Draw the Lewis Dot Structure for POCl₃.

• A.
• B.
• C.
• D.

Answer: (A)

Verified step by step guidance

1. Identify the central atom in the molecule POCl₃. Phosphorus (P) is typically the central atom because it can form multiple bonds and has a lower electronegativity compared to oxygen (O) and chlorine (Cl).
2. Determine the total number of valence electrons available for the molecule. Phosphorus has 5 valence electrons, oxygen has 6, and each chlorine has 7. Therefore, the total number of valence electrons is: 5 + 6 + (3 × 7) = 32 valence electrons.
3. Arrange the atoms around the central phosphorus atom. Place oxygen and the three chlorine atoms around phosphorus. Connect each atom to phosphorus with a single bond initially.
4. Distribute the remaining valence electrons to satisfy the octet rule for each atom. Start by completing the octet for the outer atoms (oxygen and chlorine) and then adjust the central atom if necessary. Oxygen typically forms a double bond with phosphorus to satisfy its octet.
5. Check the formal charges to ensure the most stable structure. The formal charge is calculated using the formula: Formal Charge = Valence Electrons - Nonbonding Electrons - (Bonding Electrons / 2). Adjust the bonds if necessary to minimize formal charges across the molecule.