The Correct Order of Hydration Enthalpies of Alkali Metal Ions is

Hydration or solvation is the addition of water molecules to an ion, atom, or molecule. The amount of heat energy generated by one mole of ions to create hydrated species is known as the hydration enthalpy. Energy is released when a relationship is created. Therefore, energy is released when ions contact water molecules to create bonds. Hydration enthalpy is the name given to this energy.

Answer - The Correct Order of Hydration Enthalpies of Alkali Metal Ions is Li+ Na+ K+ Rb+ Cs+.

The solvation effect causes table salt to dissolve in water. NaCl separates into sodium ion, Na+, and chloride ion, Cl, when it is introduced to water. The subsequent solvation of these ions by water molecules causes the salt to dissolve in the water. Heat energy also known as hydration energy is released when the ion becomes solvated. We are asked to rank the hydration enthalpies of alkali metal ions in the inquiry. We are aware that in the periodic table, caesium has the largest atomic size and is also the most electropositive element.

Charge-to-size ratio affects the enthalpy of hydration. The charge to size ratio will continue to decline if atomic size grows while charge stays constant. As a result, lithium ions will have the highest charge-to-size ratio and caesium ions the lowest. Charge-to-size ratio and hydration enthalpy are directly proportional. Thus, the hydration enthalpy will be in the following order: Li+ Na+ K+ Rb+ Cs+.

Summary:

The Correct Order of Hydration Enthalpies of Alkali Metal Ions is

The Correct Order of Hydration Enthalpies of Alkali Metal Ions is Li+ Na+ K+ Rb+ Cs+. Charge-to-size ratio and hydration enthalpy are directly proportional.

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