Introduction to General Chemistry ( Official )
WebCMS orange bar image
Introduction to General Chemistry ( Official )
College logo image
WebCMS text image
Introduction to General Chemistry ( Official )

Printer Friendly Version


SECTION A – Course Information

1. Course ID:

CHEM     40

Student Learning Outcomes

2. Course Title:

Introduction to General Chemistry

3. Division:

Natural Sciences Division

4. Department:

Chemistry Department

5. Subject:


6. Short Course Title:

Intro General Chemistry

7. Proposed Effective Term:

Summer 2018

The required Cover Sheet Supplemental Form can be created after completion of Section A

SECTION B – Official Course Information

1. Recommended Class Size:

a. Maximum Class Size:


Note:   If the course is new or class size of an existing course is to be changed, a Class Size Supplemental Form is required.

b. Class Size Approval Date:


Note:   Date to be entered by the Instruction Office.


2. Method of Instruction:


 Work Experience, Occupational


 Open Entry/Exit

 Lecture and Laboratory


 Independent Studies

 Distance Learning



3. Contact Hours for a Term:

Note: If not a variable unit/hour course, enter the hours in the "Low" column only. Leave the hours in the "High" column blank.








To be arranged:

         72.00 To





         54.00 To


Lab/Lecture Parity?    Yes  No

Does this course have lab parity?

If not, are you going to  apply for lab parity?                          Yes  No

To be arranged:







To be arranged:







Total Hours:    


         54.00 To


To be arranged:

         72.00 To




4. Credit Units:

  5.00 To


Note: Units of credit are based on:

1 Unit of credit per eighteen (18) hours of lecture contact hours for a term

1 Unit of credit per fifty-four (54) hours of lab, activity or clinical contact hours for a term


5. Taxonomy of Programs (TOPS) Information:

a. TOPS Code and Course Program Title:

190500 - Chemistry, General

     b.  Course Control Number:    

(To be entered by the Instruction Office Only.)


6. SAM Priority Code: [Select One]



Courses offered to apprentices only.


Advanced Occupational

Courses taken in the advanced stages of an occupational program. Each “B” level course must have a “C” level prerequisite in the same program area.


Clearly Occupational

Courses taken in the middle stages of an occupational program. Should provide the student with entry-level job skills.


Possibly Occupational

Courses taken in the beginning stages of an occupational program.





7. Please place this course into the appropriate discipline by selecting from the drop down list. The discipline placement indicates what preparation is needed to teach the course. Discipline faculty may place their courses into more than one discipline as appropriate:


8. General Course Information

a. Course Credit Status:

D Credit – Degree Applicable

b. State Transfer Code:

A Transferable, UC/CSU/Private

c. State Classification Code:

A Liberal Arts/Sciences Degrees

d. Basic Skills Status/Level:

N Not a Basic Skills Course

e. Sports/Physical Education Course:


( Only check here if the course is a physical education course.)

f. Grading Method:

Letter Grade Only

g. Number of repeats allowed:

Non-repeatable Credit - equates to 0 repeats

Note: If course is repeatable, complete the Repeatability Supplemental Form.

h. Please provide cross listed course if applicable:



9. Course Preparation

Note: If this course has any requisite, please complete the Content Review Supplemental Form and provide rationale for the requisite. If a requisite is being removed, please complete the Content Review Supplemental Form and provide rationale for removing the requisite. If a new requisite is being added, complete the Content Review Supplemental Form and provide rationale for the requisite.

a.   Prerequisite

Eligibility for MATH 71

b.   Co requisite

c.   Advisories

Eligibility for ENGL 1A

d.   None


10. Course Special Designators:

Do not edit this text box. Use the 'Add'/'Remove' command buttons above.

11. Course Program Status:

These buttons are only active when the course reaches Stage 5 in WebCMS.


 Program Applicable


 12. Funding Agency Category:

       Not Applicable

       Primarily developed using economic development funds

       Partially developed using economic development funds



SECTION C – For new transfer requests only, please complete the Transfer Status (CSU) Supplemental Form before submitting course for approval.

 CSU Transferable              CSU Approval Date:                     (mmddyyyy)                 

 Applying for CSU Transfer Status

 UC Transferable                 UC Approval Date:                      (mmddyyyy)                 

 Applying for UC Transfer Status

Note:  CSU Transfer Status must be obtained prior to submitting a request for UC Transfer Status to the UC Chancellor.


SECTION D - General Education Request

Mt. San Antonio College and CSU General Education course approvals are submitted to the Educational Design Committee and GE Subcommittee for approval.

