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The complexes K2[NiF6] and K3[CoF6] are
- a)both paramagnetic
- b)both diamagnetic
- c)paramagnetic and diamagnetic, respectively
- d)diamagnetic and paramagnetic, respectively
Correct answer is option 'D'. Can you explain this answer?
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Verified Answer
The complexes K2[NiF6] and K3[CoF6] area)both paramagneticb)both diama...
Oxidation number of Ni in K2[NiF6] is +4. +4 oxidation state of Ni attracts the F- ligands with greater force of attraction so the F- ligands enforce the unpaired electrons of Ni4+ to get paired up , so it is diamagnetic .
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The complexes K2[NiF6] and K3[CoF6] area)both paramagneticb)both diama...
Paramagnetism and Diamagnetism
Before we can answer the question, we need to understand the concepts of paramagnetism and diamagnetism.
- Paramagnetic materials have unpaired electrons, which create a magnetic moment. When placed in an external magnetic field, they are attracted towards the field.
- Diamagnetic materials have all paired electrons, which cancel out their magnetic moments. When placed in an external magnetic field, they are slightly repelled by the field.
K2[NiF6]
The complex K2[NiF6] contains nickel in the +2 oxidation state. The electronic configuration of Ni2+ is 3d8. In the presence of fluoride ions, the six 3d electrons of nickel are paired up with the six fluoride electrons, leaving two unpaired electrons in the 3d orbitals. Therefore, K2[NiF6] is paramagnetic.
K3[CoF6]
The complex K3[CoF6] contains cobalt in the +3 oxidation state. The electronic configuration of Co3+ is 3d6. In the presence of fluoride ions, the six 3d electrons of cobalt are paired up with the six fluoride electrons, leaving no unpaired electrons in the 3d orbitals. Therefore, K3[CoF6] is diamagnetic.
Conclusion
In summary, K2[NiF6] is paramagnetic because it has unpaired electrons in the 3d orbitals of nickel, while K3[CoF6] is diamagnetic because there are no unpaired electrons in the 3d orbitals of cobalt.
Before we can answer the question, we need to understand the concepts of paramagnetism and diamagnetism.
- Paramagnetic materials have unpaired electrons, which create a magnetic moment. When placed in an external magnetic field, they are attracted towards the field.
- Diamagnetic materials have all paired electrons, which cancel out their magnetic moments. When placed in an external magnetic field, they are slightly repelled by the field.
K2[NiF6]
The complex K2[NiF6] contains nickel in the +2 oxidation state. The electronic configuration of Ni2+ is 3d8. In the presence of fluoride ions, the six 3d electrons of nickel are paired up with the six fluoride electrons, leaving two unpaired electrons in the 3d orbitals. Therefore, K2[NiF6] is paramagnetic.
K3[CoF6]
The complex K3[CoF6] contains cobalt in the +3 oxidation state. The electronic configuration of Co3+ is 3d6. In the presence of fluoride ions, the six 3d electrons of cobalt are paired up with the six fluoride electrons, leaving no unpaired electrons in the 3d orbitals. Therefore, K3[CoF6] is diamagnetic.
Conclusion
In summary, K2[NiF6] is paramagnetic because it has unpaired electrons in the 3d orbitals of nickel, while K3[CoF6] is diamagnetic because there are no unpaired electrons in the 3d orbitals of cobalt.
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The complexes K2[NiF6] and K3[CoF6] area)both paramagneticb)both diama...
Due to the +4 oxidation state of Ni in K2[NiF6] it is low spin complex therefore no unpaired electrons and it is diamagnetic. In K3[CoF6] Oxidation state of Co is +3 which is high spin, unpaired electrons are present So it is paramagnetic in nature.
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The complexes K2[NiF6] and K3[CoF6] area)both paramagneticb)both diamagneticc)paramagnetic and diamagnetic, respectivelyd)diamagnetic and paramagnetic, respectivelyCorrect answer is option 'D'. Can you explain this answer?
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