The oxidation state of central metal ion and magnetic moment of Brown ring complex is (A) +1 and 2.8 B.M (B) +1 and 3.87 B.M (C) +1 and 4.8 B.M (D) +2 and 4.89 B.M

If the magnetic moment of a dioxygen species is 1.73 B.M, it may be:

the pair of metal ions that can give a spin - only magnetic moment of 3.9 BM for the complex [M(H_(2) O)_(6)]Cl_(2) is

The spin only magnetic moment of [MnBr_4]^(2-) is 5.9 B.M. Predict the geometry of the complex ion.

A magnetic moment of 1.73 B.M. will be shown by one among the following:

A complex of a certain metal ion has a magnetic moment of 4.90BM Another complex of the same metal ion in the same oxidation state has zero magnetic moment The central metal ion could be which of the following (a) Cr^(3+) ,(b) Mn^(3+) (c ) Fe^(2+)

One unpaired electron in an atom contributes a magnetic moment of 1.1 B.M. Calculate the magnetic moment of Cr

Although Cr^(3+) and Co^(2+) ions have same number of unpaired electrons but the magnetic moment of Cr^(3+) is 3.87 B.M . and that of Co^(2+) 4.87 B.M. because….

Elements of group 14 (a) exhibit oxidation state of +4 only (b) exhibit oxidation state of +2 and +4 (c) form M^(2–)" and "M^(4+) ions (d) form M^(2+)" and "M^(4+) ions

The magnetic moment of a transition metal of 3d series is sqrt48 B.M. It s electronic configuration is

An ion (Mn^(a+)) has the magnetic moment equal to 4.9 B.M What is the value of (a) :