SRJC Course Outlines

10/31/2020 10:01:47 AMCHEM 3A Course Outline as of Fall 2020

New Course (First Version)
CATALOG INFORMATION

Discipline and Nbr:  CHEM 3ATitle:  GENERAL CHEMISTRY 1:LEC  
Full Title:  General Chemistry Part 1: Lecture
Last Reviewed:5/13/2019

UnitsCourse Hours per Week Nbr of WeeksCourse Hours Total
Maximum3.00Lecture Scheduled3.0017.5 max.Lecture Scheduled52.50
Minimum3.00Lab Scheduled06 min.Lab Scheduled0
 Contact DHR0 Contact DHR0
 Contact Total3.00 Contact Total52.50
 
 Non-contact DHR0 Non-contact DHR Total0

 Total Out of Class Hours:  105.00Total Student Learning Hours: 157.50 

Title 5 Category:  AA Degree Applicable
Grading:  Grade Only
Repeatability:  00 - Two Repeats if Grade was D, F, NC, or NP
Also Listed As: 
Formerly: 

Catalog Description:
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General principles of chemistry, including atomic theory, bonding, stoichiometry, kinetic molecular theory of gases, properties of mixtures, the periodic table, and thermochemistry. Lecture portion of the first semester of a one-year program of general chemistry.

Prerequisites/Corequisites:
Course Completion or Concurrent Enrollment in CHEM 3AL; AND Course Completion of CHEM 42, or one year of high school chemistry taken within the last five years with a grade of B or higher; AND Course Completion of MATH 154 or MATH 155 or MATH 156 or higher (MATH) or appropriate placement based on AB705 mandates


Recommended Preparation:
Course Completion of ENGL 1ACourse Completion of ENGL 1A

Limits on Enrollment:

Schedule of Classes Information
Description: Untitled document
General principles of chemistry, including atomic theory, bonding, stoichiometry, kinetic molecular theory of gases, properties of mixtures, the periodic table, and thermochemistry. Lecture portion of the first semester of a one-year program of general chemistry.
(Grade Only)

Prerequisites:Course Completion or Concurrent Enrollment in CHEM 3AL; AND Course Completion of CHEM 42, or one year of high school chemistry taken within the last five years with a grade of B or higher; AND Course Completion of MATH 154 or MATH 155 or MATH 156 or higher (MATH) or appropriate placement based on AB705 mandates
Recommended:Course Completion of ENGL 1ACourse Completion of ENGL 1A
Limits on Enrollment:
Transfer Credit:CSU;UC.
Repeatability:00 - Two Repeats if Grade was D, F, NC, or NP

ARTICULATION, MAJOR, and CERTIFICATION INFORMATION

Associate Degree:Effective:Fall 2020
Inactive: 
 Area:C
Natural Sciences
 
CSU GE:Transfer Area Effective:Inactive:
 B1Physical ScienceFall 2020
 
IGETC:Transfer Area Effective:Inactive:
 5APhysical SciencesFall 2020
 
CSU Transfer:TransferableEffective:Fall 2020Inactive:
 
UC Transfer:TransferableEffective:Fall 2020Inactive:
 
C-ID:

Certificate/Major Applicable: Major Applicable Course



COURSE CONTENT

Student Learning Outcomes:
Upon completion of the course, students will be able to:
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1.  Describe matter, its transformations and corresponding energy changes according to
    prevailing chemical theories.
2.  Interpret and solve problems in a chemical context using quantitative reasoning.
 

Objectives: Untitled document
Students will be able to:
1.   Use dimensional analysis and stoichiometry to solve quantitative chemical problems.  
2.   Apply atomic theory in describing matter, including chemical nomenclature and physical and
      chemical processes.  
3.   Summarize the quantum mechanical structure of the hydrogen atom in light of its emission
      spectrum, and apply it to many-electron systems.  
4.   Calculate energy changes in calorimetry and chemical reactions.  
5.   Use the periodic table of elements to recognize trends and patterns, and to perform
      calculations.  
6.   Describe the bonding and shapes of simple compounds with a range of models.  
7.   Apply kinetic-molecular theory to the behavior of ideal and real gases.  
8.   Relate intermolecular forces to the physical properties of matter.  
9.   Calculate the effects of solute concentration on the physical properties of solutions.  
10.  Apply chemical principles to real world situations.

