Hybridisation of SO 2 and SeO 2

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SUMMARY

The hybridization of sulfur in sulfur dioxide (SO2) is definitively sp2, while selenium in selenium dioxide (SeO2) exhibits sp3 hybridization. This distinction arises from the molecular structure and state of the compounds; SO2 is a discrete gaseous molecule, whereas SeO2 exists as a solid with a polymeric chain structure. The bond angles also differ significantly, with SO2 having bond angles around 120 degrees and SeO2 ranging between 90 and 100 degrees in its solid form. The discussion emphasizes the importance of accurate representation of hybridization based on observable molecular characteristics rather than speculation.

PREREQUISITES
  • Understanding of molecular hybridization concepts
  • Familiarity with the molecular structures of SO2 and SeO2
  • Knowledge of bond angles and their significance in molecular geometry
  • Basic principles of solid-state chemistry
NEXT STEPS
  • Research the molecular geometry of sulfur and selenium compounds
  • Study the differences between discrete molecules and polymeric solids
  • Explore the concept of bond angles in various molecular states
  • Investigate the role of hybridization in predicting molecular behavior
USEFUL FOR

Chemistry students, educators, and professionals interested in molecular structure, hybridization, and the physical properties of sulfur and selenium compounds.

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Hybridisation of SO2 and SeO2

Why is the hybridisation of S in SO2 sp2 where as it is sp3 in SeO2 ?
 
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Who sais so? Or is this only based on some difference in bond angle?
 


My book.
"SO2 being a discrete molecule exists in the gaseous state. Hybridisation of S in SO2 in the gaseous state is sp2.

Selenium and tellurium dioxides are solids having polymeric chain or layer structure. It consists of a zig-zag chain. Hybridisation of Se in SeO2 is sp3"
 


What does this book want to tell us? That SO2 doesn't exist in liquid or solid form because it is a discrete molecule?
What you can say is that the bond angles in SO2 and SeO2 are about 120 deg in gas phase and in solid SeO2 between 90 and 100 degree. Would be much more honest than speculating about some hypothetical hybridization which is not observable.
In case of SeO2 (solid) assuming no hybridization at all would probably describe the molecule even better.
Get a better book.
 

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