Which of the following options are not accordance with the property mentioned against them?
(a) `F_(2)gtCl_(2)gtBr_(2)gtI_(2)` Oxodising power
(b) `MIgtMBrgtMClgtMF` Ionic character of metal halide
(c ) `F_(2)gtCl_(2)gtBr_(2)gtI_(2)` Bond dissociation enthalphy
(d) `HIltHBrltHClltHF` Hydrogen - halogen bond strength

Explanation

To solve the question, we need to analyze each option provided and determine whether the order mentioned aligns with the properties described. Let's break it down step by step:

### Step 1: Analyzing Option (a)
**Given Order:** \( F_2 > Cl_2 > Br_2 > I_2 \)
**Property:** Oxidizing power

**Analysis:**
- Oxidizing power increases with the ability of an element to gain electrons.
- Fluorine (F) has the highest oxidizing power due to its small size and high electronegativity, followed by chlorine (Cl), bromine (Br), and iodine (I).
- Thus, the order is correct.

### Step 2: Analyzing Option (b)
**Given Order:** \( MI > MBr > MCl > MF \)
**Property:** Ionic character of metal halides

**Analysis:**
- Ionic character is determined by the electronegativity difference between the metal (M) and the halogen.
- Fluorine (F) has the highest electronegativity, leading to the highest ionic character in \( MF \), followed by \( MCl \), \( MBr \), and \( MI \).
- Therefore, the order given in the question is incorrect.

### Step 3: Analyzing Option (c)
**Given Order:** \( F_2 > Cl_2 > Br_2 > I_2 \)
**Property:** Bond dissociation enthalpy

**Analysis:**
- The bond dissociation enthalpy is affected by the size of the atoms and the repulsion between electrons.
- Fluorine (F) has a lower bond dissociation enthalpy than chlorine (Cl) due to significant electron-electron repulsions in the small 2p orbital.
- The correct order should be \( Cl_2 > Br_2 > F_2 > I_2 \).
- Thus, the order given is incorrect.

### Step 4: Analyzing Option (d)
**Given Order:** \( HI < HBr < HCl < HF \)
**Property:** Hydrogen-halogen bond strength

**Analysis:**
- The bond strength decreases as the size of the halogen increases.
- HF has the strongest bond due to the small size of fluorine and high electronegativity, followed by HCl, HBr, and HI.
- Therefore, the order given is correct.

### Conclusion
The options that are not in accordance with the properties mentioned are **(b) and (c)**.

### Final Answer:
(b) and (c) are not in accordance with the properties mentioned.

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