A student checked the conductivity of 2 different solids and the results are listed in the table below explain why the students
got these results in terms of principles of chemical bonding your explanation should include a discussion of the specific particles present is fake particles present in each substance and how the behavior of these particles is related to the conductivity of the solid?
Solid copper conducts electricity because of the presence of free electrons. There are no free electrons in CuCl2(g) hence it does not conduct electricity.
Metals are known as conductors of electricity because, in the metallic bond, free electrons are attracted to metal cations by electrostatic forces. These free electrons explains the conductivity of solid metals.
However, when these metals form compounds, ions are present. These ions only conduct electricity in the liquid or aqueous states when the ions are free to move about. In the solid or gaseous state, these ions are not free hence, CuCl2(g) does not conduct electricity.
Atoms never gain protons; they become positively charge only by losing electrons. A positive ion is called a cation (pronounced: CAT-eye-on). You may have notice that the number of neutrons in each of these ions was not specified.
