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Chapter 20: Problem 40

Besides the central atom, what are the differences between \(\mathrm{CO}_{2}\) and \(\mathrm{SiO}_{2} ?\)

Short Answer

Expert verified
The main differences between CO2 and SiO2, besides the central atom, are their molecular structures, bond types, bond strength, melting points, chemical properties, and applications. CO2 has a linear structure with double bonds between carbon and oxygen atoms, making it a nonpolar gas with low melting point. SiO2 has a three-dimensional network structure with single bonds between silicon and oxygen atoms, resulting in a polar solid with a high melting point. CO2 forms carbonic acid when mixed with water, while SiO2 is insoluble in water and does not form any acid. Their differing properties make them suitable for various applications, such as CO2 for carbonated beverages and SiO2 for building materials.

Step by step solution

01

Identify the structures of CO2 and SiO2

First, we need to determine the molecular structures of CO2 and SiO2. CO2 has a linear structure, with carbon as the central atom and two oxygen atoms bonded to it. On the other hand, SiO2 has a three-dimensional network structure, with each silicon atom bonded to four oxygen atoms and each oxygen bonded to two silicon atoms.
02

Compare the types of bonds in CO2 and SiO2

In CO2, carbon forms double bonds with the two oxygen atoms, making the molecule nonpolar. In SiO2, silicon forms single bonds with the oxygen atoms, creating a polar covalent compound.
03

Compare the bond strength and melting points

Due to the double bonds present in CO2, the bond strength is greater than in SiO2, which has single bonds between silicon and oxygen. Consequently, CO2 has a lower melting point (-78.5°C or 194.65 K) and is a gas at room temperature, while SiO2 has a high melting point (around 1,710°C or 1,983.15 K) and is a solid at room temperature.
04

Analyze the differences in chemical properties

CO2 reacts with water to form carbonic acid (H2CO3), which dissociates into hydrogen and bicarbonate ions. In contrast, SiO2 is insoluble in water and does not form any acid. CO2 can act as a ligand in coordination complexes, while SiO2 typically does not.
05

Compare the uses and applications

The different properties of CO2 and SiO2 make them suitable for various applications. CO2 is used in carbonated beverages, fire extinguishers, and photosynthesis in plants, whereas SiO2 is used as a building material, an insulator in electronics, and an abrasive in cleansers. In summary, besides the central atom, the key differences between CO2 and SiO2 are their molecular structures, bond types, bond strength, melting points, chemical properties, and applications.

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Most popular questions from this chapter

The compound \(\mathrm{Pb}_{3} \mathrm{O}_{4}\) (red lead) contains a mixture of lead(II) and lead(IV) oxidation states. What is the mole ratio of lead(II) to lead(IV) in \(\mathrm{Pb}_{3} \mathrm{O}_{4} ?\)

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While selenic acid has the formula \(\mathrm{H}_{2} \mathrm{SeO}_{4}\) and thus is directly related to sulfuric acid, telluric acid is best visualized as \(\mathrm{H}_{6} \mathrm{TeO}_{6}\) or \(\mathrm{Te}(\mathrm{OH})_{6}\) a. What is the oxidation state of tellurium in Te(OH) \(_{6} ?\) b. Despite its structural differences with sulfuric and selenic acid, telluric acid is a diprotic acid with \(\mathrm{p} K_{\mathrm{a}_{1}}=7.68\) and \(\mathrm{p} K_{\mathrm{a}_{2}}=11.29 .\) Telluric acid can be prepared by hydrolysis of tellurium hexafluoride according to the equation $$ \mathrm{TeF}_{6}(g)+6 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Te}(\mathrm{OH})_{6}(a q)+6 \mathrm{HF}(a q) $$ Tellurium hexafluoride can be prepared by the reaction of elemental tellurium with fluorine gas: $$ \mathrm{Te}(s)+3 \mathrm{F}_{2}(g) \longrightarrow \mathrm{TeF}_{6}(g) $$ If a cubic block of tellurium (density \(=6.240 \mathrm{g} / \mathrm{cm}^{3} )\) measuring 0.545 \(\mathrm{cm}\) on edge is allowed to react with 2.34 \(\mathrm{L}\) fluorine gas at 1.06 \(\mathrm{atm}\) and \(25^{\circ} \mathrm{C},\) what is the pH of a solution of \(\mathrm{Te}(\mathrm{OH})_{6}\) formed by dissolving the isolated TeF \(_{6}(g)\) in 115 \(\mathrm{mL}\) solution? Assume 100\(\%\) yield in all reactions.
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