The electronic configuration of in the excited state is:
In the formation of an ethane molecule , one hybrid orbital of carbon overlaps a hybridized orbital of another carbon atom, thereby forming a C-C sigma bond. The remaining two orbitals of each carbon atom form a sigma bond with two hydrogen atoms. The unhybridized orbital of one carbon atom undergoes sidewise overlap with the orbital of a similar kind present on another carbon atom to form a weak n-bond.
In the formation of molecule, each C-atom is sp hybridized with two 2p-orbitals in an unhybridized state. One sp orbital of each carbon atom overlaps with the other along the internuclear axis forming a c- c sigma bond. The second sp orbital of each C-atom overlaps a half- filled 1s-Orbital to form a bond.
The two unhybridized 2p-orbitals of the first carbon undergo sidewise overlap with the 2p orbital of another carbon atom, thereby two carbon atoms is made up of one sigma and two n-bonds.
Q: 28. What is the total number of sigma and pi bonds in the following molecules?
A single bond is a result of the axial overlap of bonding orbitals. Hence, it contributes a sigma bond. A multiple bond (double or triple bond) is always formed as a result of the sidewise overlap of orbitals. A pi-bond is always present in it. A triple bond is a combination of two pi-bonds and one sigma bond.
Structure of can be represented as:
Hence, there are three sigma and two pi-bonds in
The structure of can be represented as:
Hence, there are five sigma bonds and one pi-bond in
Q: 29. Considering x-axis as the internuclear axis which out of the following will not form a sigma bond and why?
orbitals will not a form a sigma bond. Taking X-axis as the internuclear axis,
orbitals will undergo lateral overlapping, thereby forming a pi bond.