explain the formation of ethylene molecule on the basis of hybridisation.
Answers
Answered by
19
BONDING IN ETHENE
Important! You will find this much easier to
understand if you first read the article about the
bonding in methane.
You may also find it useful to read the article on
orbitals if you aren't sure about simple orbital
theory.
Ethene, C 2H4
The simple view of the bonding in ethene
At a simple level, you will have drawn ethene
showing two bonds between the carbon atoms.
Each line in this diagram represents one pair of
shared electrons.
Ethene is actually much more interesting than
this.
An orbital view of the bonding in ethene
Ethene is built from hydrogen atoms (1s 1) and
carbon atoms (1s 22s 22p x 12p y 1).
The carbon atom doesn't have enough unpaired
electrons to form the required number of bonds,
so it needs to promote one of the 2s 2 pair into
the empty 2p z orbital. This is exactly the same
as happens whenever carbon forms bonds -
whatever else it ends up joined to.
So the first thing that happens is . . .
Promotion of an electron
There is only a small energy gap between the 2s
and 2p orbitals, and an electron is promoted from
the 2s to the empty 2p to give 4 unpaired
electrons. The extra energy released when these
electrons are used for bonding more than
compensates for the initial input.
Important! You will find this much easier to
understand if you first read the article about the
bonding in methane.
You may also find it useful to read the article on
orbitals if you aren't sure about simple orbital
theory.
Ethene, C 2H4
The simple view of the bonding in ethene
At a simple level, you will have drawn ethene
showing two bonds between the carbon atoms.
Each line in this diagram represents one pair of
shared electrons.
Ethene is actually much more interesting than
this.
An orbital view of the bonding in ethene
Ethene is built from hydrogen atoms (1s 1) and
carbon atoms (1s 22s 22p x 12p y 1).
The carbon atom doesn't have enough unpaired
electrons to form the required number of bonds,
so it needs to promote one of the 2s 2 pair into
the empty 2p z orbital. This is exactly the same
as happens whenever carbon forms bonds -
whatever else it ends up joined to.
So the first thing that happens is . . .
Promotion of an electron
There is only a small energy gap between the 2s
and 2p orbitals, and an electron is promoted from
the 2s to the empty 2p to give 4 unpaired
electrons. The extra energy released when these
electrons are used for bonding more than
compensates for the initial input.
Answered by
17
Heya...
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Question:- explain the formation of ethylene molecule on the basis of the hybridisation
Answer
Formation and structure of ethylene molecules on the basis of hybridisation
Ethylene and other organic compounds have C = C bond, 2s and two 2p orbitals of carbon atom undergoes sp2 hybridization.
In normal state the electronic configuration of carbon atom C(6) = ls2 2s2 2px1 2py1 2pz0
At excited state the electronic configuration is C*(6) = ls2 2s1 2px1 2py1 2pz1
After sp2 hybridization the electronic configuration is C*(6) = 1s2 ψ11 ψ21 ψ31 pz1
So, ψ1, ψ2, ψ3 are sp2 hybrid orbitals. Then are hybrid orbital of one carbon atom overlaps with one hybrid orbital of another carbon atom and thus form C-C sigma (σ) bond. Two other hybrid orbitals of each carbon atom overlap with 1s orbitals of two hydrogen atoms and thus form two C-H bonds with each carbon atom. Thus the main structure of ethylene can be constructed . Due to this SP2 hybridization, the bond anglesof this ethylene arc is about 120° and all these atoms are on a plane.or plane surface
Then the 2pz orbital on each carbon atom remains with one electron each. They overlap with each other sidewise to form one C-C pi-bond.
_____________________________________________________________
Hope it helps
___________________________________________________________
Question:- explain the formation of ethylene molecule on the basis of the hybridisation
Answer
Formation and structure of ethylene molecules on the basis of hybridisation
Ethylene and other organic compounds have C = C bond, 2s and two 2p orbitals of carbon atom undergoes sp2 hybridization.
In normal state the electronic configuration of carbon atom C(6) = ls2 2s2 2px1 2py1 2pz0
At excited state the electronic configuration is C*(6) = ls2 2s1 2px1 2py1 2pz1
After sp2 hybridization the electronic configuration is C*(6) = 1s2 ψ11 ψ21 ψ31 pz1
So, ψ1, ψ2, ψ3 are sp2 hybrid orbitals. Then are hybrid orbital of one carbon atom overlaps with one hybrid orbital of another carbon atom and thus form C-C sigma (σ) bond. Two other hybrid orbitals of each carbon atom overlap with 1s orbitals of two hydrogen atoms and thus form two C-H bonds with each carbon atom. Thus the main structure of ethylene can be constructed . Due to this SP2 hybridization, the bond anglesof this ethylene arc is about 120° and all these atoms are on a plane.or plane surface
Then the 2pz orbital on each carbon atom remains with one electron each. They overlap with each other sidewise to form one C-C pi-bond.
_____________________________________________________________
Hope it helps
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