Draw the Lewis Structure for OBr2

The Lewis structure for OBr₂, or dibromine oxide, can be drawn by following these steps:

1. Count the valence electrons: Oxygen has 6 valence electrons, and each bromine (Br) has 7 valence electrons. Therefore, the total number of valence electrons is 6 (from O) + 2 * 7 (from 2 Br) = 20 valence electrons.
2. Determine the central atom: In this molecule, oxygen is the central atom since it is less electronegative than bromine.
3. Place the surrounding atoms: Connect the two bromine atoms to the oxygen atom with single bonds. This uses 4 electrons (2 for each bond).
4. Distribute the remaining electrons: After forming the bonds, we have 20 – 4 = 16 valence electrons left. We will now place the remaining electrons on the surrounding atoms; each bromine will get 6 more electrons to complete their octets, which makes 12 electrons used here (6 for each Br).
5. Place remaining electrons on the central atom: At this point, we are left with 4 electrons, which can be placed as lone pairs on the central oxygen atom, resulting in 2 lone pairs.

Putting this all together, the final Lewis structure of OBr₂ looks like this:

This structure shows that oxygen is bonded to two bromine atoms with single bonds, and it has two lone pairs of electrons, fulfilling its octet rule.