# 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.

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Hint:We have to know that the transition metal (or) element comes under the d block element. Some of the general features of transition metal such as variable oxidation state, formation of complex ions, colored ions and catalytic activity. Zinc and scandium are not taken as transition metals though they are members of the d block.

-From the periodic table, we know that the transition metals are components present in groups 3-12. -The transition metals are also called the d-block components. These components are described by their mostly involved d subshells in the free components or in their cations. The variety in the oxidation state of transitions components is because of the incomplete filling of d orbitals so that their oxidation states fluctuate from one another by solidarity.
-We have to give an example and reason why the lowest oxide of transition metal is basic in nature and the highest oxide of transition metal is acidic/amphoteric in nature.
-On account of a lower oxide of a transition metal, the metal molecule has a low oxidation state. This implies that a portion of the valence electrons of the metal atoms are not engaged with bonding. -Accordingly, it can give electrons and act as a base.
-Then again, on account of a higher oxide of a transition metal, the metal atom has a high oxidation state. This implies that the valence electrons are associated with bonding thus, they are inaccessible. -There is additionally a high effective nuclear charge.
-Subsequently, it can gain electrons and act as an acid.
-For instance, $MnO$ is basic and $M{n_2}{O_7}$ is acidic.
-In $MnO$, the oxidation state of manganese is $+ 2$ and in $M{n_2}{O_7}$, the oxidation state of manganese is $+ 7$.
-We have to give the reason and example why transition metals show higher oxidation state in fluorides and oxides.
-Oxygen and fluorine act as solid oxidizing agents due to their high electronegativities and little sizes. -Subsequently, they draw out the highest oxidation states from the transition metals. In simple words, a transition metal shows higher oxidation states in oxides and fluorides. For instance, in $Os{F_6}$ and in ${V_2}{O_5}$, the oxidation conditions of Os and V are +6 and +5 separately.
-We have to give the reason and example why the highest oxidation state is shown in oxoanions of a metal.
-Oxygen is a solid oxidizing agent because of its high electronegativity and little size. Along these, oxo-anions of a metal contain the highest oxidation state. For instance, in $Mn{O_4}^ -$, the oxidation state of Mn is +7.

Note:
We need to remember that the coordination complex is a compound that contains a central atom (ion) that is metallic and is called the coordination centre. It is bounded by array bound molecules (or) ions known as ligands (or) complexing agents. Transition metals are coordination complexes. A coordination complex whose centre comprises an atom of metal is known as a metal complex of d block element.