To draw the Lewis structure for bromate chlorate (BrO3–), we need to follow the octet rule, which states that atoms tend to form bonds in such a way that each atom has eight electrons in its valence shell.
Here are the steps to draw the Lewis structure for bromate chlorate:
- Determine the total number of valence electrons:
- Bromine (Br) has 7 valence electrons.
- Each oxygen (O) has 6 valence electrons, and there are 3 oxygen atoms, so 6 × 3 = 18 electrons.
- Add one extra electron for the negative charge: 7 + 18 + 1 = 26 valence electrons.
- Draw the skeletal structure:
- Place the bromine (Br) atom in the center and the three oxygen (O) atoms around it.
- Distribute the electrons:
- Connect each oxygen atom to the bromine atom with a single bond (each bond uses 2 electrons).
- After forming the single bonds, you have used 6 electrons (3 bonds × 2 electrons).
- You have 20 electrons left to distribute.
- Complete the octets:
- Add lone pairs to the oxygen atoms to complete their octets. Each oxygen atom needs 6 more electrons (2 lone pairs).
- After adding lone pairs to all three oxygen atoms, you have used 18 electrons (3 oxygen atoms × 6 electrons).
- You have 2 electrons left, which will be placed on the bromine atom as a lone pair.
- Check the formal charges:
- Calculate the formal charges for each atom to ensure they are as close to zero as possible.
- If necessary, form double bonds between bromine and oxygen atoms to minimize formal charges.
The final Lewis structure for bromate chlorate (BrO3–) will have bromine in the center with three oxygen atoms surrounding it. Each oxygen atom will have two lone pairs, and bromine will have one lone pair. There will be one double bond between bromine and one of the oxygen atoms to minimize formal charges.