"Lithium ion has the smallest hydration enthalpy of all the alkali metals."
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Enthalpy
of hydration is the heat energy released when new bonds are made between the
ions and water molecules. The hydration enthalpy is the enthalpy change when 1
mole of gaseous ions dissolve in sufficient water to give an infinitely dilute
solution. Hydration enthalpies are always negative.
Mz+(g)+mH2O→Mz+(aq)
Where
Mz+ (aq) represents ions surrounded by water molecules and dispersed in
the solution. As the atomic numbers increases, so do the ionic size, leading to
a decrease in absolute values of enthalpy of hydration.
Smaller
the cation, greater is the degree of hydration. Alkali metals easily lose 1
electron and therefore have high values of "oxidising potential" which
means high tendency to get oxidised and hence, powerful reducing nature in aqueous
medium. Since Li+ is small in size among all alkali metals, it has high
charge density and hence, the highest hydration energy of all the alkali
metals.
Enthalpy of hydration is the heat energy released when new bonds are made between the ions and water molecules. The hydration enthalpy is the enthalpy change when 1 mole of gaseous ions dissolve in sufficient water to give an infinitely dilute solution. Hydration enthalpies are always negative.
Mz+(g)+mH2O→Mz+(aq)
Where Mz+ (aq) represents ions surrounded by water molecules and dispersed in the solution. As the atomic numbers increases, so do the ionic size, leading to a decrease in absolute values of enthalpy of hydration.
Smaller the cation, greater is the degree of hydration. Alkali metals easily lose 1 electron and therefore have high values of "oxidising potential" which means high tendency to get oxidised and hence, powerful reducing nature in aqueous medium. Since Li+ is small in size among all alkali metals, it has high charge density and hence, the highest hydration energy of all the alkali metals.
