Hydration Energy :
When a gaseous cation or gaseous anion interacts with water, hydrated cation or hydrated anion is produced and in this process (called hydration process), the energy released is called as hydration energy.
`M_g^(+) + (H_2O)_(l) -> undersettext(Hydrated cation)(M_(aq)^(+)) + text(Hydration energy)`
`X_g^(-) + (H_2O)_(l) -> undersettext(Hydrated cation)(X_g^(-)) + text(Hydration energy)`
Hydration energy is the enthalpy change that accompanies when one mole of the gaseous ion is dissolved in water.
For example, reaction of the hydration of `Li` ion is shown as :
`Li^(+) (g) + nH_2O -> Li(H_2O)_n(aq); Delta H = - 806 kJ text(mol)^(-1)`.
The process by which polar water molecules clings (sticks) to `Na^+` and `Cl^-` is called hydration. Ions are converted to hydrated form.
`text(Hydration energies (heat of hydration)` `text(of some ions)` : `(kJ//mol)`. See Table.
`M_g^(+) + (H_2O)_(l) -> undersettext(Hydrated cation)(M_(aq)^(+)) + text(Hydration energy)`
`X_g^(-) + (H_2O)_(l) -> undersettext(Hydrated cation)(X_g^(-)) + text(Hydration energy)`
Hydration energy is the enthalpy change that accompanies when one mole of the gaseous ion is dissolved in water.
For example, reaction of the hydration of `Li` ion is shown as :
`Li^(+) (g) + nH_2O -> Li(H_2O)_n(aq); Delta H = - 806 kJ text(mol)^(-1)`.
The process by which polar water molecules clings (sticks) to `Na^+` and `Cl^-` is called hydration. Ions are converted to hydrated form.
`text(Hydration energies (heat of hydration)` `text(of some ions)` : `(kJ//mol)`. See Table.