The measure of electrical conductivity for compounds is mainly determined by what factors?

The measure of electrical conductivity for compounds is primarily influenced by the strength of the cation and anion present in the compound. Conductivity in a solution is due to the movement of charged particles, specifically ions. Strong cations and anions are those that dissociate completely in a solution, producing a higher concentration of free ions that can carry an electrical current. This is why ionic compounds, which consist of strong cations and anions, tend to exhibit higher conductivity compared to those with weaker ionic interactions.

While solubility in water is significant for determining whether a compound will dissociate into ions, it is the ability of the ions themselves (their charge and mobility) that determines the level of conductivity. Similarly, molecular weight does not directly impact conductivity since conductivity depends on the presence and concentration of charged particles rather than the mass of the molecules. Temperature can affect conductivity as well, typically increasing it with higher temperatures due to enhanced ion mobility, but the intrinsic strength of the cations and anions remains the primary determinant of a compound's ability to conduct electricity efficiently. Hence, the strength of the cation and anion is the most relevant factor in this context.