Maximum covalent character is shown by

Options

A. `NCl_(3)`
B. `PCl_(3)`
C. `AsCl_(3)`
D. `SbCl_(3)`

Answer

To determine which compound exhibits the maximum covalent character among the given options (NCl3, PCl3, Cl3, SbCl3), we can follow these steps:

### Step 1: Understand Covalent Character
Covalent character in a compound is influenced by the size of the cation (the positively charged ion). The smaller the cation, the greater the covalent character because smaller cations can polarize the electron cloud of the anion more effectively.

### Step 2: Analyze the Cations in the Given Compounds
- **NCl3**: Here, nitrogen (N) is the cation.
- **PCl3**: Here, phosphorus (P) is the cation.
- **Cl3**: This option seems incomplete or incorrect as it does not specify a cation.
- **SbCl3**: Here, antimony (Sb) is the cation.

### Step 3: Compare the Sizes of the Cations
- **N (Nitrogen)**: Smallest cation among the options.
- **P (Phosphorus)**: Larger than nitrogen.
- **Sb (Antimony)**: Larger than both nitrogen and phosphorus.

### Step 4: Determine the Trend
As we move down the group in the periodic table (from N to P to Sb), the size of the cation increases. Therefore, the covalent character decreases as we go from NCl3 to SbCl3.

### Step 5: Conclusion
Since NCl3 has the smallest cation (N), it will exhibit the maximum covalent character compared to PCl3 and SbCl3.

### Final Answer
The compound that shows the maximum covalent character is **NCl3**.

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