Determine the cell notation for the redox reaction given below. 3 cl2(g) + 2 fe(s) --> 6 cl-(aq) + 2 fe3+(aq) ) fe3+(aq) | fe(s) || cl-(aq) | cl2(g) | pt

cl2(g) | cl-(aq) | pt || fe(s) | fe3+(aq)

fe(s) | fe3+(aq) || cl2(g) | cl-(aq) | pt

cl-(aq) | cl2(g) | pt || fe3+(aq) | fe(s)

fe(s) | cl2(g) || fe3+(aq) | cl-(aq) | pt

Fe(s) | Fe3+(aq) || Cl2(g) | Cl-(aq) | Pt

Explanation:

For the given reaction -

3 Cl₂(g) + 2 Fe(s)  →  6 Cl⁻(aq) + 2 Fe³⁺(aq)  

The reaction have two halves , where there is oxidation process as well as reduction process .

Oxidation process - the process of increase in the number of oxidation state .

And ,

Reduction process - the process of reduction of the number of oxidation state .  

Hence , from the reaction ,

Oxidation process -

Fe(s) → Fe³⁺(aq)

and ,

Reduction process -

Cl₂(g) → Cl⁻(aq)

Writing the cell notation -

The oxidation half is written first and followed by the reduction process , which is separated by the salt bridge .

hence , the cell notation for the above reaction is -

Fe(s) | Fe³⁺(aq) || Cl₂(g) | Cl⁻(aq) | Pt

the electronic configuration of an atom with eight electrons is 1s²2s²2p⁴. the orbital diagrams are shown in the figure.

as per the hunds rule:

1. electrons tend to avoid being in the same orbital as per as practicable.

2. electrons in different orbitals of the same energy will have their spin parallel.

this can be illustrated from the multiplicity of the orbitals of the atom. as there are four electrons in the p orbital and p orbital has 3 sub-shells. the electrons can be fed in different ways as shown in the figure but the correct orbital diagram will be as per the hunds rule.