According to valence bond theory, which atomic orbitals of carbon may be hybridized to account for bonding? Why?
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A. Only 2p orbitals may hybridize; the 2p orbital is carbon’s highest-energy atomic orbital.
B. Only 1s and 2s orbitals of carbon may hybridize; each contains electrons to share in bonding.
C. Only 2s and 2p may hybridize; these orbitals contain valence electrons used in bonding.
D. Only 2s orbitals may hybridize; these orbitals contain valence electrons.
E. 1s, 2s, and 2p orbitals all may hybridize; these orbitals are of the same phase

Carbon has four valence electrons (2s² 2p²), in several organic compounds it forms four bonds and as this element has two types of orbitals to join, 2s and 2p, it is expected that a compound like methane has two types of C-H bonds, but this is not the case, as all its orbital atoms are the same.

In a process called hybridization, s orbitals and p orbitals are combined in an atom. Depending on the amount of p orbitals that are combined, the hybrid orbitals can be sp (one orbital 2s and one 2p are combined), sp² (the 2s orbital combines with two 2p orbitals) and sp³(the orbital 2s combines with three 2p orbitals).

shrutiagrawal1798 shrutiagrawal1798 · Answer 2 · 2022-03-11T11:08:58+01:00

The carbon atom has the presence of 6 electrons. The valence bond theory hybridized the 2s and 2p orbital for the bonding, as they have valence bonds.

What is valence bond theory?

The valence bond theory has been the atomic hybridization of the atoms that results in the formation of the bonds.

The carbon atom has 4 valence electrons present in the bonding valence orbitals. The orbitals combine as sp, sp2, sp3 orbital in order to form the bond.

Thus, since there has been the presence of valence electrons in the s and p orbitals, the 2s and 2p are involved in the hybridization. Hence, option C is correct.

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