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Considering that the angles of a regular pentagon are 108º, why is cyclopentane not planar? A) all the carbons are sp 2 hybridized, so there is considerable angle strain. B) The C-C bonds are formed by overlap of p-orbitals, so the 90º angle results in large angle strain. C) The cyclic overlap of bonding orbitals results in anti-aromaticity destabilization. D) The five C-C bonds have eclipsing strain

Considering that the angles of a regular pentagon are 108º, why is cyclopentane not planar?
 A) all the carbons are sp2 hybridized, so there is considerable angle strain.
 B) The C-C bonds are formed by overlap of p-orbitals, so the 90º angle results in large angle strain.
 C) The cyclic overlap of bonding orbitals results in anti-aromaticity destabilization. 
 D) The five C-C bonds have eclipsing strain

Grade:11

1 Answers

NANDA
18 Points
8 years ago
It is D All bonds will be eclipsed if planar and therefore to relieve itslef of the torsional strain it becomes non planar

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