Carbon on the left is the highlighted atom. Answer the questions below about the highlighted atom…
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Question “Carbon on the left is the highlighted atom. Answer the questions below about the highlighted atom…”
Answer
1. Sigma bonds are single bonds that result from the overlap of two orbitals of two atoms. They form bonds along the internuclear direction. A sigma bond is a simple single bond.
The highlighted atom is represented as:
The highlighted atom is part of 4 sigma bonds.
2. Sideways overlap of the orbitals of two atoms creates a pi bond. Multiple bonds can form a pi bond. One bond is always a Sigma bond, while the other/s are pi bonds. In a double bond between two atoms, one bond is the Sigma bond while the other is a Pi bond. A triple bond between two atoms is one of three. The other two bonds are pi bonds.
The highlighted atom is not part of any pi bond because there are no double or three-bonded around it. The highlighted atom only has single bonds, which are all sigma bond. The highlighted atom is therefore a member of 0 pi bonds.
3. You can either sp, or sp 2 hybridize carbon.
When all four valence orbitals of carbon ( one 2s and three 2p) hybridise to form four sigma bonds around carbon then it is sp3 hybridisation.
If only three of the four valence orbitals for carbon combine to form three sigma bonds, and one of the three 2p orbitals remains unhybridised for sideways overlapping to form a pi-bond, or is vacant or has a single pair of electrons, then the carbon atom is considered to have sp hybridisation.
If only 2 of 4 valence orbitals of carbon combine to form 2 Sigma bonds, and 2 of 3 2p orbitals are unhybridized to form pi bonds, or remain empty or contain one pair of electrons, then carbon is sp hybridization.
The highlighted atom, which is carbon, has four sigma bonds around its surface so it can be sp hybridized.
The orbital hybridization of the highlighted atom thus becomes sp 3
Conclusion
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