Why is an ionic solid non-conductive, but conductive in aqueous solution?

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Why is an ionic solid non-conductive, but conductive in aqueous solution?

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Answer 1 · 2016-12-04T18:14:37

Because the ions that constitute ionic compounds are not free to move in the solid state...........

Explanation:

The generic ionic solid is $M X$ $MX$ , and consists of equal number of $M^{+}$ $M^+$ and $X^{-}$ $X^-$ ions that are held together in a non-molecular, electrostatically bound lattice. The ions are not free to move in the solid state, and thus cannot carry a charge.

In certain circumstances, with certain solvents, for instance water, the ionic solid can dissolve to produce $M^{+} (a q)$ $M^(+)(aq)$ and $X^{-} (a q)$ $X^(-)(aq)$ ions that are free to move in solution. We write $M^{+} (a q)$ $M^(+)(aq)$ to represent the aquated ion, i.e. ${[M {(O H_{2})}_{6}]}_{6}^{+}$ $[M(OH_2)_6]^+$ or something similar. And in solution these ions can carry a charge in that the ions are mobile.

Water is an excellent solvent for solvating ions. However, it does not solvate all ions, and it is not the only solvent available.

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Why is an ionic solid non-conductive, but conductive in aqueous solution?

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