The stability of $Cu^{2+}$ is more than $Cu^+$ salts in aqueous solution due to

Question

$\textbf{Reduction potential of ions are given below:}$
\[ \begin{array}{ccc} \text{ClO}_4^- & \text{IO}_4^- & \text{BrO}_4^- \\ E^\circ = 1.19 \, \text{V} & E^\circ = 1.65 \, \text{V} & E^\circ = 1.74 \, \text{V} \\ \end{array} \]
The correct order of their oxidising power is:

Answer 1

To determine the stability of ions in aqueous solutions, one important factor to consider is the hydration energy. The given question asks why $Cu^{2+}$ is more stable than $Cu^+$ in aqueous solution, presenting several options.

Enthalpy of atomization: This describes the energy change when atoms are converted into gaseous atoms and is not directly related to the stability of ions in solutions.
Hydration energy: This refers to the energy released when ions are surrounded by water molecules. For $Cu^{2+}$, the hydration energy is significantly higher because it has a higher charge density compared to $Cu^+$. The strong attraction between the $Cu^{2+}$ ions and water molecules results in the release of more energy, thus stabilizing the ion in aqueous solution.
Second ionization enthalpy: This involves the energy needed to remove an additional electron from an ion. While this does affect ion formation, it is not directly relevant to stability in solution.
First ionization enthalpy: This involves the energy to remove an electron from an atom or ion, relevant to the formation of $Cu^+$ from neutral copper, but doesn't directly affect the observed stability difference in solution.

Considering all options, the correct explanation for the greater stability of $Cu^{2+}$ over $Cu^+$ in aqueous solution is due to the higher hydration energy of $Cu^{2+}$.

Therefore, the correct answer is: Hydration energy.

Answer 2

To determine the stability of ions in aqueous solutions, one important factor to consider is the hydration energy. The given question asks why $Cu^{2+}$ is more stable than $Cu^+$ in aqueous solution, presenting several options.

Enthalpy of atomization: This describes the energy change when atoms are converted into gaseous atoms and is not directly related to the stability of ions in solutions.
Hydration energy: This refers to the energy released when ions are surrounded by water molecules. For $Cu^{2+}$, the hydration energy is significantly higher because it has a higher charge density compared to $Cu^+$. The strong attraction between the $Cu^{2+}$ ions and water molecules results in the release of more energy, thus stabilizing the ion in aqueous solution.
Second ionization enthalpy: This involves the energy needed to remove an additional electron from an ion. While this does affect ion formation, it is not directly relevant to stability in solution.
First ionization enthalpy: This involves the energy to remove an electron from an atom or ion, relevant to the formation of $Cu^+$ from neutral copper, but doesn't directly affect the observed stability difference in solution.

Considering all options, the correct explanation for the greater stability of $Cu^{2+}$ over $Cu^+$ in aqueous solution is due to the higher hydration energy of $Cu^{2+}$.

Therefore, the correct answer is: Hydration energy.

The stability of \(Cu^{2+}\) is more than \(Cu^+\) salts in aqueous solution due to

The Correct Option is B

Solution and Explanation

Top Questions on p -Block Elements

Questions Asked in NEET (UG) exam