1.  The Articulation Officer submits the course directly to the CSU Chancellor for approval.

2.  Upon receiving CSU approval, the course will be placed in the CSU approved area for the Mt. SAC Associate Degree GE.



Requesting approval for inclusion on Mt. SAC and CSU General Education List?

Note:   If requesting approval for inclusion on the General Education List, the General Education Course Evaluation Supplemental Form must be completed before submitting course for approval.  If request is approved, the remainder of Section D will be completed by the Instruction Office.

1. Mt SAC General Education Applicability:

    GE Approval Date :                   (mmddyyyy)

AAB1 - Physical Sciences
ASB1 - Physical Sciences

2. CSU General Education Applicability (Requires CSU approval):

    CSU Approval Date:                   (mmddyyyy)

CSB1 - Physical Sciences
CSB3 - Laboratory Activity

3. IGETC Applicability (Requires CSU/UC approval):

    IGETC Approval Date:                   (mmddyyyy)

IG5A - Physical Science - Lecture Only
IG5C - Physical Science – Combo



SECTION E - Course Content

1. Course Descriptions

a. Catalog Description:

(Write a clear, concise course description, summarizing the course content.  Include major goals of the course, scope, requirements for successfully completing the course, and any unusual aspects of the course.)

Measurements, atomic structure, chemical equations, stoichiometry, gases, solutions, acids and bases, bonding, nomenclature, matter, and energy. Completion prepares students to take CHEM 50.

b. Class Schedule Description:



Is a course description to be printed in the Class Schedule?

(If yes, write one or two sentences condensing the catalog description for the prospective student.  Does not require as much detail as the catalog description. Limited to 130 characters, including spaces.)

Chemistry for science and engineering majors. Completion prepares students to take CHEM 50.

2. Course Outline Information

In courses that include lecture and laboratory, the topical outlines should be separate and distinct, each specific and appropriate to the activities to be conducted.

a. Lecture Topical Outline:

(The lecture topical outline should provide a detailed record of the content of the course.)

- Measurements and calculations: significant figures and dimensional analysis
- Matter: chemical and physical properties, states of matter, and conservation of mass
- Energy: specific heat capacity, phase changes, and conservation
- Periodic table: atoms, elements, ions, trends, and properties
- Atomic theory: atomic structure and electron configuration
- Nomenclature: ionic and covalent compounds
- Chemical reactions: types, chemical equations, and net ionic equations
- Chemical quantities: percent composition, moles, molar mass, and empirical formula
- Stoichiometry: mole ratios, limiting reactant, and percent yield
- Solutions: concentration, dilution, and solution stoichiometry
- Bonding: covalent, ionic, molecular shape, and polarity
- Intermolecular forces: relationship to properties of solids and liquids
- Acids and bases: properties, titrations, and pH
- Gases: properties, gas laws, and kinetic molecular theory
- Final exam

b. Lab Topical Outline:

(The lab topical outline should reflect the activities in lab.)

- Training in fundamental laboratory safety, waste disposal, and laboratory equipment and glassware
- Performing metric measurements
- Measuring and analyzing physical properties
- Measuring and quantifying energy transfer
- Classifying and naming ionic and covalent compounds
- Measuring components of a chemical reaction and applying principles of stoichiometry
- Analyzing compounds to determine chemical composition
- Preparing solutions and determining concentration
- Characterizing types of chemical reactions and writing corresponding chemical equations
- Identifying unknown substances based on physical and chemical properties
- Exploring periodic trends and atomic structure
- Determining acidity and basicity of solutions
- Drawing Lewis diagrams of compounds and building molecular models
- Exploring properties of gases
- Final exam

3. Course Measurable Objectives:

(Measurable course objectives should identify expected outcomes: specific, observable student actions – what the student should be able to do, know or feel as a result of taking this course.  A majority of objectives should reflect critical thinking, i.e. application, analysis, synthesis, and evaluation.  Course objectives should relate directly to methods of evaluation)

Provide a minimum of five (5) course measurable objectives:

1. Apply scientific notation and significant figures to properly report measured data and use dimensional analysis in problem solving.
2. Distinguish between physical and chemical properties of matter.
3. Apply the laws of conservation of mass and energy.
4. Calculate the energy resulting from temperature and phase changes.
5. Use the periodic table to determine the average atomic mass and electron configuration of the elements.
6. Calculate the number of subatomic particles in a given isotope.
7. Determine the names or formula for ionic and molecular compounds including acids.
8. Calculate the percent composition, molar masses, and empirical and molecular formula of compounds.
9. Classify and predict products and write balanced equations for chemical reactions, including net ionic equations.
10. Perform stoichiometric calculations, including limiting reactant and percent yield.
11. Determine solution concentration including dilution.
12. Distinguish between ionic and covalent bonding.
13. Determine molecular structure, shape, polarity, and intermolecular forces.
14. Determine the pH of acidic and basic solutions and perform titration calculations.
15. Perform gas law calculations and use kinetic-molecular theory to account for the properties and behavior of gases.
16. Implement safe laboratory procedures.
17. Record data and observations using standard chemical conventions, including use of significant figures and units.
18. Demonstrate proper use of laboratory equipment.
19. Perform experiments using standard chemical laboratory techniques.
20. Record and summarize observations and analyze experimental data.
21. Interpret experimental results to draw conclusions.

