14.1: General Acidity and Basicity 14.2: Lewis Bases What makes a molecule (or an atom or ion) a Lewis base? It must have a pair of electrons available to share with another atom to form a bond. The most readily available electrons are those that are not already in bonds. Bonding electrons are low in energy. Non-bonding electrons are higher in energy and may be stabilized when they are delocalized in a new bond. 14.3: Lewis Acids 14.4: Lewis Acid-Base Complexes and Molecular Orbitals 14.5: Reversibility of the Dative Bond 14.6: Coordination Complexes 14.7: Proton as a Common Lewis Acid 14.8: Proton Transfer from One Basic Site to Another and Molecular Orbital Interactions in Proton Transfers 14.9: Proton Donor Strength- pKa 14.10: The Relationship Between Structure and Bronsted-Lowry Acidity 14.11: Factors Affecting Bronsted-Lowry Acidity- Local Factors 14.12: Factors affecting Bronsted-Lowry Acidity- Distal Factors 14.13: Effects on Basicity (Attraction for Proton) 14.14: The Direction of Proton Transfer 14.15: Amino Acids and Peptides 14.16: Relative Conditions and pKa 14.17: The Meaning of pKa- Product-to-Reactant Ratio and Equilibrium Constant 14.18: pH and Buffers 14.19: Application Problems 14.20: Solutions to Selected Problems