CHEM 1412
General Chemistry II

Western Texas College

  1. Basic Course Information
    1. Lecture—Chemical equilibrium; phase diagrams and spectrometry; acid-base concepts; thermodynamics; kinetics; electrochemistry; nuclear chemistry; an introduction to organic chemistry and descriptive inorganic 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:  Need a C or higher in CHEM 1411.
    4. Required grade for enrolling in the next course in this sequence: None
  2. Student Learning Outcomes
    1. Lecture
      1. State the characteristics of liquids and solids, including phase diagrams and spectrometry.
      2. Articulate the importance of intermolecular interactions and predict trends in physical properties.
      3. Identify the characteristics of acids, bases, and salts, and solve problems based on their quantitative relationships.
      4. Identify and balance oxidation-reduction equations, and solve redox titration problems.
      5. Determine the rate of reaction and its dependence on concentration, time, and temperature.
      6. Apply the principles of equilibrium to aqueous systems using LeChâtelier’s Principle to predict the effects of concentration, pressure, and temperature changes on equilibrium mixtures.
      7. Analyze and perform calculations with the thermodynamic functions, enthalpy, entropy, and free energy.
      8. Discuss the construction and operation of galvanic and electrolytic electrochemical cells, and determine standard and non-standard cell potentials.
      9. Define nuclear decay processes.
      10. Describe basic principles of organic chemistry and descriptive inorganic chemistry.
    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 and chemical instrumentation.
      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, 13th Edition. Brown, LeMay. 2015. Pearson Prentice Hall. (ISBN: 0321864409)
    2. Required Access Code: MasteringChemistry access code is bundled with book.
    3. Required Lab Kit (ONLINE ONLY): General Chemistry v.2 Lab Kit. eScience Labs. (SKU: Kit4119)
    4. 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 5: Thermochemistry

5.1 Energy
5.2 The First Law of Thermodynamics
5.3 Enthalpy
5.4 Enthalpies of Reaction
5.5 Calorimetry
5.6 Hess’s Law
5.7 Enthalpies of Formation
5.8 Foods and Fuels

Chapter 11: Liquids and Intermolecular Forces

11.1 A Molecular Comparison of Gases, Liquids, and Solids
11.2 Intermolecular Forces
11.3 Select Properties of Liquids
11.4 Phase Changes
11.5 Vapor Pressure
11.6 Phase Diagrams
11.7 Liquid Crystals

Chapter 12: Solids and Modern Materials

12.1 Classification of Solids
12.2 Structures of Solids
12.3 Metallic Solids
12.4 Metallic Bonding
12.5 Ionic Solids
12.6 Molecular Solids
12.7 Covalent-Network Solids
12.8 Polymers
12.9 Nanomaterials

Chapter 13: Properties of Solutions

13.1 The Solution Process
13.2 Saturated Solutions and Solubility
13.3 Factors Affecting Solubility
13.4 Expressing Solution Concentration
13.5 Colligative Properties
13.6 Colloids

Chapter 14: Chemical Kinetics

14.1 Factors that Affect Reaction Rates
14.2 Reaction Rates
14.3 Concentration and Rate Laws
14.4 The Change of Concentration with Time
14.5 Temperature and Rate
14.6 Reaction Mechanisms
14.7 Catalysis

Chapter 15: Chemical Equilibrium

15.1 The Concept of Equilibrium
15.2 The Equilibrium Constant
15.3 Understanding and Working with Equilibrium Constants
15.4 Heterogeneous Equilibria
15.5 Calculating Equilibrium Constants
15.6 Applications of Equilibrium Constants
15.7 Le Châtelier’s Principle

Chapter 16: Acid-Base Equilibria

16.1 Acids and Bases: A Brief Review
16.2 Brønsted-Lowry Acids and Bases
16.3 The Autoionization of Water
16.4 The pH Scale
16.5 Strong Acids and Bases
16.6 Weak Acids
16.7 Weak Bases
16.8 Relationship between Ka and Kb
16.9 Acid-Base Properties of Salt Solutions
16.10 Acid-Base Behavior and Chemical Structure
16.11 Lewis Acids and Bases

Chapter 17: Additional Aspects of Aqueous Equilibria

17.1 The Common-Ion Effect
17.2 Buffers
17.3 Acid-Base Titrations
17.4 Solubility Equilibria
17.5 Factors that Affect Solubility
17.6 Precipitation and Separation of Ions
17.7 Qualitative Analysis for Metallic Elements

Chapter 19: Chemical Thermodynamics

19.1 Spontaneous Processes
19.2 Entropy and the Second Law of Thermodynamics
19.3 The Molecular Interpretation of Entropy and the Third Law of Thermodynamics
19.4 Entropy Changes in Chemical Reactions
19.5 Gibbs Free Energy
19.6 Free Energy and Temperature
19.7 Free Energy and the Equilibrium Constant

Chapter 20: Electrochemistry

20.1 Oxidation States and the Oxidation-Reduction Reactions
20.2 Balancing Redox Equations
20.3 Voltaic Cells
20.4 Cell Potentials Under Standard Conditions
20.5 Free Energy and Redox Reactions
20.6 Cell Potentials Under Nonstandard Conditions
20.7 Batteries and Fuel Cells
20.8 Corrosion
20.9 Electrolysis

Chapter 21: Nuclear Chemistry

21.1 Radioactivity and Nuclear Equations
21.2 Patterns of Nuclear Stability
21.3 Nuclear Transmutations
21.4 Rates of Radioactive Decay
21.5 Detection of Radioactivity
21.6 Energy Changes in Nuclear Reactions
21.7 Nuclear Power: Fission
21.8 Nuclear Power: Fusion
21.9 Radiation in the Environment and Living Systems

Chapter 24: The Chemistry of Life: Organic and Biological Chemistry

24.1 General Characteristics of Organic Molecules
24.2 Introduction to Hydrocarbons
24.3 Alkenes, Alkynes, and Aromatic Hydrocarbons
24.4 Organic Functional Groups
24.5 Chirality in Organic Chemistry
24.6 Introduction to Biochemistry
24.7 Proteins
24.8 Carbohydrates
24.9 Lipids
24.10 Nucleic Acids



Last Modified: January 17, 2017