For the 3d molecular structure of allene, how come there is no wedge and dash on the right side? The explanation given by the textbook does not make sense to me. If there are two double bonds, why does one side have to be perpendicular to the other? 1-20 Carbon-2 is sp hybridized. If the p orbitals making the pi bond between C-1 and C-2 are in the planeof the paper (putting the hydrogens in front of and behind the paper), then the other p orbital on C-2 mustbe perpendicular to the plane of the paper, making the pi bond between C-2 and C-3 perpendicular to thepaper. This necessarily places the hydrogens on C-3 in the plane of the paper. (Models will surely help.)HH,2EC=CH3model ofH.perpendicular ri bondssp14

When two parallel orbitals are overlapped with each other, pi (π) bond forms.

For the 3d molecular structure of allene, how come there is no wedge and dash on the right side? The explanation given by the textbook does not make sense to me. If there are two double bonds, why does one side have to be perpendicular to the other?

For the 3d molecular structure of allene, how come there is no wedge and dash on the right side? The explanation given by the textbook does not make sense to me. If there are two double bonds, why does one side have to be perpendicular to the other?

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter4: Polar Bonds, Polar Reactions

Section: Chapter Questions

Problem 27E

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