Learn VSEPR Theory: Carbon & Oxygen Bonding

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SUMMARY

The discussion focuses on the VSEPR (Valence Shell Electron Pair Repulsion) theory and its application to carbon and oxygen bonding, specifically in the formation of carbon monoxide (CO) through a triple bond. The user expresses confusion regarding carbon's ability to form this bond despite having only four valence electrons. The explanation involves understanding carbon's electron configuration (2s2, 2p2) and the concept of hybridization, which allows carbon to utilize its p-orbitals to achieve a stable electron configuration by forming multiple bonds.

PREREQUISITES
  • Understanding of VSEPR theory
  • Knowledge of valence bond theory
  • Familiarity with electron configuration and hybridization
  • Basic concepts of molecular orbital theory
NEXT STEPS
  • Study the hybridization of carbon in detail
  • Learn about molecular orbital theory and its application to CO
  • Explore examples of other molecules with triple bonds
  • Investigate the implications of lone pairs on molecular geometry
USEFUL FOR

Chemistry students, educators, and anyone interested in molecular bonding and the principles of VSEPR theory.

Maz88
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okay so I am learning the Valence bond theory and the VSEPR theory in chemistry. and so far its been going well.
but i don't understand how carbon and oxygen combine together forming a triple boond creating CO (carbon monoxide) because we only have 4 valence carbon electrons so how can it form a triple bond with 2 lone pairs ? please help :)
 
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can someone pleaseee help mee !
 
Since carbon's valence shell looks like 2s2, 2p2 and your p-orbital can have 3 pairs of e- (6 e-) that means you can gain up to 4- to complete its valance shell.

Try drawing out your orbitals on energy diagram for the bond (with the hybridized orbitals) and filling it in.
 

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