Question

INORGANIC CHEMISTRY

All of the following molecules are isoelectric: PO4 3-, SO4 2-, AND CLO4 -. (a) Compare the stregths of these ions as bronsted bases and explain the trends you observe. (b) Compare the stregths of these ions as oxidizing agents under basic and acidic conditions and explain the trends you observe. how are your results in parts (a) and (b) related?

Answer 1

Stronger the acid, weaker is its conjugate base and vice-versa.

a) Thus, in increasing order of basicity:- ClO₄^- < SO₄^2- < PO₄^3-

b) An oxidizing agent is one which itself undergoes reduction.

As in ClO₄^-, Cl is at its highest oxidation state i.e + 7 , it is the strongest oxidizing agent.

Similarly, in PO₄^3- , P is at its highest oxidation state i.e. +5 & in SO₄^2- , S is ints highest Oxidation state i.e +6 and are also a strong oxidizing agent. But SO₄^2- is more stable than PO₄^3-

Hence in decreasing order of oxidizing power:-

ClO₄^- > PO₄^3- > SO₄^2-