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Which of the following complexes has the highest magnetic moment?
- a)[Fe(CN)6]4-
- b)[VO(H2O)5]2+
- c)[Cr(NH3)6]3+
- d)[Co(NH3)6]3+
Correct answer is option 'C'. Can you explain this answer?
Verified Answer
Which of the following complexes has the highest magnetic moment?a)[Fe...
Higher the number of unpaired electrons, the higher is the magnetic moment. So, the correct option is [Cr(NH3)6]3+
Most Upvoted Answer
Which of the following complexes has the highest magnetic moment?a)[Fe...
Magnetic Moment of Complexes
Magnetic moment is a measure of the strength of a magnetic field created by a substance. It depends on the number of unpaired electrons in the complex.
The formula for magnetic moment is:
μ = √n(n+2) BM
where n is the number of unpaired electrons and BM is the Bohr magneton, which is a unit of magnetic moment.
The complex with the highest magnetic moment will have the highest number of unpaired electrons.
Analysis of the Given Complexes
a) [Fe(CN)6]4-
Iron in [Fe(CN)6]4- has a d6 configuration, which means it has four unpaired electrons. Therefore, its magnetic moment is:
μ = √4(4+2) BM = 4.9 BM
b) [VO(H2O)5]2
Vanadium in [VO(H2O)5]2 has a d1 configuration, which means it has one unpaired electron. Therefore, its magnetic moment is:
μ = √1(1+2) BM = 1.7 BM
c) [Cr(NH3)6]3
Chromium in [Cr(NH3)6]3 has a d3 configuration, which means it has three unpaired electrons. Therefore, its magnetic moment is:
μ = √3(3+2) BM = 3.9 BM
d) [Co(NH3)6]3
Cobalt in [Co(NH3)6]3 has a d6 configuration, which means it has four unpaired electrons. Therefore, its magnetic moment is:
μ = √4(4+2) BM = 4.9 BM
Conclusion
The complex with the highest magnetic moment is [Cr(NH3)6]3, with a magnetic moment of 3.9 BM. It has three unpaired electrons, which is one less than [Fe(CN)6]4- and [Co(NH3)6]3, but still higher than [VO(H2O)5]2, which has only one unpaired electron.
Magnetic moment is a measure of the strength of a magnetic field created by a substance. It depends on the number of unpaired electrons in the complex.
The formula for magnetic moment is:
μ = √n(n+2) BM
where n is the number of unpaired electrons and BM is the Bohr magneton, which is a unit of magnetic moment.
The complex with the highest magnetic moment will have the highest number of unpaired electrons.
Analysis of the Given Complexes
a) [Fe(CN)6]4-
Iron in [Fe(CN)6]4- has a d6 configuration, which means it has four unpaired electrons. Therefore, its magnetic moment is:
μ = √4(4+2) BM = 4.9 BM
b) [VO(H2O)5]2
Vanadium in [VO(H2O)5]2 has a d1 configuration, which means it has one unpaired electron. Therefore, its magnetic moment is:
μ = √1(1+2) BM = 1.7 BM
c) [Cr(NH3)6]3
Chromium in [Cr(NH3)6]3 has a d3 configuration, which means it has three unpaired electrons. Therefore, its magnetic moment is:
μ = √3(3+2) BM = 3.9 BM
d) [Co(NH3)6]3
Cobalt in [Co(NH3)6]3 has a d6 configuration, which means it has four unpaired electrons. Therefore, its magnetic moment is:
μ = √4(4+2) BM = 4.9 BM
Conclusion
The complex with the highest magnetic moment is [Cr(NH3)6]3, with a magnetic moment of 3.9 BM. It has three unpaired electrons, which is one less than [Fe(CN)6]4- and [Co(NH3)6]3, but still higher than [VO(H2O)5]2, which has only one unpaired electron.
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Community Answer
Which of the following complexes has the highest magnetic moment?a)[Fe...
In case of iron complex which is with strong field legand so pairing takes place that's by having lowest magnetic moment
and V only having one electron i.e lower value of the magnetic moment but in case of chromium highest number of unpaired electron I.e higher the magnetic moment
and so on but in case of Co extra magnetic moment is also count so pairing decreases thae magnetic moment
and V only having one electron i.e lower value of the magnetic moment but in case of chromium highest number of unpaired electron I.e higher the magnetic moment
and so on but in case of Co extra magnetic moment is also count so pairing decreases thae magnetic moment
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