4. Course Methods of Evaluation:

(Methods of evaluation should relate directly to measurable course objectives.  They indicate the kind of assignments or performance activities designed for a course to assess student learning.  Each course must list either substantial writing assignments (category 1) OR computational / non-computational problem solving demonstrations (category 2) if writing assignments are inappropriate (with an explanation of why substantial writing is not appropriate for the course).  Activities typically assigned in categories 3 and 4 must also be listed in this section.)

Category 1. Substantial written assignments for this course include:

10-14 lab reports with pre- and post-lab questions that require short-essay answers up to 3 to 5 sentences

If the course is degree applicable, substantial written assignments in this course are inappropriate because:

Category 2. Computational or non-computational problem solving demonstrations:

Single and multi-step calculations to convert between units, solve for unknown variables, or use stoichiometric quantities
Laboratory experiments requiring the identification of unknown substances or properties, after observing a series of known substances or properties

Category 3. Skills Demonstrations:

Hands-on lab experiments which require students to demonstrate skill with various lab techniques such as measuring and dispensing correct quantities of chemicals, recording observations and data, and safely handling and disposing of chemical waste

Category 4. Objective Examinations:

Free-response, multiple-choice, completion, matching, true or false, and essay questions on atomic structure, chemical quantities, chemical equations, bonding, acids and bases, periodic trends, solutions and gases

5. Sample Assignments:

(Assignments should be directly related to the objectives of the course.  They should be specific enough to provide real guidance to faculty and clear expectations for students.  Descriptions of the type or examples of assignments are required.  For example, rather than “term paper” state “term paper comparing and contrasting the social aspects of hunting tactics of two mammal species.”  This section must establish that the work is demanding enough in rigor and independence to fulfill the credit level specified.  The nature of the assignments must clearly demand critical thinking.  Assignments should be adequate to assure that students who successfully complete them can meet the objectives of the course.  Appropriate out-of-class work is required for credit courses.)

Provide a minimum of three (3) sample assignments:

1. Write chemical formulas for sodium chloride, potassium acetate, dinitrogen monoxide, and dihydrogen monoxide. Classify each compound as ionic or molecular.
2. Write a balanced equation for the reaction between solid magnesium and hydrochloric acid to produce hydrogen gas and aqueous magnesium chloride. Use the balanced equation to determine the volume of hydrogen gas produced at standard temperature and pressure (STP) from a reaction of 100.0 grams of magnesium with excess hydrochloric acid. Express the answer using correct significant figures and units.
3. Draw a Lewis dot structure of nitrogen trichloride. From the Lewis dot structure, determine the electron geometry, molecular geometry, and polarity of the molecule.
4. Determine the unknown concentration of a copper (II) nitrate solution by applying Beer’s law: From a 1.0M stock copper (II) nitrate solution, make a series of diluted solutions of 0.80M, 0.60M, and 0.40M. Determine the absorption of these solutions using spectrophotometry, construct a Beer’s law plot, and use the plot to determine the unknown’s concentration based on its absorption.


6. Representative Text:

(List EXAMPLES of textbooks and other data sources and materials, which may be used in this course.  Provide author, title, publisher, date of publication, and edition.)

If the course is requested to be or is CSU transferable, provide at least one (1) representative text that has been published within the last five (5) years.  A representative text is optional for a non-transferable course.

a. Book 1:

This is the most recent edition of this text:




If the text is more than 5 years old, please provide rationale for not selecting a more recent text:


  Charles Corwin


  Introductory Chemistry: Concepts and Critical Thinking



Date of Publication:



  1st Custom for Mt SAC

b. Book 2:

This is the most recent edition of this text:




If the text is more than 5 years old, please provide rationale for not selecting a more recent text:


  Mt. SAC Chemistry Department


  Chemistry 40 Laboratory Manual 2016-2017


  Mt. SAC

Date of Publication:




c. Book 3:

This is the most recent edition of this text:




If the text is more than 5 years old, please provide rationale for not selecting a more recent text:







Date of Publication: