Can a Molecule Share 4 Bonded Electrons?

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SUMMARY

Quadruple bonds, pentuple bonds, and sextuple bonds have been observed in metal-metal complexes, particularly involving heavier metals such as Tungsten and Rhenium. Carbon cannot form quadruple bonds due to its tetrahedral geometry, which limits orbital hybridization. The presence of d-orbitals in these metals allows for the formation of delta bonds, enabling higher-order bonding. The highest order bond documented is a sextuple bond, which involves the sharing of 12 electrons.

PREREQUISITES
  • Understanding of molecular geometry, specifically tetrahedral geometry
  • Knowledge of d-orbitals and their role in bonding
  • Familiarity with metal-metal bonding in coordination complexes
  • Basic concepts of covalent bonding and electron sharing
NEXT STEPS
  • Research the properties and examples of metal-metal quadruple bonds
  • Study the role of d-orbitals in bonding, particularly in transition metals
  • Explore the characteristics and applications of sextuple bonds in chemistry
  • Investigate the physical properties of compounds with high-order bonds, such as hardness and reactivity
USEFUL FOR

Chemists, materials scientists, and students interested in advanced bonding theories and the properties of transition metal complexes.

_wolfgang_
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I am wandering whether this can happen? When a molecule shares 4 pairs of bonded electons? Say like a C2 Molecule?? maybe. Could it happen or does it happen??
 
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Yes, but not for carbon.

The reason carbon can't four-bond is because of its tetrahedral geometry. Even with only half of the orbitals hybridized, one orbital on each carbon atom will still face "away" from the bond.

As it turns out, quadruple bonds, pentuple bonds, and even a sextuple bond have all been observed. Where? Metal-metal bonds in complexes, especially the heavier metals with loose electrons. I believe Tungsten and Rhenium both exhibit this odd behavior.

My theory as to why this happens? d-orbitals.
 
Char. Limit said:
My theory as to why this happens? d-orbitals.

Correct. Overlap between d-orbitals in metal-metal covalent bonds can produce a delta bond which is required to explain quadruple bonding species.
 
Haha! I knew it!

Thanks for proving me right. Honestly, sometimes physics is so screwed up I think the intuitive answer, though right in this case, could ever be correct.
 
Specifically I remember about some Rhenium and Technetium compounds with a formal Re-Re or Tc-Tc double bond.
 
Doesn't mean it can't be higher as well.
 
Hmm so can actually happen just not with carbon, i get why now because of its tetrahedral shape. Also is there any special names for these substances, as well as would you know what the most amount of bonds there are possible?
 
I don't know about the names, but I can tell you that the highest order bond observed is a sextuple bond, sharing 12 electrons.
 
Ok cool i see this happens molybdenum. Also what would happen to phsical properties? ultra hard? Ultra unreactive?
 

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