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  • The unhybridized p orbitals in each carbon atom of ethylene are perpendicular to the plane of the <img alt="\mathrm{sp^{2}}" src="https://entrancecorner.oncodecogs.com/gif.latex?%5Cmathrm%7Bsp%5E%7

The unhybridized p orbitals in each carbon atom of ethylene are perpendicular to the plane of the \mathrm{sp^{2}} hybrid orbitals. What type of bond is formed between these unhybridized p orbitals?

Option: 1

Sigma (\sigma ) bond


Option: 2

Pi(\pi) bond


Option: 3

Covalent bond


Option: 4

Hydrogen bond


Answers (1)

best_answer

The overlap of hybrid orbitals or a hybrid orbital and a 1s orbtial from hydrogen creates the sigma bond framework of the ethylene molecule. However the unhybridized \mathrm{p}_{\mathrm{z}} orbital on each carbon remains. The unhybridized pz orbitals on each carbon overlap to a \pi bond (pi).

Posted by

himanshu.meshram

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