Answer
See the explanation
Work Step by Step
Here are the Lewis structures for the given species, along with the formal charge for each central atom:
a. $POCl_{3}$:
- Lewis structure:
O=P-Cl
|
Cl Cl
- Formal charge on the central P atom: 0
b. $SO_{4}^{2-}$:
- Lewis structure:
O=S=O
|
O O
- Formal charge on the central S atom: 0
c. $ClO_{4}^{-}$:
- Lewis structure:
O
|
Cl-O
|
O O
- Formal charge on the central Cl atom: 0
d. $PO_{4}^{3-}$:
- Lewis structure:
O
|
P-O
||
O O
- Formal charge on the central P atom: 0
e. $SO_{2}Cl_{2}$:
- Lewis structure:
O=S-Cl
|
Cl
- Formal charge on the central S atom: 0
f. $XeO_{4}$:
- Lewis structure:
O
|
Xe-O
|
O O
- Formal charge on the central Xe atom: 0
g. $ClO_{3}^{-}$:
- Lewis structure:
O
|
Cl-O
|
O
- Formal charge on the central Cl atom: 0
h. $NO_{4}^{3-}$:
- Lewis structure:
O
|
N-O
|
O O
- Formal charge on the central N atom: 0
In all the given species, the central atoms obey the octet rule, and the formal charges on the central atoms are 0.
