Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 20: Problem 35

Discuss the importance of the \(\mathrm{C}-\mathrm{C}\) and \(\mathrm{Si}-\mathrm{Si}\) bond strengths and of \(\pi\) bonding to the properties of carbon and silicon.

Short Answer

Expert verified
In summary, the C-C bond strength and ability to form stable π bonds allow carbon to form diverse and stable compounds with various molecular structures. However, Si-Si bonds are weaker and less diverse due to the larger atomic size and limited π bonding, resulting in extended network structures. Therefore, the bond strengths and π bonding significantly impact the properties and chemical behavior of carbon and silicon.

Step by step solution

01

1. The Carbon-Carbon (C-C) bond strength and properties of Carbon

Carbon has a unique ability to form strong, stable covalent C-C bonds due to its small atomic size and half-filled valence shell. As a result, carbon forms a diverse range of compounds with single, double, and triple bonds between carbon atoms. These strong C-C bonds are responsible for the stability of organic compounds and the formation of complex molecular structures.
02

2. The Silicon-Silicon (Si-Si) bond strength and properties of Silicon

Silicon, also a group 14 element like carbon, has a larger atomic radius and, therefore, forms longer and weaker Si-Si bonds compared to C-C bonds. Silicon compounds tend to be relatively less stable and show a preference for single Si-Si bonds, resulting in extended network structures in many solid silicon compounds. This difference in bond strength is one reason why silicon does not possess the same level of chemical diversity and complexity as carbon.
03

3. Role of π bonding in Carbon

π bonding is the overlap of p orbitals along the inter-nuclear axis, leading to the formation of double and triple bonds between carbon atoms. The presence of π bonds strongly influences the geometry and stability of carbon compounds, allowing carbon to form planar and linear structures in cases of double and triple bonds, respectively. Moreover, π bonds in conjugated systems add stability and unique properties to organic compounds, such as color and reactivity. Therefore, π bonding significantly affects the chemical behavior and characteristics of carbon compounds.
04

4. Role of π bonding in Silicon

Silicon also has p orbitals capable of forming π bonds, but due to the larger atomic size and a low degree of p orbital overlap, π bonding in silicon is weaker than in carbon. Consequently, multiple bonds like double and triple bonds between Si atoms are relatively less common and less stable compared to those in Carbon. This limited π bonding in silicon restricts the diversity of compounds formed by silicon compared to carbon.
05

5. Conclusion

In summary, the distinct bond strengths of C-C and Si-Si bonds and the role of π bonding play essential roles in determining the properties and chemical behavior of carbon and silicon. Carbon's strong C-C bonds and ability to form stable π bonds contribute to the vast diversity and stability of organic compounds, while silicon's weaker Si-Si bonds and limited π bonding result in fewer complex structures, with an emphasis on extended frameworks and network arrangements in solid-state compounds.

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.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

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

An unknown element is a nonmetal and has a valence electron configuration of \(n s^{2} n p^{4}\). a. How many valence electrons does this element have? b. What are some possible identities for this element? c. What is the formula of the compound(s) this element would form with lithium? hydrogen? magnesium? aluminum? fluorine?

EDTA is used as a complexing agent in chemical analysis. Solutions of EDTA, usually containing the disodium salt \(\mathrm{Na}_{2} \mathrm{H}_{2} \mathrm{EDTA}\), are also used to treat heavy metal poisoning. The equilibrium constant for the following reaction is \(1.0 \times 10^{23}\) : Calculate \(\left[\mathrm{Pb}^{2+}\right]\) at equilibrium in a solution originally \(0.0010 \mathrm{M}\) in \(\mathrm{Pb}^{2+}, 0.050 \mathrm{M}\) in \(\mathrm{H}_{2} \mathrm{EDTA}^{2-}\), and buffered at \(\mathrm{pH}=6.00\).

How could you determine experimentally whether the compound \(\mathrm{Ga}_{2} \mathrm{Cl}_{4}\) contains two gallium(II) ions or one gallium(I) and one gallium(III) ion? (Hint: Consider the electron configurations of the three possible ions.)

Write equations describing the reactions of Sn with each of the following: \(\mathrm{Cl}_{2}, \mathrm{O}_{2}\), and \(\mathrm{HCl}\).

Write a balanced equation describing the reduction of \(\mathrm{H}_{2} \mathrm{SeO}_{4}\) by \(\mathrm{SO}_{2}\) to produce selenium.
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Making Measurements

Read Explanation

Chemical Reactions

Read Explanation

Chemistry Branches

Read Explanation

Inorganic Chemistry

Read Explanation

Nuclear Chemistry

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.

Sign-up for free