Active Outline

General Information

Course ID (CB01A and CB01B)
CHEMD001A
Course Title (CB02)
General Chemistry I
Course Credit Status
Credit - Degree Applicable
Effective Term
Fall 2024
Course Description
This course provides an introduction to the structure and reactivity of matter at the molecular level, as well as an application of critical reasoning to modern chemical theory and structured numerical problem-solving. Students will learn the development of molecular structure from rudimentary quantum mechanics, including an introduction to ionic and covalent bonding; chemical problem solving involving both formula and reaction stoichiometry employing the unit analysis method, and be introduced to thermochemistry and a discussion of the first law of thermodynamics.
Faculty Requirements
Course Family
Not Applicable

Course Justification

This course is a major preparation requirement in the discipline of Chemistry at all CSUs and UCs. This course meets a general education requirement for °®¶¹´«Ã½ GE, CSU GE, and IGETC. This course is a part of the Biological Sciences AS degree. This is the first of three courses in the General Chemistry sequence of classes where students are introduced to foundational topics in chemistry.

Foothill Equivalency

Does the course have a Foothill equivalent?
No
Foothill Course ID

Course Philosophy

Formerly Statement

Course Development Options

Basic Skill Status (CB08)
Course is not a basic skills course.
Grade Options
  • Letter Grade
  • Pass/No Pass
Repeat Limit
0

Transferability & Gen. Ed. Options

Transferability
Transferable to both UC and CSU
°®¶¹´«Ã½ GEArea(s)StatusDetails
2GBX°®¶¹´«Ã½ GE Area B - Natural SciencesApproved
CSU GEArea(s)StatusDetails
CGB1CSU GE Area B1 - Physical ScienceApproved
CGB3CSU GE Area B3 - Science Laboratory ActivityApproved
IGETCArea(s)StatusDetails
IG5AIGETC Area 5A - Physical ScienceApproved
IG5CIGETC Area 5C - Science LaboratoryApproved
C-IDArea(s)StatusDetails
CHEMChemistryApproved(CHEM D001A or CHEM D01AH) & (CHEM D001B or CHEM D01BH) required for C-ID CHEM 110 (CHEM D001A or CHEM D01AH) & (CHEM D001B or CHEM D01BH) & (CHEM D001C or CHEM D01CH) required for C-ID 120 S

Units and Hours

Summary

Minimum Credit Units
5.0
Maximum Credit Units
5.0

Weekly Student Hours

TypeIn ClassOut of Class
Lecture Hours3.06.0
Laboratory Hours6.00.0

Course Student Hours

Course Duration (Weeks)
12.0
Hours per unit divisor
36.0
Course In-Class (Contact) Hours
Lecture
36.0
Laboratory
72.0
Total
108.0
Course Out-of-Class Hours
Lecture
72.0
Laboratory
0.0
NA
0.0
Total
72.0

Prerequisite(s)

CHEM D025. or CHEM D030A or satisfactory score on the Chemistry Placement Test; and intermediate algebra or equivalent (or higher), or appropriate placement beyond intermediate algebra

Corequisite(s)

Advisory(ies)

EWRT D001A or EWRT D01AH or ESL D005.

Limitation(s) on Enrollment

(Not open to students with credit in the Honors Program related course.)

Entrance Skill(s)

General Course Statement(s)

(See general education pages for the requirements this course meets.)

Methods of Instruction

Lecture and visual aids

Discussion of assigned reading

Discussion and problem solving performed in class

Quiz and examination review performed in class

Homework and extended projects

Collaborative learning and small group exercises

Laboratory experience which involve students in formal exercises of data collection and analysis

Laboratory discussion sessions and quizzes that evaluate the preceding week's laboratory exercises

Assignments

  1. Reading
    1. Required readings from the textbook in preparation for the scheduled lecture. This may include entire chapters or sections from the chapters covering topics included in this outline.
    2. Required readings from the laboratory manual as a preparation for the scheduled experiment in order to provide students with familiarity about the specific laboratory protocols and related safety precautions necessary for successful completion of the experiment.
  2. Writing
    1. Homework assignments based on classroom discussion/lecture may include answering questions from end-of-chapter exercises or other sources as deemed appropriate by the instructor.
    2. Periodic quizzes and mid-term examinations based on material discussed in lectures and/or reading assignments
  3. Laboratory assignments
    1. Pre-lab exercise: The pre-lab assignment for the scheduled laboratory experiment to be completed prior to beginning of each new experiment. This assignment may be identical to that provided in the laboratory manual or substituted with other appropriate assignments determined by the instructor.
    2. Report: Data obtained in laboratory exercises are to be entered in the assigned laboratory manual or a laboratory notebook. Necessary calculations required to obtain the final results from the experiment must be completed in the manual or the notebook as to be determined by the instructor. Detailed lab reports incorporating results and discussions from the experiment will be required.

