Why Li have maximum hydration enthalpy than other elements of its group?

The heat energy released when new bonds are made between the ions and water molecules is known as the hydration enthalpy of the ion. Because Li+ is much smaller than the other alkali metal cations, it’s hydration energy is the highest.

Why does enthalpy of hydration increase down Group 1?

The size of the hydration enthalpy is governed by the amount of attraction between the ions and the water molecules. The attractions are stronger the smaller the ion. For example, hydration enthalpies fall as you go down a group in the Periodic Table. The attractions are stronger the more highly charged the ion.

Which cation has the highest hydration energy?

Hydration energy is directly proportional to charge present on ion, and it is inversely proportional to size of ion. Among given ions Al3+ A l 3 + have more charge and least size. So, Al3+ A l 3 + has highest hydration energy.

Why lithium is the strongest reducing agent whereas its ionization enthalpy is highest?

Lithium ion is small in size and has high ionization enthalpy. Thus, Li has a greater tendency to lose electrons in solution than other alkali metals. The Large amount of hydration energy makes it the strongest reducing agent in spite of its highest ionisation enthalpy.

Why does hydration enthalpy of alkali metals decrease with increase in ionic size?

Hydration enthalpy decreases down the group because down the group size of the atom increases because of addition of extra valence shells.

Why does lithium have high hydration enthalpy?

The degree of hydration is dependent on the size of the ion. The smaller the size of the cation formed, the greater the degree of hydration. Since lithium is the smallest (in size) among all the alkali metals, it is known to have the highest hydration energy among all alkali metals. …

Why does enthalpy change of hydration decrease down the group?

Smaller the ion, the higher the hydration enthalpy will be because smaller atoms can accommodate a large number of water molecules around it and get hydrated. Hydration enthalpy decreases down the group the size of the atom increases due to the addition of extra valence shells.

Why does hydration energy decrease down a group?

Why lithium is the strongest reducing agent among alkali metals in aqueous state?

Alkali metals are good reducing agents as they readily lose their electrons due to low ionization enthalpy. Moreover, due to its small size $Li$ has very high hydration enthalpy. So, $Li$ has a high tendency to lose electrons in solution. Hence, $Li$ is the strongest reducing agent.

Why do alkali metals have low hydration enthalpy?

Since size of atoms increases down the group in alkali metals and charge remains the same Hydration enthalpy decreases down the group which means Lithium have highest hydration enthalpy and Caesium have lowest hydration enthalpy among alkali metals.