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Chapter 6: Problem 2

Molecules with formulae of the form \(C_{n} H_{2 n+1}\) (e.g. \(C H_{3}, C_{2} H_{5}\) ) are called "radicals" and are extremely reactive. Using Lewis structures, explain the reactivity of these molecules.

Short Answer

Expert verified
Radicals have unpaired electrons in their Lewis structures, causing high reactivity.

Step by step solution

01

Understand the Basic Structure

Molecules with the formula \(C_n H_{2n+1}\) have one carbon atom with fewer hydrogens than it can maximally accommodate, resulting in an unpaired electron. This occurs because each carbon normally forms four bonds, but here it forms three with hydrogen, leaving one electron unsatisfied.
02

Draw the Lewis Structure for a Simple Example

Take \(CH_3\) as an example. Carbon, having four valence electrons, would bond with three hydrogen atoms. The Lewis structure shows three C-H bonds and one unpaired electron on the carbon atom, making it a radical.
03

Identify the Unpaired Electron

Recognize that the unpaired electron is the source of reactivity in radical molecules. In \(CH_3\), the unpaired electron on carbon is seeking another electron to pair with, making it highly reactive.
04

Explain Reactivity Using Lewis Structure

Because radicals have an unpaired electron, they tend to react quickly with other atoms or molecules to achieve a stable electron pair. The Lewis structure emphasizes this by showing the unpaired electron clearly.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Radicals
Radicals are intriguing chemical species that exhibit unique properties due to having open valence shells. These molecules, characterized by their general formula \(C_nH_{2n+1}\), include a carbon atom bonded to hydrogens. Importantly, one electron remains unpaired. This unpaired electron forms the essence of a radical, introducing a balance of instability and high reactivity.
  • Radicals are often short-lived and highly reactive.
  • The "unpaired electron" is a key feature that seeks stability by forming a bond.
Examining the Lewis structure of radicals such as \(CH_3\) helps visualize their incomplete octet, indicating their readiness to react in chemical processes.
Unpaired Electron
An unpaired electron is what makes radicals like \(CH_3\) fascinating yet reactive. In a typical Lewis structure, you can easily identify this electron as it does not pair with any other electron. This leaves the molecule in a state of imbalance, as every atom prefers paired electrons for stability.
  • Unpaired electrons create a sense of electron deficiency in the molecule.
  • They drive the molecule to quickly find and pair with other electrons from nearby atoms or molecules.
This electron-seeking behavior accounts for a significant part of the chemical reactivity seen in radicals.
Chemical Reactivity
The chemical reactivity of radicals stems from their quest to achieve stable electron configurations. Radicals like \(C_nH_{2n+1}\) molecules undergo various reactions to satisfy their unpaired electron. These reactions are typically fast-paced, as the radicals aggressively search for electrons.
  • Radicals can easily disrupt stable molecules by grabbing electrons.
  • This reactivity allows them to initiate and propagate chain reactions.
Understanding this aggressive reactivity explains why radicals play critical roles in complex chemical processes, including combustion and polymerization.
Carbon Hydrogen Bonds
Carbon-hydrogen (C-H) bonds form a crucial part of radical structures despite the presence of an unpaired electron. These bonds contribute significantly to the molecule's properties. Each hydrogen atom shares its electron with carbon, forming a strong covalent bond that is usually stable under normal conditions.
  • C-H bonds are essential in stabilizing the base structure of radicals.
  • Despite the unpaired electron, C-H bonds resist breaking, lending a "backbone" to the molecule.
In the context of radicals, the C-H bonds, along with the unpaired electron, determine how and with what the radical will react in its pursuit of stability.

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Most popular questions from this chapter

Compounds with formulae of the form \(C_{n} H_{2 n+2}\) are often referred to as "saturated" hydrocarbons. Using Lewis structures, explain how and in what sense these molecules are "saturated."
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