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Chapter 8: Q3 CYL (page 424)

Acetic acid, H3CC(O)OH, is the molecule that gives vinegar its odor and sour taste. What is the hybridization of the two carbon atoms in acetic acid?

Short Answer

Expert verified

The sp3d hybridization of H3C and sp2 of C(O)OH.

Step by step solution

01

Define hybridization

Hybridization is a concept in organic chemistry that is used to explain chemical bonding when the valence bond theory fails to provide an adequate explanation. This hypothesis is particularly useful for explaining organic molecules' covalent bonding.

02

Explanation

The hybridization in H3C is sp3 and C(O)OH is sp2.


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Most popular questions from this chapter

For the first ionization energy for an \({{\rm{N}}_2}\) molecule, what molecular orbital is the electron removed from?

Sulfuric acid is manufactured by a series of reactions represented by the following equations:

\(\begin{array}{l}{{\rm{S}}_{\rm{8}}}{\rm{(s) + 8}}{{\rm{O}}_{\rm{2}}}{\rm{(g)}} \to {\rm{8S}}{{\rm{O}}_{\rm{2}}}{\rm{(g)}}\\{\rm{2S}}{{\rm{O}}_{\rm{2}}}{\rm{(g) + }}{{\rm{O}}_{\rm{2}}}{\rm{(g)}} \to {\rm{2S}}{{\rm{O}}_{\rm{3}}}{\rm{(g)}}\\{\rm{S}}{{\rm{O}}_{\rm{3}}}{\rm{(g) + }}{{\rm{H}}_{\rm{2}}}{\rm{O(l)}} \to {{\rm{H}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}{\rm{(l)}}\end{array}\)

Draw a Lewis structure, predict the molecular geometry by VSEPR, and determine the hybridization of sulfur for the following:

(a) circular \({{\rm{S}}_{\rm{8}}}\)molecule

(b) \({\rm{S}}{{\rm{O}}_{\rm{2}}}\)molecule

(c) \({\rm{S}}{{\rm{O}}_{\rm{3}}}\)molecule

(d) \({{\rm{H}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}\)molecule (the hydrogen atoms are bonded to oxygen atoms)

Calculate the bond order for an ion with this configuration: \({\left( {{{\bf{\sigma }}_{{\bf{2s}}}}} \right)^{\bf{2}}}{\left( {{\bf{\sigma }}_{{\bf{2s}}}^{\bf{*}}} \right)^{\bf{2}}}{\left( {{{\bf{\sigma }}_{{\bf{2px}}}}} \right)^{\bf{2}}}{\left( {{{\bf{\pi }}_{{\bf{2py}}}}{\bf{,}}{{\bf{\pi }}_{{\bf{2pz}}}}} \right)^{\bf{4}}}{\left( {{\bf{\pi }}_{{\bf{2py}}}^{\bf{*}}{\bf{,\pi }}_{{\bf{2pz}}}^{\bf{*}}} \right)^{\bf{3}}}\).

Why is the concept of hybridization required in valence bond theory?

Write Lewis structures for \({\rm{N}}{{\rm{F}}_{\rm{3}}}\) and \({\rm{P}}{{\rm{F}}_{\rm{5}}}\). On the basis of hybrid orbitals, explain the fact that \({\rm{N}}{{\rm{F}}_{\rm{3}}}\), \({\rm{P}}{{\rm{F}}_{\rm{3}}}\), and \({\rm{P}}{{\rm{F}}_{\rm{5}}}\) are stable molecules, but \({\rm{N}}{{\rm{F}}_{\rm{5}}}\) does not exist.
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