Ambiguous oxidation state of phosphorus in phosphorous acid

I was doing a question in which we were required to find the oxidation state of $\ce{H3PO3}$. I knew the structure that is:


![Phosphorous  acid](https://i.stack.imgur.com/0KgdN.png)


Now, phosphorus being less electronegative than oxygen gets $+2,+1,+1$ charge from respective oxygens. Now we see that in case of hydrogen, it is taught that **phosphorus being more electronegative than hydrogen** thus it gets $-1$ charge from it, and finally adding all the charges we get Oxidation state of Phosphorus $=+3$.


Now my doubt is that I found on the internet that **hydrogen is more electronegative than phosphorus** that is, electronegativity of hydrogen$=2.2$ whereas electronegativity of phosphorus$= 2.19$.


Therefore, phosphorus must get $+1$ from hydrogen thus oxidation state of phosphorus $=+5$ but I know this is wrong and the probable reason I could figure out is that hydrogen is more stable in $+1$ form. Therefore, oxidation state of phosphorus is $-1$.


Please tell me if this reason is correct or please add to it.


