/*! 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 34 Explain why not all oxidation re... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 19: Problem 34

Explain why not all oxidation reactions involve oxygen.

Short Answer

Expert verified
Not all oxidation reactions involve oxygen because oxidation is defined as the loss of electrons from a species, and this can occur in chemical reactions without the presence of oxygen. For example, the reaction between sodium metal (Na) and chlorine gas (Cl鈧�) to form sodium chloride (NaCl) involves the transfer of electrons from sodium to chlorine, even though oxygen is not present. Oxidation is a more general concept that encompasses any chemical reaction in which electron transfer occurs, regardless of the specific elements involved.

Step by step solution

01

Define Oxidation

Oxidation is a chemical reaction that involves the loss of electrons from an atom or molecule. In other words, the species that undergoes oxidation loses electrons and becomes more positively charged. Initially, oxidation reactions were thought to involve only oxygen because the most commonly observed oxidizing agents were oxygen-containing compounds. However, the concept of oxidation has expanded to encompass all chemical reactions where electron transfer occurs.
02

Provide an Example of Oxidation without Oxygen

Let's consider an example of an oxidation reaction that does not involve oxygen. A simple example is the reaction between sodium metal (Na) and chlorine gas (Cl鈧�) to form sodium chloride (NaCl), which is table salt. The balanced reaction can be written as: \[ 2Na + Cl_2 \rightarrow 2NaCl \] During the reaction, sodium loses an electron to become a positively charged ion (Na鈦�), while chlorine gains an electron to become a negatively charged ion (Cl鈦�). Thus, the oxidation half-reaction can be written as: \[ Na \rightarrow Na^+ + e^- \] Here, sodium is undergoing oxidation, even though oxygen is not involved in the reaction.
03

Conclusion

In conclusion, not all oxidation reactions involve oxygen because oxidation is defined as the loss of electrons from a species, and this can occur in chemical reactions without the presence of oxygen. The example of sodium reacting with chlorine to form sodium chloride demonstrated an oxidation reaction without the involvement of oxygen. Oxidation is a more general concept that encompasses any chemical reaction in which electron transfer occurs, regardless of the specific elements involved.

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!

Key Concepts

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

Electron Transfer
In the world of chemistry, electron transfer is a fundamental concept that underlies many reactions. Essentially, it involves the movement of electrons from one atom, ion, or molecule to another. This process is pivotal because it results in changes to the charge state of the participating species.
During an electron transfer, one entity will lose electrons while another will gain them. This is typically observed in redox reactions, where oxidation (loss of electrons) and reduction (gain of electrons) occur simultaneously.
  • The species that loses electrons becomes more positive, turning into an oxidized form.
  • The species that gains electrons becomes more negative, forming a reduced state.
Understanding electron transfer offers insights into why certain reactions happen and how materials change at a molecular level. It's a cornerstone in explaining how batteries work, how metals corrode, and even how our bodies produce energy.
Oxidation Definition
The term oxidation has evolved over time. Originally, it was associated strictly with reactions involving oxygen. For instance, rusting of iron was considered a classic oxidation process because oxygen was a reactant.
However, today, the definition is broader. Oxidation now pertains to any chemical reaction where there is a loss of electrons, irrespective of oxygen. This change in understanding means that many reactions previously not classified as oxidation are now included.
For example:
  • Oxidation can occur without oxygen being present, as long as electron loss happens.
  • The entity that loses electrons is oxidized, becoming more positive.
This expanded definition is crucial for understanding a wide array of chemical processes beyond just those involving oxygen.
Sodium Chloride Formation
The formation of sodium chloride, or table salt, from sodium and chlorine is a prime example of oxidation occurring without oxygen. Here's what happens:
  • Sodium (Na), a shiny metal, donates an electron to become Na鈦�.
  • Chlorine (Cl鈧�), a pungent gas, accepts the electron to form two chloride ions (Cl鈦�).
The chemical reaction is:
\[ 2Na + Cl_2 \rightarrow 2NaCl \]
This reaction involves electron transfer, where sodium undergoes oxidation and chlorine undergoes reduction.
This reaction illustrates how oxidation doesn't always require oxygen. Instead, it's the electron transfer that defines the oxidation process. Such processes are central to chemistry, demonstrating how materials transform and interact in various environments.

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

Balance the following redox chemical equation. Rewrite the equation in full ionic form, then derive the net ionic equation and balance by the half- reaction method. Give the final answer as it is shown below but with the balancing coefficients. \(\mathrm{KMnO}_{4}(\mathrm{aq})+\mathrm{FeSO}_{4}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq}) \rightarrow\) \(\mathrm{Fe}_{2}\left(\mathrm{SO}_{4}\right)_{3}(\mathrm{aq})+\mathrm{MnSO}_{4}(\mathrm{aq})+\) \(\quad \mathrm{K}_{2} \mathrm{SO}_{4}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(1)\)

Determine the oxidation number of the boldface element in the following formulas for ions a. \({N H}_{4}+\) b. \(A s O_{4} 3-\) c. \({C r O}_{4}^{2-}\)

Use the half-reaction method to balance the redox equations. Begin by writing the oxidation and reduction half-reactions. Leave the balanced equation in ionic form. Challenge \(\mathrm{N}_{2} \mathrm{O}(\mathrm{g})+\mathrm{ClO}^{-}(\mathrm{aq}) \rightarrow \mathrm{NO}_{2}^{-}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})\) (in basic solution)

Describe what is happening to electrons in each half reaction of a redox process

Before you attempt to balance the equation for a redox reaction, why do you need to know whether the reaction takes place in acidic or basic solution?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Making Measurements

Read Explanation

The Earths Atmosphere

Read Explanation

Nuclear Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Chemistry Branches

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.