Consider the following statements `:`
Statement `:1 HBr` is a stronger acid than `HI` because of hydrogen bonding.
Statement `:2 F^(-)` ion has higher hydration energy than `Cl^(-)`
Statement `:3 O_(2)` is more powerful oxidising agent than `F_(2)` becuase it contains three `'O'`.
Statement `:4 ` fluorine does not form polyhalides.
and arrange in the order of true `//` false.

Options

A. `T T T F`
B. `F T F T `
C. `T F T F`
D. `F F T T `

Explanation

To analyze the given statements and arrange them in order of true and false, we will evaluate each statement one by one.

### Step 1: Evaluate Statement 1
**Statement 1:** HBr is a stronger acid than HI because of hydrogen bonding.

- **Analysis:**
- HBr and HI are both hydrogen halides. As we move down the group from HF to HI, the bond strength decreases due to the increasing size of the halogen atoms.
- HI has a longer bond length and weaker bond strength compared to HBr, which means HI can dissociate more easily in solution, making it a stronger acid.
- Therefore, the statement that HBr is stronger than HI due to hydrogen bonding is **false**.

### Step 2: Evaluate Statement 2
**Statement 2:** F⁻ ion has higher hydration energy than Cl⁻.

- **Analysis:**
- Hydration energy is influenced by the size and charge density of the ion. F⁻ is smaller than Cl⁻, which means it has higher charge density.
- The smaller size of F⁻ leads to stronger interactions with water molecules, resulting in higher hydration energy.
- Thus, this statement is **true**.

### Step 3: Evaluate Statement 3
**Statement 3:** O₂ is a more powerful oxidizing agent than F₂ because it contains three 'O'.

- **Analysis:**
- The oxidizing ability of a species is determined by its standard reduction potential (SRP). Fluorine (F₂) has a higher SRP than oxygen (O₂), which means F₂ is a stronger oxidizing agent.
- The number of oxygen atoms does not determine the oxidizing power; rather, it is the inherent properties of the molecules.
- Therefore, this statement is **false**.

### Step 4: Evaluate Statement 4
**Statement 4:** Fluorine does not form polyhalides.

- **Analysis:**
- Polyhalides are formed when halogens can utilize their empty d-orbitals to bond with other halogens. However, fluorine has no empty d-orbitals due to its small size and electron configuration.
- Therefore, fluorine cannot form polyhalides, making this statement **true**.

### Final Arrangement
Now, we can summarize the evaluations:
1. Statement 1: False
2. Statement 2: True
3. Statement 3: False
4. Statement 4: True

Thus, the order of true and false statements is: **False, True, False, True (FTFT)**.