• Brønsted–Lowry Base: A molecule that can accept a proton (H+). It has at least one pair of electrons ready to bond with that lonely proton.

  • Real World Example: Imagine the proton as a lonely person on Valentine's Day. The Brønsted–Lowry base is like a friend with an extra ticket to a concert! 🎵

• Lewis Acid & Base

  • Lewis Acid: A molecule that accepts an electron pair.
  • Lewis Base: A molecule that donates an electron pair.
  • Real World Example: Think of the Lewis Acid as someone who has a vacant seat in their car and the Lewis Base as someone offering a GPS (electron pair) for the journey.🚗

Arrhenius, Brønsted–Lowry, and Lewis Theories: While the Arrhenius and Brønsted–Lowry theories have their charm, the Lewis theory is the broad-minded friend in the group! It includes a wider range of substances.

Both ammonia (NH3) and the hydroxide ion (OH-) are multitaskers! They can act as both Brønsted–Lowry and Lewis bases.

• They’re like those friends who are equally good at cooking and singing. 🍳🎤

BF3 (boron trifluoride) + NH3 (ammonia): In this bonding session, ammonia donates an electron pair to BF3. So, ammonia is the Lewis base and BF3 is the Lewis acid.

• Real World Example: This is like two puzzle pieces fitting perfectly without needing an extra piece (proton) to connect them.