Draw the Lewis Structure for HSO4

To draw the Lewis structure for HSO₄ (sulfuric acid), we need to follow a series of steps to ensure we accurately represent the molecule’s electron distribution.

1. Count the total number of valence electrons: Sulfur (S) has 6 valence electrons, oxygen (O) has 6 valence electrons each, and hydrogen (H) has 1 valence electron. Therefore, for HSO₄:
   – Sulfur: 6 electrons
   – Oxygen: 4 × 6 = 24 electrons
   – Hydrogen: 1 electron
   Total = 6 + 24 + 1 = 31 valence electrons.
2. Determine the central atom: In HSO₄, sulfur is the central atom because it is less electronegative and can form more bonds than the surrounding atoms.
3. Arrange the atoms: We will start placing the atoms around the sulfur. We will draw the sulfur atom in the center with four oxygen atoms bonded to it.
4. Connect the atoms with single bonds: Draw single bonds from sulfur to each of the four oxygen atoms. This uses up 8 of the valence electrons (2 electrons per bond, and there are 4 bonds).
5. Distribute the remaining valence electrons: After forming the four bonds, we have a total of 23 valence electrons left. Place three lone pairs on each of the three oxygen atoms and one double bond with the fourth oxygen. Each lone pair accounts for 2 electrons, totaling 12 electrons used (6 lone pairs), leaving us with 11 electrons. We can then place a double bond between sulfur and one oxygen. This double bond uses 2 electrons, thus having 9 electrons remaining.
6. Place the hydrogen atom: Attach a hydrogen atom to one of the singly bonded oxygen atoms. Now, all atoms have a full valence shell. The hydrogen uses 1 of the 9 remaining electrons.
7. Check the formal charges: Make sure the formal charges on each atom sum to zero. The sulfur atom will have a +6 charge, while the oxygen atoms and hydrogen will balance this out, typically resulting in a net charge of 0.

The final Lewis structure for HSO₄ shows sulfur in the center, bonded to four oxygen atoms: one with a single bond with hydrogen attached and one double-bonded oxygen, complemented by lone pairs around the other oxygens, conveying that sulfuric acid has a tetrahedral shape with resonance structures.