The reaction of white phosphorus with aqueous $NaOH$ gives phosphine along with another phosphorus containing compound. The reaction type, the oxidation states of phosphorus in phosphine and the other product respectively are
- redox reaction, $- 3$ and $- 5$
- redox reaction, $+ 3$ and $+ 5$
- disproportionation reaction, $- 3$ and $+ 5$
- disproportionation reaction, $- 3$ and $+ 3$
The Correct Option is C
Solution and Explanation
However, + 1 oxidation number is not given in any option, one might think that $NaH_2P O_2$ has gone to further decomposition on heating. $2NaH_2P O_2\, \, \xrightarrow{\Delta}\, \, \, Na_2H\, ^{+5}_{P} O_4 +PH_3$
Top Questions on Redox reactions
- Which of the following is a redox reaction, but not a combination reaction?
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The reaction given above is a redox reaction because in this case:- CBSE Class X - 2024
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- The oxidation states not shown by Mn in the given reaction is:
\( 3MnO_4^{2-} + 4H^+ \rightarrow 2MnO_4^- + MnO_2 + 2H_2O \)
A. +6
B. +2
C. +4
D. +7
E. +3
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[Given, atomic number: V = 23, Cr=24, Mn 25, Fe 26, Co 27, Ni 28, Cu = 29, Ir = 77]- JEE Advanced - 2024
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Concepts Used:
Redox Reactions
Redox Reaction:
Redox reactions are chemical reactions where oxidation and reduction take place simultaneously. In this type of reaction, there is a gain of electrons for one chemical species while the other loses electrons or simply involves transfer of electrons. The species that loses electrons is oxidized while the one that gains electrons is reduced.
Types of Redox Reactions:
Redox reactions can be differentiated into 4 categories namely combination reactions, decomposition reactions, displacement reactions, and disproportionation reactions. Each is explained separately below:
Combination Reaction:
In this, the molecules combine to form new compounds. For example, when magnesium reacts to nitrogen.
Decomposition Reaction:
Opposite to the combination reaction, here there is a breakdown of compounds to simpler substances. For example, electrolysis of water.
Displacement Reaction:
In this, the more reactive metal will displace the less reactive one in a chemical reaction. The reactivity of an element is represented in a series called the reactivity series (arranged in decreasing order of reactivity) which makes it easier to determine the chemical reaction and its products.
Disproportionation Reaction:
This is a peculiar type of reaction where an element showing a particular oxidation state will be oxidized and reduced simultaneously. Another thing to note is that these reactions will always have an element that can exhibit three oxidation states.