Final answer:
Lewis structures for NO3⁻, SO4²⁻, CO3²⁻, and PO4³⁻ involve arranging atoms to minimize formal charges, connecting with bonds, and adding lone pairs to satisfy the octet rule, while accounting for the ion's overall charge.
Step-by-step explanation:
The question involves writing Lewis structures for various polyatomic ions. Lewis structures are diagrams that represent the valence electrons of atoms within a molecule.
To write Lewis structures for the ions NO3⁻, SO4²⁻, CO3²⁻, and PO4³⁻, start by counting the valence electrons for each atom and including the extra electrons or positive charges indicated by the ion's charge.
Arrange the atoms to minimize formal charges, connect them with single or multiple bonds as needed, and then add lone pairs to satisfy the octet rule (or duet for hydrogen atoms).
Below are the Lewis structures for the ions:
- NO3⁻ (Nitrate ion): The nitrogen atom is the central atom with double bonds to one oxygen atom and single bonds to the other two oxygen atoms. Each oxygen atom has a full octet, and the overall charge of the ion is -1.
- SO4²⁻ (Sulfate ion): Sulfur is the central atom with double bonds to two oxygen atoms and single bonds to the other two. Each oxygen atom has a full octet, and the overall charge of the ion is -2.
- CO3²⁻ (Carbonate ion): Carbon is the central atom with double bonds to one oxygen atom and single bonds to the other two. Each oxygen atom has a full octet, and the overall charge of the ion is -2.
- PO4³⁻ (Phosphate ion): Phosphorus is the central atom with double bonds to one oxygen atom and single bonds to the other three. Each oxygen atom has a full octet, and the overall charge of the ion is -3.
Note that for all these structures, resonance may occur, meaning that the double or triple bonds are delocalized among the oxygen atoms.