Question

Consider the following and choose the correct option.
Statement -1 :Both $\left[Co\right(ox{)}_3{]}^{3-}and[Co{F}_6{]}^{3-}$ are paramagnetic
Statement 2 :$CoC{l}_3.3N{H}_3$ complex is non conducting.
Statement 3 : The number of all possible isomers for the complex $\left[Pt\right(N{O}_2\left)\right(py\left)\right(OH\left)\right(N{H}_3\left)\right]$ is six
Statement 4: The oxidatation state of iron in brown ring complex $\left[Fe\right(H_{2}O{)}_{5}NO]S{O}_4$ is +2 where $NO$ is $N{O}^{+}$

• A. FTFF
• B. TTTT
• C. FFTF
• D. TTTF

Answer 1

The correct option is A FTFF

Statement -1 : Number of unpaired electron present in $\left[Co\right(ox{)}_3{]}^{3-}and[Co{F}_6{]}^{3-}$ are 0 and 4 respectively. Oxalate is a strong field and fluoride is a weak field ligand. So this statement is false.

Statement -2 : Conduction is due to the presence of ions outside the coordination sphere and hence $CoC{l}_3.3N{H}_3$ is non- conducting.

Statement - 3 : The given complex is a type of [Mabcd] compound where the M is metal and a,b,c,d are 4 different ligands attached to it. This type of complex forms 3 geometrical isomers.

Statement 4 : Since the overall charge on the coordination sphere, $\left[Fe\right(H_{2}O{)}_{5}N{O}^{+}{]}^{2+}$ is +2, the sum of oxidation states of all elements in it should be equal to +1.