How come ionic bonds do not conduct electricity and metallic bonds do?
1 Answer
Because the ions bound by ionic bonds ARE NOT FREE TO MOVE in the solid-state....
Explanation:
On the other hand, in a metallic lattice, each atom is considered to contribute one or more of its valence electrons to the overall structure. The electrons are said to be delocalized, i.e. not associated with a particular and free to move over the entire structure, and conduct a current.
The ions in a solid ionic lattice are conversely NOT free to move. In solution, however, anions and cations exist as solvated particles....an aqueous solution of common salt will conduct a current.....
As given, this equation represents a chemical reaction, in that strong electrostatic bonds have been broken, and new substances, the aquated ions, have been formed. That the reaction is reversible does not alter this condition.
