The Question is from neet-chemistry classification-of-elements halogens-group-17, and it was created by the author A.RAMA NAGESWARARAO

Question

Which of the following statements regarding the oxidizing power of interhalogen compounds is INCORRECT?

A.RAMA NAGESWARARAO · Accepted Answer

## CORE INFORMATION
✓ **Answer**: A
## CONCEPT FRAMEWORK
	**Primary Concept**: Oxidizing power of interhalogen compounds
	**Related Topics**: Halogen chemistry, Redox reactions, Electronegativity
	**Prerequisites**: Understanding of oxidation states, electronegativity, and periodic trends.
## SOLUTION PATHWAY
**Given Information**:
	Multiple-choice question about the oxidizing power of interhalogen compounds.
**Method & Steps**:
	1. **Analyze the oxidizing power of interhalogen compounds**: Interhalogen compounds are generally stronger oxidizing agents than halogens (except F2). This is due to the polar nature of the X-Y bond in interhalogens, making them more reactive.
	Reasoning: The X-Y bond is weaker than the X-X or Y-Y bonds in diatomic halogens, making interhalogens more reactive and thus stronger oxidizing agents.
	2. **Compare the oxidizing power within interhalogens**:  Oxidizing power generally decreases with increasing electronegativity difference between the two halogens.
	Working: For a given central halogen, oxidizing power decreases as the size of the other halogen increases. For example, ClF > ClF3 > ClF5.
	Key Point: The more positive oxidation state of the central halogen, the higher the oxidizing power (generally). 
	3. **Consider the given options**: Evaluate each statement based on the established principles.
	Result: Option A is incorrect as it states interhalogens are weaker oxidizing agents than halogens, which contradicts the established principle.
	Verification: The other options align with the principles of interhalogen oxidizing power.
## OPTION ANALYSIS
[A] :x: **Incorrect**: Interhalogen compounds are generally *stronger* oxidizing agents than halogens (except $F_2$).  The X-Y bond in interhalogens is weaker than the X-X bond in diatomic halogens, making them more reactive.
[B] ✓: **Correct**: ClF is a better oxidizing agent than BrF. Chlorine is more electronegative than bromine, leading to a more polar and reactive bond in ClF.
[C] ✓: **Correct**: The oxidizing power of ClF, ClF3, and ClF5 decreases in the order ClF > ClF3 > ClF5. This is because the oxidation state of chlorine decreases from +1 to +5, and generally, a lower positive oxidation state leads to a weaker oxidizing agent (within the same central halogen).
[D] ✓: **Correct**: BrCl is a stronger oxidizing agent than IBr. Chlorine is more electronegative than iodine, resulting in a more polar and reactive Br-Cl bond.
## LEARNING AIDS
	**Common Mistakes**:
		1. Confusing the trend of oxidizing power within interhalogens with the trend between interhalogens and halogens: Remember interhalogens (except those with fluorine) are generally stronger oxidizing agents than halogens.
		2. Ignoring the effect of electronegativity difference: The greater the electronegativity difference, the stronger the oxidizing power (generally).
	**Quick Tips**:
		1. Remember that $F_2$ is the strongest oxidizing agent among halogens.
		2. For a central halogen, higher positive oxidation state generally implies stronger oxidizing power (with exceptions).

A.RAMA NAGESWARARAO · Answer

The correct Option is "Interhalogen compounds are weaker oxidizing agents than halogens."

A.RAMA NAGESWARARAO · Answer

ClF is a better oxidizing agent than BrF.

A.RAMA NAGESWARARAO · Answer

The oxidizing power of ClF, ClF3, and ClF5 decreases in the order ClF > ClF3 > ClF5.

A.RAMA NAGESWARARAO · Answer

BrCl is a stronger oxidizing agent than IBr.

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