Which of the following species is most ionic.

Options

A. `SnCl_(4)`
B. `C Cl_(4)`
C. `SnCl_(2)`
D. `SnI_(2)`

Explanation

To determine which of the following species is most ionic, we can follow these steps:

### Step 1: Understand Ionic and Covalent Character
Ionic character in a compound is influenced by the size and charge of the ions involved. Smaller cations and larger anions typically lead to greater covalent character due to increased polarization. Conversely, larger cations and smaller anions tend to result in more ionic character.

### Step 2: Identify the Given Species
The species in question are:
1. SnCl4
2. SnCl2
3. SnI2
4. C (Carbon)

### Step 3: Analyze the Oxidation States
- SnCl4: Tin is in the +4 oxidation state.
- SnCl2: Tin is in the +2 oxidation state.
- SnI2: Tin is in the +2 oxidation state.
- C: Not relevant as it does not form ionic compounds in this context.

### Step 4: Apply Fajan's Rule
According to Fajan's rule, the polarization of an anion by a cation increases with:
- A smaller cation (higher charge density).
- A larger anion.

In our case:
- SnCl4 has a +4 charge, which means it has a smaller ionic radius compared to Sn in +2 state.
- SnCl2 and SnI2 both have Sn in the +2 state, but the anions differ.

### Step 5: Compare the Anions
- Cl- (Chloride) is smaller than I- (Iodide).
- Thus, SnCl2 (with Cl-) will have a larger ionic character compared to SnI2 (with I-), because the smaller chloride ion will be less polarized by the Sn cation.

### Step 6: Conclusion
Since SnCl2 has the larger cation (Sn in +2 state) and a smaller anion (Cl-), it will exhibit the most ionic character among the given species.

### Final Answer
The species that is most ionic is **SnCl2**.

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