Question

Which of the following compounds is the most stable?

O A. CuCl2
O B. AgCI
O C. AICI3
O D. LICI

Answer 1

The most stable compound among the given options is AgCl

Therefore the correct option is B.

Step-by-step explanation:

In order to determine the stability of these compounds, we can analyze their respective cations and anions. Silver (Ag) and chloride (Cl) have more similar sizes and charges compared to other elements in the given options. The formation of AgCl involves the reaction:

`\[ Ag^+_((aq)) + Cl^-_((aq)) \rightarrow AgCl_((s)) \]`

The
`\( Ag^+ \)` cation has a single positive charge, and the
`\( Cl^- \)` anion has a single negative charge. The attractive forces between these ions lead to the formation of a stable ionic lattice, making AgCl a relatively stable compound.

Additionally, the ionic character of AgCl is significant, contributing to its stability. Ionic character increases with the electronegativity difference between the elements. In this case, the electronegativity difference between silver and chlorine is considerable, enhancing the ionic character of AgCl.

Furthermore, the solubility product constant
`(\(K_(sp)\))` can be considered. AgCl has a low solubility due to a small
`\(K_(sp)\)` value, indicating that only a small fraction of the compound dissolves in water. This limited solubility further supports the stability of AgCl as it tends to maintain its solid state.

In conclusion, the combination of favorable ion sizes, charges, ionic character, and low solubility makes AgCl the most stable compound among the options provided.

Therefore the correct option is B.