QQuestionChemistry
QuestionChemistry
"Describe the hybrid orbitals used by the central atom(2$) and the type(2$) of bonds formed in SO^2.
Hybridization:
Number of bonds:
σ
π"
3 months agoReport content
Answer
Full Solution Locked
Sign in to view the complete step-by-step solution and unlock all study resources.
Step 1: Determine the hybridization of the central atom (Sulfur) in SO^2.
Sulfur forms three bonds in SO^2, two single bonds with oxygen atoms and one double bond with another oxygen atom. To accommodate this, sulfur will use sp^2 hybridization.
Step 2: Explain sp^2 hybridization.
sp^2 hybridization is a combination of one s orbital and two p orbitals to form three hybrid orbitals with equal energy and geometry. The three hybrid orbitals are arranged in a trigonal planar geometry, making a 120 -degree angle with each other.
Final Answer
Hybridization: The central atom, sulfur, in SO^2 uses sp^2 hybridization. Number of bonds: Sulfur forms a total of three bonds: two σ bonds with one oxygen atom and one π bond with another oxygen atom. σ and π bonds: Sulfur forms two σ bonds and one π bond in SO^2.
Need Help with Homework?
Stuck on a difficult problem? We've got you covered:
- Post your question or upload an image
- Get instant step-by-step solutions
- Learn from our AI and community of students