The ground state electronic configurations of some elements, P, Q, R, S and T (these symbols represent the some of the known elements given in the periodic table) are as follows.
(P) : $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{2}$
(Q) : $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{1}$
(R) : $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{1}$
(S) : $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{6} 4 s^{1}$
(T) : $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{1} 4 s^{2} 4 p^{6}$
Match the electronic configurations of the elements with the properties given below and select the
correct sequence by choosing the correct code given.
(i) Element forms a cation which is isoelectronic with $P^{3 -}$ .
(ii) Element which in its compounds can show a maximum oxidation state of +6 and that is coloured too.
(iii) Element has largest atomic radius and highest first ionisation energy in the respective period.
(iv) Element which has intermediate value of electronegativity and its oxide forms salts with strong acids and bases

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