Mind Map: How Far and How Fast?

1. Reaction Reversibility

• Examples of Reversible Reactions:

  • Cyanohydrin formation: reversible in water (Chapter 6).

  • Proton transfer:

    • HCl → nearly complete transfer to water (strong acid).

    • Carboxylic acids → partial transfer (Chapter 8).

• Irreversible Reactions:

  • Loss of gaseous products like SO₂ and HCl (Chapter 10).

• Tetrahedral Intermediate Behavior:

  • Can collapse back to reactant (ester) or proceed to products (acid + alcohol) (Chapter 10).

2. Relative Stability of Compounds

• Key Determinants of Stability:

  • Stability of conjugate base influences acid strength (Chapter 8).

  • Examples:

    • F⁻ more stable than CH₃⁻ (fluorine > carbon in electronegativity) (Chapter 8).

    • Oximes more stable than imines (due to delocalization from electronegative substituents) (Chapter 11).

3. Reaction Rates

• Reaction-Specific Differences:

  • Benzaldehyde reduces 400x faster than acetophenone in isopropanol (Chapter 6).

  • Amines react rapidly with acetic anhydride (hours at room temperature), alcohols react very slowly without a base (Chapter 10).

  • Secondary/tertiary amides are challenging to hydrolyze but succeed with strong base and minimal water (Chapter 10).

  • Acyclic hemiacetals form slowly but are accelerated by acid or base (Chapter 11).

4. Understanding Reaction Dynamics

• Key Questions:

  • Why can some reactions run forwards or backwards?

  • Why are some products formed irreversibly while others reach equilibrium?

  • Why are some reactions fast and others slow?

• Practical Application:

  • Control reaction speed to favor desired products and minimize undesired ones.

  • Use equilibrium and stability principles to optimize yields.