The halide ion easiest to oxides is :

Options

A. `F^(-)`
B. `Cl^(-)`
C. `Br^(-)`
D. `I^(-)`

Answer

To determine which halide ion is the easiest to oxidize, we need to analyze the properties of the halide ions. The halide ions we are considering are fluoride (F⁻), chloride (Cl⁻), bromide (Br⁻), and iodide (I⁻).

### Step 1: Understand Oxidation
Oxidation refers to the loss of electrons. Therefore, when we talk about a halide ion being oxidized, we are referring to its ability to lose an electron and convert into its corresponding halogen.

### Step 2: Analyze the Halide Ions
The halide ions are:
- F⁻ (fluoride)
- Cl⁻ (chloride)
- Br⁻ (bromide)
- I⁻ (iodide)

### Step 3: Consider the Trends in Halogens
In the periodic table, as we move down the group of halogens from fluorine to iodine, the size of the atoms increases. This increase in size affects the stability of the halide ions:
- Fluoride (F⁻) is the smallest and has a high electronegativity.
- Iodide (I⁻) is the largest and has a lower electronegativity.

### Step 4: Determine the Ease of Oxidation
The ease of oxidation generally increases with the size of the halide ion because larger ions have a lower ionization energy, making it easier for them to lose an electron. Therefore, we can summarize:
- F⁻ is less likely to oxidize because it is very stable due to its small size and high electronegativity.
- Cl⁻ is more likely to oxidize than F⁻, but less than Br⁻.
- Br⁻ is more likely to oxidize than Cl⁻.
- I⁻ is the most likely to oxidize because it is the largest and least electronegative.

### Conclusion
Based on the above analysis, the halide ion that is easiest to oxidize is **I⁻ (iodide)**.