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In a metallic lattice the attractive forces/bonds between metal ions and the surrounding mobile sea of electrons are strong. Strong attractive forces/bonds require a high temperature to be overcome/broken. E.g. The MP for chromium is 1900oC, and for iridium, 2450oC.

(* Some metals have low melting points such as Mercury, -39oC, and the Group 1 metals: Li = 180oC, Na = 98oC, rubidium = 39oC, caesium = 29oC.)

The attractions, between the polar solvent molecules and the metallic lattice cations/electrons, are not strong enough to pull them from the lattice. (Also: electrons are too tiny to be successfully surrounded by solvent molecules.)

Non-polar molecules have no permanently charged parts that can be attracted to the charged cations/electrons.

The mobile sea of electrons can move within the metallic lattice to be an electric current.

Even when the metallic lattice has been broken by high temperatures, so that the metal is in the liquid state, there is still a mobile sea of electrons which can move to be an electric current. (E.g. Liquid mercury conducts.)

The mobile sea of electrons can move around metal cations in the lattice as the cations are moved. This allows the metal to change shape without breaking.


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