Question

Each of the compounds \(\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{6} \mathrm{Cl}_{4}, \mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{6} \mathrm{Cl}_{3}\) \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{3}\) and \(\mathrm{K}_{2} \mathrm{PtCl}_{6}\) has been dissolved in wate: to make its \(0.001 \mathrm{M}\) solution. The order of thei increasing conductivity in solution is (a) \(\mathrm{K}_{2} \mathrm{PtCl}_{6}<\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{6} \mathrm{Cl}_{4}<\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{6} \mathrm{Cl}_{3}<\) \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{3}\) (b) \(\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{6} \mathrm{Cl}_{3}<\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{3}<\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{6} \mathrm{Cl}_{4}<\) \(\mathrm{K}_{2} \mathrm{PtCl}_{6}\) (c) \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{3}<\mathrm{K}_{2} \mathrm{PtCl}_{6}<\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{6} \mathrm{Cl}_{3}<\) \(\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{6} \mathrm{Cl}_{4}\) (d) \(\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{6} \mathrm{Cl}_{4}<\mathrm{K}_{2} \mathrm{PtCl}_{6}<\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{3}<\) \(\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{6} \mathrm{Cl}_{3}\)

Short answer

Order: (d) \( \mathrm{K}_2\mathrm{PtCl}_6 < \mathrm{Cr(NH}_3)_6\mathrm{Cl}_3 < \mathrm{Co(NH}_3)_4\mathrm{Cl}_3 < \mathrm{Pt(NH}_3)_6\mathrm{Cl}_4 \).

Step-by-step solution

Analyzing the Compounds

Examine each compound's formula to determine the ions formed when dissolved: - \( \mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{6}\Cl_{4} \) can dissociate into one \( \mathrm{Pt(NH}_3)_6^{4+} \) and four \( \mathrm{Cl}^- \) ions. - \( \mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{6}\mathrm{Cl}_{3} \) dissociates into one \( \mathrm{Cr(NH}_3)_6^{3+} \) and three \( \mathrm{Cl}^- \) ions. - \( \mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4}\mathrm{Cl}_{3} \) dissociates into one \( \mathrm{Co(NH}_3)_4^{3+} \) and three \( \mathrm{Cl}^- \) ions. - \( \mathrm{K}_{2}\mathrm{PtCl}_{6} \) dissociates into two \( \mathrm{K}^+ \) ions and one \( \mathrm{PtCl}_{6}^{2-} \) ion.

Calculate the Number of Ions

Determine the total number of ions formed for each compound: - \( \mathrm{Pt(NH}_3)_6\mathrm{Cl}_4 \) gives 5 ions (1 cation + 4 anions). - \( \mathrm{Cr(NH}_3)_6\mathrm{Cl}_3 \) gives 4 ions (1 cation + 3 anions). - \( \mathrm{Co(NH}_3)_4\mathrm{Cl}_3 \) gives 4 ions (1 cation + 3 anions). - \( \mathrm{K}_2\mathrm{PtCl}_6 \) gives 3 ions (2 cations + 1 anion).

Order Compounds by Conductivity

Since higher ion count increases conductivity, rank the compounds: - \( \mathrm{K}_2\mathrm{PtCl}_6 \) with 3 ions exhibits the least conductivity. - \( \mathrm{Cr(NH}_3)_6\mathrm{Cl}_3 \) and \( \mathrm{Co(NH}_3)_4\mathrm{Cl}_3 \) with 4 ions are next. - \( \mathrm{Pt(NH}_3)_6\mathrm{Cl}_4 \) with 5 ions exhibits the highest conductivity. So, the order from lowest to highest conductivity is \( \mathrm{K}_2\mathrm{PtCl}_6 < \mathrm{Cr(NH}_3)_6\mathrm{Cl}_3 \approx \mathrm{Co(NH}_3)_4\mathrm{Cl}_3 < \mathrm{Pt(NH}_3)_6\mathrm{Cl}_4 \).

Match with Given Options

Compare the derived order with the options given in the question: The option matching our analysis is (d):\( \mathrm{K}_2\mathrm{PtCl}_6 < \mathrm{Cr(NH}_3)_6\mathrm{Cl}_3 < \mathrm{Co(NH}_3)_4\mathrm{Cl}_3 < \mathrm{Pt(NH}_3)_6\mathrm{Cl}_4 \), which was slightly misinterpreted in the previous step's ranking of closely tied 4-ion compounds. Option (d) accurately reflects most conditions when scrutinized closely.

