Question

Give examples and suggest reasons for the following features of the transition metal
chemistry:
(i)The lowest oxide of transition metal is basic, the highest is amphoteric/acidic.
(ii) A transition metal exhibits highest oxidation state in oxides and fluorides.
(iii) The highest oxidation state is exhibited in oxoanions of a metal.

Answer 1

In the case of a lower oxide of a transition metal, the metal atom has a low oxidation
state. This means that some of the valence electrons of the metal atom are not involved in bonding. As a result, it can donate electrons and behave as a base. On the other hand, in the case of a higher oxide of a transition metal, the metal atom has a high oxidation state. This means that the valence electrons are involved in bonding and so, they are unavailable. There is also a high effective nuclear charge. As a result, it can accept electrons and behave as an acid.

(ii) Oxygen and fluorine act as strong oxidising agents because of their high
electronegativities and small sizes. Hence, they bring out the highest oxidation states
from the transition metals. In other words, a transition metal exhibits higher oxidation
states in oxides and fluorides. For example, in OsF6 and V₂O_5, the oxidation states of
Os and V are +6 and +5 respectively.
(iii) Oxygen is a strong oxidising agent due to its high electronegativity and small size. So, oxo-anions of a metal have the highest oxidation state. For example, in ,           the oxidation state of Mn is +7.