Well, SeO2 is a bent molecule. It has 2 lone pairs on the Se central atom, giving it bond angles of 109.5 degrees. Because it's bent, it is polar. We also know (hopefully) that all polar molecules exhibit Dipole-Dipole IMFs. And all molecules exhibit London Dispersion Forces (LDFs). Because it doesn't have any Hydrogen atoms, we can rule out Hydrogen Bonding. So it's just Dipole-dipole and LDFs.
London dispersion forces, instantaneous dipole- dipole interaction. CSe2 is non polar. The bonds are expected to be non-polar as the electronegativities for Se and C are identical. As the molecule is linear like CO2 and CS2 any bond dipole would in any event cancel.
London Dispersion
Gravitational, Coulombic, Frictional, Intermolecular, Viscous etc
Potential energy from intermolecular forces
All molecules (and noble gases) experience London dispersion forces with other molecules. CH3COOH is a polar molecule and polar molecules also experience dipole - dipole forces. Because CH3COOH also has an OH group the O of one molecule is strongly attracted to the H (attached to the O) on another molecule. This unusually strong type of dipole-dipole force is called a hydrogen bond. Hydrogen bonds are going to be the most important type of intermolecular force within a group of CH3COOH molecules.
Forces acting on a point such that it gives a null vector by vector addition law, then such type of forces are called balanced forces.
In almost all hydrocarbons, the only type of intermolecular forces that exists is the London forces (Van der Waals forces).
intermolecular forces
Intramolecular forces are not intermolecular forces !
Hydrogen fluoride, with the chemical formula HF, is a colorless gas that is the principal source of fluorine. The type of intermolecular forces that exist in HF are London forces, dipole-dipole.
You think probable to intermolecular forces.
Dipole
ionic
yes it is - gentle warming will change it to vapor though.
London Dispersion Forces
The intermolecular forces are ionic for CoCl2 cobalt chloride. For COCl2 Phosgene they are polar covalent.
These are intermolecular forces.
London Dispersion