The compound that has the higest ionic character associated with the X-Cl bond is :

Options

A. `PCl_(5)`
B. `BCl_(3)`
C. `C Cl_(4)`
D. `SiCl_(4)`

Explanation

To determine which compound has the highest ionic character associated with the X-Cl bond, we will follow these steps:

### Step 1: Understand Ionic Character
Ionic character in a bond is primarily determined by the difference in electronegativity between the two atoms involved in the bond. The greater the difference, the more ionic the bond is.

### Step 2: Identify the Compounds
We need to identify the compounds that contain the X-Cl bond. Common elements that can bond with chlorine (Cl) include silicon (Si), phosphorus (P), sulfur (S), and carbon (C).

### Step 3: Find Electronegativity Values
We will look up the electronegativity values for the relevant elements:
- Chlorine (Cl) has an electronegativity of approximately 3.16.
- Silicon (Si) has an electronegativity of approximately 1.90.
- Phosphorus (P) has an electronegativity of approximately 2.19.
- Sulfur (S) has an electronegativity of approximately 2.58.
- Carbon (C) has an electronegativity of approximately 2.55.

### Step 4: Calculate Electronegativity Differences
Now we will calculate the electronegativity differences for each compound:
1. **SiCl4**: |3.16 - 1.90| = 1.26
2. **PCl3**: |3.16 - 2.19| = 0.97
3. **SCl2**: |3.16 - 2.58| = 0.58
4. **CCl4**: |3.16 - 2.55| = 0.61

### Step 5: Determine the Maximum Difference
From the calculated differences:
- SiCl4: 1.26
- PCl3: 0.97
- SCl2: 0.58
- CCl4: 0.61

The maximum electronegativity difference is 1.26, which corresponds to SiCl4.

### Step 6: Conclusion
Thus, the compound that has the highest ionic character associated with the X-Cl bond is **SiCl4**.