For the ions Zn^{2+}, Ni^{2+} and Cr^{3+} whi | vedclass

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(D) The colour of transition metal ions is due to the presence of unpaired electrons which allow $d-d$ transitions.Electronic configurations:$Zn^{2+}

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Only $Zn^{2+}$ is colourless and $Ni^{2+}$ and $Cr^{3+}$ are coloured.

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(D) The colour of transition metal ions is due to the presence of unpaired electrons which allow $d-d$ transitions.Electronic configurations:$Zn^{2+} (Z=30): [Ar] 3d^{10} 4s^0$ (All electrons are paired,so it is colourless).$Ni^{2+} (Z=28): [Ar] 3d^8 4s^0$ (Has $2$ unpaired electrons,so it is coloured).$Cr^{3+} (Z=24): [Ar] 3d^3 4s^0$ (Has $3$ unpaired electrons,so it is coloured).Therefore,only $Zn^{2+}$ is colourless,while $Ni^{2+}$ and $Cr^{3+}$ are coloured.

For the ions $Zn^{2+}, Ni^{2+}$ and $Cr^{3+}$ which among the following statements is correct?
(Atomic number of $Zn = 30, Ni = 28$ and $Cr = 24$)

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For the ions $Zn^{2+}, Ni^{2+}$ and $Cr^{3+}$ which among the following statements is correct?(Atomic number of $Zn = 30, Ni = 28$ and $Cr = 24$)