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Chapter 10: Problem 11

Describe the geometry around each of the three central atoms in the \(\mathrm{CH}_{3} \mathrm{COOH}\) molecule.

Short Answer

Expert verified
The geometry around the first C atom in the \(\mathrm{CH}_{3} \mathrm{COOH}\) molecule is tetrahedral, around the second C atom is trigonal planar, and around the O atom is bent or V-shaped.

Step by step solution

01

Identify the central atoms

The \(\mathrm{CH}_{3} \mathrm{COOH}\) molecule has three central atoms: the C in \(\mathrm{CH}_{3}\), the C in \(\mathrm{COOH}\), and the O in \(\mathrm{COOH}\). It is necessary to examine each central atom separately.
02

Determining geometry around the first C atom

The first C atom (in \(\mathrm{CH}_{3}\)) is bonded to three H atoms and to the second C atom (in \(\mathrm{COOH}\)). It has no lone pairs of electrons, meaning it has a total of 4 electron groups. This is consistent with the tetrahedral geometry, which has bond angles of approximately \(109.5^\circ\).
03

Determining geometry around the second C atom

The second C atom (in \(\mathrm{COOH}\)) is bonded to the first C atom, to an O atom via a double bond and to another O atom via a single bond. It has no lone pairs of electrons and a total of 3 electron groups. This corresponds to a trigonal planar geometry, having bond angles of approximately \(120^\circ\).
04

Determining geometry around the O atom

The O atom (in \(\mathrm{COOH}\)) bonded to the hydrogen atom and to the second C atom, and it also has two lone pairs of electrons, making a total of 4 electron groups around it. This suggests a bent (or V-shaped) geometry, considering that the lone pairs will distort standard bond angles to be less than \(109.5^\circ\).

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Most popular questions from this chapter

Compare the Lewis and molecular orbital treatments of the oxygen molecule.

Specify which hybrid orbitals are used by carbon atoms in these species: (a) \(\mathrm{CO},\) (b) \(\mathrm{CO}_{2},\) (c) \(\mathrm{CN}^{-}\).

What is the relationship between the dipole moment and bond moment? How is it possible for a molecule to have bond moments and yet be nonpolar?

Draw Lewis structures and give the other information requested for the following molecules: (a) \(\mathrm{BF}_{3}\). Shape: planar or nonplanar? (b) \(\mathrm{ClO}_{3}^{-}\). Shape: planar or nonplanar? (c) \(\mathrm{H}_{2} \mathrm{O}\). Show the direction of the resultant dipole moment. (d) \(\mathrm{OF}_{2}\). Polar or nonpolar molecule? (e) \(\mathrm{SeO}_{2}\). Estimate the OSeO bond angle.

Consider the reaction $$ \mathrm{BF}_{3}+\mathrm{NH}_{3} \longrightarrow \mathrm{F}_{3} \mathrm{~B}-\mathrm{NH}_{3} $$ Describe the changes in hybridization (if any) of the \(B\) and \(N\) atoms as a result of this reaction
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