State the reason for the following :
(i) Cu (I) ion is not stable in an aqueous solution.
(ii) Unlike `Cr^(3+),Mn^(2+),Fe^(3+)` and the subsequent other `M^(2+)` ions of the 3d series, the 4d and 5d series metals generally do not form stable oxidation states.

Complete the following chemical equation: (i) MnO_(4)^(-)(aq)+s_(2)O_(3)^(2-)(aq)+H_(2)O(I) to (ii) MnO_(4)^(-) +NO_(2)^(-)+H^(+) to State reason for the following : (i) Cu(I) ion is not stable in an aqueous solution. (ii) Unlike Cr^(3+),Mn^(2+),Fe^(3+) and the subsequently other M^(2+) ions of the 3d series of elements, the 4d and the 5d series metals generally do not form stable cationic species.

Assertion : Cu^+ ion is not stable in aqueous solution. Reason : Cu^+ contains 3d-filled subshell.

In 3d series , Mn shows highest oxidation state . Why ?

Among the following pairs of ions the lower oxidation state in aqueous solution is more stable than the other in

In 3d series highest oxidation state is shown by

How would you account for the following : (i) Cr^(2+) is reducing in nature while with the same d-orbital configuration (d^(4)),Mn^(2+) is oxidising in nature. (ii) In the transition series of metals, the metal which exhibits the greatest number of oxidation states occurs in the middle of the series.