Learn VSEPR Theory: Carbon & Oxygen Bonding

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The discussion focuses on understanding the bonding between carbon and oxygen, specifically the formation of a triple bond in carbon monoxide (CO). The user expresses confusion over how carbon, with only four valence electrons, can form a triple bond while also having two lone pairs. A suggestion is made to visualize the bonding by drawing the orbitals on an energy diagram, including hybridized orbitals. Clarification is provided that carbon can utilize its p-orbitals to accommodate additional electrons, allowing for the formation of a triple bond. Understanding these orbital interactions is crucial for mastering VSEPR theory and valence bond theory in chemistry.
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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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