Question

Consider the following statements and arrange in the order of true/ false as given in the codes.
$S_1$: Both $\left[Co\right(ox{)}_3{]}^{3-}$ and $[Co{F}_6{]}^{3-}$ are paramagnetic.
$S_2:CoC{l}_{3}3N{H}_3$ complex is non-conducting.
$S_3$: The number of 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.
$S_4$: The oxidation state of iron in brown ring complex $\left[Fe\right(H_{2}O{)}_{5}N{O}^{+}]S{O}_4$ + II where NO is $N{O}^{+}$.

• A. F T T T
• B. T T T T
• C. F T T F
• D. T T T F

Answer 1

Answer: (C)

F T T F

In solution, $\left[Co\right(N{H}_3{)}_{3}C{l}_3]$ does not dissociate into ions. It exists as neutral molecule. Hence, its aqueous solution does not conduct electricity.
Both linkage and geometrical isomerism are possible in the complex $\left[Pt\right(N{O}_2\left)\right(py\left)\right(OH\left)\right(N{H}_3\left)\right]$. Hence it shows six isomers.
Hence both statements are correct.
The complex $[Co{F}_6{]}_3$ contains 5 unpaired electrons. Hence, it is paramagnetic. In the complex $\left[Co\right(ox{)}_3{]}_3$ all the electrons are paired. Hence it is diamagnetic.
The oxidation state of iron in the complex $Fe\left(H_{2}O\right)5N{O}^{+}]S{O}_2$ is +1.
Hence both the statements are false.