What is the Lewis structure for F2O?

The Lewis structure for F₂O, which is fluorine dioxide, illustrates how the valence electrons are arranged among the atoms in the molecule.

To draw the Lewis structure:

1. First, count the total number of valence electrons. Fluorine (F) has 7 valence electrons, and oxygen (O) has 6. Therefore, for F₂O, the total number of valence electrons is 7 + 7 + 6 = 20.
2. Next, place the oxygen atom in the center as it is less electronegative than fluorine. Connect the two fluorine atoms to the oxygen atom with single bonds.
3. This initial structure uses 4 electrons (2 for each bond), leaving us with 16 electrons to distribute.
4. Now, complete the octet for each fluorine atom by adding 6 electrons (3 lone pairs) around each fluorine. This uses up 12 electrons, leaving us with 4 electrons.
5. Finally, place the remaining 4 electrons as two lone pairs on the oxygen atom to complete its octet. Oxygen now has 8 electrons (2 from the bonding pairs and 4 from the lone pairs).

In conclusion, the Lewis structure for F₂O consists of an oxygen atom with two single bonds to two fluorine atoms, and it has two lone pairs of electrons on the oxygen, with each fluorine also having three lone pairs.