Q. 15

(a) Which metal i

Answer :

(a) Cu is the only metal in the first transition series (3d series) that exhibits +1 oxidation state more frequently.


The electronic configuration of Cu is 3d10 4s1. So, when it loses one ‘s’ electron, it acquires a stable 3d10 configuration. Thus, it shows +1 oxidation state more frequently.


(b) We know that the colour of cations depend upon the number of unpaired electrons present in the d-orbital.


So, the electronic configuration of the following cations are:-


1. Sc (Atomic number 21) = [Ar]3d14s2 and Sc3+ = 3d04s0. As discussed, since d-orbital is empty, it is colourless.


2. V (atomic number 23) = [Ar]3d34s2 and V3+ = 3d24s0. As d-orbital is having 2 unpaired electrons, it undergoes d-d transition and gives green colour.


3. Ti (Atomic number 22) = [Ar]3d24s2 and Ti4+ = 3d04s0. As ‘d’ orbital is empty, it is colourless.


4. Mn (Atomic number 25) = [Ar]3d54s2 and Mn2+ = 3d54s0. As ‘d’ orbital has 5 unpaired electrons, it undergoes d-d transition and gives pink colour.


Thus, V3+ and Mn2+ ions are coloured in their aqueous solution due to presence of unpaired ‘d’ electrons.


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