When CU reacts with`AgNO_(3)` solution , the reaction takes place is f:

Options

A. Oxidation of Cu
B. Reducing of Cu
C. Oxidation Of Ag
D. Raducing of `No_(3)^(-)`

Explanation

To solve the question of what happens when copper (Cu) reacts with silver nitrate (AgNO₃) solution, we can follow these steps:

### Step 1: Identify the Reactants
The reactants in this reaction are copper (Cu) and silver nitrate (AgNO₃).

### Step 2: Determine the Type of Reaction
This is a displacement reaction. In this type of reaction, a more reactive metal displaces a less reactive metal from its compound.

### Step 3: Check the Reactivity of Metals
Copper (Cu) is more reactive than silver (Ag). Therefore, Cu will displace Ag from AgNO₃.

### Step 4: Write the Balanced Chemical Equation
The balanced chemical equation for the reaction is:
\[ 2 \text{AgNO}_3 (aq) + \text{Cu} (s) \rightarrow 2 \text{Ag} (s) + \text{Cu(NO}_3)_2 (aq) \]

### Step 5: Analyze the Oxidation States
- In AgNO₃, silver (Ag) is in the +1 oxidation state.
- In the products, silver (Ag) is in the 0 oxidation state (elemental form).
- Copper (Cu) starts in the 0 oxidation state and goes to +2 in copper(II) nitrate (Cu(NO₃)₂).

### Step 6: Identify Oxidation and Reduction
- **Oxidation**: Copper (Cu) is oxidized from 0 to +2.
- **Reduction**: Silver (Ag) is reduced from +1 to 0.

### Step 7: Conclusion
The overall reaction involves the oxidation of copper and the reduction of silver. The nitrate ion (NO₃⁻) remains unchanged during the reaction.

### Final Answer
The reaction that takes place when Cu reacts with AgNO₃ is:
\[ 2 \text{AgNO}_3 (aq) + \text{Cu} (s) \rightarrow 2 \text{Ag} (s) + \text{Cu(NO}_3)_2 (aq) \]