Catalog Description

Prerequisite: Completion of CHEM A or equivalent with grade of "C" or better; and completion of MATH D or MATH G with grade of "C" or better, or placement by matriculation assessment process, or equivalent; and satisfactory score on the Chemistry Placement Examination
Advisory: Eligibility for ENGL 1A strongly recommended
Hours: 162 (54 lecture, 108 laboratory)
Description: Introduction to the general principles of chemistry with emphasis upon quantitative relationships. Properties of matter related whenever possible to present concepts of atomic structure and to the periodic table. Includes atomic structure, the mole concept, gas laws, stoichiometry, redox, states of matter, solutions, and an introduction to modern theories of chemical bonding through related lecture and laboratory exercises. Students enrolling in CHEM 1A after having completed CHEM 3A will lose credit for CHEM 3A. Note: Not open to students who have completed CHEM 3B. CHEM 1A/1B sequence may be started any semester. (C-ID CHEM 110) (combined with CHEM 1B, C-ID CHEM 120S) (CSU, UC-with unit limitation)

Course Student Learning Outcomes

  • CSLO #1: Demonstrate proficiency in solving problems and analyzing data related to chemical formulas and stoichiometry.
  • CSLO #2: Demonstrate proficiency in solving problems and analyzing data related to thermodynamics.
  • CSLO #3: Demonstrate proficiency in solving problems and analyzing data related to atomic and molecular structure.
  • CSLO #4: Demonstrate proficiency in solving problems and analyzing data related to states of matter.
  • CSLO #5: Demonstrate proficiency in scientific communication.

Effective Term

Fall 2022

Course Type

Credit - Degree-applicable

Contact Hours

162

Outside of Class Hours

108

Total Student Learning Hours

270

Course Objectives

Given a periodic chart, an ion chart, a strong and weak electrolyte chart, and a calculator, students will perform the following on written examinations, on laboratory exercises, or in laboratory experiments:
Lecture Objectives:
1. decide if a given change is a chemical change or a physical change;
2. convert within the metric system and between English and metric systems;
3. calculate numerical problem answers in proper scientific notation and to the proper number of significant figures using dimensional analysis;
4. calculate the numbers of protons, neutrons, and electrons for given atoms and ions;
5. solve problems involving atomic number, mass number, and numbers of protons, neutrons, and electrons;
6. compute the percent abundance or average atomic mass of an element;
7. solve problems involving grams, moles, and particles;
8. calculate the percent composition of a given compound;
9. determine the empirical and/or molecular formula for a given compound from the given composition;
10. Determine the chemical formulas for given chemical names, determine the chemical names for given chemical formulas;
11. construct balanced chemical equations;
12. construct ionic and net ionic equations;
13. solve the oxidation states for given chemical formulas;
14. solve stoichiometry problems involving grams, moles, and particles;
15. solve stoichiometry problems involving a limiting reagent;
16. solve problems using molarity;
17. solve stoichiometry problems involving molarity;
18. solve problems involving specific heat, mass, and temperature;
19. solve stoichiometry problems involving enthalpy;
20. compute the enthalpy of reaction by combining other equations;
21. compute the enthalpy of reaction by using enthalpy of formations;
22. solve problems involving wavelength, frequency, and energy;
23. compute the wavelength, frequency, and energy of an electron transition;
24. diagram atomic orbitals;
25. determine the quantum numbers for an electron in an atom;
26. write the electron configuration for given elements and ions;
27. determine the electron configuration and atomic properties for an element from its location on the periodic chart;
28. draw the electron dot formulas for given chemical names or formulas;
29. determine the shape and polarity of a molecule;
30. determine the correct hybridization of atomic orbitals for given compounds;
31. solve problems correlating the Valence Bond Theory with the molecular shapes predicted by the VSEPR theory;
32. write molecular orbital configurations for given compounds;
33. prepare molecular orbital diagrams for given compounds;
34. solve gas problems involving grams, pressure, volume, temperature, and number of moles;
35. solve stoichiometry problems involving gas volumes;
36. solve gas problems involving Dalton's Law and Graham's Law;
37. identify and explain the behavior of metals, semiconductors, and insulators using molecular orbital diagrams;
38. explain the existence of the various states of matter using the Kinetic-Molecular Theory;
39. infer solubility, vapor pressure, melting point, and boiling point trends;
40. prepare and interpret phase diagrams;
41. identify solids by type using bonding between the basic units;
42. determine density of solids using crystal structures;
43. solve problems involving molality, molarity, and mass percent;
44. solve problems involving colligative properties.
Laboratory Objectives:
1. Perform laboratory experiments to reinforce the concepts, to teach basic laboratory technique, and to prepare for more advanced work in chemistry;
2. develop skills for keeping and maintaining a proper scientific lab notebook;
3. develop techniques for measurement and recording data with correct significant figures;
4. use appropriate equipment to measure mass and volume in order to determine density;
5. determine the empirical formula of a compound;
6. investigate different types of chemical reactions;
7. write chemical formulas for given chemical names, write chemical names for given chemical formulas;
8. identify strong electrolytes, weak electrolytes, and nonelectrolytes in an aqueous solution;
 write ionic and net ionic equations;
9. given the equation for an oxidation-reduction reaction, identify the substance oxidized and the substance reduced, as well as the oxidizing agent and the reducing agent;
10. determine the oxidation states of chemical formulas;
11. determine the concentration of a solution through titration;
12. using a calorimeter, determine the specific heat of a substance;
13. atomic structure will be investigated by observing line spectra of elements;
14. determine the Rydberg constant by observing line spectra of hydrogen;
15. determine the Lewis Structure, shape, and polarity of a molecule/ion;
16. practice writing the correct hybridization of atomic orbitals for given compounds;
17. investigate problems correlating the Valence Bond Theory with the molecular shapes predicted by the VSEPR theory;
18. practice writing molecular orbital configurations for given compounds;
19. experimentally determine the molar mass of gas;
20. determine standard molar volume and the molar mass of a metal using gas laws;
21. determine the enthalpy of fusion and enthalpy of vaporization of a liquid;
22. investigate colligative properties using freezing point depression;
23. exhibit cooperative and individual skills in the collection and analysis of data;
24. develop clear, cogent reporting of experimental observations, analysis and conclusions using the scientific method.
A minimum of 20 of the 32 (maximum) lab sessions during the semester will be experiments which require the student to obtain, record, and analyze observations and measurements. A range of 22-24 lab sessions of this type is most commonly scheduled.

