Ochem W.2 slide flashcard

What do acids do in acid-base chemistry?

Acids donate protons (H+).

What do bases do in acid-base chemistry?

Bases accept protons.

Define Bronsted-Lowry acids.

Substances that donate protons.

What are Lewis acids?

Electron pair acceptors.

How does electronegativity affect bond polarity?

Polar bonds occur when atoms with differing electronegativities are bonded together.

What is an example of a non-polar molecule?

Carbon dioxide (CO2) is non-polar due to linear geometry.

What is resonance in chemistry?

Delocalization of electrons within molecules.

What has more stability in resonance structures?

More covalent bonds, less charge separation, and complete valence shells.

Explain the concept of pKa.

Defines the strength of an acid; lower pKa means a stronger acid.

How does solubility change with pH?

Solute solubility can be impacted by pH; for example, phenylethylamine is more soluble at lower pH due to protonation.

What is the acid-base equilibrium constant (Keq)?

The ratio of product concentrations to reactant concentrations at equilibrium.

What does a lower pKa indicate about an acid's strength?

It indicates that the acid is stronger.

What does an electron withdrawing group do to anions?

It stabilizes anions, leading to higher acidity.

What effect do larger anions have on stability?

Larger anions are generally more stable.

What does the curved arrow mechanism demonstrate?

It shows electron flow in acid/base reactions.

What is a key feature of resonance structures?

Lone pairs, double bonds, and triple bonds can move.

What is the importance of pKa values?

They help determine the relative acidity and stability of species.

What occurs during acid-base reactions according to the dynamics?

Reactions can be reversible, favoring the formation of weaker acids and bases.

What role does solvent play in acid/base reactions?

Solvents influence acid/base reactions via the levelling effect.

What are the criteria for identifying acid/base reactions?

Identify acid, base, conjugate acid (CA), and conjugate base (CB).

What does the inductive effect refer to?

Electronegative atoms stabilize the negative charge of conjugate bases.