STATEMENT-1: In the reaction : `Cl_(2)+ OH^(-) to Cl^(-) + ClO_(4)^(-)` chlorine is oxidised only
STATEMENT-2: Oxidation and reduction cannot take place alone.

Answer

To analyze the statements provided in the question, we will break down the reaction and evaluate the oxidation states of chlorine in each species involved.

### Step-by-Step Solution:

1. **Identify the Reaction**:
The reaction given is:
\[ \text{Cl}_2 + \text{OH}^- \rightarrow \text{Cl}^- + \text{ClO}_4^- \]

2. **Determine Oxidation States**:
- In \(\text{Cl}_2\), the oxidation state of chlorine (Cl) is 0 (elemental form).
- In \(\text{Cl}^-\), the oxidation state of Cl is -1.
- In \(\text{ClO}_4^-\), we need to calculate the oxidation state of Cl. The overall charge is -1, and oxygen has an oxidation state of -2. Since there are four oxygens:
\[ \text{Let the oxidation state of Cl be } x. \]
\[ x + 4(-2) = -1 \implies x - 8 = -1 \implies x = +7. \]
Thus, the oxidation states are:
- Cl in \(\text{Cl}_2\): 0
- Cl in \(\text{Cl}^-\): -1
- Cl in \(\text{ClO}_4^-\): +7

3. **Identify Oxidation and Reduction**:
- **Oxidation** is defined as an increase in oxidation state. Here, Cl changes from 0 in \(\text{Cl}_2\) to +7 in \(\text{ClO}_4^-\), indicating oxidation.
- **Reduction** is defined as a decrease in oxidation state. Here, Cl changes from 0 in \(\text{Cl}_2\) to -1 in \(\text{Cl}^-\), indicating reduction.

4. **Evaluate Statement 1**:
- The statement claims that "chlorine is oxidized only." However, since chlorine is both oxidized (to +7) and reduced (to -1) in this reaction, **Statement 1 is incorrect**.

5. **Evaluate Statement 2**:
- The statement claims that "oxidation and reduction cannot take place alone." This is not true, as there are reactions where only oxidation or only reduction occurs. For example:
- Oxidation: \( \text{Na} \rightarrow \text{Na}^+ + e^- \) (only oxidation).
- Reduction: \( \text{Cl}_2 + 2e^- \rightarrow 2\text{Cl}^- \) (only reduction).
Therefore, **Statement 2 is also incorrect**.

### Conclusion:
Both statements are incorrect.