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Chapter 17: Problem 62

Why can oxidation nerer occur without reduction?

Short Answer

Expert verified
Oxidation involves losing electrons, and reduction involves gaining them. Since electrons lost by one substance must be gained by another, oxidation cannot occur without reduction.

Step by step solution

01

Understand Oxidation

Oxidation is the loss of electrons from a substance during a chemical reaction. It often involves the addition of oxygen or the removal of hydrogen.
02

Understand Reduction

Reduction is the gain of electrons by a substance during a chemical reaction. It often involves the removal of oxygen or the addition of hydrogen.
03

Recognize the Electron Exchange

In any chemical reaction involving oxidation and reduction, electrons are transferred from one substance to another. This is known as a redox reaction.
04

Concept of Redox Reactions

In a redox reaction, one substance loses electrons (oxidized) and another gains those electrons (reduced). Hence, the two processes are interconnected.
05

Conclusion

Since electrons lost by one substance in oxidation must be gained by another substance in reduction, oxidation cannot occur without reduction and vice versa.

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Key Concepts

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

Oxidation
Oxidation is a fundamental concept in the study of chemical reactions. It involves the loss of electrons by a molecule, atom, or ion. During this process, the oxidized substance often either gains oxygen or loses hydrogen. For instance, when iron rusts, it undergoes oxidation as it combines with oxygen to form iron oxide. Key points to remember about oxidation:
  • It is the loss of electrons.
  • Involves the addition of oxygen or removal of hydrogen.
  • Leads to an increase in the oxidation state of the substance.
Understanding oxidation is crucial for grasping the interconnected nature of redox reactions.
Reduction
Reduction is essentially the opposite of oxidation. It involves the gain of electrons by a molecule, atom, or ion. During this process, the reduced substance often either loses oxygen or gains hydrogen. For example, in the process of photosynthesis, carbon dioxide is reduced to glucose. Important points about reduction include:
  • It is the gain of electrons.
  • Involves the removal of oxygen or addition of hydrogen.
  • Results in a decrease in the oxidation state of the substance.
Comprehending reduction helps in understanding how electrons are transferred in redox reactions.
Electron Transfer
The core of redox reactions is the transfer of electrons from one substance to another. This electron transfer is what links oxidation and reduction together. Here’s how it works:
  • One substance loses electrons (oxidized).
  • Another substance gains those electrons (reduced).
This interdependence ensures that oxidation cannot occur without a corresponding reduction. Visualize the flow of electrons; it's a bit like a relay race where the baton (electrons) is passed from one runner (substance) to another. Each transfer completes a crucial part of the race, making it impossible for one runner to finish alone.
Chemical Reactions
Chemical reactions involve the transformation of reactants into products. Redox reactions are specific types of chemical reactions where oxidation and reduction occur simultaneously. Understanding the essentials of chemical reactions helps in grasping redox processes:
  • Reactants interact to form products.
  • Energy changes often occur, like in exothermic or endothermic reactions.
  • Redox reactions involve electron exchanges between substances.
By focusing on electron movement, we can see why oxidation and reduction are inseparable. In every redox reaction, the loss of electrons by one substance is balanced by the gain of electrons by another, making them two sides of the same coin.

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Most popular questions from this chapter

Slate the charge and purpose of the anode and the cathode in an electrolytic or volatic cell.

Balance these reactions: (a) \(\mathrm{Mo-O}_{u}(s)+\mathrm{MnO}_{4}^{-}(a q) \rightarrow \mathrm{MoO}_{4}(s)+\mathrm{Mn}^{2}(a q)\) (acidic solution) (b) \(\mathrm{BrO}^{-}(a q)+\mathrm{Cr}\left(\mathrm{OH}_{4}^{-}(a q) \longrightarrow\right.\) \(\mathrm{Br}^{-}\left(\mathrm{aq}_{)}\right)+\mathrm{CrO}_{4}^{-}(\mathrm{aq})\) (basic solution) (c) \(\mathrm{S}_{2} \mathrm{O}^{2}-(a q)+\mathrm{MnO}_{4}^{-}(a q) \rightarrow\) \(\mathrm{SO}_{4}^{2}(a q)+\mathrm{MnO}_{2}(s)\) (basic solution)

(a) \(\mathrm{Al}\) is oxidized and loses 3 electrons. \(\mathrm{H}\) is reduced and gains 1 electron. \(\mathrm{Al}\) is the reducing agent and \(\mathrm{HNO}_{3}\) is the oxidizing agent. (b) Ni is oxidized and loses 2 electrons. Cu is reduced and gains 2 electrons. \(\mathrm{Ni}\) is the reducing agent and \(\mathrm{CuSO}_{4}\) is the axidioing agent. (c) C is oxidized and loses 1 electron. \(O\) is reduced and gains 2 electrons. \(\mathrm{C}_{2} \mathrm{H}_{6}\) is the reducing agent and \(\mathrm{O}_{2}\) is the oxidizing agent.

How many grams of zinc are reguired to reduce Fe3+ when \(25.0 \mathrm{~mL}\) of \(1.2 \mathrm{M} \mathrm{FeCl}\) are reacted? $$ \mathrm{Zn}+\mathrm{Fe}^{3+} \rightarrow \mathrm{Zn}^{2+}+\mathrm{Fe}

The chemical reactions taking place during discharge in a lead storage battery are $$ \begin{gathered} \mathrm{Pb}+\mathrm{SO}^{-} \longrightarrow \mathrm{PbSO}_{4} \\ \mathrm{PbO}_{2}+\mathrm{SO}_{4}^{2}+4 \mathrm{H}^{+} \longrightarrow \mathrm{PbSO}_{4}+2 \mathrm{H}_{4} \mathrm{O} \end{gathered} $$ (a) Complete each half-reaction by supplying electrons. (b) Which reaction is oxidation, and which is reduction? (c) Which reaction occurs at the anode of the battery?
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