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Chapter 17: Problem 66

Oxidation may be described as a(n) _______ of electrons or as an increase in ________.

Short Answer

Expert verified
Oxidation may be described as a(n) loss of electrons or as an increase in oxidation state.

Step by step solution

01

Fill in the first blank: Oxidation in terms of electron transfer

Oxidation is a process in which a chemical species loses one or more electrons. Thus, we can say oxidation is a(n) "loss" of electrons.
02

Fill in the second blank: Oxidation in terms of another property

As a species loses electrons, its charge increases. Oxidation can also be described as an increase in "oxidation state" or simply "oxidation number." So the completed sentence is: Oxidation may be described as a(n) loss of electrons or as an increase in oxidation state.

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Key Concepts

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

Electron Transfer
Electron transfer is a critical concept in understanding oxidation. When a chemical species loses electrons, it undergoes oxidation. This means that during a reaction, electrons are transferred from one atom or molecule to another. This process is crucial because it drives many chemical reactions forward.

Here are some key points about electron transfer:
  • Electrons are negatively charged subatomic particles found in atoms.
  • In a chemical reaction, electrons can move from one chemical species to another.
  • The species that loses electrons undergoes oxidation, while the one that gains electrons undergoes reduction.
So, whenever you hear about electron transfer in reactions, remember it's about the movement of electrons from one place to another. This movement influences how chemical reactions happen and helps us understand the changes in chemical species.
Oxidation State
Oxidation state, also known as oxidation number, is a numeric value that we assign to elements in a molecule or ion to indicate how many electrons an atom has gained, lost, or shared during bond formation. It helps us track electron flow in chemical reactions.

Key aspects of oxidation state include:
  • An increase in oxidation state means the species is losing electrons and is hence oxidized.
  • A decrease indicates the species is gaining electrons, meaning it is reduced.
  • Each element in a molecule has an oxidation state, which can help predict the result of redox reactions.
Understanding the change in oxidation state is crucial. It shows us the electron balance in reactions and helps identify which species are oxidized or reduced.
Chemical Species
The term chemical species refers to different forms of molecules, ions, atoms, or radicals that participate in a chemical reaction. Each species has unique chemical properties that determine its reactivity and behavior in reactions.

Features of chemical species include:
  • They are identified by their distinct molecular structures and compositions.
  • Chemical species can undergo oxidation or reduction, which involves electron transfer.
  • The type of species in a reaction determines the reaction's course and its products.
By understanding chemical species, you can predict how different substances will interact in a reaction and what kind of transformations to expect as a result of these interactions.

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Most popular questions from this chapter

Consider the oxidation-reduction reaction \(\mathrm{Mg}(s)+\mathrm{Cu}^{2+}(a q) \rightarrow \mathrm{Mg}^{2+}(a q)+\mathrm{Cu}(s)\) Sketch a galvanic cell that uses this reaction. Which metal ion is reduced? Which metal is oxidized? What half-reaction takes place at the anode in the cell? What half-reaction takes place at the cathode?

Elemental bromine can be prepared by treatment of seawater with chlorine gas. \(\mathrm{Cl}_{2}(g)+2 \mathrm{NaBr}(a q) \rightarrow \mathrm{Br}_{2}(a q)+2 \mathrm{NaCl}(a q)\) Identify the atoms that are oxidized and reduced, and specify the oxidizing and reducing agents.

How is an oxidation-reduction reaction set up as a galvanic cell (battery)? How is the transfer of electrons between reducing agent and oxidizing agent made useful?

Assign oxidation states to all of the atoms in each of the following: a. \(\mathrm{NaHSO}_{4}\) b. \(\mathrm{CaCO}_{3}\) c. \(\mathrm{KMnO}_{4}\) d. \(\mathrm{MnO}_{2}\)

In each of the following reactions, identify which element is oxidized and which is reduced by assigning oxidation states. a. \(2 \mathrm{B}_{2} \mathrm{O}_{3}(s)+6 \mathrm{Cl}_{2}(g) \rightarrow 4 \mathrm{BCl}_{3}(l)+3 \mathrm{O}_{2}(g)\) b. \(\operatorname{GeH}_{4}(g)+\mathrm{O}_{2}(g) \rightarrow \operatorname{Ge}(s)+2 \mathrm{H}_{2} \mathrm{O}(g)\) c. \(\mathrm{C_{2} H_{4}(g)+C l_{2}(g) \rightarrow C_{2} H_{4} C l_{2}(l)}\) d. \(\mathrm{O}_{2}(g)+2 \mathrm{F}_{2}(g) \rightarrow 2 \mathrm{OF}_{2}(g)\)
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