Understanding Acids and Bases

What is a Lewis acid?

• A Lewis acid is an electron pair acceptor.

• A Lewis acid is a proton donor.

• A Lewis acid is a neutral molecule.

• A Lewis acid is an electron pair donor.

What is a Lewis base?

• A Lewis base is an electron pair acceptor.

• A Lewis base is a proton donor.

• A Lewis base is a substance that increases the concentration of hydroxide ions.

• A Lewis base is an electron pair donor.

How does the Lewis theory differ from the Brønsted-Lowry theory?

• Lewis theory focuses on electron pairs, while Brønsted-Lowry theory focuses on proton transfer.

• Brønsted-Lowry theory focuses on electron pairs, while Lewis theory focuses on acid-base strength.

• Lewis theory is based on acid-base strength, while Brønsted-Lowry theory is based on electron pairs.

• Lewis theory only applies to gases, while Brønsted-Lowry theory applies to all states of matter.

Define a Brønsted-Lowry acid.

• A Brønsted-Lowry acid is a substance that forms salts in solution.

• A Brønsted-Lowry acid is a substance that donates a proton (H+) in a chemical reaction.

• A Brønsted-Lowry acid is a substance that neutralizes bases.

• A Brønsted-Lowry acid is a substance that accepts a proton (H+).

Define a Brønsted-Lowry base.

• A Brønsted-Lowry base is a substance that donates protons.

• A Brønsted-Lowry base is a substance that accepts protons.

• A Brønsted-Lowry base is a substance that remains neutral in reactions.

• A Brønsted-Lowry base is a substance that increases acidity.

What is an Arrhenius acid?

• A substance that decreases the concentration of H+ ions in solution.

• A substance that increases the concentration of OH- ions in solution.

• A neutral substance that does not affect ion concentration in solution.

• An Arrhenius acid is a substance that increases the concentration of H+ ions in solution.

What is an Arrhenius base?

• A substance that increases hydrogen ion concentration in water.

• An Arrhenius base is a substance that increases hydroxide ion concentration in water.

• A substance that decreases hydroxide ion concentration in water.

• A substance that neutralizes acids without producing hydroxide ions.

How do Arrhenius acids and bases differ from Lewis acids and bases?

• Arrhenius acids are always strong, while Lewis acids are always weak.

• Lewis acids produce hydroxide ions in water, while Arrhenius acids do not.

• Arrhenius bases accept protons, while Lewis bases donate protons.

• Arrhenius acids and bases are defined by their ion production in water, while Lewis acids and bases are defined by their ability to accept or donate electron pairs.

Provide an example of a Lewis acid and explain why it fits the definition.

• Aluminum chloride (AlCl3)

• Sodium chloride (NaCl)

• Hydrochloric acid (HCl)

• Water (H2O)

Provide an example of a Brønsted-Lowry acid and its conjugate base.

• Sulfuric acid (H2SO4) and its conjugate base, sulfate ion (SO4^2-)

• Nitric acid (HNO3) and its conjugate base, nitrate ion (NO3-)

• Acetic acid (CH3COOH) and its conjugate base, acetate ion (CH3COO-)

• Hydrochloric acid (HCl) and its conjugate base, chloride ion (Cl-).