A complex of platinum,ammonia,and chloride pr | vedclass

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(C) To determine the number of ions produced,we look at the dissociation of the coordination compounds in water:$1$. $[Pt(NH_3)_4]Cl_4 \rightarrow [Pt

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$[Pt(NH_3)_5Cl]Cl_3$

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(C) To determine the number of ions produced,we look at the dissociation of the coordination compounds in water:$1$. $[Pt(NH_3)_4]Cl_4 \rightarrow [Pt(NH_3)_4]^{4+} + 4Cl^-$ ($5$ ions total)$2$. $[Pt(NH_3)_2Cl_4]$ does not dissociate into ions as it is a neutral complex.$3$. $[Pt(NH_3)_5Cl]Cl_3 \rightarrow [Pt(NH_3)_5Cl]^{3+} + 3Cl^-$ ($4$ ions total)$4$. $[Pt(NH_3)_4Cl_2]Cl_2 \rightarrow [Pt(NH_3)_4Cl_2]^{2+} + 2Cl^-$ ($3$ ions total)Since the question states that the complex produces $4$ ions per molecule,the correct structure is $[Pt(NH_3)_5Cl]Cl_3$.

$A$ complex of platinum,ammonia,and chloride produces four ions per molecule in the solution. Which structure is consistent with this observation?

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