/*! 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 Why must the number of electrons... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 17: Problem 40

Why must the number of electrons lost in the oxidation equal the number of electrons gained in the reduction? Is it possible to have "leftover" electrons in a reaction?

Short Answer

Expert verified
In redox reactions, the number of electrons lost in oxidation must equal the number of electrons gained in reduction to maintain charge balance and adhere to the conservation of electrons principle. This ensures that the reaction is complete and reaches its stable, lowest-energy state. Having "leftover" electrons would result in unstable radicals, which indicates an incomplete reaction. Therefore, it is not possible to have leftover electrons in a typical redox reaction.

Step by step solution

01

Understanding Redox Reactions

Redox reactions, short for "reduction-oxidation" reactions, are chemical processes in which one reactant is oxidized (loses electrons) and another reactant is reduced (gains electrons). In simpler terms, oxidation is a process where a substance loses electrons, while reduction is a process where a substance gains electrons.
02

Recognize The Role of Electrons

In redox reactions, electrons are being transferred between species. This transfer of electrons allows substances to change their oxidation states. The change in oxidation states, in turn, causes the observed chemical changes in a redox reaction.
03

Electron Balance in Redox Reactions

In a redox reaction, the number of electrons lost by the oxidized species must equal the number of electrons gained by the reduced species. This condition ensures that the reaction is balanced in terms of charge and that no "leftover" electrons are present. The conservation of electrons principle dictates that electrons cannot be created or destroyed during a chemical reaction; they can only change their location or be transferred between species.
04

No Leftover Electrons

If there were "leftover" electrons in a reaction, it would mean that the charges are not balanced and that the reaction is not complete. Incomplete redox reactions would result in reactive intermediates with unpaired electrons, called radicals, which are highly unstable and reactive. Most common redox reactions strive for a stable, lowest-energy state by ensuring that electrons are fully transferred between species, leaving no leftover electrons.
05

Conclusion

In redox reactions, the number of electrons lost in the oxidation process must equal the number of electrons gained in the reduction process, ensuring that the charges are balanced and adhering to the conservation of electrons principle. This balance prevents the formation of unstable radicals and ensures that the reaction reaches its stable, lowest-energy state with no leftover electrons.

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

"Jump-starting" a dead automobile battery can be dangerous if precautions are not taken, because of the production of an explosive mixture of _________ and _________ gases in the battery.

Does an oxidizing agent donate or accept electrons? Does a reducing agent donate or accept electrons?

At which electrode (anode/cathode) do species gain electrons in a galvanic cell?

What process is represented by the corrosion of a metal? Why is corrosion undesirable?

Balance each of the following half-reactions. a. \(\mathrm{N}_{2}(g) \rightarrow \mathrm{N}^{3-}(s)\) b. \(\mathrm{O}_{2}^{2-}(a q) \rightarrow \mathrm{O}_{2}(g)\) c. \(\mathrm{Zn}(s) \rightarrow \mathrm{Zn}^{2+}(a q)\) d. \(\mathrm{F}_{2}(g) \rightarrow \mathrm{F}^{-}(a q)\)
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Nuclear Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Making Measurements

Read Explanation

Kinetics

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.