Final answer:
In the equation N₂ + 3H₂ → 2NH₃, N₂ can be considered a Lewis acid and H₂ a Lewis base, as there are no protons exchanged to categorize them as Brønsted-Lowry acids or bases.
Step-by-step explanation:
In the chemical equation N2 + 3H2 → 2NH3, there are no protons (H+) being donated or accepted, which means the reactants cannot be directly identified as Brønsted-Lowry acids or bases. However, if we look at the reaction from a Lewis acid-base perspective, we can say that N2 is acting as a Lewis acid because it is accepting a pair of electrons from H2, which is acting as a Lewis base.
The Lewis definition considers acids and bases in terms of electron pair donors and acceptors rather than proton donors and acceptors. It's also worth noting that in other reactions, ammonia (NH3) can act as a Brønsted-Lowry base because it readily accepts protons.