Explain, with reference to the outer electrons, the type of bonding in sodium chloride and whether it would be a good conductor of electricity.

Because sodium chloride is a compound that consists of a metal and a non-metal, we know that the bonding present in sodium chloride is ionic. This means that electrons are given and taken in order for the two elements to have a full outer shell. Sodium, being in group one, has one electron in its outermost shell. In order for a sodium ion to have a full outer shell, therefore, it must lose one electron (thus making an Na⁺ ion). Chlorine, on the other hand, is in group 7 - it therefore has 7 electrons in its outermost shell, and thus needs to gain one electron for a full electron shell. The chloride ion that is produced is therefore Cl^-.Because of the ions present in this compound, sodium chloride is therefore a good conductor of electricity because the ions present are able to conduct a current. However, this is only the case when the ionic compound is in an aqueous solution, as this allows the ions to flow. Solid ionic compounds would therefore not conduct electricity but aqueous ionic compounds would.