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Chapter 10: Problem 13

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

Short Answer

Expert verified
The first Carbon atom (from left) in the \(\mathrm{CH}_{3} \mathrm{COOH}\) molecule exhibits a tetrahedral geometry. The second Carbon atom (from right) exhibits a trigonal planar geometry. The Oxygen atom in the \(\mathrm{OH}\) group exhibits a bent or V-shaped geometry.

Step by step solution

01

Draw the Lewis Structure

Start by drawing the Lewis structure of the acetic acid \(\mathrm{CH}_{3} \mathrm{COOH}\) molecule. The molecule consists of 2 central Carbon (C) atoms, 4 Hydrogen (H) atoms and 2 Oxygen (O) atoms, one of which is attached to a Hydrogen atom forming a Hydroxyl group. After drawing the lewis structure, you can see that one Carbon atom is bonded to three Hydrogen atoms and the other Carbon atom. The second Carbon atom is bonded to an Oxygen atom and the Hydroxyl group.
02

Understand the Geometry of the First Carbon Atom

Looking at the first Carbon atom (from left), you would find that there are three sigma bonds with Hydrogen atoms and one sigma bond with the other Carbon atom. According to the VSEPR theory, four electron regions (four sigma bonds in this case) result in a tetrahedral geometry. Therefore, the geometry around the first Carbon atom is tetrahedral.
03

Understand the Geometry of the Second Carbon Atom

Now, considering the second Carbon atom (from right), you would see that there are sigma bonds with the first Carbon atom, with one Oxygen atom and the Hydroxyl group. According to the VSEPR theory, three atom regions result in a trigonal planar geometry. Therefore, the geometry around the second Carbon atom is trigonal planar.
04

Understand the Geometry of the Oxygen Atom

The Oxygen atom in the Hydroxyl group is bonded to the Carbon atom and a Hydrogen atom and has two lone pairs. According to the VSEPR theory, two bonding pairs and two lone pairs result in a bent or V-shaped geometry. Therefore, the geometry around the Oxygen atom in \(\mathrm{OH}\) is bent or V-shaped.

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Most popular questions from this chapter

Predict the geometry of sulfur dichloride \(\left(\mathrm{SCl}_{2}\right)\) and the hybridization of the sulfur atom.

The allene molecule \(\mathrm{H}_{2} \mathrm{C}=\mathrm{C}=\mathrm{CH}_{2}\) is linear (the three \(\mathrm{C}\) atoms lie on a straight line \() .\) What are the hybridization states of the carbon atoms? Draw diagrams to show the formation of sigma bonds and pi bonds in allene.

For each pair listed here, state which one has a higher first ionization energy and explain your choice: (a) \(\mathrm{H}\) or \(\mathrm{H}_{2},\) (b) \(\mathrm{N}\) or \(\mathrm{N}_{2},\) (c) \(\mathrm{O}\) or \(\mathrm{O}_{2},\) (d) \(\mathrm{F}\) or \(\mathrm{F}_{2}\).

Describe the hybridization of phosphorus in \(\mathrm{PF}_{5}\).

Draw the Lewis structure for the \(\mathrm{BeCl}_{4}^{2-}\) ion. Predict its geometry and describe the hybridization state of the Be atom.
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