In the reaction P4+3 KOH+3 H2 O →PH3+3 KH2 PO2 phosphorous is: (a) Oxidized (b) Reduced (c) Oxid

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In the reaction P4+3 KOH+3 H2 O →PH3+3 KH2 PO2 phosphorous...

In the reaction $\mathrm{P}_{4}+3 \mathrm{KOH}+3 \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{PH}_{3}+3 \mathrm{KH}_{2} \mathrm{PO}_{2}$
phosphorous is:
(a) Oxidized
(b) Reduced
(c) Oxidized and reduced
(d) Neither oxidized nor reduced

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Key Concepts

Oxidation-Reduction Reaction

This concept involves the transfer of electrons between chemical species, leading to changes in their oxidation states. In these reactions, one species undergoes oxidation (loss of electrons) while another undergoes reduction (gain of electrons). Understanding oxidation-reduction is crucial for analyzing how electron flow affects the chemical behavior of substances.

Oxidation State

An oxidation state is a number assigned to an atom in a chemical compound that represents its degree of oxidation. It helps in tracking electron transfer in reactions and determining which atoms are oxidized or reduced, serving as a fundamental tool for balancing chemical equations and understanding reaction mechanisms.

Disproportionation Reaction

A disproportionation reaction is a particular type of redox reaction where a single element undergoes both oxidation and reduction simultaneously, forming two different products with distinct oxidation states. This concept is key to explaining how the same element can be transformed into compounds where its oxidation number increases in one product and decreases in another.

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