4 Bonds Carbon Can Form

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Solution

The reason is to have those bonds all 4 pairs of electrons must be present betwixt ii carbon atoms and simply on 'one' side of each carbon atom which is geometrically impossible for all kinds of hybrid orbitals. No! Carbon-Carbon quadra bond is invalid. ... It is bonded covalently with iv other Carbon cantlet.

From a Lewis point of view, there is no reason why carbon can't form a quadruple bailsatisfying the Octet Rule and leaving no electrons for further bonding. But information technology implies that C2 is a perfectly stable molecule, like N2, and that just isn't the case.

If we go on to the valence-bail model, in which bonds upshot from the overlap of atomic orbitals, we come across a better caption: carbon cannot form a quadruple bond because it doesn't have plenty atomic orbitals pointing in the right directions. sp hybridization leaves two p orbitals over, while sp2 hybridization leaves one p orbital.

Valence-bond theory predicts two possible bonding states for C2:

1. double bond with all electrons paired, :C=C: (every bit seen in Alkene)

2. a triple bond with two unpaired electrons, .C(Triple)C. (As seen in Alkyne)

These are called resonance structures, and both must be considered every bit partial representations of the real situation.

Source: https://byjus.com/question-answer/why-can-t-carbon-form-bond-of-4-electrons-with-another-carbon/