Drawing a Lewis Dot Structure for Octathiocane (S8)

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SUMMARY

The Lewis dot structure for octathiocane (S8) requires careful consideration of formal charges and the octet rule. A straight chain configuration initially results in terminal sulfurs carrying a negative charge, leading to an overall net negative charge. Adjusting electron pairs can alleviate charge issues but risks violating the octet rule for adjacent sulfurs. The correct structure maintains net neutrality while ensuring all atoms adhere to the octet rule.

PREREQUISITES
  • Understanding of Lewis dot structures
  • Knowledge of formal charges in molecular structures
  • Familiarity with the octet rule
  • Basic principles of sulfur bonding and lone pair interactions
NEXT STEPS
  • Research advanced techniques for drawing Lewis structures for larger molecules
  • Study the properties and bonding behavior of sulfur in organic compounds
  • Learn about resonance structures and their impact on molecular stability
  • Explore molecular geometry and its relation to electron pair repulsion
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Chemistry students, educators, and professionals involved in molecular modeling and structural chemistry will benefit from this discussion.

rmjmu507
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Homework Statement


How can I draw a Lewis dot structure for octathiocane (S8) which is non-cyclic, net neutral, and which does not violate the octet rule?


Homework Equations


None.


The Attempt at a Solution


First, I tried drawing a straight chain molecule, but the two terminal sulfurs each have a negative charge, giving a net negative charge overall.

I then tried pushing an electron pair from one of the terminal sulfurs inwards, which solves the charge issue but makes the penultimate sulfur on one side violate the octet rule...

I'm stumped. Any advice?
 
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- It is a straight chain.
- One end has a 1- formal charge, the other has a 0 formal charge. (Net charge=0)
- Sulfur can change lone pairs to bonds.

You should be able to figure it out with this, if not let me know. :D
 

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