Organic Chemistry I: Course Syllabus and Topic Overview

Course Structure and Main Topics

This syllabus outlines the structure and major topics covered in a college-level Organic Chemistry I course. The course is organized by weekly topics, exams, and key concepts fundamental to understanding organic chemistry.

• Weeks 1-2: Introduction and Foundations

  • Syllabus and Course Policies: Overview of course expectations and resources.

  • Introduction to Organic Chemistry: Definition, scope, and importance of organic chemistry in science and industry.

  • Bonding: Types of chemical bonds (covalent, ionic), electron sharing, and bond formation.

  • Formal Charge: Calculation and significance in molecular structures.

  • Lewis Structures: Drawing molecules to represent bonding and lone pairs.

  • Hybrid Orbitals: Concept of orbital hybridization (sp, sp2, sp3).

  • Bond Angles: Geometric considerations in molecular shape.

• Weeks 3-4: Molecular Forces and Nomenclature

  • Intermolecular Forces: Types (hydrogen bonding, dipole-dipole, London dispersion) and their effects on physical properties.

  • Functional Group Overview: Introduction to key functional groups in organic molecules (alkanes, alkenes, alkynes, alcohols, etc.).

  • Alkane Reactions: Basic reactions involving alkanes, such as combustion and halogenation.

  • Nomenclature (IUPAC): Systematic naming of organic compounds according to IUPAC rules.

• Week 5: Exam 1

  • Assessment: Covers foundational topics including bonding, structure, and nomenclature.

• Weeks 6-7: Conformational and Stereochemical Analysis

  • Straight Chain Conformational Analysis: Study of different spatial arrangements of atoms in alkanes.

  • Newman Projections: Visual representation of conformations around single bonds.

  • Cycloalkanes: Structure and properties of ring-shaped alkanes.

  • Cyclohexane Chair Conformational Analysis: Analysis of the most stable conformations of cyclohexane.

  • Substituted Cycloalkanes: Effects of substituents on ring stability and reactivity.

• Weeks 8-9: Reactions and Mechanisms

  • Substitution Reactions: Mechanisms and types (SN1, SN2).

  • Chlorination of Methane: Example of a radical substitution reaction.

  • Chain Reactions: Steps in radical chain mechanisms (initiation, propagation, termination).

• Weeks 10-11: Thermodynamics and Kinetics

  • Energy and Kinetics: Study of reaction rates and energy changes.

  • Transition State Theory: Concept of activation energy and transition states.

  • Thermodynamics: Enthalpy, entropy, and free energy in chemical reactions.

• Week 12: Exam 2

  • Assessment: Covers conformational analysis, reactions, and thermodynamics.

• Weeks 13-14: Stereochemistry

  • Intro to Stereochemistry: Study of spatial arrangement of atoms in molecules.

  • Optical Rotation: Measurement of chiral compounds' ability to rotate plane-polarized light.

  • R/S Nomenclature: System for designating absolute configuration at chiral centers.

  • Enantiomers and Diastereomers: Types of stereoisomers.

  • Fischer Projections: Two-dimensional representations of stereochemistry.

  • E/Z Nomenclature: Designation for double bond stereochemistry.

• Weeks 15-16: Nucleophilic Substitution and Halides

  • Nucleophilic Aliphatic Substitution: Mechanisms and factors affecting SN1 and SN2 reactions.

  • Alkyl Halides: Structure, reactivity, and uses in organic synthesis.

• Final Weeks: Review and Final Exam

  • Review: Comprehensive review of all course topics.

  • Final Exam: Cumulative assessment covering the entire course.

Key Terms and Concepts

• Functional Group: A specific group of atoms within a molecule responsible for characteristic chemical reactions.

• Hybridization: The mixing of atomic orbitals to form new hybrid orbitals suitable for the pairing of electrons.

• Enantiomer: One of two stereoisomers that are mirror images of each other but not superimposable.

• Activation Energy (): The minimum energy required for a chemical reaction to occur.

• Transition State: A high-energy state during a reaction where bonds are partially formed and broken.

Example: Drawing a Lewis Structure

• Step 1: Count total valence electrons.

• Step 2: Draw a skeletal structure.

• Step 3: Distribute electrons to satisfy the octet rule.

• Step 4: Assign formal charges as needed.

Example Equation: Gibbs Free Energy

The relationship between enthalpy, entropy, and free energy is given by:

Additional info:

• This syllabus is typical for a first-semester organic chemistry course and provides a logical progression from foundational concepts to more advanced topics such as stereochemistry and reaction mechanisms.