Course Outline for Chemistry 31
Introduction to College Chemistry

Effective: Fall 2016
SLO Rev: 01/24/2017
Catalog Description:

CHEM 31 - Introduction to College Chemistry

4.00 Units

Elementary concepts of chemistry with emphasis on mathematical calculations; includes nomenclature, stoichiometry, atomic structure, gas laws, and acids and bases. Designed for majors in science and engineering.
Prerequisite: MTH 55 or MTH 55B.
1905.00 - Chemistry, General
Optional
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. describe matter and energy;
  2. classify states of matter and describe phase changes using the kinetic molecular theory;
  3. distinguish between elements/compounds/mixtures; physical/chemical, intensive/extensive, endothermic/exothermic changes and/or properties;
  4. solve unit conversion problems, including metric system and metric to English, and density problems, using dimensional analysis;
  5. convert between the three temperature scales Celcius, Kelvin and Fahrenheit;
  6. solve mathematical problems using algebraic equations, significant figures and units correctly;
  7. describe basic atomic structure using simple quantum theory, and Bohr Theory;
  8. state electron configurations and orbital diagrams, and their relationship to placement on the periodic table;
  9. name salts, common acids and binary molecular compounds by both systematic and common methods;
  10. describe the mole concept and use it in various calculations such as amount conversion problems, percent composition, and determination of empirical/molecular formulas when given percent composition;
  11. perform all levels of stoichiometric calculations (mass, gas and solution) including limiting reagent problems;
  12. perform calculations using the Gas Laws;
  13. define ionic and covalent bonds and give properties of each;
  14. draw Lewis structures for simple covalent molecules and polyatomic ions;
  15. classify chemical reactions by type, perform mass balance of chemical equations, and predict products (such as single and double replacement, combination, decomposition and combustion);
  16. perform calculations involving molarity and percent concentrations for solutions;
  17. classify solutes as electrolytes or nonelectrolytes, and write net ionic equations to determine if reaction has occurred;
  18. define acids and bases by Arrehenius and Bronsted-Lowry theories, write acid dissociation reactions, including the use of hydronium ion (H3O+), and identify conjugate acids and conjugate bases in acid/base reactions;
  19. perform precision acid/base titration calculations;
  20. perform simple pH calculations;
  21. satisfactorily perform the following laboratory procedures and techniques:
    a. safely handle chemicals and equipment in the laboratory;
    b. read and record measured quantities from various analytical instruments, correctly recording the certain digits and estimating the uncertain digit;
    c. weigh chemicals to 0.001 grams using a top-loading balance;
    d. quantitatively transfer solid and liquid chemicals from one container to another;
    e. correctly use a Bunsen burner;
    f. accurately measure liquid volumes using analytical volumetric glassware such as graduated cylinders, burets, and volumetric pipets;
    g. perform gravity filtrations quantitatively;
    h. perform acid/base titrations using known and unknown solutions;
    i. measure temperature;
    j. accurately and comprehensively observe chemical and physical changes and record such information in a scientifically correct form;
    k. construct models of simple molecules using model kits and Lewis structures;
    l. perform error and precision analysis of data by calculating averages, relative ranges and percent errors.
    m. guided experiment design and writing of simple laboratory experiment procedures
    n. quality narrative explanations of observations and/or results.
Course Content:

Course Content (Lecture):

  1. Review of relevant mathematics; scientific notation, significant figures, dimensional analysis
  2. Definitions and classifications of matter and energy
  3. Atomic structure and periodicity
  4. Chemical nomenclature of ionic compounds, binary covalent compounds and common acids 
  5. The mole concept including amount conversions, and all levels and variations of stoichiometric calculations
  6. Chemical bonding (ionic and covalent), Lewis structures for simple molecules
  7. The Gas Laws (for ideal gases only)
  8. Reactions: balancing equations, classification, prediction of product
  9. Solutions: definitions, molarity and percent concentrations
  10. Net ionic equations
  11. Arrhenius and Bronsted-Lowry acid-base theories
  12. pH calculations and solution stoichiometry including titration calculations

Course Content (Laboratory):

  1. Measurement of mass, volume, density, temperature
  2. Measurement of % composition and determination of empirical formula
  3. Gravimetric analysis and filtration
  4. Observe, classify and analyze various types of chemical reactions
  5. Construction of molecular models from Lewis structures
  6. Collection of gases; measurement of pressure, volume and temperature
  7. Conductivity of substances and solutions
  8. Preparation of solutions
  9. Acid/Base titration
  10. Data analysis, calculation of average, relative range, percent error, including graphical analysis
  11. Safe handling of chemicals and proper techniques for use of scientific instrumentation



Methods of Instruction:
  1. Classroom and laboratory demonstrations
  2. Distance Education
  3. Individual and group work in the laboratory
  4. Lecture, informal with student questions encouraged
  5. Safe and proper respect for chemicals and scientific apparatus are constantly stressed
  6. Use of models, animations, movies, interactive software, online homework, periodic tables, films and overlays
Assignments and Methods of Evaluating Student Progress:
  1. Laboratory assignment: design an experiment for separating an unknown mixture of salt and sand and determine the percentage by weight of salt and sand in the mixture. Determine the precision and accuracy of the results
  2. Homework: 10-12 homework problems per chapter taken from the text. Example: Complete chapter 3 problems 29-39, 43,47, 49,53,57,61,63, 107.
  1. Home Work
  2. Quizzes
  3. A minimum of eight written laboratory reports based on departmentally approved experiments and graded on criteria that may include the following 1) Description of experimental procedures 2) Completeness of data collected 3) Quality of data collected 4) Computational precision and accuracy 5) Accuracy and precision of laboratory results 6) Proper use of symbolic notation 7) Quality of analysis of scientific principles explored 8) 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. (Critical Thinking) Analyze experimental data and explain chemical processes at the molecular level.
  2. (Communication) Communicate chemical concepts, understand definitions, and interpret experimental results
  3. (Development of the Whole Person) Recognize and appreciate the impact of the scientific principles of chemistry in day-to-day life
Textbooks (Typical):
  1. Nivaldo J. Tro (2015). Introduction Chemistry (5th). Prentice Hall.
  1. Donna Gibson, et al,. In-House Laboratory Manual for Chemistry 31. Chabot College, .
  • Safety goggles approved for chemistry laboratory
  • Scientific calculator
  • Laboratory coat/apron (optional)
Abbreviated Class Schedule Description:
Elementary concepts of chemistry with emphasis on mathematical calculations; includes nomenclature, stoichiometry, atomic structure, gas laws, and acids and bases. Designed for majors in science and engineering.
Prerequisite: MTH 55 or MTH 55B.
Discipline:
Chemistry*