Pi Bonds Cannot Rotate

[Inderpal Singh 2L]

Why can Pi Bonds not Rotate? I cannot visualize it properly.

[Leo Naylor 2F]

Pi bonds cannot rotate because they are p-orbitals overlapping side-by-side, so that both electron density areas are "touching." Hope this helps.

[Jagveer 1I]

To add on, for the molecule to rotate about the double bond, the π-bond would need to break and then reform. It is not possible for a π-bond to remain intact and rotate.

[SahajDole_1C]

Pi bonds cannot rotate because the p orbitals overlap and cause a double bond which is more stronger and thus it cannot rotate

[Melis Kasaba 2B]

For a pi bond, there has to be a parallel orientation of the p orbitals so they overlap. If the bond were to rotate, that would break it.

[BKoh_2E]

Here is an image that may help you visualize it!

[105618850]

Pi bonds overlap parallel to one another meaning that rotation is not possible. If there was any form of rotation, the bond would be broken as a result.

[Navdha Sharma 3J]

Pi-bonds overlap side-by-side. If they rotate, they will break. Hence, pi bonds do not rotate.

[Annette Fishman]

Rotation around a single bond occurs readily, while rotation around a double bond is restricted. The pi bond prevents rotation because of the electron overlap both above and below the plane of the atoms.

[Jason Knight - 1F]

Pi bonds are present in double and triple bonded molecules. For example, a double bond has one pi bond and a triple bond has two pi bonds. Pi bonds cannot rotate because that would require the break of the parallel orientation of the p-orbitals.

[apurva-3E]

They cannot rotate because there are p orbitals overlapping side by side. Try to visualize this in your head after looking at a picture of the pi bond.

[David Y]

if the bond were to rotate it would break because they are parallel

[Chance Herbert 3A]

I remember in Dr. Lavelle's lecture on types of bonds he held a marker in his hands parallel to demonstrate how pi bonds do not allow for rotation. If rotation were to occur, the bond would have to be broken which was represented by the marker falling from his hands. I am totally visual as well and I feel like this video gives a great representation if you are still struggling! Hope this helps! https://www.youtube.com/watch?v=7tH8Xe5u8A0

[Tatyana Bonnet 2H]

They don't rotate because they are connected side by side, if one atom were to rotate they would no longer be side to side breaking the pi bond. Therefore, pi bonds keep a structure in its plane unless broken.

[Joel Meza 3I]

This picture does a pretty good job at showing how a pi bond would break.

[Nathaly Cruz 2D]

When rotating, would the pi bond break because it is no longer parallel?

[Caelin Brenninkmeijer 1G]

When rotating, would the pi bond break because it is no longer parallel?

Correct! Pi bonds don't allow atoms to rotate, so if the atom is no longer parallel, there is no pi bond. This is because pi bonds have electron densities on each side of the internuclear axis, preventing the bond to exist if the atoms bonded are not 180º.

[David Facio 3C]

Think of it like the base you make when you lock arms with another person to give your friend a boost over a fence. If one of the persons serving as the base tried rotating their arms, it would be less stable, and under pressure, the base would break. Similarly, Pi bonds can't rotate, or else they'd simply break.

[LovepreetSran_3H]

Pi-bonds overlap in a parallel, making it unable to rotate.

[Hannah Lechtzin 1K]

Pi bonds rely on two p orbitals overlapping side by side. Think of two figure eights overlapping long side to long side. If one of those two figure eights were to turn, then they would no longer overlap side to side. If this occurs with two p-orbitals the bond breaks so pi bonds cannot rotate.

[Gian Boco 2G]

In a pi bond orbitals are overlapping outside of the intermolecular axis. Thus, rotating the bond about that axis would break the pi bond. On the other hand, sigma bonds overlap along this axis and thus allowing rotation.

[Charlie Russell 2L]

The two p-orbitals overlap. Think of a LADDER. You cannot move 1 ring of the ladder without moving the other unless you break it (the bond breaks).

[Nathaly Cruz 2D]

When rotating, would the pi bond break because it is no longer parallel?

Correct! Pi bonds don't allow atoms to rotate, so if the atom is no longer parallel, there is no pi bond. This is because pi bonds have electron densities on each side of the internuclear axis, preventing the bond to exist if the atoms bonded are not 180º.

Thank you for the explanation :)

[America Ramirez 3H]

you basically have two regions of the p-orbital overlapping and you cant rotate one without rotating another and thus breaking the pi bond.

[Aditya Desai 1A]

that's why at high temperatures, you have cis-trans isomerization (the high temperature breaks the pi bond and the molecule rotates around the sigma bond)

[Wenhan Li_3d]

there are two p orbital overlapping and parrallel to each other so you can not rotate on without breaking the other one.

[Milli Zunich 3I]

If it helps visualize, I sometimes think of it like one of those plastic rulers from elementary school. If you try to twist it to make the ends meet, the whole thing shatters. Not saying molecules can shatter, but you get the gist.

[Michelle Argueta 1E]

Pi bonds are unable to rotate due to the orientation of overlapping in a parallel manner; making one atom rotate would break symmetry of side by side and cause the bond between them to break.

[Nishan Reddy 3K]

Since they are just p orbitals that are next to each other interacting, they do not rotate

[905767718]

Since pi bonds are placed on top of each other, I imagine it as two eclairs that are glued to each other and since they are each bound to atoms but also to each other, the only way they can move is if they separate. This means that they can only rotate if their bond is broken.