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(D) The enthalpy of atomisation is the enthalpy change that accompanies the total separation of all atoms in a chemical substance.The extent of metall

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$Cr, Zn$

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(D) The enthalpy of atomisation is the enthalpy change that accompanies the total separation of all atoms in a chemical substance.The extent of metallic bonding an element undergoes decides the enthalpy of atomisation. The more extensive the metallic bonding of an element, the higher will be its enthalpy of atomisation.$Cr$ $(3d^5 4s^1)$ has the highest enthalpy of atomisation for the first row of transition elements due to the maximum number of unpaired electrons available for metallic bonding.$Zn$ $(3d^{10} 4s^2)$ has a completely filled $d$-orbital and has no unpaired electrons to participate in the formation of metallic bonds. Therefore, the metallic bonding in zinc is the weakest, resulting in the lowest enthalpy of atomisation.

Column $A$	Column $B$
$(1)$ $V^{4+}$	$(a)$ Colorless
$(2)$ $Ti^{3+}$	$(b)$ Pink
$(3)$ $Ti^{4+}$	$(c)$ Purple
$(4)$ $Mn^{2+}$	$(d)$ Blue
	$(e)$ Violet

The elements with the highest and the lowest enthalpy of atomisation respectively, for first row transition elements are:

Similar Questions

Which element from the following does $NOT$ exhibit a spin-only magnetic moment in the $+3$ oxidation state?

$Zn$ and $Cd$ metals do not show variable valency because

Match Column $A$ with Column $B$:

Column $A$ Column $B$

$(1)$ $V^{4+}$ $(a)$ Colorless

$(2)$ $Ti^{3+}$ $(b)$ Pink

$(3)$ $Ti^{4+}$ $(c)$ Purple

$(4)$ $Mn^{2+}$ $(d)$ Blue

$(e)$ Violet

What are the $d-$block elements in the modern periodic table known as?

The magnetic moment of a metal ion of the first transition series is $2.83 \ BM$. Therefore,it will have how many unpaired electrons?

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