Organic Chemistry Chapter 3: Acids and Bases

These flashcards cover fundamental concepts of acids and bases as discussed in Organic Chemistry, specifically focusing on Bronsted-Lowry definitions, Ka and pKa values, resonance, induction, and the leveling effect.

What is a Bronsted-Lowry acid?

A Bronsted-Lowry acid is defined as a substance that donates a proton.

What defines a Bronsted-Lowry base?

A Bronsted-Lowry base is defined as a substance that accepts a proton.

What is a conjugate acid?

A conjugate acid is the species formed when a base accepts a proton.

What is a conjugate base?

A conjugate base is the species formed when an acid donates a proton.

What do curved arrows represent in acid-base reactions?

Curved arrows represent the movement of electron density during bond formation and bond breaking.

What does a larger Ka value indicate about an acid?

A larger Ka value indicates a stronger acid.

How do pKa values relate to acid strength?

A lower pKa value indicates a stronger acid.

What is the effect of resonance on acidity?

Resonance can stabilize a negative charge, thereby increasing the strength of the corresponding acid.

What is induction in terms of acidity?

Induction refers to the electron-withdrawing effects of nearby electronegative atoms which can stabilize a conjugate base.

Define the leveling effect in solvents.

The leveling effect occurs when a solvent, like water, can act as an acid or base, thus limiting the strengths of acids and bases that can exist in that solvent.

What does ARIO stand for in acidity assessment?

ARIO stands for Atom, Resonance, Induction, and Orbital, which are factors used to assess stability of conjugate bases.

Why can't strong acids like sulfuric acid exist in water?

Strong acids like sulfuric acid will react with water to form H3O+, effectively quenching their acidity.

What determines the stability of a cationic acid?

The more stable the cationic acid is, the less acidic it becomes.