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Reduction of the metal centre in aqueous permanganate ion involves
- a)3 electrons in neutral medium
- b)5 electrons in neutral medium
- c)3 electrons in alkaline medium
- d)5 electrons in acidic medium
Correct answer is option 'A,D'. Can you explain this answer?
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Reduction of the metal centre in aqueous permanganate ion involvesa)3 ...
In acidic medium
Change in oxidation state of Mn = 7 – 2 = 5
Thus electrons lost = 5
In neutral medium
In neutral medium
Change in oxidation state of Mn = 7 – 4 = 3
∴ Electrons lost = 3
∴ Electrons lost = 3
Most Upvoted Answer
Reduction of the metal centre in aqueous permanganate ion involvesa)3 ...
Reduction of the metal centre in aqueous permanganate ion involves the transfer of electrons. The reduction potential of permanganate ion (MnO4-) is dependent on the pH of the solution. The reduction can occur in both acidic and alkaline mediums, resulting in different numbers of electrons being transferred.
In acidic medium:
In an acidic medium, permanganate ion can be reduced to manganese(II) ion (Mn2+). The reduction reaction involves the transfer of 5 electrons. The overall reaction can be represented as follows:
MnO4- + 8H+ + 5e- → Mn2+ + 4H2O
In alkaline medium:
In an alkaline medium, permanganate ion can be reduced to manganate ion (MnO42-). The reduction reaction involves the transfer of 3 electrons. The overall reaction can be represented as follows:
2MnO4- + 4OH- + 3e- → 2MnO42- + 2H2O
Therefore, the correct options for the reduction of the metal centre in aqueous permanganate ion are options A and D. In a neutral medium, neither of these reactions occurs, so the reduction of the metal centre does not involve either 3 or 5 electrons.
To summarize:
- In an acidic medium, the reduction of permanganate ion involves the transfer of 5 electrons.
- In an alkaline medium, the reduction of permanganate ion involves the transfer of 3 electrons.
- In a neutral medium, the reduction of permanganate ion does not occur.
It is important to note that the reduction potential of permanganate ion is highly dependent on the pH of the medium. This is because the redox reaction involves the transfer of protons (H+) along with the electrons.
In acidic medium:
In an acidic medium, permanganate ion can be reduced to manganese(II) ion (Mn2+). The reduction reaction involves the transfer of 5 electrons. The overall reaction can be represented as follows:
MnO4- + 8H+ + 5e- → Mn2+ + 4H2O
In alkaline medium:
In an alkaline medium, permanganate ion can be reduced to manganate ion (MnO42-). The reduction reaction involves the transfer of 3 electrons. The overall reaction can be represented as follows:
2MnO4- + 4OH- + 3e- → 2MnO42- + 2H2O
Therefore, the correct options for the reduction of the metal centre in aqueous permanganate ion are options A and D. In a neutral medium, neither of these reactions occurs, so the reduction of the metal centre does not involve either 3 or 5 electrons.
To summarize:
- In an acidic medium, the reduction of permanganate ion involves the transfer of 5 electrons.
- In an alkaline medium, the reduction of permanganate ion involves the transfer of 3 electrons.
- In a neutral medium, the reduction of permanganate ion does not occur.
It is important to note that the reduction potential of permanganate ion is highly dependent on the pH of the medium. This is because the redox reaction involves the transfer of protons (H+) along with the electrons.
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Reduction of the metal centre in aqueous permanganate ion involvesa)3 electrons in neutral mediumb)5 electrons in neutral mediumc)3 electrons in alkaline mediumd)5 electrons in acidic mediumCorrect answer is option 'A,D'. Can you explain this answer?
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