In the compound, CH2=CH-CH2-CH2-C ≡CH, the C2-C3 bond is of the type (a) s p-s p^2 (b) s p^3-5 p

Name: Problem 85, Chapter 23: A Complete Resource Book in Chemistry for JEE Main
Uploaded: 2021-09-11T20:05:18-08:00
Duration: 1 min 45 s
Channel: Vasu Makani
Description: In the compound, CH2=CH-CH2-CH2-C ≡CH, the C2-C3 bond is of the type (a) s p-s p^2 (b) s p^3-5 p^3 (c) sp-sp^3 (d) s p^2-s p^3

step 1 Hi, in this problem, we are given structure of an organic compound as shown here. Out of the giv

Question

In the compound, $\mathrm{CH}_{2}=\mathrm{CH}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{C} \equiv \mathrm{CH}$, the $\mathrm{C}_{2}-\mathrm{C}_{3}$ bond is of the type (a) $s p-s p^{2}$ (b) $s p^{3}-5 p^{3}$ (c) $\mathrm{sp}-\mathrm{sp}^{3}$ (d) $s p^{2}-s p^{3}$

   In the compound, $\mathrm{CH}_{2}=\mathrm{CH}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{C} \equiv \mathrm{CH}$, the
$\mathrm{C}_{2}-\mathrm{C}_{3}$ bond is of the type
(a) $s p-s p^{2}$
(b) $s p^{3}-5 p^{3}$
(c) $\mathrm{sp}-\mathrm{sp}^{3}$
(d) $s p^{2}-s p^{3}$

A Complete Resource Book in Chemistry for JEE Main

A.K. Singhal 3rd Edition

Chapter 23, Problem 85

Instant Answer

Solved by Expert Vasu Makani

09/11/2021

Step 1

According to the IUPAC rules, the carbon atom with the lowest number is the one that is substituted. In this compound, both terminal carbon atoms are substituted, so both could be given the number 1. However, the double bond gets higher priority than the triple Show more…

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In the compound, $\mathrm{CH}_{2}=\mathrm{CH}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{C} \equiv \mathrm{CH}$, the $\mathrm{C}_{2}-\mathrm{C}_{3}$ bond is of the type (a) $s p-s p^{2}$ (b) $s p^{3}-5 p^{3}$ (c) $\mathrm{sp}-\mathrm{sp}^{3}$ (d) $s p^{2}-s p^{3}$

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Key Concepts

Carbon Hybridization

Carbon atoms use hybrid orbitals (sp3, sp2, sp) to form bonds in organic molecules. The type of hybridization affects both the geometry around the carbon atom and the number and type of bonds it can form, such as single, double, or triple bonds.

Sigma and Pi Bonds

A sigma bond is formed through the head?on overlap of hybrid orbitals and establishes the primary framework of a molecule, while a pi bond arises from the sideways overlap of unhybridized p orbitals. In multiple bonds, the sigma component holds the atoms together, and the additional pi bond(s) provide extra bonding strength.

Orbital Overlap in Bond Formation

For a stable covalent bond to form, the orbitals of the bonding atoms must have compatible geometries and phases. Even when two carbons have different hybridizations—such as sp2 and sp3—their hybrid orbitals can overlap end-to-end to form a sigma bond, which is key to determining the nature of the bond between them.

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