Oxygen is a non polar molecule so its molecules have only Vander waal's forces of attraction.
The molecules haves secondary types of bondings as 1- Dipole-Dipole interaction, 2- Vander waal's bonding and 3- Hydrogen bonding, depending upon nature of molecules.
Van der Waals forces are usually considered to includedipole - dipole interactionsdipole- induced dipole interactionsinstantaneous dipole - induced dipole interactions (London dispersion forces)These are electrostatic in nature, and cause an attraction between molecules
They vary depending on the molecules under consideration. They are all electrostatic in nature deriving from the interaction of permanent or instantaneous dipoles. They are lumped together as Van der Waals forces but can be considered to be of 3 types:-Keesom forces permanent dipole dipole interactionsDebye forces; permanent dipole interaction with induced dipole,London dispersion forces ; interaction between two instantaneous dipoles.
Solids are held together but different types of intermolecular forces. The nature of these forces depends on the compound. In nonpolar substances, only dispersion forces at work. In polar compounds, dipole-dipole forces also hold the molecules together. Since dipole-dipole forces are stronger than dispersion forces, polar compounds usually have a higher melting point than nonpolar ones.
When molecules are close together, a slight attraction can develop between the oppositely charged regions of nearby molecules. Apex------They form temporary, weak dipole attractions between molecules.
Solids are held together but different types of intermolecular forces. The nature of these forces depends on the compound. In nonpolar substances, only dispersion forces at work. In polar compounds, dipole-dipole forces also hold the molecules together. Since dipole-dipole forces are stronger than dispersion forces, polar compounds usually have a higher melting point than nonpolar ones.
HF has a much higher boiling point than other halogens because HF is a very polar bond and is capable of hydrogen bonding between molecules. Hydrogen bonding is the strongest type of intermolecular force of attraction. where as all other halogens has dipole-dipole forces and van der Waal's forces of attraction between molecules, but these are weaker than hydrogen bonding and so it has a lower boiling point because it is easier to separate molecules of them from each other during the change from liquid to gas.
Dipole-dipole interactions are of electrostatic nature.
the nature of symmetry of a field due to a dipole is cylindrical in nature
Water's polar nature affects its ability to dissolve different substances because of the charges of its molecules. Since its oxygen atom is negatively charged and its hydrogen atoms are positively charged, it makes it strong enough to tear apart other polar substances that are poured into it.
This is because of its polar nature - water molecules have a strong dipole, therefore, the water molecules attract each other more than most other molecules do.
Depending on the exact nature of the polar molecule, the most significant forces would be hydrogen bonding or dipole-dipole forces.