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This isĬorrect option is: D Questions & Answers - Magnetic Nature of Ni complexes - MCQġ) How do you calculate the magnetic moment of ions of transition elements?Ģ) What are the strong field and weak field ligands?Ĥ) What is the hybridization & structure of 2-? Question-4) Transition metals show paramagnetic behavior. Note: The charge on metal ions is equal to the charge on the complex since water is a neutral ligand. * Fe 2+ ion has more number of unpaired electrons. * The outer shell electronic configurations of metal ions in the above complexes are shown below. Hence the electronic configurations of metal ions coordinated to water are same as in isolated ions. * As mentioned in previous question, the electronic configuration of metal ions is not much affected by weak field ligand water. Question-3) Among the following ions, which one will have highest Whereas there is only one unpaired electron in Cu 2+ and hence CuSO 4.5H 2O shows lowest degree of paramagnetism.Ĭorrect option is: 'b'. Hence MnSO 4.4H 2O shows greater paramagnetic nature. Mn 2+ ion has more number of unpaired electrons. * The paramagnetic nature of a compound is proportional to the number of unpaired electrons in it. * All the metal ions in the above compounds are divalent and their outer shell electronic configurations are shown below. * In presence of water, which is a weak field ligand, the configurations of metal ions in hydrated compounds reflect those in isolated gaseous ions i.e., no pairing of electrons is possible as the interaction with water molecules is weak.

& Online Coaching Related questions Question-2) Among the following the lowest degree of paramagnetism per mole of the compound at 298 K will be shown by: As there are unpaired electrons in the d-orbitals, NiCl 4 2- is paramagneticĪnd is referred to as a high spin outer orbital complex.īEST CSIR NET - GATE - SET Study Material Therefore, Ni 2+ undergoes sp 3 hybridization to make bonds with Cl - ligands in * Again in NiCl 4 2-, there is Ni 2+ ion, However, in presence of weak field Cl - ligands, NO pairing of d-electrons occurs. Thus 2- isĭiamagnetic. It is said to be a low spin inner orbital complex.

The emptyģd, 3s and two 4p orbitals undergo dsp 2 hybridization to make bonds with CN - ligands in square planar geometry. * In presence of strong field CN - ions, all the electrons are paired up. * In 2-, there is Ni 2+ ion for which the electronic configuration in the valence shell is 3d 8 4s 0. The empty 4s and three 4p orbitals undergo sp 3 hybridization and form bonds with CO ligands to give Ni(CO) 4. Thus Ni(CO) 4 is * All of these 10 electrons are pushed into 3d orbitals and get paired up when strong field CO ligands approach Ni atom. * The valence shell electronic configuration of ground state Ni atom is 3d 8 4s 2. Question-1) Amongst Ni(CO) 4, 2- and NiCl 4 2-:Ī) Ni(CO) 4 and NiCl 4 2- are diamagnetic and 2- is paramagnetic.ī) 2- and NiCl 4 2- are diamagnetic and Ni(CO) 4 is paramagnetic.Ĭ) Ni(CO) 4 and 2- are diamagnetic and NiCl 4 2- is paramagnetic.ĭ) Ni(CO) 4 is diamagnetic 2- and NiCl 4 2- are paramagnetic. 2- HYBRIDIZATION-STRUCTURE- PARAMAGNETIC Hybridization-Ni(CO)4 | 2-| 2- | Structure-Parmagnetic-Diamagnetic-Examples-dsp2