Choose the correct statement regarding oxy acids of halogens

Options

A. F does not form oxy acid
B. `HClO_(4)` is stronger acid than `HBrO_(4)`
C. All oxy acids are monobasic
D. `HClO_(4)` is stronger oxidising agent than `HBrO_(4)`

Answer

To solve the question regarding the correct statements about the oxy acids of halogens, we will analyze each statement step by step.

### Step 1: Analyze Statement A
**Statement A:** "F does not form oxoacid."

**Explanation:**
Fluorine (F) is the most electronegative element and has a very small atomic size. Due to its high electronegativity and small size, it lacks d-orbitals, which are necessary for forming higher oxidation states. Fluorine primarily exhibits a -1 oxidation state and cannot act as a central atom in oxoacids, which require positive oxidation states. Therefore, this statement is correct.

### Step 2: Analyze Statement B
**Statement B:** "HClO4 is a stronger acid than HBrO4."

**Explanation:**
HClO4 (perchloric acid) is indeed a stronger acid than HBrO4 (perbromic acid). This is because chlorine (Cl) is more electronegative than bromine (Br), which means that Cl pulls electron density towards itself more effectively. This makes the hydrogen in HClO4 more easily removable as H+, thus making HClO4 a stronger acid compared to HBrO4. Therefore, this statement is also correct.

### Step 3: Analyze Statement C
**Statement C:** "All oxy acids are monobasics."

**Explanation:**
Oxy acids typically have one replaceable hydrogen atom, which means they can donate one proton (H+) in solution. This characteristic makes them monobasic. Therefore, this statement is correct.

### Step 4: Analyze Statement D
**Statement D:** "HClO4 is a stronger oxidizing agent than HBrO4."

**Explanation:**
This statement is incorrect. HBrO4 is actually a stronger oxidizing agent than HClO4. The reason lies in the ability of bromine to accept electrons due to its larger size and the weaker overlap between its orbitals and those of oxygen. In contrast, chlorine has a strong back-bonding effect that stabilizes its oxidation state, making it less effective as an oxidizing agent. Therefore, this statement is incorrect.

### Conclusion
From the analysis, we conclude that:
- Statement A is correct.
- Statement B is correct.
- Statement C is correct.
- Statement D is incorrect.

Thus, the correct statements regarding the oxy acids of halogens are A, B, and C.

### Final Answer
The correct statements regarding oxy acids of halogens are A, B, and C.

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