Lecture 11 – Acidity and Basicity, Interactions Overview

A collection of vocabulary flashcards derived from the lecture on acidity, basicity, and molecular interactions, focused on key concepts and definitions relevant to the topic.

Acidity

The strength of a compound to lose a proton, typically in relation to functional groups.

Hydroxyl Group

An –OH functional group that can lose a proton and contribute to acidity.

Deprotonation

The removal of a proton (H+) from a molecule, increasing its negative charge.

Inductive Effect

An electronic effect whereby a neighboring atom pulls electrons away from a functional group, increasing acidity.

Resonance Stabilization

A phenomenon where a molecule can be represented by multiple structures, enhancing stability and acidity.

Thiols

Organic compounds containing sulfur, analogous to alcohols, but typically better acids.

Basicity

The ability of a compound to accept protons (H+), typically involving functional groups like amines.

Conjugate Base

The species that remains after an acid donates a proton; influences the acidity of the original acid.

Hydrogen Bond

A type of attractive interaction where a hydrogen atom covalently bonded to an electronegative atom is attracted to another electronegative atom.

Electrostatic Interaction

The attraction between positively and negatively charged particles.

Hydrophobic Effect

A tendency for non-polar substances to aggregate in aqueous solutions to minimize their exposure to water.

Steric Hinderance

The prevention of molecular interactions due to the presence of bulky groups that cause repulsion.

Functional Groups

Specific groups of atoms that give molecules distinct properties and dictate their behavior in chemical reactions.

Carboxylic Acid

A weak acid characterized by the presence of a carboxyl group (–COOH), which can easily donate a proton.

Amines

Organic compounds derived from ammonia (NH3) by replacing one or more hydrogen atoms with alkyl or aryl groups; they are basic in nature.