Question
In all the oxyacids of phosphorus, each phosphorus atom is in sp3 hybrid state, i.e., it is tetrahedrally bonded to neighbouring four atoms. All these acids contain P - OH bonds, the hydrogen atom of which are ionisable imparting acidic nature to the compound. The ous acids (oxidation state of P = +1 or +3) also have P - H bonds in which hydrogens are not ionisable (P and hydrogen have nearly same electronegativity). The presence of P - H group in these acids imparts reducing properties. The structure of the various acids are drawn below (note that the tetrahedral shape of phosphorus is not shown only for convenience of representation).
There is very little difference in acid strength in the series H3PO4, H3PO3 and H3PO2 because
- phosphorus in these acids exists in different oxidation states
- the hydrogen in these acids are not all bonded to phosphorus
- phosphorus is not a highly electronegative element
- phosphorus oxides are less basic
The correct answer is: the hydrogen in these acids are not all bonded to phosphorus
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