Physical Properties:

* Low melting and boiling points: This is because the forces holding the molecules together (intermolecular forces) are relatively weak compared to the strong ionic bonds in ionic compounds.

* Poor conductors of electricity: Covalent compounds usually don't have free-moving electrons, which are necessary for electrical conductivity.

* Many are gases or liquids at room temperature: Their weak intermolecular forces allow them to exist as gases or liquids, rather than solids.

* Often soluble in non-polar solvents: Like dissolves like. Covalent compounds, being non-polar themselves, tend to dissolve in other non-polar solvents.

* Variable hardness: Covalent compounds can range from very hard (e.g., diamond) to very soft (e.g., wax) depending on the specific molecule and how it interacts with other molecules.

Chemical Properties:

* Form by sharing electrons: This is the defining characteristic of covalent bonding.

* Often exist as discrete molecules: The atoms in a covalent compound are linked together in specific arrangements, forming distinct molecules.

* Can be quite reactive: Many covalent compounds readily participate in chemical reactions, forming new bonds.

* Can be organic or inorganic: While organic compounds (containing carbon) are almost always covalent, many inorganic compounds also form covalent bonds.

Important Note: These are general properties, and there are exceptions to each. The specific properties of a covalent compound depend on the types of atoms involved, the structure of the molecule, and the strength of the intermolecular forces.