The ionic radii of $Rb^{+}$ and $I^{-}$ are $1.46 \ \mathring{A}$ and $2.16 \ \mathring{A}$,respectively. The most probable type of structure exhibited by it is:
- A$CsCl$ type
- B$ZnS$ type
- C$NaCl$ type
- D$CaF_2$ type
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The energy that opposes the dissolution of an ionic solid in a solvent is:
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The radii and charges of six ions are given below:
Ion $J^{+}$ $L^{+}$ $M^{2+}$ $X^{-}$ $Y^{-}$ $Z^{2-}$ Radius $(nm)$ $0.14$ $0.18$ $0.15$ $0.14$ $0.18$ $0.15$
If the ionic compounds $JX$,$LY$,and $MZ$ have the same crystal structure,then the correct order of their lattice energy is:
| Ion | $J^{+}$ | $L^{+}$ | $M^{2+}$ | $X^{-}$ | $Y^{-}$ | $Z^{2-}$ |
| Radius $(nm)$ | $0.14$ | $0.18$ | $0.15$ | $0.14$ | $0.18$ | $0.15$ |
If the ionic compounds $JX$,$LY$,and $MZ$ have the same crystal structure,then the correct order of their lattice energy is:
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