Brønsted-Lowry Theory:
* Focuses on the transfer of protons (H+) during acid-base reactions.
* Acid: A substance that donates a proton (H+).
* Base: A substance that accepts a proton (H+).
How a substance acts as a Brønsted-Lowry base:
1. Presence of a lone pair: Brønsted-Lowry bases typically have a lone pair of electrons. This lone pair is available to form a bond with a proton (H+).
2. Reaction with an acid: When a Brønsted-Lowry base reacts with an acid, it accepts a proton from the acid. This forms a new bond between the base and the proton.
Example:
* Ammonia (NH3) is a Brønsted-Lowry base. It has a lone pair of electrons on the nitrogen atom.
* Water (H2O) can act as both a Brønsted-Lowry acid and base.
* As an acid: It can donate a proton (H+), forming the hydroxide ion (OH-).
* As a base: It can accept a proton (H+), forming the hydronium ion (H3O+).
Key points to remember:
* Brønsted-Lowry bases are not necessarily hydroxide-containing compounds.
* They can be molecules, ions, or even atoms.
* The ability of a substance to act as a base depends on its specific chemical structure and the reaction conditions.
