Consider the following statement :

${\mathrm{S}}_1$ - d-block metal have high melting points because of participation of $\left(\mathrm{n}-1\right)d e^{-}$ in interatmoic metallic bonding $\left(\mathrm{n}\to \mathrm{outermost} \mathrm{shell}\right)$.

${\mathrm{S}}_2 -$ metal-metal bonding in compounds of transition elements increases from top to bottom in a group.

The correct option is-

The high melting and boiling points of the d-block metals is attributed to the involvement of a greater number of electrons from the $\left(\mathrm{n}-1\right)d e^{-}$ in addition to the ns-electrons in the interatomic metallic bonding. In any row the melting points of these metals rise to a maximum at $d^5$ except for anomalous values of Mn and Tc and fall regularly as the atomic number increases.

The metallic depends upon the ease of a metal of loosing electrons. When we move from left to right across the periodic table, there is an increase in the number of protons and electrons which further leads to an increase in nuclear forces on the electrons which makes it difficult for them to lose electrons, therefore the metallic character while moving left to right decreases. As the atomic radius is increased there is an increase in the metallic character as well. Therefore, while moving top to bottom, the metallic character of the elements is increased. 

Both the given statement are correct.

Therefore, the correct option is (C).