What is the Lewis Structure for H3PO4?

The Lewis structure for H₃PO₄, also known as phosphoric acid, can be drawn by following these steps:

1. Count the total number of valence electrons: Phosphorus (P) has 5 valence electrons, each hydrogen (H) has 1, and each oxygen (O) has 6. For H₃PO₄, the total number of valence electrons is 5 (P) + 3(1) (H) + 4(6) (O) = 32 electrons.
2. Determine the central atom: Phosphorus is the central atom because it is less electronegative than oxygen.
3. Draw single bonds between the central atom and surrounding atoms: Connect the phosphorus atom to the three hydrogen atoms and one oxygen atom with single bonds. This uses up 8 electrons (4 bonds × 2 electrons).
4. Distribute the remaining electrons: Place the remaining 24 electrons around the oxygen atoms to satisfy the octet rule. Each oxygen atom should have 8 electrons, including the electrons in the bonds.
5. Form double bonds if necessary: To satisfy the octet rule for phosphorus, form double bonds between phosphorus and the remaining three oxygen atoms. This will use up the remaining electrons.

The final Lewis structure for H₃PO₄ shows phosphorus at the center with single bonds to three hydrogen atoms and one oxygen atom, and double bonds to the remaining three oxygen atoms. Each oxygen atom has a complete octet, and phosphorus also has a complete octet.