Why are oxides with lower oxidation number of metals are basic while those with higher oxidation numbers are acidic in case of d-block elements?
1oxidation state increases frm left 2 rite across a period in the d-block as the metallic charectr reduces frm left 2 ite along the period. More basic means more metallic! I am not sure! :) i jus tried :)
Basic generally metals
Acidic generally non metals
1Lesser oxidation number in the d-block elements means greater tendency to donate electrons, which is a characteristic of a base....
Thus less oxidation number means more basic behavior......
Similar expalantion for the ones with higher oxdn numbers..
1that may be...abhisek..
@subham oxidation number increases till almost meiddle of the deries and then decreases...
11One reason that I can think is that the elements with lower oxidation no. can give away their
electrons completely,i.e, donate so they form basic oxides ( the reason may be for this is, the
nuclear charge on them is lesser as compared to the right hand side members of the d-block
after Mn) Where as in the case of the right hand side members, nuclear force is more so they
share electrons and form covlent compounds which are more acidic in comparison.
11I only explained on the basis of the increase in nuclear charge as we move from left to right of the periodic table.
Now the outer orbital electrons can be easily donated since the nuclear charge on them is l
ess than for the the inner ones, like as we remove the outer electrons the no. of electrons
decreases and no. of protons increases, as a result the nuclear charge too increases, hence
the inner electrons are can't be donated so they form bonds by sharing, and hence form
more acidic oxides than their low oxidation states.
This is what the conclusion I got after reading the transition elements from a book