Methods of Evaluation

  1. Homework assignments based on end-of-chapter problems from the primary text will be evaluated for completion to test comprehension of lectures.
  2. Periodic quizzes will be used to test the comprehension of topics covered during the lecture and will be evaluated for accuracy of responses.
  3. A minimum of two mid-term examinations will be used to evaluate the ability of students to a) solve problems, b) outline various concepts covered in the lecture, and c) demonstrate an understanding of reading assignments. These will be evaluated for accuracy to assess student progress in achieving various learning outcomes.
  4. A comprehensive final examination in any chosen format (multiple choice questions or free response) will be based on all the course material covered during the entire quarter and evaluated for accuracy of responses.
  5. Pre-lab assignments will be evaluated for completeness and level of preparedness required for safe and timely execution of laboratory protocols and experiments.
  6. Report sheets and/or laboratory reports will be evaluated for successful completion of laboratory experiments as well as accuracy of data analysis and interpretation. Students will work both individually and collaboratively towards the completion of the laboratory experiments.
  7. A comprehensive laboratory examination or periodic quizzes will be used to evaluate the student understanding of the various concepts discussed in the different experiments performed during the course. Concepts evaluated will include: a) general laboratory protocol b) comprehension of data analysis and interpretation and c) critical thinking as it pertains to the scientific method

Essential Student Materials/Essential College Facilities

Essential Student Materials
  • Safety goggles
Essential College Facilities
  • Fully equipped chemical laboratory including, at a minimum, the following: consumable chemicals, chemical balances, glassware, molecular models, melting point apparatus, laptops with data acquisition modules, fume hoods, chemical disposal facilities, lockable student storage areas, periodic tables, and laboratory technician, Lecture room with a periodic table

Examples of Primary Texts and References

AuthorTitlePublisherDate/EditionISBN
Silberberg and Amateis.Chemistry: The Molecular Nature of Matter and ChangeMcGraw-Hill9th edition, 2021978-1-260-24021-4.
°®¶¹´«Ã½ Chemistry Department°®¶¹´«Ã½ Chemistry Department General Chemistry Laboratory Manual(/chemistry/Chem1A.html)2022

Examples of Supporting Texts and References

None.

Learning Outcomes and Objectives

Course Objectives

  • Examine contributions by investigators of diverse cultures and times to the body of chemical knowledge, with an emphasis on physical and chemical conceptual frameworks.
  • Investigate the critical aspects of measurement.
  • Explore the historical development of understanding the structure of the atom.
  • Assess the development of the Periodic Table of Elements in light of modern atomic theory.
  • Differentiate the causes and types of molecular bonding.
  • Appraise the effect of quantum mechanics on formulation of molecular structure.
  • Employ systematic nomenclature to the identification of molecules.
  • Utilize the principles of stoichiometry to analyze compounds, chemical mixtures, and reactions.
  • Examine the prominent characteristics of solutions.
  • Classify the major types of chemical reactions.
  • Apply the essential principles of thermodynamics to chemical systems.

CSLOs

  • Identify and explain trends in the periodic table.

  • Construct balanced reaction equations and illustrate principles of stoichiometry.

  • Apply the first law of thermodynamics to chemical reactions.

