Question

Which statement explains why the theory of orbital hybridization is important to our understanding of chemical bonding?

 

1-Hybridization provides a theory in which orbitals are not localized on specific atoms.

 

2-Lewis structures do not depict hybridization, so another theory was required.

 

3-There are not enough atomic orbitals to explain experimentally observed molecular shapes.

 

4-Use of atomic orbitals to describe bonding in some molecules does not result in the experimentally observed bond angles.

Answer 1

Answer = option 4

Use of atomic orbitals to describe bonding in some molecules does not result in experimentally observed bond angles.

Hybridization is introduced to explain the geometry of bonding orbitals in valance bond theory.Hybridization is a concept of general chemistry, it is used in both organic and inorganic one. Its relatively big importance for organic chemistry is due to the fact that it is the only simple model which can explain (approximately) molecular geometry of organic compounds

How does the carbon form four bonds if it has only two half-filled p orbitals available for bonding? A hint comes from the experimental observation that the four C-H bonds in methane are arranged with tetrahedral geometry about the central carbon, and that each bond has the same length and strength. In order to explain this observation, valence bond theory relies on a concept called orbital hybridization. In this picture, the four valence orbitals of the carbon (one 2s and three 2p orbitals) combine mathematically (remember: orbitals are described by equations) to form four equivalent hybrid orbitals, which are named sp3 orbitals because they are formed from mixing one s and three p orbitals. In the new electron configuration, each of the four valence electrons on the carbon occupies a single sp3 orbital.