  19. describe types of nuclear radiation, isotopes and their half-life, nuclear reactions, units, and medical/industrial uses;
  20. perform laboratory experiments in an efficient, safe and purposeful manner;
  21. collect and analyze scientific data;
  22. use an electronic balance and various pieces of volumetric glassware;
  23. record laboratory observations in a useful, detailed manner;
  24. perform a titration.
Course Content:

Course Content (Lecture):

  1. Matter and energy   
  2. Simple atomic theory, excluding quantum mechanics or wave theory
  3. Compounds and chemical bonds
  4. Intermolecular forces
  5. Moles and simple stoichiometry
  6. States of matter and gas laws
  7. Chemical energy, including specific heat calculations and nutrition calculations
  8. Water and solutions 
    1. molarity, including solution preparation and simple stoichiometry calculations
    2. equivalents/normality-simple calculations
    3. percent concentrations
    4. electrolytes
    5. net ionic equations
  9. Acid/Base chemistry
    1. Arrhenius theory
    2. Bronsted-Lowry theory
    3. pH scale and simple calculations
    4. hydrolysis 
    5. buffers
  10. Equilibrium
    1. definition
    2. LeChatelier's Principle
  11. Kinetic Molecular Theory
  12. Oxidation-reduction
    1. definitions of oxidation and reduction
    2. recognition of redox reactions
  13. Introduction to nuclear chemistry
    1. alpha, beta, gamma and positron decay
    2. half-life and simple calculations
    3. biological effects of radiation
    4. medical applications of radiation

Course Content (Laboratory):

  1. Measurements
    1. accuracy
    2. precision
    3. basic significant figures
    4. common units of measurements
    5. metric units
    6. English units
  2. Safety in the laboratory and proper disposal of waste materials
  3. Techniques of collecting and analyzing data to reach conclusions
  4. Qualitative and quantitative experiments in the laboratory, including 
    1. conductivity of solutions
    2. measurement of density
    3. direct observations of reactions
    4. experimentation with gas laws
    5. experimentation with acids/bases including pH measurement, titration and buffers.



Methods of Instruction:
  1. Audio-visual materials, which may include any of the following: a. molecular models b. periodic tables c. films d. transparencies e. computer simulations f. PowerPoint presentations
  2. Demonstrations of chemical reactions and related phenomena
  3. Informal lecture with student questions encouraged
  4. Laboratory experimentation, including individual and group work
  5. Lecture/Discussion
  6. Distance Education
Assignments and Methods of Evaluating Student Progress:
  1. Reading 1) Read the chapter on measurements in your textbook. Be able to answer all the end- of-chapter questions. 2) Read the laboratory discussion/procedure for titration. Be able to answer the pre-lab questions.
  2. Laboratory 1) Titrate a sample of unknown concentration of a monoprotic acid against a standardized base to determine the concentration. 2) Determine the density of various samples by taking appropriate measurements. 3) Observe what happens when samples of copper, zinc and magnesium are added to hydrochloric acid. Describe what you observe and write balanced equations for the reactions.
  1. Home Work
  2. Quizzes
  3. A minimum of 10 written laboratory reports based on departmentally approved experiments and graded on criteria that may include the following 1) Completeness of data collected 2) Quality of data collected 3) Computational precision and accuracy 4) Proper use of symbolic notation 5) Quality of analysis of scientific principles explored 6) Quality of narrative explanations and reasoning
  4. Exams/Tests
  5. Final Examination
Upon the completion of this course, the student should be able to:
  1. analyze experimental data and explain chemical processes at the molecular level;
  2. communicate chemical concepts, understand definitions, and interpret experimental results;
  3. recognize and appreciate the impact of the scientific principles of chemistry in day-to-day life.
Textbooks (Typical):
  1. Timberlake, K. (2012). General, Organic and Biological Chemistry (4th). Pearson.
  • Safety goggles approved for Chemistry laboratory
  • Scientific calculator
  • Laboratory coat/apron
Abbreviated Class Schedule Description:
Chemistry of inorganic compounds, atomic theory, bonding, equations, gas laws, solutions, acid-base theory and oxidation-reduction. Designed to meet the requirements of certain programs in allied health and technological fields and for general education.
Prerequisite: MTH 65, MTH 65B or MTH 65L or MTH 53 or MTH 53B.
Discipline:
Chemistry*