why the lowest oxide of transition metals is always basic and the highest oxide is always acidic?
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The d block elements of periodic table are called as Transition elements.
They have partially filled d orbitals. Transition elements have variable oxidation state.
Metals with lower oxidation state are generally low oxide metals.They have valence electrons which will not be involved in bonding. Thus, these metals can donate electrons and because of this reason they acts as Basic.
Metals with higher oxidation state are generally higher oxide metals in which all the valence electrons are involved in bonding and so they don't have free electrons and they will be deficient of electrons so they accept electrons and thus act as acidic
For example :
In Mn₂O₇, Manganese is in the +7 oxidation state, so it is acidic in nature
Where as Mno has low oxidation state, so basic in nature
They have partially filled d orbitals. Transition elements have variable oxidation state.
Metals with lower oxidation state are generally low oxide metals.They have valence electrons which will not be involved in bonding. Thus, these metals can donate electrons and because of this reason they acts as Basic.
Metals with higher oxidation state are generally higher oxide metals in which all the valence electrons are involved in bonding and so they don't have free electrons and they will be deficient of electrons so they accept electrons and thus act as acidic
For example :
In Mn₂O₇, Manganese is in the +7 oxidation state, so it is acidic in nature
Where as Mno has low oxidation state, so basic in nature
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