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. 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.
      2. 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: The Central Science w/Mastering Chemistry, 14th Edition. Brown, LeMay. 2018. Pearson Prentice Hall. (ISBN: 9780134292816)
    2. Required Access Code: MasteringChemistry access code is bundled with book.
    3. Required Lab Book (ON-CAMPUS ONLY): Laboratory Experiments for Chemistry: The Central Science, 14th Edition. Brown, LeMay, Bursten, Murphy, Woodward, Stoltzfus, Nelson & Kemp. 2018. Pearson. (ISBN 9780134566207)
    4. Required Lab Kit (ONLINE ONLY): General Chemistry 1. Hands- On Learning. (SKU: Kit SP-3005-CK-02) (ISBN: 2818560391982)
    5. Calculators: scientific calculator
  6. Grading Breakdown
    1. Campus/Online
      Lecture Homework                 10%
      Lecture Quizzes                      10%
      Lecture Midterm                      25%
      Lecture Final Exam                 25%
      Lab Reports                             15%
      Lab Final Exam                       15%
    2. 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: Introduction: Matter and Measurement

1.1 The Study of Chemistry
1.2 Classifications of Matter
1.3 Properties of Matter
1.4 The Nature of Energy
1.5 Uncertainty in Measurement
1.6 Dimensional Analysis

Chapter 2: Atoms, Molecules, and Ions

2.1 The Atomic Theory of Matter
2.2 The Discovery of Atomic Structure
2.3 The Modern View of Atomic Structure
2.4 Atomic Weights
2.5 The Periodic Table
2.6 Molecules and Molecular Compounds
2.7 Ions and Ionic Compounds
2.8 Naming Inorganic Compounds
2.9 Some Simple Organic Compounds

Chapter 3: Chemical Reactions and Reaction Stoichiometry

3.1 Chemical Equations
3.2 Simple Patterns of Chemical Reactivity
3.3 Formula Weights
3.4 Avogadro’s Number and the Mole
3.5 Empirical Formulas from Analyses
3.6 Quantitative Information from Balanced Equations
3.7 Limiting Reactants

Chapter 4: Reactions in Aqueous Solution

4.1 General Properties of Aqueous Solutions
4.2 Precipitation Reactions
4.3 Acids, Bases, and Neutralization Reactions
4.4 Oxidation-Reduction Reactions
4.5 Concentrations of Solutions
4.6 Solution Stoichiometry and Chemical Analysis

Chapter 6: Electronic Structure of Atoms

6.1 The Wave Nature of Light
6.2 Quantized Energy and Photons
6.3 Line Spectra and the Bohr Model
6.4 The Wave Behavior of Matter
6.5 Quantum Mechanics and Atomic Orbitals
6.6 Representations of Orbitals
6.7 Many-Electron Atoms
6.8 Electron Configurations
6.9 Electron Configurations and the Periodic Table

Chapter 7: Periodic Properties of the Elements

7.1 Development of the Periodic Table
7.2 Effective Nuclear Charge
7.3 Sizes of Atoms and Ions
7.4 Ionization Energy
7.5 Electron Affinity
7.6 Metals, Nonmetals, and Metalloids
7.7 Trends for Groups 1A and Group 2A Metals
7.8 Trends for Selected Nonmetals

Chapter 8: Basic Concepts of Chemical Bonding

8.1 Lewis Symbols and the Octet Rule
8.2 Ionic Bonding
8.3 Covalent Bonding
8.4 Bond Polarity and Electronegativity
8.5 Drawing Lewis Structures
8.6 Resonance Structures
8.7 Exceptions to the Octet Rule
8.8 Strengths and Lengths of Covalent Bonds

Chapter 9: Molecular Geometry and Bonding Theories

9.1 Molecular Shapes
9.2 The VSEPR Model
9.3 Molecular Shape and Molecular Polarity
9.4 Covalent Bonding and Orbital Overlap
9.5 Hybrid Orbitals
9.6 Multiple Bonds
9.7 Molecular Orbitals
9.8 Bonding in Period 2 Diatomic Molecules

Chapter 10: Gases

10.1 Characteristics of Gases
10.2 Pressure
10.3 The Gas Laws
10.4 The Ideal-Gas Equation
10.5 Further Applications of the Ideal-Gas Equation
10.6 Gas Mixtures and Partial Pressures
10.7 The Kinetic-Molecular Theory of Gases
10.8 Molecular Effusion and Diffusion
10.9 Real Gases: Deviations from Ideal Behavior



Last Modified: August 25, 2017