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Chapter 4: Problem 41

Is it possible to have a reaction in which oxidation occurs and reduction does not? Explain.

Short Answer

Expert verified
No, it's not possible. Oxidation and reduction reactions are two halves of the same process. For oxidation to occur, reduction must also occur, because the electrons lost during oxidation have to be gained by another substance, indicating reduction. This is why they are always paired together in a redox reaction.

Step by step solution

01

Understanding Redox Reactions

Redox (or reduction-oxidation) reactions include all chemical reactions in which atoms have their oxidation states changed. In other words, redox reactions are a family of reactions that are concerned with the transfer of electrons between species.
02

Defining Oxidation and Reduction

Oxidation is defined as a process where a substance loses electrons. On the other hand, reduction is a process in which a substance gains electrons. Both these processes occur simultaneously in a redox reaction.
03

Analyzing the Interdependence of Oxidation and Reduction

The two halves of a redox reaction, oxidation and reduction, cannot occur independently. If a substance is oxidized, it means it has lost electrons, but those electrons have to be gained by another substance; hence reduction takes place. Oxidation and reduction always occur together, meaning if one substance is getting oxidized, another substance must be getting reduced. This relationship between oxidation and reduction is commonly known as 'redox pair'.

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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 redox reactions, and it involves the loss of electrons by a molecule, atom, or ion. An easy way to remember this is through the mnemonic "OIL RIG", where OIL stands for "Oxidation Is Loss". When a substance undergoes oxidation, it increases its oxidation state.

Here are some key points about oxidation:
  • During oxidation, the substance losing electrons often results in the material having a more positive charge.
  • Common examples include the rusting of iron, where iron loses electrons to oxygen in the air, forming iron oxide.
  • Oxidation does not occur in isolation; it is always paired with reduction, as electrons must go somewhere.
Understanding oxidation is crucial, as it plays a role in numerous biological and chemical processes that are essential to life and technology.
Reduction
Reduction accompanies oxidation and involves the gain of electrons. Using the same mnemonic "OIL RIG", where RIG stands for "Reduction Is Gain", we can clearly see that when one substance gains electrons, its oxidation state decreases.

Important aspects of reduction include:
  • In a redox reaction, reduction results in the substance having a more negative charge due to the gained electrons.
  • Reduction is essential in processes like photosynthesis, where carbon dioxide is reduced to form glucose.
  • Just like oxidation, reduction cannot happen alone; it must be paired with oxidation to complete the electron transfers.
By understanding reduction, we see why it's impossible to have an oxidation process without a corresponding reduction event happening in tandem.
Electron Transfer
Electron transfer is the principal mechanism driving redox reactions. It refers to how electrons are relocated from one atom, ion, or molecule to another during the processes of oxidation and reduction.

Here鈥檚 what you should know about electron transfer:
  • The movement of electrons creates a redox pair, where one entity is oxidized (loses electrons) and another is reduced (gains electrons).
  • Redox reactions, including electron transfer, are crucial in energy production, such as in cellular respiration and battery operations.
  • The balance of electron transfer ensures that the total charge is conserved within a chemical reaction.
Understanding electron transfer helps explain why oxidation and reduction are two sides of the same coin, each requiring the other to proceed.

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Most popular questions from this chapter

Predict the outcome of the reactions represented by the following equations by using the activity series, and balance the equations. (a) \(\mathrm{Cu}(s)+\mathrm{HCl}(a q) \longrightarrow\) (b) \(\mathrm{I}_{2}(s)+\operatorname{NaBr}(a q) \longrightarrow\) (c) \(\mathrm{Mg}(s)+\mathrm{CuSO}_{4}(a q) \longrightarrow\) (d) \(\mathrm{Cl}_{2}(g)+\mathrm{KBr}(a q) \longrightarrow\)

Describe the basic steps involved in gravimetric analysis. How does this procedure help us determine the identity of a compound or the purity of a compound if its formula is known?

A \(5.00 \times 10^{2} \mathrm{~mL}\) sample of \(2.00 \mathrm{M} \mathrm{HCl}\) solution is treated with \(4.47 \mathrm{~g}\) of magnesium. Calculate the concentration of the acid solution after all the metal has reacted. Assume that the volume remains un- changed.

A 22.02-mL solution containing \(1.615 \mathrm{~g} \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}\) is mixed with a 28.64-mL solution containing \(1.073 \mathrm{~g}\) \(\mathrm{NaOH}\). Calculate the concentrations of the ions remaining in solution after the reaction is complete. Assume volumes are additive.

Sulfites (compounds containing the \(\mathrm{SO}_{3}^{2-}\) ions) are used as preservatives in dried fruits and vegetables and in wine making. In an experiment to test the presence of sulfite in fruit, a student first soaked several dried apricots in water overnight and then filtered the solution to remove all solid particles. She then treated the solution with hydrogen peroxide \(\left(\mathrm{H}_{2} \mathrm{O}_{2}\right)\) to oxidize the sulfite ions to sulfate ions. Finally, the sulfate ions were precipitated by treating the solution with a few drops of a barium chloride \(\left(\mathrm{BaCl}_{2}\right)\) solution. Write a balanced equation for each of the preceding steps.
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