Among the following complexes (K–P)
K3[Fe(CN)6] (K), [Co(NH3)6]Cl3 (L), Na3[Co(oxalate)3] (M), [Ni(H2O)6]Cl2 (N), K2[Pt(CN)4] (O) and [Zn(H2O)6] (NO3)2 (P) the diamagnetic complexes are :
(L) : [Co(NH3)6]Cl3
(M) : Na3[Co(Ox)3]
(O) : K2[Pt(CN)4]
(P) : [Zn(H2O)6] (NO3)2
To determine which complexes are diamagnetic, we need to understand that diamagnetic substances have all electrons paired, meaning no unpaired electrons. This depends on the oxidation state of the central metal ion and its electron configuration in the complex.
Step 1: Identify the central metal ion and its oxidation state in each complex.
Step 2: Determine the number of unpaired electrons for each metal ion in its complex.
Step 3: List the diamagnetic complexes: L, M, O, P.
Thus, the correct option is: L, M, O, P.
Crystal Field Theory: Explains how ligands affect the d orbitals of metal ions, leading to splitting and electron pairing.
Oxidation State Calculation: For a complex, sum of oxidation states of all atoms equals total charge. Example: In [Co(NH3)6]Cl3, let oxidation state of Co be x. x + 6*(0) = +3, so x = +3.
Electron Configuration: Determine dn configuration based on oxidation state. Example: Fe3+ has atomic number 26, so electron configuration is [Ar] 3d5.
Magnetic Property: Diamagnetic if all electrons paired (no unpaired electrons), paramagnetic if unpaired electrons present.