In the reaction P4+3 KOH+3 H2 O ⟶PH3+3 KH2 PO2 phos- phorus is (a) oxidized (b) reduced (c) oxid

step 1 Hello, good evening student. So in this question we have to tell the in the given reaction, phos

In the reaction P4+3 KOH+3 H2 O ⟶PH3+3 KH2 PO2 phos- phorus...

In the reaction
$\mathrm{P}_{4}+3 \mathrm{KOH}+3 \mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{PH}_{3}+3 \mathrm{KH}_{2} \mathrm{PO}_{2}$ phos-
phorus is
(a) oxidized
(b) reduced
(c) oxidized and reduced
(d) neither oxidized nor reduced

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Key Concepts

Oxidation

Oxidation refers to the process in which an element or compound loses electrons during a chemical reaction, often leading to an increase in its oxidation state. This concept is central in understanding redox reactions as it helps determine how electrons are redistributed between substances.

Reduction

Reduction is the complementary process to oxidation, where an element or compound gains electrons in a chemical reaction, resulting in a decrease in its oxidation state. Recognizing reduction is essential in the study of redox reactions since it clarifies which species is acting as the oxidizing agent.

Disproportionation Reaction

A disproportionation reaction is a specific type of redox reaction in which a single element undergoes both oxidation and reduction, forming two different products containing the element in distinct oxidation states. This concept is crucial for understanding scenarios where the same element simultaneously increases and decreases its oxidation state within the reaction.

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