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.

In the transition series of metals, the metal which exhibits the greatest number of oxidation states occurs in the middle of the series. Explain.

How would you account for the following: (i) Cr^(2+) is reducing in nature while with the same d-orbital configuration (d^(4)) Mn^(3+) is an oxidising agent (ii) In a transition series of metals, the metal which exhibits the greatest number of oxidation state occurs in the middle of the series.

How would you account for the following? (i) Cr^(2+) is reducing in nature while with the same d-orbital configuration (d^14) Mn^(3+) is an oxidising agent. (ii) In a transition series of metals, the metal which exhibits the greatest number of oxidation states occurs in the middle of the series. (iii) Metal-metal bonding is more frequent for the 4d and the 5d series of transition metals than for the 3d series.

How would you account for the following: (i) Cr^(2+) is reducing in nature while with the same d-orbital configuration (d^4) Mn^(3+) is an oxidising agent. (ii) In a transition series of metals, the metal which exhibits the greatest number of oxidation state occurs in the middle of the series.

How would you account for the following ? In a transition series of metals, the metal which exhibits the greatest number of oxidation states occurs in the middle of the series.

Which of the 3d series of the transition metals exhibits the largest number of oxidation states and why?