/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 40 Besides the central atom, what a... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

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掳C or 194.65 K) and is a gas at room temperature, while SiO2 has a high melting point (around 1,710掳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.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Although the earth was formed from the same interstellar material as the sun, there is little elemental hydrogen \(\left(\mathrm{H}_{2}\right)\) in the earth's atmosphere. Explain.

Although He is the second most abundant element in the universe, it is very rare on the earth. Why?

In large doses, selenium is toxic. However, in moderate intake, selenium is a physiologically important element. How is selenium physiologically important?

The resistivity (a measure of electrical resistance) of graphite is \((0.4 \text { to } 5.0) \times 10^{-4}\) ohm \(\cdot \mathrm{cm}\) in the basal plane. (The basal plane is the plane of the six-membered rings of carbon atoms.) The resistivity is 0.2 to 1.0 ohm \(\cdot \mathrm{cm}\) along the axis perpendicular to the plane. The resistivity of diamond is \(10^{14}\) to \(10^{16} \mathrm{ohm} \cdot \mathrm{cm}\) and is independent of direction. How can you account for this behavior in terms of the structures of graphite and diamond?

What is nitrogen fixation? Give some examples of nitrogen fixation.
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Making Measurements

Read Explanation

Chemical Analysis

Read Explanation

Nuclear Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.