The following complexes are given:1. text{tra | vedclass

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(D) Analysis of optical activity:$1$. $	ext{trans}-[Co(NH_3)_4Cl_2]^+$ has a plane of symmetry,so it is optically inactive.$2$. $	ext{cis}-[Co(NH_3)

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$2$ is optically active; $1$,$3$ are optically inactive

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(D) Analysis of optical activity:$1$. $	ext{trans}-[Co(NH_3)_4Cl_2]^+$ has a plane of symmetry,so it is optically inactive.$2$. $	ext{cis}-[Co(NH_3)_2(en)_2]^{3+}$ lacks a plane of symmetry and is chiral,so it is optically active.$3$. $	ext{trans}-[Co(NH_3)_2(en)_2]^{3+}$ has a plane of symmetry,so it is optically inactive.Analysis of colour:$4$. $[NiCl_4]^{2-}$ ($Ni^{2+}$: $d^8$ configuration) is coloured due to $d-d$ transitions.$5$. $[TiF_6]^{2-}$ ($Ti^{4+}$: $d^0$ configuration) is colourless due to the absence of $d-d$ transitions.$6$. $[CoF_6]^{3-}$ ($Co^{3+}$: $d^6$ configuration) is coloured due to $d-d$ transitions.Comparing with options,option $D$ correctly states that $2$ is optically active,while $1$ and $3$ are optically inactive.

The following complexes are given:
$1$. $\text{trans}-[Co(NH_3)_4Cl_2]^+$
$2$. $\text{cis}-[Co(NH_3)_2(en)_2]^{3+}$
$3$. $\text{trans}-[Co(NH_3)_2(en)_2]^{3+}$
$4$. $[NiCl_4]^{2-}$
$5$. $[TiF_6]^{2-}$
$6$. $[CoF_6]^{3-}$
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The following complexes are given:$1$. $\text{trans}-[Co(NH_3)_4Cl_2]^+$ $2$. $\text{cis}-[Co(NH_3)_2(en)_2]^{3+}$ $3$. $\text{trans}-[Co(NH_3)_2(en)_2]^{3+}$ $4$. $[NiCl_4]^{2-}$ $5$. $[TiF_6]^{2-}$ $6$. $[CoF_6]^{3-}$ Choose the correct code: