1. Determine the central atom: Bromine (Br) is the least electronegative element and will be the central atom.
2. Calculate the total number of valence electrons:
* Bromine (Br) has 7 valence electrons.
* Oxygen (O) has 6 valence electrons each, and there are three oxygen atoms.
* The negative charge adds one more electron.
* Total valence electrons: 7 + (6 x 3) + 1 = 26
3. Arrange the atoms and form single bonds: Place the three oxygen atoms around the bromine atom, connecting them with single bonds.
4. Distribute the remaining electrons to satisfy the octet rule: Each oxygen atom will have two lone pairs of electrons to complete its octet.
5. Draw the resonance structures: To achieve the best possible Lewis structure for bromate, you need to move the electrons around. You can do this by moving a lone pair from one of the oxygen atoms to form a double bond with the bromine. Since there are three oxygen atoms, you can draw three resonance structures.
Here are the three resonance structures of bromate ion:
[Image of the three resonance structures of the bromate ion]
Key points:
* Each resonance structure contributes to the overall structure of the bromate ion.
* The actual structure of the bromate ion is a hybrid of all three resonance structures.
* The negative charge is delocalized over all three oxygen atoms.
Let me know if you'd like me to explain any specific aspect in more detail!
