How do sp hybridization takes place in chemistry?
Answers
Answered by
1
Hybridization was introduced to explain molecular structure when the valence bond theory failed to correctly predict them. It is experimentally observed that bond angles in organic compounds are close to 109o, 120o, or 180o. According to Valence Shell Electron Pair Repulsion (VSEPR) theory, electron pairs repel each other and the bonds and lone pairs around a central atom are generally separated by the largest possible angles.
Introduction
Carbon is a perfect example showing the need for hybrid orbitals. As you know, Carbon's ground state configuration is:

According to Valence Bond Theory, carbon should form two covalent bonds, resulting in a CH2, because it has two unpaired electrons in its electronic configuration. However, experiments have shown that CH2CH2 is highly reactive and cannot exist outside of a reaction. Therefore, this does not explain how CH4can exist. To form four bonds the configuration of carbon must have four unpaired electrons.
The only way CH4 it can be explained is is, the 2s and the 3 2p orbitals fused together to make four, equal energy sp3 hybrid orbitals. That would give us the following configuration:

Now that carbon has four unpaired electrons it can have four equal energy bonds. The hybridization of orbitals is also greatly favored because hybridized orbitals are lower in energy compared to their separated, unhybridized counterparts. This results in more stable compounds when hybridization occurs. Also, major parts of the hybridized orbitals, or the frontal lobes, overlap better than the lobes of unhybridized orbitals. This leads to better bonding.
The next section will explain the various types of hybridization and how each type helps explain the structure of certain molecules.
sp3 hybridization
sp3 hybridization can explain the tetrahedral structure of molecules. In it, the 2s orbitals and all three of the 2p orbitals hybridize to form four sp orbitals, each consisting of 75% p character and 25% s character. The frontal lobes align themselves in the manner shown below. In this structure, electron repulsion is minimized.
I hope it help you.....
Please mark me brainlist
And follow me....
Introduction
Carbon is a perfect example showing the need for hybrid orbitals. As you know, Carbon's ground state configuration is:

According to Valence Bond Theory, carbon should form two covalent bonds, resulting in a CH2, because it has two unpaired electrons in its electronic configuration. However, experiments have shown that CH2CH2 is highly reactive and cannot exist outside of a reaction. Therefore, this does not explain how CH4can exist. To form four bonds the configuration of carbon must have four unpaired electrons.
The only way CH4 it can be explained is is, the 2s and the 3 2p orbitals fused together to make four, equal energy sp3 hybrid orbitals. That would give us the following configuration:

Now that carbon has four unpaired electrons it can have four equal energy bonds. The hybridization of orbitals is also greatly favored because hybridized orbitals are lower in energy compared to their separated, unhybridized counterparts. This results in more stable compounds when hybridization occurs. Also, major parts of the hybridized orbitals, or the frontal lobes, overlap better than the lobes of unhybridized orbitals. This leads to better bonding.
The next section will explain the various types of hybridization and how each type helps explain the structure of certain molecules.
sp3 hybridization
sp3 hybridization can explain the tetrahedral structure of molecules. In it, the 2s orbitals and all three of the 2p orbitals hybridize to form four sp orbitals, each consisting of 75% p character and 25% s character. The frontal lobes align themselves in the manner shown below. In this structure, electron repulsion is minimized.
I hope it help you.....
Please mark me brainlist
And follow me....
raaj25:
Please mark me brainlist...
Please
Answered by
0
When one s orbital hybridizes with one p orbital,leaving 2 unhybridized orbitals,it is sp hybridization.
Similar questions