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Chapter 6: Problem 1

\(\mathrm{CO}_{2}\) Answer: First draw a dot diagram, then examine it via VSEPR: Draw a dot diagram: Apply VSEPR: Determine the molecule's shape: There are two electron The molecule groups \(180^{\circ}\) apart around is linear. the central \(C\) atom. \((S N=2)\)

Short Answer

Expert verified
The molecular geometry of the CO2 molecule is determined by drawing its Lewis structure, which shows a central Carbon atom double-bonded to two Oxygen atoms. Applying the VSEPR theory reveals that there are two electron groups around the central Carbon atom, causing them to be \(180^{\circ}\) apart. Therefore, the molecular geometry of CO2 is linear.

Step by step solution

01

Draw the Lewis Structure

First, we need to draw the Lewis structure of the CO2 molecule, which will help us determine the positions of the atoms and the electron pairs around the central atom (Carbon). The molecule has two Oxygen atoms bonded to the central Carbon atom. Carbon has 4 valence electrons, and Oxygen has 6 valence electrons, making a total of 16 electrons in the molecule. The Lewis structure of CO2 is as follows: O=C=O In this Lewis structure: - The central Carbon atom is double-bonded to each of the two Oxygen atoms. - Each Oxygen atoms have two lone pairs of electrons.
02

Apply the VSEPR Theory

Now we will apply the VSEPR theory to determine the arrangement of electron pairs around the central Carbon atom in the CO2 molecule. In VSEPR theory, the electron pairs around an atom repel each other, so they try to stay as far apart as possible. The bonding pairs (shared by atoms) and lone pairs (not bonded but attached to an atom) around the central atom will define its electron pair geometry. In CO2, the central Carbon atom has two bonding pairs and no lone pairs. We will consider the bonding pairs as electron groups.
03

Determine the Molecule's Shape

Using VSEPR theory, the molecular geometry is determined by the electron groups around the central Carbon atom. In the CO2 molecule, there are two electron groups, so they try to stay as far apart as possible according to VSEPR theory. They will be \(180^{\circ}\) apart, which means the CO2 molecule has a linear geometry. This explains why the Carbon atom is double-bonded to each of the two Oxygen atoms in a straight line. So, the molecular geometry of the CO2 molecule is linear.

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Most popular questions from this chapter

White phosphorus, \(\mathrm{P}_{4}\), consists of four phosphorus atoms, with each atom bonded to the other three. Draw the three-dimensional shape of this molecule, showing all valence electrons and bond angles. (Hint: Begin by drawing one atom bonded to the three others using VSEPR theory, and then make the remaining connections.)

What do we mean by intermolecular forces? What evidence is there that they exist?

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Consider the molecule \(\mathrm{N}_{2} \mathrm{O}\) (connected \(\mathrm{N}-\mathrm{N}-\mathrm{O})\) (a) Draw the dot diagram. (b) Draw the molecule's three-dimensional shape, and label the numeric value of all bond angles. (c) What is the shape of this molecule? (d) Draw in the individual bond dipole moments. (e) Is the molecule polar? If yes, draw the molecular dipole moment vector.

One student claims \(\mathrm{XeF}_{4}\) will be polar. Another claims it will be nonpolar. Which is right, and why?
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