Question:
$K_4[Fe(CN)_6]$ is diamagnetic and $[Fe(H_2O)_6 ]Cl_3$ is paramagnetic.
Hybridisation of central metal m $K_4[Fe(CN)_6] is \,sp^3d^2,$ while in $[Fe(H_2O)_6]Cl_3\, is\, d^2\, sp^3$
$K_4[Fe(CN)_6]$ is diamagnetic and $[Fe(H_2O)_6 ]Cl_3$ is paramagnetic.
Hybridisation of central metal m $K_4[Fe(CN)_6] is \,sp^3d^2,$ while in $[Fe(H_2O)_6]Cl_3\, is\, d^2\, sp^3$
Updated On: Jul 6, 2022
- Both Assertion and Reason are true and Reason is the correct explanation of Assertion.
- Both Assertion and Reason are true and Reason is not the correct explanation of Assertion.
- Assertion is true but Reason is false.
- Both Assertion and Reason are false.
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The Correct Option is C
Solution and Explanation
In $K_4[Fe(CN)_6],Fe $ is present as $Fe^{2+}$.
$Fe^{2+} = [Ar] 3d^6, 4s^0$
Since, all eiecrons are paired, it is diamagnetic in nature.
In $[Fe(H_2O)_6]Cl_3$, Fe is present as $Fe^{3+}$
$Fe^{3+} = [Ar] 3d^5, 4s^0$
$[Fe(H_2O)_6)^{3+} =[Ar]$
Since, it contains five unpaired electrons, it is paramagnetic in nature.
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Concepts Used:
Coordination Compounds
A coordination compound holds a central metal atom or ion surrounded by various oppositely charged ions or neutral molecules. These molecules or ions are re-bonded to the metal atom or ion by a coordinate bond.
Coordination entity:
A coordination entity composes of a central metal atom or ion bonded to a fixed number of ions or molecules.
Ligands:
A molecule, ion, or group which is bonded to the metal atom or ion in a complex or coordination compound by a coordinate bond is commonly called a ligand. It may be either neutral, positively, or negatively charged.