1. Draw the Lewis Structure:
* Count valence electrons: H (1) + S (6) + O (3 * 6) + 1 (negative charge) = 26 valence electrons.
* Connect atoms: Place sulfur (S) in the center, surrounded by three oxygens (O). Connect each oxygen to sulfur with a single bond.
* Complete octets: Place lone pairs on the oxygen atoms to complete their octets.
* Add the hydrogen: Place the hydrogen on one of the oxygen atoms.
* Check for formal charges: The sulfur atom should have a formal charge of +1, and one of the oxygen atoms should have a formal charge of -1. This is the most stable arrangement.
2. Count Electron Domains:
* Electron domains: These are regions of electron density around the central atom. In HSO₃⁻, sulfur has four electron domains:
* Three single bonds to oxygen atoms
* One double bond to an oxygen atom
3. Determine Hybridization:
* Hybridization: The hybridization of an atom is determined by the number of electron domains around it.
* Four electron domains = sp³ hybridization
Therefore, the hybridization of the central sulfur atom in HSO₃⁻ is sp³.
