How do you account for the reducing behaviour of $H_{3}PO_{2}$ on the basis of its structure?

(N/A) The structure of $H_{3}PO_{2}$ (hypophosphorous acid) contains two $P-H$ bonds and one $P=O$ bond,along with one $P-OH$ bond.
Because of the presence of two $P-H$ bonds,$H_{3}PO_{2}$ acts as a strong reducing agent.
The $H$ atoms bonded directly to the $P$ atom are responsible for its reducing character.