Which of the following is coloured as well as | vedclass

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(D) To be coloured,a complex must have $d-d$ transitions (usually requiring unpaired electrons or charge transfer). To be paramagnetic,it must have at

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$[Cu(NH_3)_4]^{2+}$

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(D) To be coloured,a complex must have $d-d$ transitions (usually requiring unpaired electrons or charge transfer). To be paramagnetic,it must have at least one unpaired electron.$(A)$ $K_2[PtCl_6]$: $Pt^{4+}$ is $5d^6$,low spin,diamagnetic.$(B)$ $K_4[Fe(CN)_6]$: $Fe^{2+}$ is $3d^6$,$CN^-$ is a strong field ligand,$d^2sp^3$ hybridization,diamagnetic.$(C)$ $[Ni(dmg)_2]$: $Ni^{2+}$ is $3d^8$,$dsp^2$ hybridization,square planar,diamagnetic.$(D)$ $[Cu(NH_3)_4]^{2+}$: $Cu^{2+}$ is $3d^9$,$dsp^2$ hybridization,one unpaired electron in $d_{x^2-y^2}$ orbital,paramagnetic and coloured due to $d-d$ transition.

Which of the following is coloured as well as paramagnetic?

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Which of the following pairs of complexes both show optical activity?

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In which of the following orders are the given complex ions arranged correctly with respect to their decreasing spin-only magnetic moment?
$(i)$ $[FeF_{6}]^{3-}$
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$(iv)$ $[Cu(NH_{3})_{4}]^{2+}$

The coordination number,oxidation number,number of electrons in $d$-orbital,and number of unpaired electrons respectively in the complex $[Co(NH_3)_4CO_3]ClO_4$ are . . . . . . .

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