Problem 60
Page 425
Section: Cumulative Problems
Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory,and Molecular Orbital Theory
Given information
Given compound has the molecular formula 
.
This compound has two double bonds.
Step-by-step explanation
The valence bond electronic configuration of carbon and hydrogen is as follows:
According to the configuration, it is seen that Carbon can form only two bonds because there are two unpaired electrons in its p-orbital. But this does not happen.
According to valence bond theory, the s and p -orbital of carbon are hybridized and form four hybrid orbital. Therefore, it can form four bonds.
Case (I): When the hybridization is 
.
In the above image, the unhybridized p-orbital of carbon forms one pi-bond.
Case(II): When the hybridization is 
.
In the above image, the two unhybridized p-orbital of carbon form two pi-bonds.
Case (III): When the hybridization is 
In the above image, there is no unhybridized p-orbital so all the bonds are sigma bonds. There is no pi-bond.
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This problem is similar to
Principles of Chemistry Molecular Approach
Chemistry: A Molecular Approach
Chemistry: Structure and Properties
