CUET Preparation Today
$ \text{Cu}$ exist as $ \text{Cu}^{+}$ and $ \text{Cu}^{2+}$ ion. Which of the following statements is correct? |
$ \text{Cu}^{2+}$ in aqueous solution undergoes disproportionation reaction $ \text{Cu}^{+}$ is $3d^{10}$ and $ \text{Cu}^{2+}$ is $3d^9$ but $ \text{Cu}^{2+}$ is more stable. stability of $ \text{Cu}^{+}$ and $ \text{Cu}^{2+}$ depends on nature of copper salt $ \text{Cu}^{+}$ and $ \text{Cu}^{2+}$ are equally stable |
$ \text{Cu}^{+}$ is $3d^{10}$ and $ \text{Cu}^{2+}$ is $3d^9$ but $ \text{Cu}^{2+}$ is more stable. |
The correct answer is Option (2) → $ \text{Cu}^{+}$ is $3d^{10}$ and $ \text{Cu}^{2+}$ is $3d^9$ but $ \text{Cu}^{2+}$ is more stable. $ \text{Cu}^{2+}$ is more stable than $ \text{Cu}^{+}$ in aqueous solutions, primarily due to its higher hydration energy $ \text{Cu}^{2+}$ has a greater charge density than $ \text{Cu}^{+}$ leading to stronger interactions with water molecules. This results in a more negative (greater) hydration enthalpy, making the ion more stable in aqueous solution. |
