101 - Considering the graph below, which compares the lattice enthalpy (Fajan's lattice enthalpy) of ionic compounds a to e formed from main group elements of period 4 of the periodic table, which statement is correct? [Figure: Bar graph showing lattice enthalpy (kJ·mol$^{-1}$) on the y-axis with values around 1000 and 4000 marked, and ionic compounds a, b, c, d, e on the x-axis. Compound d has the tallest bar (near 4000), while a, b, c, e have shorter bars (near 1000).]
[(1)] If the cation of compound c has a charge of $+2$, the anion of compound a cannot be a halide ion.
[(2)] If a and b have similar cations, the elements forming their anions can be in the same period of the periodic table.
[(3)] If the ions of compound e have no noble gas electron configuration, then from the charges of the cation and anion in it, we can be certain that the charge of the cation and anion is greater than in the other compounds.
[(4)] If the ionic radius of the anion of compound b is smaller than the ionic radius of the anion of compound d, and their electrical charges are equal, then the ratio of the ionic radius of the cation in b to the ionic radius of the cation in d is greater than $\dfrac{b}{d}$.
\textbf{101 -} Considering the graph below, which compares the lattice enthalpy (Fajan's lattice enthalpy) of ionic compounds \textbf{a} to \textbf{e} formed from main group elements of period 4 of the periodic table, which statement is correct?
\textit{[Figure: Bar graph showing lattice enthalpy (kJ·mol$^{-1}$) on the y-axis with values around 1000 and 4000 marked, and ionic compounds a, b, c, d, e on the x-axis. Compound d has the tallest bar (near 4000), while a, b, c, e have shorter bars (near 1000).]}
\begin{enumerate}
\item[(1)] If the cation of compound c has a charge of $+2$, the anion of compound a cannot be a halide ion.
\item[(2)] If a and b have similar cations, the elements forming their anions can be in the same period of the periodic table.
\item[(3)] If the ions of compound e have no noble gas electron configuration, then from the charges of the cation and anion in it, we can be certain that the charge of the cation and anion is greater than in the other compounds.
\item[(4)] If the ionic radius of the anion of compound b is smaller than the ionic radius of the anion of compound d, and their electrical charges are equal, then the ratio of the ionic radius of the cation in b to the ionic radius of the cation in d is greater than $\dfrac{b}{d}$.
\end{enumerate}