Step 1: Definition of hybridization:
Hybridization is intermixing of atomic orbitals of different shapes and nearly the same energy to give the same number of orbitals of the same shape, equal energy and orientation such that there is minimum repulsion between these hybridized orbitals. The new orbitals thus formed are known as hybrid orbitals.
a)
CH3Cl
Step 1: Definition of hybridization:
Hybridization is intermixing of atomic orbitals of different shapes and nearly the same energy to give the same number of orbitals of the same shape, equal energy and orientation such that there is minimum repulsion between these hybridized orbitals. The new orbitals thus formed are known as hybrid orbitals.
Step 2: Lewis’s structure of the compound:
Draw the Lewis structure of given compound to visualize the number and types of bonds of each carbon atoms. After that number each carbon atoms to analyze the hybridization. Lewis’s structure of given molecular formula can be drawn as.
Step 3: Hybridization of carbon:
Carbon can make maximum
4 bonds
If all are sigma
σ bonds
⇒sp3 hybridisation
If
3 sigma and one
π bonds
⇒sp2 hybridisation
If
2 sigma and
2 π bonds
⇒sp hybridization.
∵ We know,
Single bond= Always sigma bond
Double bond=1σ bond +1π bond
Triple bond=1σ bond+2π bond
![](https://df0b18phdhzpx.cloudfront.net/ckeditor_assets/pictures/1643057/original_21.png)
There is only one carbon atom present in given molecular formula and according to structure, it is making
4 sigma bonds (single bond) with the help of one
s hybrid orbital
& 3p hybrid orbital. Hence, given carbon is
sp3 hybridized.
Final answer: Hybridisation of carbon is
sp3
(b)
(CH3)2CO
Step 1: Definition of hybridization:
Hybridization is intermixing of atomic orbitals of different shapes and nearly the same energy to give the same number of orbitals of the same shape, equal energy and orientation such that there is minimum repulsion between these hybridized orbitals. The new orbitals thus formed are known as hybrid orbitals.
Step 2: Lewis’s structure of the compound:
Draw the Lewis structure of given compound to visualize the number and types of bonds of each carbon atoms. After that number each carbon atoms to analyze the hybridization.
Lewis’s structure of given molecular formula can be drawn as.
Step 3: Hybridization of carbon: Carbon can make maximum
4 bonds.
If all are sigma
σ bonds
⇒sp3 hybridisation
If
3 sigma and one
π bonds
⇒sp2 hybridisation
If
2 sigma and
2 π bonds
⇒sp hybridization.
∵ We know,
Single bond= Always sigma bond
Double bond=1σ bond +1π bond
Triple bond=1σ bond+2π bond
![](https://df0b18phdhzpx.cloudfront.net/ckeditor_assets/pictures/1643130/original_22.png)
There are three carbon atoms present in given molecular formula and according to structure,
C1 and
C3 are making
4 sigma bonds (single bond) with the help of one
s hybrid orbital
& 3p hybrid orbital and
C2 making
3σ bonds
(3σ bond +1π bond) with the help of one
s hybrid orbital
& 2p hybrid orbital. Hence,
C1 and
C3 carbons are
sp3 and
C2 carbon is
sp2 hybridized.
Final answer: Hybridisation of carbons:
C1 C2 C3
sp3 sp2 sp3
(c)
CH3CN
Step 1: Definition of hybridization:
Hybridization is intermixing of atomic orbitals of different shapes and nearly the same energy to give the same number of orbitals of the same shape, equal energy and orientation such that there is minimum repulsion between these hybridized orbitals. The new orbitals thus formed are known as hybrid orbitals.
Step 2: Lewis’s structure of the compound:
Draw the Lewis structure of given compound to visualize the number and types of bonds of each carbon atoms. After that number each carbon atoms to analyze the hybridization.
Lewis’s structure of given molecular formula can be drawn as.
Step 3: Hybridization of carbon: Carbon can make maximum
4 bonds
If all are sigma
σ bonds
⇒sp3 hybridisation
If
3 sigma and one
π bonds
⇒sp2 hybridisation
If
2 sigma and
2 π bonds
⇒sp hybridization.
