CHEM 1411
General Chemistry I

Western Texas College

  1. Basic Course Information
    1. Lecture—Fundamental principles of chemistry for majors in the sciences, health sciences, and engineering; topics include measurements, fundamental properties of matter, states of matter, chemical reactions, chemical stoichiometry, periodicity of elemental properties, atomic structure, chemical bonding, molecular structure, solutions, properties of gases, and an introduction to thermodynamics and descriptive chemistry.
    2. Lab—the required laboratory activities will reinforce the lecture material; introduction of the scientific method, experimental design, data collection and analysis, and preparation of laboratory reports.
    3. Any required prerequisites:  C or higher in Math 1314 or equivalent.
    4. Required grade for enrolling in the next course in this sequence: Need a C or higher in CHEM 1411 in order to take CHEM 1412
  2. Student Learning Outcomes
    1. Lecture
      1. Define the fundamental properties of matter.
      2. Classify matter, compounds, and chemical reactions.
      3. Determine the basic nuclear and electronic structure of atoms.
      4. Identify trends in chemical and physical properties of the elements using the Periodic Table.
      5. Describe the bonding in and the shape of simple molecules and ions.
      6. Solve stoichiometric problems.
      7. Write chemical formulas.
      8. Write and balance equations.
      9. Use the rules of nomenclature to name chemical compounds.
      10. Define the types and characteristics of chemical reactions.
      11. Use the gas laws and basics of the Kinetic Molecular Theory to solve gas problems.
      12. Determine the role of energy in physical changes and chemical reactions.
      13. Convert units of measure and demonstrate dimensional analysis skills.
    2. Lab
      1. Use basic apparatus and apply experimental methodologies used in the chemistry laboratory.
      2. Demonstrate safe and proper handling of laboratory equipment and chemicals.
      3. Conduct basic laboratory experiments with proper laboratory techniques.
      4. Make careful and accurate experimental observations.
      5. Relate physical observations and measurements to theoretical principles.
      6. Interpret laboratory results and experimental data, and reach logical conclusions.
      7. Record experimental work completely and accurately in laboratory notebooks and communicate experimental results clearly in written reports.
      8. Design fundamental experiments involving principles of chemistry.
      9. Identify appropriate sources of information for conduction laboratory experiments involving principles of chemistry.
  3. Testing Requirements
    1. Campus
      1. The midterm and lecture exam must be proctored by an approved testing organization. (I would use the WTC counseling center)
      2. Students are not allowed to use their book or notes of any kind while taking their proctored tests and exams. A periodic table will be provided.
      3. Students are allowed to use a calculator.
    2. Online
      1. The midterm and final exam must be proctored by an approved testing organization. (Ask your instructor for more details.)
      2. Students are not allowed to use their book or notes of any kind while taking their proctored tests and exams. A periodic table will be provided.
      3. Students are allowed to use a calculator.
  4. Course Requirements
    1. Campus/Online
      1. Lecture: homework assignments; weekly quizzes; midterm and final exam
      2. Lab: lab reports; final exam
      3. Quizzes and exams are timed.
  5. Information on Books and Other Course Materials
    1. Required Book:  Chemistry: A Molecular Approach, 5th Edition. Tro, Nivaldo J. 2020. Pearson. (ISBN: 9780134874371)
    2. Required Access Code: MasteringChemistry access code is bundled with book.
    3. Required Lab Kit (ONLINE ONLY): General Chemistry 1. Hands- On Learning. (SKU: Kit SP-3005-CK-02) (ISBN: 2818560391982) Please contact the WTC bookstore to purchase the kit.
    4. Required Calculators: scientific calculator
    5. Recommended: Quick Study Academic: Chemistry. Jackson, Mark. D. (ISBN: 978-142321859-3)
    6. Recommended: Quick Study Academic: Chemistry Equations & Answers. Jackson, Mark. D. (ISBN: 978-142320189-2)
  6. Grading Breakdown
    1. Campus/Online

    Lecture Homework                  10%
    Lecture Quizzes                       5%
    Lecture Exams                         10%
    Lecture Midterm                      20%
    Lecture Final Exam                 25%
    Lab Reports                             15%
    Lab Final Exam                       15%

    1. A final semester grade will be based as follows:

    A = 89.5% and above
    B = 79.5 – 89.49
    C = 69.5 – 79.49
    D = 59.5 – 69.49
    F = 59.49% and below
    I = Incomplete (failure to complete the requirements of the course)

  7. Other Policies, Procedures and important dates. Please refer to the WTC Catalog for the following:
    1. Campus Calendar
    2. Final exam schedule
    3. How to drop a class
    4. Withdrawal information
    5. Student Conduct/Academic Integrity
    6. Students with disabilities
  8. Course Content
Chapter 1: Matter, Measurement, and Problem Solving

