Question

Which among d block elements have the lowest boiling point and highest boiling point?

Answer 1

Hint : We know that the Periodic table is a great source of information about the elements and their relation to each other. Changes of different periodic properties. Also, this helps to predict the properties of the elements even if they are not discovered. Inert gases are from group $18.$ Which is on the extreme right side of the periodic table.

Complete Step By Step Answer:
To answer this question the periodic properties of the elements from the different groups should be known. The periodic properties have opposite trends between left to right and top to bottom. The elements in periodic tables are arranged in a way that every element of each group shows similar physical characteristics and chemical characteristics. In the periodic table, all the elements are arranged by atomic numbers. Generally, on the left side of the periodic table, elements are metallic in nature. Moving from left to right the metallic character decreases and the non-metallic character increases. At the extreme right elements are non-metallic in nature.
d-block elements with more number of unpaired ${{e}^{-~}}$ have high boiling points as more is the number of unpaired ${{e}^{-}},$ stronger is the metallic bonding which results in high enthalpy of atomization. Thus more amount of heat is required to weaken these metallic bonds. Hence having a high boiling point. So, Chromium with electronic configuration $4{{s}^{1}}3{{d}^{5}}$ having five unpaired ${{e}^{-}}s~$ will have the highest boiling point due to the formation of stronger metallic bonds. On the other hand, $Zn$ and $Hg$ have the lowest boiling point due to the absence of unpaired $d-{{e}^{-}}s.$

Note :
Remember that In the case of inert gases, the force of attraction is weak Van Der Waals interaction, which depends on the size of the element. With the increasing size of the element Vander Waal interaction increases, as well as the boiling point.