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The d-And-f-Block Elements
Explain the following giving an appropriate reason in each case.
O2 and F2 both stabilise higher oxidation states of metals but O2 exceeds F2 in doing so.
O2 and F2 both stabilise high oxidation states with metal but the tendency is greater in oxygen than fluorine. It is because O2 bears -2 charges for each oxygen atom while F2 bears only -1 for each atom thus the force of attraction between the metal atom and O2-ion is greater than the force between the same metal atom and F- ion. Thus, oxygen has the ability to form multiple bonds with transition element whereas fluorine does not have the ability to form multiple bonds with transition elements. Hence, O2 gets the higher state of metals.
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The outer electronic configuration of copper is 3d10 4s1, yet it is considered transition element. Why?
Name the first element of 3rd transition series.
Though copper, silver and gold have completely filled sets of d-orbitals yet they are considered as transition metals. Why?
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