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Manganate ion is paramagnetic and permanganate ion is diamagnetic. How can we find this out?
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Mowarin Emmanuel
Manganate ion is paramagnetic and permanganate ion is diamagnetic. How can we find this out?
In permanganate ion (MnO4^-), the oxidation number of Mn is +7. Ground state electronic configuration of Mn^7+ ion is [Ar] 3d0 4s0. There is no unpaired electron and hence, permanganate ion is diamagnetic. But in manganate (MnO4^2-) ion, the oxidation number of Mn is +6. The ground state electronic configuration of Mn^6+ is [Ar] 3d1. Mn^6+ contains an unpaired electron in 3d sub-shell. So, manganate ion is paramagnetic. Its calculated spin only magnetic moment = √{n*(n+2)} B. M. = √{1*(1+2)} = √3 =1.732 B. M.
In permanganate ion (MnO4^-), the oxidation number of Mn is +7. Ground state electronic configuration of Mn^7+ ion is [Ar] 3d0 4s0. There is no unpaired electron and hence, permanganate ion is diamagnetic. But in manganate (MnO4^2-) ion, the oxidation number of Mn is +6. The ground state electronic configuration of Mn^6+ is [Ar] 3d1. Mn^6+ contains an unpaired electron in 3d sub-shell. So, manganate ion is paramagnetic. Its calculated spin only magnetic moment = √{n*(n+2)} B. M. = √{1*(1+2)} = √3 =1.732 B. M.
In permanganate ion (MnO4^-), the oxidation number of Mn is +7. Ground state electronic configuration of Mn^7+ ion is [Ar] 3d0 4s0. There is no unpaired electron and hence, permanganate ion is diamagnetic. But in manganate (MnO4^2-) ion, the oxidation number of Mn is +6. The ground state electronic configuration of Mn^6+ is [Ar] 3d1. Mn^6+ contains an unpaired electron in 3d sub-shell. So, manganate ion is paramagnetic. Its calculated spin only magnetic moment = √{n*(n+2)} B. M. = √{1*(1+2)} = √3 =1.732 B. M.
Hope this helps.
In permanganate ion (MnO4^-), the oxidation number of Mn is +7. Ground state electronic configuration of Mn^7+ ion is [Ar] 3d0 4s0. There is no unpaired electron and hence, permanganate ion is diamagnetic. But in manganate (MnO4^2-) ion, the oxidation number of Mn is +6. The ground state electronic configuration of Mn^6+ is [Ar] 3d1. Mn^6+ contains an unpaired electron in 3d sub-shell. So, manganate ion is paramagnetic. Its calculated spin only magnetic moment = √{n*(n+2)} B. M. = √{1*(1+2)} = √3 =1.732 B. M.
Hope this helps.
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In Manganate ion Mn (+6) means 3d1 system. It's paramagnetic due to one unpaired electron.
In parmanganate ion Mn(+7) means 3d0 system, that's why it is diamagnetic.
In Manganate ion Mn (+6) means 3d1 system. It's paramagnetic due to one unpaired electron.
In parmanganate ion Mn(+7) means 3d0 system, that's why it is diamagnetic.
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