Choose the best Lewis structure for OCl2: 0 9-3- 0 &78-&: 0 {=0=d; 9-i_c; 0 j-g-d;
The Correct Answer and Explanation is:
The best Lewis structure for OCl₂ (dichlorine monoxide) is:
..
:Cl–O–Cl:
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Correct Lewis Structure:
- Oxygen (O) is the central atom.
- Each chlorine (Cl) atom is single-bonded to oxygen.
- Oxygen has 2 lone pairs, and each Cl atom has 3 lone pairs.
- The structure satisfies the octet rule for all atoms.
Step-by-Step Explanation:
1. Count total valence electrons:
- Oxygen (Group 16) = 6 valence electrons
- Chlorine (Group 17) = 7 valence electrons × 2 = 14
- Total = 6 + 14 = 20 valence electrons
2. Choose the central atom:
- Oxygen is less electronegative than chlorine, so O is central.
3. Form single bonds:
- Connect each Cl to O with a single bond:
- Each bond = 2 electrons × 2 bonds = 4 electrons used
- Remaining electrons: 20 – 4 = 16 electrons
4. Distribute remaining electrons as lone pairs:
- Start by giving 3 lone pairs (6 electrons) to each Cl to complete their octets:
- 6 electrons × 2 Cl = 12 electrons
- Remaining electrons: 16 – 12 = 4
- Place the remaining 4 electrons as 2 lone pairs on the central oxygen.
5. Check octet rule:
- Oxygen has 2 bonding pairs + 2 lone pairs = 8 electrons → satisfies octet
- Each Cl has 1 bond + 3 lone pairs = 8 electrons → also satisfies octet
6. Formal charge check (optional but supports structure stability):
- All atoms have a formal charge of zero → the structure is stable.
Conclusion:
The best Lewis structure for OCl₂ has oxygen in the center, bonded by single bonds to two chlorine atoms, with lone pairs completing the octets. All atoms follow the octet rule and the structure minimizes formal charges, making it the most accurate and stable representation.
