For the octahedral complexes of `Fe^(3+)` in `SCN^-` (thiocyanato-S) and in `CN^-` ligand environments, the difference between the spin-only magnetic moments in Bohr magnetons (when approximated to the nearest integer) is [Atomic number of Fe = 26]

For the complex [Fe(CN)_6]^(3-) , write the hybridization type, magnetic character and spin nature of the complex. (At. number : Fe = 26)

For the complex K_3[Fe(CN)_5NO] identify the cental atom and ligands.

The spin magnetic moment of the complex [Fe(CN)_6]^(4-) is ................. .

Assume that each iron atom has a permanent magnetic moment equal to 2 Bohr magneton . The number density of atoms in iron is 8.52 xx 10^28 m^-3 . Find the maximum value of intensity of magnetisation.

Consider the following complex ions, P, Q and R. P = [FeF_6]^(3-), Q = [V(H_2O)_6]^(2+) and R = [Fe(H_2O)_6]^(2+) . The correct order of the complex ions, according to their spin-only magnetic moment values (in B.M.) is

Assume that each iron atom has a permanent magnetic moment equal to 2 Bohr magneton . The number density of atoms in iron is 8.52 xx 10^28 m^-3 . Find the maximum value of magnetic induction in an iron bar.

If hydrogen atoms (in the ground state ) are passed through an homogeneous magnetic field, the beam is split into two parts. This interaction with the magnetic field shows that the atoms must have magnetic moment. However, the moment cannot be due to the orbital angular momentum since l=0. Hence one must assume existence of intrinsic angular momentum, which as the experiment shows, has only two permitted orientations. Spin of the electron produce angular momentum equal to S=sqrt(s(s+1))(h)/(2pi) where S=+(1)/(2) . Total spin of an atom = +(n)/(2) " or "-(n)/(2) where n is the number of unpaired electrons. The substance which contain species with unpaired electrons in their orbitals behave as paramagnetic substances. The paramagnetism is expressed in terms of magnetic moment. The magnetic moment of an atom mu_(s)sqrt(s(s+1))(eh)/(2pimc)=sqrt((n)/(2)((n)/(2)+1))(eh)/(2pimc)" "s=(n)/(2) impliesmu_(s)=sqrt(n(n+1)) B.M. 1. B.M. (Bohr magneton)= (eh)/(4pimc) If magnetic moment is zero the substance is diamagnetic. If an ion of _(25)Mn has a magnetic moment of 3.873 B.M. Then oxidation state of Mn in ion is :

If hydrogen atoms (in the ground state ) are passed through an homogeneous magnetic field, the beam is split into two parts. This interaction with the magnetic field shows that the atoms must have magnetic moment. However, the moment cannot be due to the orbital angular momentum since l=0. Hence one must assume existence of intrinsic angular momentum, which as the experiment shows, has only two permitted orientations. Spin of the electron produce angular momentum equal to S=sqrt(s(s+1))(h)/(2pi) where S=+(1)/(2) . Total spin of an atom = +(n)/(2) " or "-(n)/(2) where n is the number of unpaired electrons. The substance which contain species with unpaired electrons in their orbitals behave as paramagnetic substances. The paramagnetism is expressed in terms of magnetic moment. The magnetic moment of an atom mu_(s)sqrt(s(s+1))(eh)/(2pimc)=sqrt((n)/(2)((n)/(2)+1))(eh)/(2pimc)" "s=(n)/(2) impliesmu_(s)=sqrt(n(n+1)) B.M. 1. B.M. (Bohr magneton)= (eh)/(4pimc) If magnetic moment is zero the substance is diamagnetic. Which of the following ion has lowest magnetic moment?

Explain why [Fe(H_2O)_6]^(3+) has magnetic moment value of 5.92 B.M. whereas [Fe(CN)_6]^(3-) has a value of only 1.74 BM.

What do you understand by weak field and strong field ligands? With the help of crystal field theory calculate the number of unpaired electrons in octahedral complexes of Fe^(3+) in the presence of weak field ligand.