Cuprous ion is colourless while cupric ion is coloured because
Both have half filled $p $ and $d-$ orbitals
Cuprous ion has incomplete $d-$ orbital and cupric ion has a complete $d-$ orbital
Both have unpaired electrons in the $d-$ orbitals
Cuprous ion has a complete $ d-$ orbital and cupric ion has an incomplete $ d-$ orbital
A transition metal ' $\mathrm{M}$ ' among $\mathrm{Sc}, \mathrm{Ti}, \mathrm{V}, \mathrm{Cr}, \mathrm{Mn}$ and $\mathrm{Fe}$ has the highest second ionisation enthalpy. The spin only magnetic moment value of $\mathrm{M}^{+}$ion is. . . . . . .$\mathrm{BM}$ (Near integer)
(Given atomic number $\mathrm{Sc}: 21, \mathrm{Ti}: 22, \mathrm{~V}: 23, \mathrm{Cr}$ : $24, \mathrm{Mn}: 25, \mathrm{Fe}: 26)$
Which is heaviest among the following
Assertion : Cuprous ion $(Cu^+)$ has unpaired electrons while cupric ion $(Cu^{2+})$ does not.
Reason : Cuprous ion $(Cu^+)$ is colourless whereas cupric ion $(Cu^{2+})$ is blue in the aqueous solution.
The aqueous solution of transition metal salt changes colour from pink to blue, when concentrated hydrochloric acid is added to it. The change In colour is due to
In the first transition series, the highest $B.P. $ and $M.P.$ is of