Atoms and Molecules
The Scientific Approach to Knowledge
The Classification of Matter
Physical and Chemical Changes and Physical and Chemical Prosperities
Energy: A Fundamental Part of Physical and Chemical Change
The Units of Measurement
The Reliability of a Measurement
Solving Chemical Problems
Analyzing and interpreting Data

Chapter 2: Atoms and Elements

Brownian Motion: Atoms Confirmed
Early Ideas About the Building Blocks of Matter
Modern Atomic Theory and the Laws that Led to It
Discovery of an Electron
The Structure of an Atom
Subatomic Particles: Protons, Neutrons, and Electrons in the Atoms
Finding Patterns: The Periodic Law and the Periodic Table
Atomic Mass: The Average Mass of an Element’s Atoms
Molar Mass: Counting Atoms by Weighing Them

Chapter 3: Molecules, and Compounds

Hydrogen, Oxygen, and water
Chemical Bonds
Representing Compounds: Chemical Formulas and Molecular Models
The Atomic-Level View of Elements and Compounds
Ionic Compounds: Formulas and Names
Molecular Compounds: Formulas and Names
Summary of Inorganic Nomenclature
Formula Mass and Mole Concept for Compounds
Composition of Compounds
Determining a Chemical Formula from Experimental Data
Organic Compounds

Chapter 4: Chemical Quantities and Chemical Reactions

Climate Change and the Combustion of Fossil Fuels
Writing and Balancing Chemical equations
Reaction Stoichiometry: How Much Carbon Dioxide
Stoichiometric relationships:  Limiting Reactant, theoretical Yield, and Percent Yield
Three examples of chemical reactions: Combustion, Alkali metals and Halogens

Chapter 5: Introduction to Solutions and Aqueous reactions

Molecular Gastronomy and the Spherified cherry
Solution Concentrations
Solution Stoichiometry
Types of Aqueous Solutions and solubility
Precipitation Reactions
Representing Aqueous Reactions: Molecular, ionic and net ionic equations
Gas-evolution reactions
Oxidation-reduction reactions

Chapter 6: Gases

Supersonic Skydiving and the Risk of Decompression
Pressure: The Result of Molecular Collisions
The Simple Gas Laws: Boyle’s Law, Charles’s Law, and Avogadro’s Law
The Ideal Gas Law
Applications of the Ideal-Gas Equation: Molar Volume, Density, and Molar Mass of a Gas
Mixtures of Gases and Partial Pressures
Gases in Chemical Reactions: Stoichiometry Revisited
Kinetic Molecular Theory: A Model for Gases
Mean Free path, Diffusion, and Effusion of Gasses
Real Gases: The Effects of Size and Intermolecular Forces

Chapter 8: The Quantum-Mechanical Model of an Atom

Schrodinger’s Cat
The Nature of Light
Atomic Spectroscopy and the Bohr Model
The Wave Nature of Matter: The de Broglie Wavelength, the Uncertainty Principle, and Indeterminacy
Quantum Mechanics and Atoms
The Shapes of Atomic Orbitals

Chapter 9: Periodic Properties of the Elements

Nerve Single Transmission
Development of the Periodic Table
Electron Configurations: How electrons Occupy Orbitals
Electron Configurations, Valance Electrons, and the Periodic Table
The Explanatory Power of the Quantum-Mechanical Model
Periodic Trends in the Size of Atoms and Effective Nuclear Charge
Ions: Electron Configurations, Magnetic Properties, Ionic Radii, and Ionization Energy
Electron Affinities and Metallic Character
Periodic trend summary

Chapter 10: Chemical Bonding I: The Lewis Model

Bonding Models and AIDS Drugs
Types of Chemical Bonds
Representing Valence Electrons with Dots
Ionic Bonding: Lewis Symbols and Lattice Energies
Covalent Bonding: Lewis Structures
Electronegativity and Bond Polarity
Lewis Structures of Molecular Compounds and Polyatomic Ions
Resonance and Formal Charge
Exceptions to the Octet Rule: Odd- Electron Species, Incomplete Octets, and Expanded Octets
Bond Energies and Bond Lengths
Bonding in Metals: The Electron Sea Model

Chapter 11: Chemical Bonding II: Molecular Shapes, Valance Bond Theory, and Molecular Orbital Theory

Morphine: A molecular imposter
VESPR Theory: The Five Basic Shapes
VESPR Theory: The Effect of Lone Pairs
VESPR Theory: Predicting Molecular Geometries
Molecular Shape and Polarity
Valance Bond Theory: Orbital Overlap as a Chemical Bond
Valance Bond Theory: Hybridization of Atomic Orbitals
Molecular Orbital Theory: Electron Delocalization


Last Modified: November 15, 2019