Topic 1: Review and Introduction to Organic Chemistry

Learning Objectives

This section introduces foundational concepts in organic chemistry, emphasizing both theoretical principles and practical skills. Students are expected to develop a strong understanding of molecular structure, bonding, and the application of green chemistry principles.

• Green Chemistry Principles: Focus on sustainable chemical practices, including atom economy, reaction mass efficiency, and process mass index.

• Atomic Orbital Theory: Explains the behavior of electrons in atoms and their role in chemical bonding.

• Valence Bond Theory: Describes how atomic orbitals combine to form chemical bonds.

• Molecular Orbital Theory: Provides a quantum mechanical description of molecular bonding.

• Hybridization: Emphasizes the formation of sp, sp2, and sp3 hybrid orbitals in organic molecules.

• Bond Properties: Includes bond length, bond strength, electronegativity, and molecular polarity.

• Lewis Structures: Visual representations of molecules showing all valence electrons.

• Intermolecular Forces: Covers van der Waals forces, dipole-dipole interactions, and hydrogen bonding.

• Ways of Representing Organic Molecules: Includes Lewis structures, condensed formulas, bond-line diagrams, and resonance forms.

• Sawhorse, Newman, Fischer, and Haworth Projections: Methods for visualizing molecular geometry.

• Resonance: Delocalization of electrons in molecules with conjugated systems.

• Functional Groups: Identification and classification of key organic functional groups.

Key Terms and Definitions

• Atom Economy: A measure of the efficiency of a chemical reaction in terms of how much of the reactants end up in the desired product. Equation:

• Reaction Mass Efficiency (RME): The percentage of the total mass of reactants that is converted into the desired product. Equation:

• Process Mass Index (PMI): The ratio of the total mass used in a process to the mass of the product obtained. Equation:

• Hybridization: The mixing of atomic orbitals to form new hybrid orbitals suitable for bonding.

• Resonance: The phenomenon where a molecule can be represented by two or more valid Lewis structures.

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

Expected Student Competencies

Upon completion of this topic, students should be able to:

• Communicate (verbally or in writing) the theory of valence bond and molecular orbital models.

• Discuss and identify relevant green chemistry principles and perform related calculations.

• Calculate and interpret atom economy, reaction mass efficiency, and process mass index for chemical reactions.

• Accurately draw electron configuration diagrams and orbital diagrams.

• Determine the number of valence electrons, bond angles, and bond lengths in molecules.

• Identify hybridization states, bond angles, and construct bond-line and condensed structural formulas.

• Describe and classify intermolecular forces for non-polar and polar molecules.

• Draw and interpret various representations of organic molecules, including 3D bond-line structures.

• Use curved arrows to depict resonance and predict resonance structures.

• Choose and justify the best resonance structure for a given molecule.

• Identify and classify major organic functional groups, such as alcohols, amines, ethers, carbonyls, and carboxylic acids.

• Classify alcohols, haloalkanes, and amines as primary, secondary, or tertiary.

Table: Classification of Organic Functional Groups

Additional info:

• Some content inferred from standard organic chemistry curricula, such as the inclusion of key equations and the classification table.

• Expanded definitions and examples provided for clarity and completeness.