Which of following statement is wrong

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Highest oxidation state of an element is more stable for the 5d series element than the other two elements above to it in that group.

In any group of d-Block elements third element (5d series) have more 1st ionization energy which is less than the other two elements above to it.

Irregularities in $E_{M / M^{2 +}}^{0}$ of 3d series elements is due to irregularities in sublimation energies and ionization energies

Melting points of 5d series elements are more than the corresponding 3d and 4d elements in their groups.

answer is A.

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Detailed Solution

A) From first element to second element in a group of d-block. IP decreases due to increase in size but 3rd element have more IP due to decrease in size L (lanthanoid contraction) and increase in effective nuclear charge.
B) $Δ G^{0} = Δ H^{0} - T Δ S^{0}, Δ G^{0} = - n F E^{0} = \frac{Δ H^{0} - T Δ S^{0},}{n F}$ $H^{0}$
depends on heat of sublimation, ionization energies and hydration energies of transition metals. Since these are irregular due to different number of electrons participating in bonds irregularities in IP values as explained in the E0 values are also irregular.
$\begin{array}{l} Δ G^{0} {=nFE}^{0} \\ = E^{0} = \frac{Δ H^{0} - T Δ S^{0}}{n F} \end{array}$
C) Second electron has to be removed from (n-1) orbital which requires more energy. Also the number of exchange pairs (increased as in option B) decreases which requires more energies. Because of these reasons the 2nd IP of V is more than Ti.
D) Unlike the p-block elements the stability of higher oxidation state increases down the group.