Which of the following is the correct Lewis dot structure for the molecule OF2?

• A. F:O:F, where O has two lone pairs and each F has three lone pairs
• B. F-O-F, where O has one lone pair and each F has three lone pairs
• C. F=O=F, where O has one lone pair and each F has two lone pairs
• D. F-O-F, where O has three lone pairs and each F has two lone pairs

Answer: (A)

Verified step by step guidance

1. Step 1: Determine the total number of valence electrons for the molecule OF2. Oxygen (O) has 6 valence electrons, and each fluorine (F) has 7 valence electrons. Since there are two fluorines, calculate the total as \$6 + 2 \times 7$.
2. Step 2: Draw a skeletal structure with oxygen as the central atom bonded to the two fluorine atoms. Connect each fluorine to oxygen with a single bond initially.
3. Step 3: Distribute the remaining valence electrons as lone pairs to satisfy the octet rule for each atom. Remember that fluorine atoms typically have three lone pairs, and oxygen should have enough lone pairs to complete its octet after bonding.
4. Step 4: Check the formal charges on each atom to ensure the most stable Lewis structure. The formal charge is calculated by \(\text{Formal charge} = \text{Valence electrons} - \text{Nonbonding electrons} - \frac{1}{2} \times \text{Bonding electrons}\).
5. Step 5: Compare the possible Lewis structures based on the octet rule and formal charges. The correct structure will have all atoms with full octets and minimal formal charges, which corresponds to oxygen having two lone pairs and each fluorine having three lone pairs.