According to valence bond theory, which atomic orbitals of carbon may be hybridized to account for bonding? Why? .
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

C. Only 2s and 2p may hybridize; these orbitals contain valence electrons used in bonding.

Explanation:

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).

199.26 or with sig figs 2.0 x 10^2

Explanation: you take the # of molecules and divide it by avagadros number which is 6.022141 x 10^23