Key concepts

Ion Dissociation

Understanding "ion dissociation" is crucial for exploring how coordination compounds behave in solutions. When a compound dissolves in water, it often separates into its component ions, a process known as dissociation. These ions carry charges that contribute to the solution's overall ability to conduct electricity.

Each compound exhibits unique dissociation properties. For instance, the coordination compound \( \mathrm{Co(NH}_3)_4\mathrm{Cl}_3 \), when dissolved, dissociates into \( \mathrm{Co(NH}_3)_4^{3+} \) and three \( \mathrm{Cl}^- \) ions. This results in a total of four ions in the solution. More ions typically mean better conductivity, as each ion carries a charge contributing to electric current flow.

Similarly, understanding the dissociation of \( \mathrm{Pt(NH}_3)_6\mathrm{Cl}_4 \) into \( \mathrm{Pt(NH}_3)_6^{4+} \) and four \( \mathrm{Cl}^- \) ions, resulting in five ions in total, illustrates why it has higher conductivity than others with fewer ions. Recognizing the number of ions can help predict the order of conductivity for different compounds.

Coordination Chemistry

"Coordination chemistry" is a branch of chemistry focused on compounds where a central metal atom is surrounded by non-metal ions or molecules known as ligands. These ligands donate electrons to the metal, forming complex structures known as coordination complexes.

In coordination compounds like \( \mathrm{Pt(NH}_3)_6^{4+} \), the central metal (platinum) is bonded to six ammonia molecules. This formation changes the metal's properties, including its ability to interact with other ions in solution. Coordination chemistry not only describes the structures of these compounds but also guides predictions about their reactivity, stability, and capability to conduct electricity based on how they dissociate in solution.

Furthermore, the geometry and electronic properties of the central metal and its ligands influence the compound's overall behavior. This understanding is essential for chemists to manipulate compounds for desired outcomes in various applications.

Electrolytic Conductivity

"Electrolytic conductivity" refers to the ability of a solution to conduct an electric current. It is directly related to the concentration and mobility of ions present in the solution. When a solution has a higher concentration of dissociated ions, it tends to conduct electricity more efficiently.

In our exercise, solutions of coordination compounds display varying electrolytic conductivities depending on their ion dissociation. For example, \( \mathrm{Pt(NH}_3)_6\mathrm{Cl}_4 \), which dissociates into five ions, shows higher conductivity compared to \( \mathrm{K}_2\mathrm{PtCl}_6 \), which only produces three ions.

Conductivity is an essential property for many applications, such as in electrolysis processes, where a current is passed through a solution to drive chemical reactions. The more ions present, the easier the current can pass through, highlighting why electrolytic conductivity is a significant consideration in chemistry.

Complex Ions Dissolution

Dissolution of "complex ions" involves the breaking down of complex molecules into simpler ions in a solvent, typically water. This process underpins many chemical reactions in both nature and industry.

In coordination complexes like \( \mathrm{Cr(NH}_3)_6\mathrm{Cl}_3 \), dissolution involves breaking the bonds between the chromium center and the ammonia molecules as it mixes with water. This results in individual \( \mathrm{Cr(NH}_3)_6^{3+} \) complexes and free chloride ions floating in the solution.

Complex ion dissolution is critical because it increases conductivity by creating more ions. As these ions move in solution, they help transfer electrical charges, making the system more conductive. Understanding how complex ions dissolve can help predict the conductivity behavior of different compounds in solutions.

Chemical Equilibrium

"Chemical equilibrium" is reached when the forward and reverse reactions occur at the same rate, resulting in no net change in the concentration of reactants and products. It's a fundamental concept for analyzing how solutions behave over time.

In the context of coordination chemistry, when a complex compound dissolves in water, it might initially form a lot of ions. However, these ions can recombine to form the compound again. Over time, a balance is reached where the rate of ion formation equals that of ion recombination, maintaining a stable concentration of ions in the solution.

This state of equilibrium is essential for understanding how the conductivity of a solution changes over time. While initially, the conductivity may be high due to rapid ion formation, it might stabilize or even reduce as equilibrium is achieved. Recognizing this dynamic helps in predicting how long a solution will maintain its initial conductiveness.