# What is the number of acidic hydrogens and the n-factor of hypophosphorous acid?

My teacher said that the hydrogen which is directly linked with oxygen or more electronegative atom is an acidic hydrogen, and that the $$n$$-factor for an acid is the number of acidic hydrogens.

Then why is the $$n$$-factor of phosphinic acid $$\ce{H3PO2}$$ is 1? I saw its structure, all $$\ce{H}$$ atoms are linked to a more electronegative atom:

• Please note that the concept of "n-factors" is only used in Indian chemistry books but not in real chemistry. May 26 at 7:26
• Related for phosphorous acid: chemistry.stackexchange.com/questions/122736/… May 26 at 10:44

The structure of hypophosphorous acid is $$\ce{HO-PH2=O}$$. The electronegativity of phosphorus is near the same as for hydrogen. The oxygen causes slight polarization of $$\ce{P-H}$$ bond, making $$\ce{H}$$ slighly acidic, but acidity of the $$\ce{H-P}$$ is negligible in water environment.

Note that if putting rare exceptions and circumstances aside, we do not consider hydrocarbons as acids either. Even $$\ce{NH3}$$ is very weakly acidic, reacting very slowly with solvated electrons in liquid ammonia.

Note also that electronegativity is a synthetic parameter. Relative element electronegativities are not the decisive and only factor, but just a rough indicator of possible acidity. Compare e.g. acidity of hypochlorous acid $$\ce{H-O-Cl}$$ and perchloric acid $$\ce{H-O-ClO3}$$. It is clear that the effective shift of electron density (leading to bond polarization of acids) and charge delocalization of anionic conjugate bases have much bigger effect than the general element electronegativity.

Element Pauling electronegativity
$$\ce{H}$$ 2.20
$$\ce{P}$$ 2.19
$$\ce{C}$$ 2.55
$$\ce{N}$$ 3.04
$$\ce{O}$$ 3.44

As Poutnik explains, phosphorus is not more electronegative than hydrogen, but "electronegativity" is not the real criterion for rendering an attached hydrogen atom acidic.

Electronegativity is essentially a combination of electron affinity with ionization energy, whereas making an attached hydrogen acidic is instead a combination of electron affinity minus bond strength between the element and hydrogen (if the bond with hydrogen is weak, the hydrogen may be dissociated as a proton even if the attached atom has low electron affinity, as is the case with iodine).

The net result is that the acidity of an attached hydrogen atom correlates with the group the atom is in: Group 16 and 17 elements, whose electron configurations are just short of a noble gas, have relatively high electron affinities compared with their bond strengths to hydrogen, and it is these elements that then tend to acidity hydrogen atoms in water solvent.

So hydrogen attached to sulfur, let us say, is likely to be acidic in water solution, whereas hydrogen attached to nitrogen is not given the different group/electron configuration associated with nitrogen.