Solveeit Logo
Login

Question

Question: In the organic compound \(C{H_2} = CH - C{H_2} - C{H_2} - C \equiv CH\), the pair of hybridized orbi...

In the organic compound CH2=CH−CH2−CH2−C≡CHC{H_2} = CH - C{H_2} - C{H_2} - C \equiv CH, the pair of hybridized orbitals involved in the formation of C2−C3{C_2} - {C_3} is:

Explanation

Solution

We have to know that the formation of a similar number of orbitals containing the same properties of different kinds of orbitals (s and p) of carbon atom is known as hybridization and orbitals produced are called hybridized orbitals.

Complete step by step answer:
We have to know that sigma bonds are formed by hybrid orbitals of carbon form and those orbitals which do not participate in hybridization to form pi (p) bonds.
A sigma bond is always a single bond. One sigma and one pi bond are found in double bonds. One sigma and two pi bonds are found in triple bonds. Based on the number of sigma bonds in an atom of carbon, we can determine its hybridization.
In −C−C - C - C bond, the type of hybridization on the carbon atom is sp3s{p^3}.
In >C=C<> C = C < bond, the type of hybridization on the carbon atom is sp2s{p^2}.
In −C≡C−- C \equiv C - bond, the type of hybridization on the carbon atom is spsp.
Let us now number the carbon atoms in the given structure.
The given structure is,
CH2=CH−CH2−CH2−C≡CHC{H_2} = CH - C{H_2} - C{H_2} - C \equiv CH
We can give the numbered structures as,
C1H2=C2H−C3H2−C4H2−C5≡C6H\mathop C\limits^1 {H_2} = \mathop C\limits^2 H - \mathop C\limits^3 {H_2} - \mathop C\limits^4 {H_2} - \mathop C\limits^5 \equiv \mathop C\limits^6 H
We know that, when double and triples are found at equivalent positions, we have to give preference to the double bond when we numbered the carbon chain.
We can give the hybridization on each carbon as,
The hybridization on carbon one is sp2s{p^2}.
The hybridization on carbon two is sp2s{p^2}.
The hybridization on carbon three is sp3s{p^3}.
The hybridization on carbon four is sp3s{p^3}.
The hybridization on carbon five is spsp.
The hybridization on carbon six is spsp.
C1H2=C2H−C3H2−C4H2−C5≡C6H sp2 sp2 sp3 sp3 sp sp  \mathop C\limits^1 {H_2} = \mathop C\limits^2 H - \mathop C\limits^3 {H_2} - \mathop C\limits^4 {H_2} - \mathop C\limits^5 \equiv \mathop C\limits^6 H \\\ {\text{s}}{{\text{p}}^2}{\text{ s}}{{\text{p}}^2}{\text{ s}}{{\text{p}}^3}{\text{ s}}{{\text{p}}^3}{\text{ sp sp}} \\\
We can see that the pair of hybridized orbitals involved in the formation of C2−C3{C_2} - {C_3} bond is sp2−sp3s{p^2} - s{p^3}.
In the compound CH2=CH−CH2−CH2−C≡CHC{H_2} = CH - C{H_2} - C{H_2} - C \equiv CH, sp2−sp3s{p^2} - s{p^3} is the pair of hybridized orbitals that is involved in the formation of C2−C3{C_2} - {C_3} bond.

Note:
We know that the geometry of the molecule depends on the hybridization.
If a compound contains single bonds, then it is sp3s{p^3} hybridized. Example for sp3s{p^3} hybridized molecule is methane. Generally, alkanes come under sp3s{p^3} hybridization. Molecules that have sp3s{p^3} hybridization will have tetrahedral geometry.
If a compound contains double bonds, then it is sp2s{p^2} hybridized. Example for sp2s{p^2} hybridized molecule is ethene. Generally, alkenes come under sp2s{p^2} hybridization. Molecules that have sp2s{p^2} hybridization will have trigonal planar geometry.
If a compound contains triple bonds, then it is spsp hybridized. Example for spsp hybridized molecule is ethyne. Generally, alkynes come under spsp hybridization.