The process of `AgCN+KCNtoK[Ag(CN)_(2)]` involves the oxidation of Ag.

Explanation

To determine whether the statement "The process of AgCN + KCN to K[Ag(CN)₂] involves the oxidation of Ag" is true or false, we need to analyze the oxidation states of silver (Ag) in both the reactants and products.

### Step-by-step Solution:

1. **Identify the Reactants and Products**:
- Reactants: AgCN and KCN
- Product: K[Ag(CN)₂]

2. **Determine the Oxidation State of Ag in AgCN**:
- In AgCN, the cyanide ion (CN⁻) has a charge of -1.
- Let the oxidation state of Ag be \( x \).
- The overall charge of AgCN is neutral (0), so we can set up the equation:
\[ x + (-1) = 0 \]
- Solving for \( x \):
\[ x = +1 \]
- Therefore, the oxidation state of Ag in AgCN is +1.

3. **Determine the Oxidation State of Ag in K[Ag(CN)₂]**:
- In K[Ag(CN)₂], the cyanide ion (CN⁻) still has a charge of -1.
- There are two cyanide ions, contributing a total charge of -2.
- Let the oxidation state of Ag in K[Ag(CN)₂] also be \( y \).
- The overall charge of the complex ion K[Ag(CN)₂] is neutral (0), so we can set up the equation:
\[ y + 2(-1) = 0 \]
- Solving for \( y \):
\[ y - 2 = 0 \implies y = +1 \]
- Therefore, the oxidation state of Ag in K[Ag(CN)₂] is also +1.

4. **Compare the Oxidation States**:
- In both AgCN and K[Ag(CN)₂], the oxidation state of Ag remains +1.
- Since there is no change in the oxidation state of Ag, we conclude that Ag is not oxidized in this reaction.

5. **Conclusion**:
- The statement that the process involves the oxidation of Ag is false because the oxidation state of Ag does not change during the reaction.

### Final Answer:
The statement is **false**.