General Chemistry II (CHE117) Syllabus and Study Guide

General Chemistry II: Course Overview and Study Guide

Course Description

This course is a systematic study of thermodynamics, kinetics, equilibrium, electrochemistry, nuclear chemistry, and an introduction to organic chemistry. It is designed for students pursuing science, engineering, and health-related majors.

• Credits: 3 credits, 3 contact hours per week

• Prerequisites: CHE 115, CHE 116, and MTH 112 or MTH 130

• Instructor: Ahsan Marion

Course Learning Outcomes

• Perform calculations related to kinetics, equilibrium, thermodynamics, oxidation-reduction reactions, and basic buffer systems.

• Explain and apply the basic theories of kinetics, equilibrium, thermodynamics, and electrochemistry.

• Recognize, compare, and explain the structures of organic compounds and coordination complexes.

• Assess and describe the physical and chemical properties of compounds based on an understanding of their structure.

Core Course Content

• Chemical Kinetics

• Chemical Equilibrium

• Acid-Base Equilibria

• Thermodynamics

• Electrochemistry

• Characteristics of the Nonmetals and Coordination Compounds

• Introduction to Organic Chemistry

Key Topics and Chapter Objectives

Chemical Kinetics (Chapter 14)

Chemical kinetics studies the rates of chemical reactions and the factors affecting them.

• Reaction Rates: Calculate reaction rates and average rates from experimental data.

• Rate Laws: Determine rate laws and reaction orders using experimental data.

• Integrated Rate Laws: Use integrated rate laws for zero, first, and second-order reactions.

• Arrhenius Equation: Understand the effect of activation energy and temperature on reaction rates.

• Catalysis: Differentiate between homogeneous and heterogeneous catalysts.

Example: For a first-order reaction, the integrated rate law is:

$\ln [A]_t = -kt + \ln [A]_0$

Chemical Equilibrium (Chapter 15)

Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products.

• Equilibrium Constant (K): Write and calculate equilibrium expressions for chemical reactions.

• Le Châtelier's Principle: Predict the effect of changes in concentration, temperature, and pressure on equilibrium position.

• ICE Tables: Use ICE (Initial, Change, Equilibrium) tables to solve equilibrium problems.

Example: For the reaction $aA + bB \rightleftharpoons cC + dD$, the equilibrium constant is:

$K_c = \frac{[C]^c[D]^d}{[A]^a[B]^b}$

Acid-Base Equilibria (Chapter 16)

This topic covers the properties of acids and bases, their equilibria, and calculations involving pH and buffer solutions.

• Brønsted-Lowry Theory: Acids are proton donors; bases are proton acceptors.

• pH and pOH: Calculate pH, pOH, and concentrations of H+ and OH- ions.

• Weak Acids and Bases: Use $K_a$ and $K_b$ to solve for equilibrium concentrations.

• Buffers: Understand buffer solutions and calculate their pH using the Henderson-Hasselbalch equation.

Example: The Henderson-Hasselbalch equation for a buffer is:

$pH = pK_a + \log \left( \frac{[A^-]}{[HA]} \right)$

Aqueous Equilibria (Chapter 17)

This chapter focuses on solubility equilibria and the behavior of sparingly soluble salts.

• Solubility Product (Ksp): Calculate the solubility of salts and predict precipitation.

• Common Ion Effect: Understand how the presence of a common ion affects solubility.

• Complex Ion Formation: Apply equilibrium concepts to complex ions.

Example: For $AgCl (s) \rightleftharpoons Ag^+ (aq) + Cl^- (aq)$, the solubility product is:

$K_{sp} = [Ag^+][Cl^-]$

Thermodynamics (Chapter 18)

Thermodynamics examines the energy changes in chemical reactions, including enthalpy, entropy, and free energy.

• First Law of Thermodynamics: Energy is conserved in chemical processes.

• Enthalpy (ΔH): Calculate heat changes at constant pressure.

• Entropy (ΔS): Measure the disorder or randomness of a system.

• Gibbs Free Energy (ΔG): Predict spontaneity of reactions using:

$\Delta G = \Delta H - T\Delta S$

Electrochemistry (Chapter 19)

Electrochemistry studies the relationship between chemical reactions and electricity.

• Oxidation-Reduction (Redox) Reactions: Assign oxidation numbers and balance redox equations.

• Electrochemical Cells: Understand galvanic (voltaic) and electrolytic cells.

• Cell Potentials: Calculate standard cell potentials using standard reduction potentials.

Example: The standard cell potential is:

$E_{cell}^\circ = E_{cathode}^\circ - E_{anode}^\circ$

Nuclear Chemistry (Chapter 20)

Nuclear chemistry involves the study of changes in atomic nuclei, including radioactive decay and nuclear reactions.

• Types of Radiation: Alpha, beta, and gamma decay.

• Balancing Nuclear Equations: Write and balance equations for nuclear processes.

• Radioactive Decay Law: Calculate the amount of radioactive material remaining after a given time.

Example: The radioactive decay law is:

$N = N_0 e^{-kt}$

Coordination Chemistry (Chapter 22)

This topic introduces coordination compounds, their structures, and nomenclature.

• Complex Ions: Identify ligands, coordination numbers, and write formulas for coordination compounds.

• Nomenclature: Name coordination compounds according to IUPAC rules.

Introduction to Organic Chemistry (Chapter 23)

Organic chemistry is the study of carbon-containing compounds and their properties.

• Functional Groups: Recognize and name common functional groups (alkanes, alkenes, alkynes, alcohols, ethers, aldehydes, ketones, carboxylic acids, amines, etc.).

• Isomerism: Understand structural and geometric isomers.

Lab Techniques and Procedures

Laboratory experiments are designed to reinforce lecture concepts and develop practical skills in measurement, observation, and data analysis.

CHE118 Experiment	CHE117 Lecture Connection
Calibration Curve Review	Review of CHE115, quantitative analysis, and calibration curves
Spectrophotometric Determination of Iron in a Vitamin	Application of Beer-Lambert Law, solution concentrations
Kinetics of the Crystal Violet and Sodium Hydroxide Reaction	Chemical kinetics, rate laws, and reaction order (CHE117 Ch. 14)
Determination of K for a Chemical Reaction	Chemical equilibrium, equilibrium constant (CHE117 Ch. 15)
Systems in Equilibrium	Le Châtelier’s Principle, equilibrium shifts (CHE117 Ch. 15)
Titration of a Commercial Antacid	Acid-base titration, buffer systems (CHE117 Ch. 16)
Qualitative Analysis of Anions	Solubility equilibria, precipitation reactions (CHE117 Ch. 17)
Qualitative Analysis of Cations	Complex ion formation, solubility (CHE117 Ch. 17, 22)
Measurement of Enthalpy Changes	Thermodynamics, enthalpy (CHE117 Ch. 18)
Potentiometric Titration of Redox Systems	Electrochemistry, redox titration (CHE117 Ch. 19)
Biochemistry & Organic Molecules	Organic chemistry, functional groups (CHE117 Ch. 23)

Grading and Assessment

• Grades are based on quizzes (20%) and tests (80%).

• Lowest test score is not dropped.

• Letter grades are assigned according to standard percentage ranges (A: 90-100%, B: 80-89.9%, etc.).

Academic Integrity and Policies

• Cheating, plagiarism, and other forms of academic dishonesty are strictly prohibited.

• Students are expected to adhere to all college policies regarding attendance, assignments, and conduct.

Additional Info

• Blackboard is used for all assignments and course materials.

• Calculator (non-programmable) is required for exams and quizzes.

• Students are encouraged to use college resources such as tutoring and library services.