What is the increasing order of hydration ent | vedclass

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Question

(A) The hydration enthalpy of ions depends on their ionic size. Smaller ions have higher charge density and thus higher hydration enthalpy. The ionic

Vedclass · Accepted Answer

$Cs^{+} < Rb^{+} < K^{+} < Na^{+} < Li^{+}$

Vedclass · Answer

(A) The hydration enthalpy of ions depends on their ionic size. Smaller ions have higher charge density and thus higher hydration enthalpy. The ionic size of alkali metal ions increases down the group as $Li^{+} < Na^{+} < K^{+} < Rb^{+} < Cs^{+}$. Therefore, the hydration enthalpy decreases as the size increases. The correct increasing order of hydration enthalpies is $Cs^{+} < Rb^{+} < K^{+} < Na^{+} < Li^{+}$.

List-$I$	List-$II$
$A$. Slaked lime	$I$. $NaOH$
$B$. Dead burnt plaster	$II$. $Ca(OH)_2$
$C$. Caustic soda	$III$. $Na_2CO_3 \cdot 10H_2O$
$D$. Washing soda	$IV$. $CaSO_4$

What is the increasing order of hydration enthalpies of alkali metal ions?

Similar Questions

Match List-$I$ with List-$II$:

List-$I$ List-$II$

$A$. Slaked lime $I$. $NaOH$

$B$. Dead burnt plaster $II$. $Ca(OH)_2$

$C$. Caustic soda $III$. $Na_2CO_3 \cdot 10H_2O$

$D$. Washing soda $IV$. $CaSO_4$

Choose the correct answer from the options given below:

Which of the following is the correct order of increasing solubility for the given compounds?

Hydrogen,by donating one electron,forms $H^+$. In this property,it resembles

Among alkali metals,which element do you expect to be least electronegative and why?

Why are lithium salts commonly hydrated and those of the other alkali metal ions usually anhydrous?

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