To solve the question regarding the correct order of properties among the given options, we will analyze each statement step by step.
### Step 1: Analyze Ionic Mobility Order
- **Given:** Fe³⁺ and Fe²⁺
- **Concept:** Ionic mobility is inversely proportional to size. A higher positive charge leads to a smaller ionic size.
- **Conclusion:** Fe³⁺ has a smaller size than Fe²⁺ because it has a higher charge. Therefore, Fe²⁺ will have higher ionic mobility than Fe³⁺.
- **Order:** Fe²⁺ > Fe³⁺ (in terms of ionic mobility)
### Step 2: Analyze Hydrated Radius Order
- **Given:** F⁻, Cl⁻, Br⁻, I⁻
- **Concept:** The hydrated radius is inversely proportional to ionic size. As we go down the group of halogens, the size of the ions increases.
- **Conclusion:** The order of size from smallest to largest is F⁻ < Cl⁻ < Br⁻ < I⁻. Therefore, the hydrated radius will be the opposite: I⁻ has the largest size and thus the smallest hydrated radius.
- **Order:** F⁻ < Cl⁻ < Br⁻ < I⁻ (in terms of hydrated radius)
### Step 3: Analyze Bond Polarity Order
- **Given:** PH₃, AsH₃, SbH₃
- **Concept:** Bond polarity decreases down the group due to decreasing electronegativity.
- **Conclusion:** Phosphorus is more electronegative than arsenic and antimony. Thus, the bond polarity order will be PH₃ > AsH₃ > SbH₃.
- **Order:** PH₃ > AsH₃ > SbH₃ (in terms of bond polarity)
### Step 4: Analyze Electronegativity Order
- **Given:** S, C, H, B
- **Concept:** Electronegativity values are as follows: S (2.58), C (2.55), H (2.20), B (2.04).
- **Conclusion:** The order of electronegativity from highest to lowest is S > C > H > B.
- **Order:** S > C > H > B (in terms of electronegativity)
### Final Conclusion
Based on the analysis:
1. The order for ionic mobility is correct.
2. The order for hydrated radius is correct.
3. The order for bond polarity is incorrect.
4. The order for electronegativity is correct.
Thus, the correct options are 1, 2, and 4.
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