Question

After my research, I have learnt that dipole-dipole forces only exist between polar covalent molecules.

I am aware that covalent networks are not molecules, thus they obviously cannot be classified as a polar covalent molecule. However, covalent networks such as SiC are overall rendered polar, and I have read that SiC does experience dipole-dipole forces between its compounds.
I don’t understand how SiC can experience dipole-dipole forces as it is not made up of molecules - or am I mistaken here? Are covalent networks made up of molecules?
I would be grateful for any help in clearing up my confusion on the overarching question of: Do covalent networks such as SiC experience dipole-dipole forces, and if so, does this force exist between silicon carbide molecules?

Answer 1

Covalent network compounds like SiC can experience dipole-dipole forces despite not consisting of individual molecules. SiC is overall polar due to the difference in electronegativity between silicon and carbon atoms, leading to a net dipole moment.

Step-by-step explanation:

Covalent network compounds, such as SiC, do not consist of individual molecules. Instead, they have a giant 3-dimensional network of covalent bonds. However, these compounds can still experience dipole-dipole forces despite not having individual molecules. In the case of SiC, the compound is overall polar due to the difference in electronegativity between silicon and carbon atoms, leading to a net dipole moment. This allows dipole-dipole interactions to occur between SiC compounds.