Reason : All halogens are coloured.
Chlorate ion : $ClO _3^{\ominus}$
Per chlorate ion : $ClO _4^{\ominus}$
$(A)$ Acidic order : $HC1O < HClO _3^{+5}< HClO _4^{+7}$ Conjugate base order : $ClO ^{-}> ClO _3^{-}> ClO _4^{-}$
| $(B)$ Hypochlorite ion $\left( ClO ^{\circ}\right)$ : | (image) Linear shape |
| Chlorate ion $\left( ClO _3^{\ominus}\right)$ : | (image) Trigonal pyramidal shape |
| Perchlorate ion $\left( ClO _4^{\circ}\right)$ : | (image) Perfect tetrahedral shape due to resonance |
In chlorate ion bond angle changes due to presence of lone pair on chlorine atom. While hypochlorite ion is linear and perchlorate ion is tetrahedral and there is no effect of lone pair on hypochlorite ion.
$(C)$ Disproportionation reaction of
$(i)$ hypochlorite ion : $3 ClO ^{\circ} \rightarrow 2 Cl ^{-}+ ClO _3^{\ominus}$
$(ii)$ Chlorate ion : $4 ClO _3^{\circ} \rightarrow 3 ClO _4^{\circ}+ Cl ^{\circ}$
$(D)$ $ClO ^{-}+ SO _3^{2-} \rightarrow SO _4^{2-}+ Cl ^{\circ}$
Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.