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4. In Part 1 of this experiment, CoCl, 6H,O reacts with ammonium chloride, ammonium hydroxide, and hydrogen peroxide to produ
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a) The balanced equation for the given reaction is :

2CoCl2·6H2O(s) + 2NH4Cl(s) + 10NH4OH(aq) + H2O2(aq) = 2[Co(NH3)6]Cl3(s) + 24H2O(l)

b) The activated charcoal/charcoal serves as a catalyst for the reaction that forms the bonds between NH4OH or NH3(aq) and Co. Conveniently, it also catalyzes the transformation of Co2+ into Co3+ by the H2O2.

c) H2O2 must be added slowly and in 1 ml portions, as it is unstable and decomposes to form water, oxygen gas and heat. There is liberation of oxygen gas occurring at that time, which causes effervences or bubbling and even heat is produced, so to prevent any accident to occur and to let the reaction go on smoothly, hydrogen peroxide must be added in the before said manner. The purpose of the hydrogen peroxide (H2O2) is to convert the cobalt from Co2+ to Co3+.

d) The total number of ligands attached to the central metal ion is called its coordination numbEr. In other words, coordination number is the number of ligands in the coordination sphere of the complex compound. Hence, the coordination number of Co in [Co(NH3)6]Cl3 is 6.

A neutral coordination compound normally consists of a complex ion—a transition metal ion with attached ligands—and counter ions, anions or cations needed to produce a neutral compound.​​​​​​​ In this case  [Co(NH3)6]3+ will be the complex ion and Cl- will be the counter ion. Complex ions are ions with a central metal ion bonded to one or more molecules or ions. A counter ion is the ion that accompanies an ionic species in order to maintain electric neutrality.

Actually [Co(NH3)6]Cl3 is a neutral complex, but if only [Co(NH3)6]3+ complex ion is considered, then it has the charge 3+.

The oxidation state of Co in CoCl2·6H2O is +2, as the 2 Cl atoms contain charge of 1- each, so to make the addition of charges of both Co and Cl equal to 0, the oxidation state of Co will be 2+.  Let the oxidation state of Co be x

x+2(-1) = 0 ; x-2 = 0 ; x = +2

The oxidation state of Co in [Co(NH3)6]Cl3 is +3.

Let the oxidation state of Co be x

As there are 6 ammonia ligands which are neutral and hence carry no charge. The chlorine ligands carry a charge of -1 each and thus they have -3 charge on them. But as the molecule in whole is a neutral the coordination sphere must carry a charge of +3. So, the oxidation state of Co is +3.   

In the complex [Co(NH3)6]Cl3 the oxidation state of Co +3.

So, the electronic configuration of Co3+ will be [Ar]3d6. So it has 2 paired electrons and 4 unpaired electrons, i.e. Co has 6 d-electrons in the given complex.

(Note : If you liked the answer then please give a thumbs up. As you didn't mention which question is to be answered, I answered the first one according to HOMEWORKLIB RULES. If you have any doubts, then please comment.)

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