We are asked to label all the bonds in SO2.
Step 1: Sulfur (EN = 2.5) is less electronegative than oxygen (EN = 3.5) so sulfur is the central atom.
Step 2: The total number of valence electrons present in SO2 is:
Group Valence Electrons
S 6A 1 × 6 e– = 6 e–
O 6A 2 × 6 e– = 12 e–
Total: 18 valence e–
Step 3: Oxygen prefers to form 2 bonds. The Lewis structure is:
Label all bonds in SO2.
The hybridization of the S atom in SO2 is sp2.
δ: S(sp2) - O(p)
Lone pair in sp2 orbital
δ: S (p) - O(sp2)
π: S(p) - O(p)
π: S(p) - O(sp2)
Lone pair in p orbital
δ: S(p) - O(p)
π: S(sp2) - O(p)
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Valence Shell Electron Pair Repulsion Theory concept. You can view video lessons to learn Valence Shell Electron Pair Repulsion Theory. Or if you need more Valence Shell Electron Pair Repulsion Theory practice, you can also practice Valence Shell Electron Pair Repulsion Theory practice problems.
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Based on our data, we think this problem is relevant for Professor Frey, Statler, & Steele's class at UTAH.