Explain why n2h4 acts as bronsted lowry base but n20 does not
To understand why N2H4 acts as a Bronsted-Lowry base, we need to recall the definitions of acids and bases according to the Bronsted-Lowry theory.
According to the Bronsted-Lowry theory, an acid is a species that donates a proton (H+) in a chemical reaction, while a base is a species that accepts a proton.
N2H4, also known as hydrazine, has a structure where each nitrogen atom is bonded to two hydrogen atoms. Due to the electronegativity difference between nitrogen and hydrogen, the N-H bond is polar, with hydrogen being slightly positive and nitrogen being slightly negative.
In a chemical reaction, hydrazine can donate one of its hydrogen atoms, which essentially means it donates a proton (H+). This proton donation qualifies hydrazine as a Brønsted-Lowry base.
On the other hand, N2O, commonly known as nitrous oxide or laughing gas, consists of a nitrogen atom bonded to two oxygen atoms. Nitrous oxide does not possess any hydrogen atoms. Since it lacks hydrogen, it cannot donate a proton and therefore cannot act as a Brønsted-Lowry base.