Answer: A. All ionic metal compounds contain a metal cation and a non-metal anion held by electrostatic attraction. When molten, the ions are free to move and electrolysis liberates the metal at the cathode — true for every ionic metal compound (e.g. molten NaCl → Na; molten \(\text{Al}_2\text{O}_3\) → Al; molten \(\text{PbBr}_2\) → Pb).
B is wrong: the metal forms the cation (positive ion) by losing electrons, never the anion. C is wrong: many ionic compounds are insoluble in water — AgCl, \(\text{BaSO}_4\), \(\text{PbI}_2\). Solubility is not a universal property.
D is wrong: ionic solids do not conduct electricity because the ions are fixed in the lattice. They conduct only when molten or dissolved. So only A is true for all ionically bonded metal compounds.
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