General Education Information

  • Approved College Associate Degree GE Applicability
    • AA/AS - Physical Sciences
    • AS - Physical Science Lab
  • CSU GE Applicability (Recommended-requires CSU approval)
    • CSUGE - B1 Physical Science
    • CSUGE - B3 Lab Activity
  • Cal-GETC Applicability (Recommended - Requires External Approval)
    • IGETC Applicability (Recommended-requires CSU/UC approval)
      • IGETC - 5A Physical Science
      • IGETC - 5C Laboratory Science

    Articulation Information

    • CSU Transferable
    • UC Transferable

    Methods of Evaluation

    • Objective Examinations
      • Example: Compare and contrast the following terms: limiting reactant, excess reactant, theoretical yield, actual yield, and percent yield.
    • Problem Solving Examinations
      • Example: (1) To a beaker containing 25 g of zinc, 25 mL of 0.100 M HCl is added. Decide which reactant is the limiting reactant and justify your answer with the appropriate calculations. Rubric grading. (2) Calculate the grams of oxygen produced by the decomposition of 25 grams of hydrogen peroxide. Rubric grading. (3) If 95.5 grams of zinc reacts with excess hydrochloric acid producing 2.5 grams of hydrogen, calculate the percent yield.
    • Reports
      • Example: Students will be taking own generated data or instructor provided data and analyze that information. Students then reports that information within the provided lab manual. Students will be evaluated based on calculations and results of the experiment. Example: prepare a report for the Formula of a Hydrate laboratory.
    • Skill Demonstrations
      • Example: Students will be tasked to perform analyze an unknown sample and perform calculations. Students are evaluated on accuracy and precision of the identity of the unknown sample.

    Repeatable

    No

    Methods of Instruction

    • Laboratory
    • Lecture/Discussion
    • Distance Learning

    Lab:

    1. Instructors assign a stoichiometric lab experiment. They go over safety precautions and give a brief demonstration of key lab techniques. Students are then asked to perform the experiment as instructed and analyze the data while the instructor facilitates the experiment.

    Lecture:

    1. The instructor presents lecture on stoichiometric unit conversions with multimedia presentation tools. Example problems on gas laws, stoichiometry, chemical bonding, and solutions are incorporated into the lecture at various points of the presentation. Students should be actively engaged, problem solving, and asking questions. Several example questions may be provided as the instructor assess the student learning.

    Distance Learning

    1. The instructor delivers the topic on gas laws either through a live or recorded video conference lecture or a pre-recorded lecture video. The recorded video lecture can be from a slide lecture presentation or a OneNote style video. The students are responsible for attending or watching the videos provided. After watching the videos, students are tasked to work on the homework assignment. Then complete the lab activity found within the lab kits. There are additional gas law experiments that are recorded that students watch on their own. They generate their own data or are given data to analyze and then tasked to finish the remainder of the lab report.”

    Typical Out of Class Assignments

    Reading Assignments

    1. Read a section from the textbook. Be prepared to use the content to participate in the classroom and to complete assigned problems from the textbook. For example: Read the section on stoichiometry from the textbook. Be prepared to use the content to participate in the classroom and to complete assigned problems from the textbook. 2. Read a laboratory and prepare a prelaboratory report. For example: Read the Scientific Measurement laboratory and prepare a prelaboratory report.

    Writing, Problem Solving or Performance

    1. Write the prelaboratory report for a laboratory. For example: Write the prelaboratory report for the Scientific Measurement laboratory. 2. Solve problems. For example: Calculate the energy required to raise the temperature of 50 grams of water 50 K. 3. Perform laboratory experiments and determine the percent error. For example: Perform the Formula of a Hydrate laboratory and determine the percent error.

    Other (Term projects, research papers, portfolios, etc.)

    Students will be instructed and evaluated on the proper use of a scientific notebook.

    Required Materials

    • Chemistry: A molecular Approach
      • Author: Nivaldo J. Tro
      • Publisher: Pearson
      • Publication Date: 2020
      • Text Edition: 5th
      • Classic Textbook?: No
      • OER Link:
      • OER:
    • Laboratory Manual for Chemistry: A Molecular Approach
      • Author: Nivaldo J. Tro, John J. Vincent, Erica J. Livingston
      • Publisher: Pearson
      • Publication Date: 2020
      • Text Edition: 5th
      • Classic Textbook?: No
      • OER Link:
      • OER:

    Other materials and-or supplies required of students that contribute to the cost of the course.

    calculator, laboratory packet, laboratory coat, laboratory goggles, and laboratory notebook