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Chapter 10: Problem 76

The compounds carbon tetrachloride \(\left(\mathrm{CCl}_{4}\right)\) and silicon tetrachloride \(\left(\mathrm{SiCl}_{4}\right)\) are similar both in geometry and hybridization. However, \(\mathrm{CCl}_{4}\) does not react with water but \(\mathrm{SiCl}_{4}\) does. Explain the difference in their chemical reactivities. (Hint: The first step of the reaction is believed to be the addition of a water molecule to the Si atom in \(\mathrm{SiCl}_{4}\).)

Short Answer

Expert verified
\(CCl_{4}\) is nonpolar and does not react with water, which is polar. On the other hand, \(SiCl_{4}\) is polar and can react with water. The first step of the reaction between \(SiCl_{4}\) and water involves the addition of a water molecule to the silicon atom, explaining the difference in chemical reactivities of \(CCl_{4}\) and \(SiCl_{4}\).

Step by step solution

01

Understanding the Problem

We're trying to understand why \(CCl_{4}\) and \(SiCl_{4}\) react differently with water, even though they're similar both in terms of their geometry and hybridization. This difference in reaction will be related to the properties and structures of these two compounds. We need to compare their bonds and interactions with water.
02

Structure and Properties of \(CCl_{4}\) and \(SiCl_{4}\)

Both \(CCl_{4}\) and \(SiCl_{4}\) have a tetrahedral structure because of the hybridization of the central atom. Their polarities are determined by the electronegativity of the central atom and the atoms around it. In \(CCl_{4}\), carbon and chlorine have similar electronegativities, resulting in nonpolar bonds and a nonpolar molecule overall. On the other hand, in \(SiCl_{4}\), silicon is less electronegative than chlorine, resulting in polar bonds and a polar molecule overall.
03

Reactivity with Water

Based on Step 1 and 2, we can deduce that the reactions of these two compounds with water are very different because water is a polar compound. In the case of \(SiCl_{4}\), the polar \(Si-Cl\) bonds can interact with the polar \(H_{2}O\) molecules, facilitating the reaction. In contrast, the nonpolarity of \(CCl_{4}\) causes it to be unreactive with polar molecules like water. Thus the \(SiCl_{4}\) will react with water, while the \(CCl_{4}\) will not.

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Most popular questions from this chapter

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

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.

Assume that the third-period element phosphorus forms a diatomic molecule, \(\mathrm{P}_{2}\), in an analogous way as nitrogen does to form \(\mathrm{N}_{2}\). (a) Write the electronic configuration for \(\mathrm{P}_{2}\). Use \(\left[\mathrm{Ne}_{2}\right]\) to represent the electron configuration for the first two periods. (b) Calculate its bond order. (c) What are its magnetic properties (diamagnetic or paramagnetic)?

How would you distinguish between a sigma bond and a pi bond?

Use valence bond theory to explain the bonding in \(\mathrm{Cl}_{2}\) and \(\mathrm{HCl}\). Show how the atomic orbitals overlap when a bond is formed
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