Question

Compare the stability of +2 oxidation state for the elements of the first transition series.

Answer 1

Sc			+3
Ti		+2	+3	+4
V		+2	+3	+4	+5
Cr		+2	+3	+4	+5	+6
Mn		+2	+3	+4	+5	+6	+7
Fe		+2	+3	+4		+6
Co		+2	+3	+4
Ni		+2	+3	+4
Cu	+1	+2
Zn		+2

From the table above, it is evident that Mn exhibits oxidation states ranging from +2 to +7. The number of oxidation states increases as one moves from Sc to Mn. On moving from Mn to Zn, the number of oxidation states decreases due to a decrease in the number of available unpaired electrons.

The relative stability of the +2 oxidation state increases as one moves from left to right across the period. This is because, on moving from left to right, the increasing nuclear charge increases the sum of the first and second ionization enthalpies, making it progressively more difficult to remove the third electron from the d-orbital.

Answer 2

Firstly, in the first half of the transition series, the sum of the first- and second-ionisation enthalpies increases with atomic number. Hence, the standard reducing potential (E°) is low and negative. Hence, the tendency to form M²⁺ ions decreases. Hence, the +2 oxidation state is more stable in the first half. The greater stability of the +2 oxidation state is due to half-filled d-subshells (d⁵) in Mn²⁺, fully filled d-subshells (d¹⁰) in Zn^2+, and high negative hydration enthalpy in nickel.