Arrange the following compounds in increasing order of their ionic character `:`
`SnC_(2),SnCl_(4),SiCl_(4),SnF_(4),SnF_(2)`

Options

A. `3Å`
B. `5.33Å`
C. `6.88Å`
D. `48Å`

Explanation

To arrange the compounds SnC₂, SnCl₄, SiCl₄, SnF₄, and SnF₂ in increasing order of their ionic character, we will follow these steps:

### Step 1: Understand Ionic and Covalent Character
Ionic character refers to the extent to which a compound exhibits ionic bonding, while covalent character refers to the extent to which a compound exhibits covalent bonding. According to Fajans' rules, the covalent character in an ionic compound is influenced by the charge and size of the ions involved. A higher charge and smaller size of the cation lead to greater covalent character, which in turn means lower ionic character.

### Step 2: Determine the Oxidation States
Identify the oxidation states of the cations in each compound:
- **SnC₂**: Sn has an oxidation state of +2.
- **SnCl₄**: Sn has an oxidation state of +4.
- **SiCl₄**: Si has an oxidation state of +4.
- **SnF₄**: Sn has an oxidation state of +4.
- **SnF₂**: Sn has an oxidation state of +2.

### Step 3: Compare Cation Charges
From the oxidation states, we see:
- SnC₂ and SnF₂ have a +2 charge.
- SnCl₄, SiCl₄, and SnF₄ have a +4 charge.

### Step 4: Analyze the Size of Anions
The size of the anions also plays a crucial role in determining covalent character:
- Fluorine (F) is smaller than chlorine (Cl).
- Therefore, for the same cation charge, compounds with Cl will have a higher covalent character compared to those with F.

### Step 5: Compare Covalent Character
Now, we compare the covalent character based on cation charge and anion size:
- **SiCl₄**: +4 charge on Si and larger Cl anion → higher covalent character.
- **SnCl₄**: +4 charge on Sn and larger Cl anion → high covalent character.
- **SnF₄**: +4 charge on Sn and smaller F anion → lower covalent character than SnCl₄.
- **SnC₂** and **SnF₂**: +2 charge on Sn → higher ionic character compared to +4 compounds.

### Step 6: Final Comparison
Now we can arrange the compounds based on their covalent character, which inversely relates to ionic character:
1. **SiCl₄** (most covalent, least ionic)
2. **SnCl₄**
3. **SnF₄**
4. **SnCl₂**
5. **SnF₂** (least covalent, most ionic)

### Conclusion
The increasing order of ionic character is:
**SiCl₄ < SnCl₄ < SnF₄ < SnCl₂ < SnF₂**