Question 25 2.5 pts What is the correct Lewis structure for oxygen difluoride molecule, OF
?
F::O::F
F::O::F
F::O::F
F::O::F
:F::O::F:
The Correct Answer and Explanation is:
ChatGPT said:
The correct Lewis structure for the oxygen difluoride (OF₂) molecule is the last option (fifth one):
:F–O–F:
Each fluorine (F) atom has three lone pairs, and the oxygen (O) atom has two lone pairs, with single bonds connecting O to each F atom.
Explanation
Oxygen difluoride (OF₂) consists of one oxygen atom bonded to two fluorine atoms. To determine the correct Lewis structure, follow these steps:
1. Count Valence Electrons:
- Oxygen (O) has 6 valence electrons.
- Fluorine (F) has 7 valence electrons, and there are two F atoms.
Total valence electrons = 6 (O) + 7×2 (F) = 20 electrons
2. Determine Atom Placement:
Oxygen is less electronegative than fluorine, so it is the central atom, with the two fluorines bonded to it.
3. Create Single Bonds:
Create single bonds between O and each F:
- 2 single bonds = 2×2 = 4 electrons used
- Remaining electrons = 20 – 4 = 16 electrons
4. Distribute Remaining Electrons as Lone Pairs:
- Each F needs 3 lone pairs (6 electrons), so 2 Fs = 12 electrons
- 4 electrons remain, which go as 2 lone pairs on O
Now, each atom has a full octet:
- Fluorines: 1 bond + 6 electrons = 8 electrons
- Oxygen: 2 bonds + 4 electrons (2 lone pairs) = 8 electrons
5. Check Formal Charges:
All atoms have formal charges of zero. This confirms that this is the most stable structure.
6. Molecular Shape:
Though not required for the Lewis structure itself, it’s worth noting:
OF₂ has a bent shape due to the two lone pairs on oxygen (similar to H₂O), and the bond angle is slightly less than 109.5° due to lone pair repulsion.
Conclusion:
The correct Lewis structure is the one showing oxygen in the center, with two single bonds to fluorine atoms, and lone pairs properly distributed::F–O–F:
