Which of the following 3d-metal ion will give | vedclass

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(B) The enthalpy of hydration $(\Delta_{hyd}H)$ is directly proportional to the charge density of the ion.Charge density is defined as $\frac{	ext{ch

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$Mn^{2+}$

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(B) The enthalpy of hydration $(\Delta_{hyd}H)$ is directly proportional to the charge density of the ion.Charge density is defined as $\frac{	ext{charge}}{	ext{size}}$.For the given $3d$-metal ions $(Cr^{2+}, Mn^{2+}, Fe^{2+}, Co^{2+})$,the charge is the same $(+2)$.Therefore,the ion with the largest ionic radius will have the lowest charge density and consequently the lowest enthalpy of hydration.According to periodic trends,the ionic radius decreases across the $3d$ series due to increasing effective nuclear charge.Among the given ions,$Mn^{2+}$ has the largest ionic radius.Thus,$Mn^{2+}$ has the lowest enthalpy of hydration.

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

Which of the following $3d$-metal ion will give the lowest enthalpy of hydration $(\Delta_{hyd}H)$ when dissolved in water?

Similar Questions

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

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