Final answer:
Covalent compounds have lower melting and boiling points, are more flammable, exhibit poor conductivity, and their solubility in water varies compared to ionic compounds which have higher melting and boiling points, conduct electricity when dissolved, and are typically water-soluble.
Step-by-step explanation:
The properties of covalent compounds and ionic compounds differ significantly because of the differences in the types of bonds present in these compounds. Covalent compounds, which consist of molecules held together by shared pairs of electrons, tend to have lower melting and boiling points, be more flammable, and exhibit poorer conductivity compared to ionic compounds. This is due to their weaker intermolecular forces compared to the strong ionic bonds found in ionic compounds that form crystal lattices.
Ionic compounds, on the other hand, are generally hard crystalline solids which have high melting points and high boiling points. They are typically soluble in water and can conduct electricity when either in a molten state or dissolved in a solution. Conversely, covalent compounds do not conduct electricity well, as they lack free-moving electrons, and their solubility in water can be quite variable.
In summary, the properties that differ between covalent and ionic compounds due to bond type are: conductivity, melting point, boiling point, and solubility. Covalent compounds do not typically vary in color strictly due to bond type; mass and flammability are not solely dependent on bond type, as these can be influenced by other factors as well.