Outline

  1. Examine contributions by investigators of diverse cultures and times to the body of chemical knowledge, with an emphasis on physical and chemical conceptual frameworks.
    1. Historical development of chemical principles
    2. Application of chemistry to topics such as environmental stewardship and traditional medicine.
  2. Investigate the critical aspects of measurement.
    1. Comparison of SI and British systems of units
    2. Problem solving using dimensional analysis
    3. Limitations of measurement and statistical methods
      1. Precision versus accuracy
      2. Significant figures
      3. Standard deviation
  3. Explore the historical development of understanding the structure of the atom.
    1. Historical development of atomic theory
      1. Proust's Law of Definite Proportions
      2. Dalton's Law of Multiple Proportions
      3. Dalton's atomic theory
      4. Millikan oil drop experiment
      5. Thompson cathode-ray tubes
      6. Rutherford nuclear deflection experiment
    2. Sub-atomic structure
      1. Protons, neutrons, and electrons
      2. Nuclei
    3. Nomenclature of atoms
      1. Atomic number, atomic mass, mass number
      2. Isotopes
    4. The Bohr Model of the atom
      1. Quantization of energy
      2. Ground and excited states
      3. Electronic transitions
    5. Development of modern quantum theory
      1. Electromagnetic spectrum
      2. Wave-particle duality of light
    6. Implications of elementary quantum mechanics
      1. Heisenberg Uncertainty Principle
      2. Wavefunctions
      3. The Born interpretation
      4. Quantum numbers
      5. Orbital shapes
      6. Nodes and degeneracy
      7. Electron spin
      8. Extension to polyelectronic atoms
    7. Electronic configurations
      1. Hund's Rule
      2. The Aufbau Principle
      3. Pauli Exclusion Principle
    8. Ions
      1. Cations
      2. Anions
  4. Assess the development of the Periodic Table of Elements in light of modern atomic theory.
    1. History of the Periodic Table
    2. Periodic trends of the elements
      1. Ionization energy
      2. Electronic affinity
      3. Atomic radii
      4. Ionic radii
      5. Electronegativity
    3. Survey of elemental groups
  5. Differentiate the causes and types of molecular bonding.
    1. Types of chemical bonds
      1. Covalent
      2. Ionic
      3. Metallic
      4. Coordinate covalent
    2. Relationship of bond type to electronegativity
    3. Dipole moments
    4. Lattice energy
    5. Bond enthalpies
  6. Appraise the effect of quantum mechanics on formulation of molecular structure.
    1. Lewis structures of organic and inorganic substances
      1. The octet rule
      2. Exceptions to the octet rule
      3. Resonance structures
      4. Formal charge
    2. VSEPR theory
      1. Molecular geometries
      2. Hybridization of atomic orbitals in organic and inorganic molecules/ions
    3. Molecular orbital theory
      1. Bonding and antibonding orbitals
      2. Sigma and pi bonds in simple organic molecules such as alkanes, alkenes, alkynes, and aromatics
      3. Bond order
      4. Paramagnetism
      5. Homonuclear diatomic molecules
      6. Heteronuclear diatomic molecules
      7. Delocalized bonding in organic molecules such as benzene
  7. Employ systematic nomenclature to the identification of molecules.
    1. Ionic compounds with fixed cation charge
    2. Ionic compounds with variable charge cations
    3. Binary covalent compounds
    4. Acids
    5. Simple organic substances
  8. Utilize the principles of stoichiometry to analyze compounds, chemical mixtures, and reactions.
    1. Historical development of stoichiometry
      1. Law of Conservation of Mass
      2. Avogadro's Hypothesis
    2. Stoichiometry
      1. The mole
      2. Molar mass
      3. Avogadro's number
    3. Percent composition of compounds
      1. Calculation from combustion analysis
      2. Calculation from given masses
    4. Determine compound formulas
      1. Empirical formula
      2. Structural formula
    5. Balance simple chemical equations
    6. Identify limiting reagents
    7. Calculate percent yield
  9. Examine the prominent characteristics of solutions.
    1. Homogeneous versus heterogeneous mixtures
    2. Solvent and solute
    3. Strong and weak electrolytes
    4. Molarity
    5. Dilution of solutions
  10. Classify the major types of chemical reactions.
    1. Precipitation reactions
      1. Molecular equations
      2. Complete ionic equations
      3. Net ionic equations
    2. Acid-base reactions
      1. Titration
      2. Equivalence point
    3. Oxidation-reduction reactions
      1. Oxidation states
      2. Balancing oxidation-reduction reactions
    4. Combustion reactions in organic substances such as hydrocarbons and alcohols
  11. Apply the essential principles of thermodynamics to chemical systems.
    1. State functions
    2. Forms of energy
      1. Kinetic and potential
      2. Chemical and mechanical
    3. First Law of Thermodynamics
      1. Exothermic versus endothermic processes
      2. Constant pressure versus constant volume
      3. Hess's Law
      4. Enthalpy of formation
      5. The standard state
    4. Calorimetry
      1. Specific heat
      2. Heat capacity

Lab Topics

  1. Laboratory methodology
    1. Maintaining a laboratory notebook
    2. Writing laboratory reports
  2. Chemical safety
  3. Chemical Disposal
    1. Materials safety data sheets (MSDS)
    2. Laboratory environment
      1. Separation of waste streams
      2. Proper disposal methods
      3. Environmental hazards of improper waste disposal
    3. Personal safety
      1. Maintaining laboratory cleanliness
      2. Chemical labeling
      3. Segregation of chemicals by hazard
      4. Secondary containment
    4. Emergency situations
      1. Safety goggles
      2. Limiting chemical exposure
      3. Safety showers
      4. Eyewash stations
      5. Proper use of fire extinguishers
      6. Fires
      7. Earthquakes
      8. Evacuation procedures
  4. Physical measurement
    1. Gravimetric analysis
      1. Taring
      2. Mass by difference
    2. Volumetric analysis
  5. Laboratory techniques
    1. Proper ignition of Bunsen burners
    2. Solid filtration
    3. Use of pipettes
  6. Chemical analysis
    1. Gravimetric analysis of a hydrate
    2. Titration
      1. Acid-base
        1. Use of indicators
        2. Relationship of endpoint to equivalence point
      2. Redox
    3. Conductivity
    4. Calorimetry
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