∵ We know,
Single bond= Always sigma bond
Double bond=1σ bond +1π bond
Triple bond=1σ bond+2π bond
![](https://df0b18phdhzpx.cloudfront.net/ckeditor_assets/pictures/1643185/original_23.png)
There are two carbon atoms present in given molecular formula and according to structure,
C1 is making
4 sigma bonds (single bond) with the help of one
s hybrid orbital
& 3p hybrid orbital and
C2 making
2σ bonds
(2σ bonds+2π bonds) with the help of one
s hybrid orbital
& one
p hybrid orbital.
Hence,
C1 is
sp3 and
C2 is
sp hybridized.
Final answer: Hybridisation of carbons:
C1 C2
sp3 sp
(d)
HCONH2
Step 1: Definition of hybridization:
Hybridization is intermixing of atomic orbitals of different shapes and nearly the same energy to give the same number of orbitals of the same shape, equal energy and orientation such that there is minimum repulsion between these hybridized orbitals. The new orbitals thus formed are known as hybrid orbitals.
Step 2: Lewis’s structure of the compound:
Draw the Lewis structure of given compound to visualize the number and types of bonds of each carbon atoms. After that number each carbon atoms to analyze the hybridization.
Lewis’s structure of given molecular formula can be drawn as.
Step 3: Hybridization of carbon: Carbon can make maximum
4 bonds
If all are sigma
σ bonds
⇒sp3 hybridisation
If
3 sigma and one
π bonds
⇒sp2 hybridisation
If
2 sigma and
2 π bonds
⇒sp hybridization.
∵ We know,
Single bond= Always sigma bond
Double bond=1σ bond +1π bond
Triple bond=1σ bond+2π bond
![](https://df0b18phdhzpx.cloudfront.net/ckeditor_assets/pictures/1643234/original_24.png)
There is only one carbon atom present in given molecular formula and according to structure, it is making
3 sigma bonds
(3σ bond+1π bond) with the help of
1s hybrid orbital
& 2p hybrid orbital. Hence, given carbon is
sp2 hybridized..
Final answer: Hybridisation of carbons is
sp2
(e)
CH3CH=CHCN
Step 1: Definition of hybridization:
Hybridization is intermixing of atomic orbitals of different shapes and nearly the same energy to give the same number of orbitals of the same shape, equal energy and orientation such that there is minimum repulsion between these hybridized orbitals. The new orbitals thus formed are known as hybrid orbitals.
Step 2: Lewis’s structure of the compound:
Draw the Lewis structure of given compound to visualize the number and types of bonds of each carbon atoms. After that number each carbon atoms to analyze the hybridization.
Lewis’s structure of given molecular formula can be drawn as.
Step 3: Hybridization of carbon: Carbon can make maximum
4 bonds.
If all are sigma
σ bonds
⇒sp3 hybridisation
If
3 sigma and one
π bonds
⇒sp2 hybridisation
If
2 sigma and
2 π bonds
⇒sp hybridization.
∵ We know,
Single bond= Always sigma bond
Double bond=1σ bond +1π bond
Triple bond=1σ bond+2π bond
![](https://df0b18phdhzpx.cloudfront.net/ckeditor_assets/pictures/1643259/original_24.png)
There are four carbon atoms present in given molecular formula and according to structure,
C1 making
4 sigma bonds (single bond) with the help of one
s hybrid orbital
& 3p hybrid orbital and
C2 and
C3 making
3σ bonds
(3σ bond +1π bond) with the help of one
s hybrid orbital
& 2p hybrid orbital while
C4 making
2σ bonds
(2σ bond +2π bond) with the help of one
s hybrid orbital and one
p hybrid orbital.
Hence,
C1 is
sp3,
C2,
C3 are
sp2 and
C4 is
sp hybridized.
Final answer: Hybridisation of carbons:
C1 C2 C3 C4
sp3 sp2 sp2 sp