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briefly explain why the two pi-bonds of an alkyne triple bond are required to be oriented perpendicular to one another. (sp hybridization)

Sagot :

Ethyne (C2H2) is a linear molecule with a triple bond among the 2 carbon atoms. The hybridization is consequently sp. The orientation of the pi bonds is that they're perpendicular to 1 another.

Sigma bonds form between two atoms. Pi bonds form from p- orbital overlap.

  • Both to the hydrogen atoms and to one another, the sp hybrid orbitals create sigma bonds. Pi bonds are created between the Py and pzo. Orbitals on each carbon atom. These side-to-side overlaps are above and below the molecule's plane, much like with ethene.
  • The two pi bonds are oriented so that they are parallel to one another (see figure below). While the other pi bond is in front of and behind the page, the first pi bond is above and below the molecule's line as shown.
  • Sigma bonds are often the only kind of single bonding between atoms. A double bond is made up of one sigma bond and one pi bond. Triple bonds are made up of one sigma bonds and pi bonds.

To know more about Sigma bond   visit : https://brainly.com/question/27879143

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