Pi bonds and Sigma bonds

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Akshay Anand
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Joined: Fri Sep 29, 2017 7:07 am

Pi bonds and Sigma bonds

Postby Akshay Anand » Sat Nov 25, 2017 11:27 am

What hybrid orbitals bond together in a linear molecule of ethyne? (H-C---C-H). The three dashes between carbons represent a triple bond. How exactly do each hybrid orbital bond to form sigma and pi bonds?

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Re: Pi bonds and Sigma bonds

Postby miznaakbar » Sat Nov 25, 2017 4:28 pm

For ethyne, each carbon is bonded to two atoms, therefore it will have two hybridized orbitals. This will lead to the formation of two sp hybridized orbitals and leaves 2 regular p orbitals. Now when we draw the orbitals, we will have two sp orbitals sticking out of the sides of each C atom. Both the C atoms also have 2 p orbitals each. Where the two sp orbitals of the C atoms overlap, a sigma bond forms. Where the H atoms' s orbitals overlap with both the C atoms' other sp orbital, there is another two sigma bonds. Now where the p orbitals of both the C atoms overlap, there are two pi bonds. This explanation is probably pretty difficult to visualize, so here is a great khan academy video that pretty much explains all of this for the ethyne molecule, hope it helps! https://www.khanacademy.org/science/org ... -jay-final

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