50 questions · timed · auto-graded
We know that CO is a neutral ligand and K carries a charge of +1. Therefore, the complex can be written as K+[Co(CO)4]- . Therefore, the oxidation number − of Co in the given complex is -1. Hence, option (iii) is correct.
During salt analysis, a number of basic radicals are detected with the help of the colour changes they exhibit with different reagents. These colour changes are a result of the coordination compounds or complexes that the basic radicals form with different ligands.
[Ni(CO)4]
The process of extraction of some of the metals from their ores involves the formation of complexes. For example, in aqueous solution, gold combines with cyanide ions to form [Au(CN)2]. From this solution, gold is later extracted by the addition of zinc metal.
[Mn(H2O)6]2+
$\text{Then, µ}=\sqrt{\text{n}(\text{n}+2)}$
$=\sqrt{\text{3}(\text{3}+2)}$
$=\sqrt{15}$
$=\text{~}4\text{BM}$
$\text{Then, µ}=\sqrt{4(4+2)}$
$=\sqrt{24}$
$=\text{~}5\text{BM}$
Hence, [Fe(H2O)6]2+ has the highest magnetic moment value.
[Co(NH3)4Cl(NO2)]Cl
[Co(NH3)3Cl3]
3
The given complex can be written as Co(NH3)6 Cl2.
Thus, [Co(NH3)6]+ along with two Cl- ions are produced.
In each of the given complex, Fe is in +3 oxidation state. As C2O42- is didentate chelating ligand, it forms chelate rings and hence (c) out of complexes given above is the most stable complex.
