206- Referring to the figure below, A, B, and C indicate the lattice energies of which halide compounds, and with larger cations of the same group, the lattice energy of the network changes more? (Read the options from right to left.) [Figure: Graph of lattice energy (kJ/mol) vs. halide ions $\text{F}^-$, $\text{Cl}^-$, $\text{Br}^-$, $\text{I}^-$, showing three curves A, B, C decreasing from approximately 1100, 800, 700 to 600 kJ/mol respectively]
[(1)] K, Na and F, Li
[(2)] Na, Li and K, I
[(3)] Li, Na and K, F
[(4)] K, Na and Li, I
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\textbf{206-} Referring to the figure below, A, B, and C indicate the lattice energies of which halide compounds, and with larger cations of the same group, the lattice energy of the network changes more? (Read the options from right to left.)
\textit{[Figure: Graph of lattice energy (kJ/mol) vs. halide ions $\text{F}^-$, $\text{Cl}^-$, $\text{Br}^-$, $\text{I}^-$, showing three curves A, B, C decreasing from approximately 1100, 800, 700 to 600 kJ/mol respectively]}
\begin{enumerate}
\item[(1)] K, Na and F, Li
\item[(2)] Na, Li and K, I
\item[(3)] Li, Na and K, F
\item[(4)] K, Na and Li, I
\end{enumerate}
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