Topics and Scope
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I. Basic Tools and Problem Solving
    A. Metric system and units
    B. Dimensional analysis and conversions
    C. Significant figures
 
II. Stoichiometry
    A. Amount of substance and molar mass
    B. Mass calculations
    C. Limiting reactants and yields
    D. Concentration and solution stoichiometry
    E. Gas stoichiometry
    F. Energy calculations
 
III. Atomic Theory
    A. States of matter
    B. Nomenclature of simple compounds
    C. Chemical composition
         1. Mass fraction
         2. Empirical formulas
         3. Molecular formulas
    D. Chemical reactions
         1. Balancing
         2. Precipitation
         3. Acid-base
         4. Oxidation-reduction
 
IV. Structure of the Atom
    A. Light and the electromagnetic spectrum
    B. Emission spectra
    C. Bohr model of hydrogen
    D. Quantum mechanical model of the atom
    E. Quantum numbers
    F. Writing electron configurations
 
V. Thermochemistry
    A. Calorimetry
    B. Pressure-Volume (PV) work
    C. Energy vs. enthalpy
    D. Hess's law
    E. Enthalpies of formation
    F. Reaction enthalpies
    G. Bond energies and reaction enthalpies
 
VI. Periodic Trends
    A. Atomic size
    B. Ionization energy
    C. Electronegativity
    D. Ionic radius
 
VII. Bonding and Molecular Structure
    A. Ionic bonding
    B. Born-Haber cycle
    C. Lewis structures
    D. Valence Shell Electron Pair Repulsion (VSEPR) Theory
    E. Covalent bond order, polarity, energy and length
    F. Hybridization of atomic orbitals
    G. Valence Bond (VB) theory
    H. Molecular Orbital (MO) theory
 
VIII. Kinetic Molecular Theory of Gases
    A. Molecular scale understanding of gas pressure and temperature
    B. Development and applications of the ideal gas law
    C. Dalton's law of partial pressures
    D. Graham's law of effusion and diffusion
    E. Approximating real gases with the van Der Waals equation
 
IX. Intermolecular Forces (IMF)
    A. Molecular polarity
    B. Types of intermolecular forces
    C. Physical properties and IMF
    D. Phases and phase diagrams
 
X. Liquids and Solids
    A. Properties of the liquid state
    B. Uniqueness of water
    C. Structure, properties and bonding in the solid state
    D. Structure of crystalline solids

Assignments:
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1. Specific reading and study assignments from the textbook (20-30 pages per week)
2. Completion of recommended homework problems (0-30 per week)
3. Midterm exams (3-5 per semester), quizzes (0-4 per semester), final exam
4. Research paper

Methods of Evaluation/Basis of Grade.
Writing: Assessment tools that demonstrate writing skill and/or require students to select, organize and explain ideas in writing.Writing
0 - 0%
None
This is a degree applicable course but assessment tools based on writing are not included because this course includes essay exams that fulfil the writing component of the course.
Problem solving: Assessment tools, other than exams, that demonstrate competence in computational or non-computational problem solving skills.Problem Solving
0 - 40%
Homework problems
Skill Demonstrations: All skill-based and physical demonstrations used for assessment purposes including skill performance exams.Skill Demonstrations
0 - 0%
None
Exams: All forms of formal testing, other than skill performance exams.Exams
40 - 100%
Midterm exams, quizzes, final exam
Other: Includes any assessment tools that do not logically fit into the above categories.Other Category
0 - 20%
Research project


Representative Textbooks and Materials:
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Chemistry: The Molecular Nature of Matter and Change. 8th ed. Silberberg, Martin and Amateis, Patricia. McGraw-Hill. 2018
Chemistry. 13th ed. Chang, Raymond and Overby, Jason. McGraw-Hil. 2019
General Chemistry. 4th ed. McQuarrie, Donald and Rock, Peter and Gallogly, Ethan. University Science Books. 2010 (classic)
Chemistry: The Science in Context. 5th ed. Gilbert, Thomas and Kirss, Rein and Foster, Natalie. W. W. Norton. 2017
Chemistry: A Molecular Approach. 4th ed. Tro, Nivaldo. Prentice Hall. 2017

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