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Electronegativity and Hybridisation

Double bonds ...

Question

Double bonds between carbon $(C)$ atoms is due to overlapping of two p-orbitals forming:

A

sigma bond

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B

pi bond

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C

ionic bond

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D

co-ordinate bond

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Solution

The correct option is B pi bond
A pi bond is formed by lateral (sideways) overlap of orbitals. Whereas a sigma bond is obtained by axial (head-on) overlap of orbitals.
Double bonds between carbon $(C)$ atoms is due to overlapping of two p-orbitals forming a pi bond.

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Similar questions

Q. When a double bond is formed between two atoms, one of the bonds is a sigma bond and the other is a pi bond. The pi bond is created by the overlap of:

Q. The formation of a double bond in an oxygen molecule is explained below. Arrange the given points in a sequential order.
(a) 2p

_{y}

orbitals of each oxygen atom overlap laterally/sidewise to form a pi bond.
(b) Thus, a double bond between two oxygen atoms in which one p

_{z}

_{z}

sigma bond and p

_{y}

_{y}

π

bond is formed.
(c) All the three 2p orbitals are perpendicular to each other. Hence 2p

_{z}

orbitals of each oxygen atom overlap end to end to form a sigma bond.
(d) The electronic configuration of oxygen is

O

^{2}

^{2}

_{x}^{1}

_{y}^{2}

_{z}^{1}

Q. Linear overlapping of any two pure atomic p - orbitals lead to sigma bond formation.

Q. Assertion :The carbon-carbon double bond energy in

C_{2} H_{4}

is more than the carbon-carbon single bond energy in

C_{2} H_{6}

σ

-orbital has greater electron overlap between the atoms because its component

σ

-orbitals are directed toward each other, whereas the component

π

-orbitals making-up the

π

-orbital are directed perpendicular to the inter-nuclear axis.

Q. Assertion :Formation of a pi bond restricts the rotation of the bond. Reason: While rotating the double bond, the perpendicular laterally overlapped p orbitals will reach non overlapping position.

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