Dipole-dipole interactions, London dispersion interactions (sometimes referred to as Van der Waals interactions), hydrogen bonds, and ionic bonds are the four basic intermolecular interaction types in charge of a compound's physical characteristics.
- Ionic bonds, in contrast to covalent bonds, are not directional or specific to particular atoms, but instead interact with the entire cluster of ions to form a lattice:
- The dipole moment, which is denoted by an arrow, determines the degree and direction of polarity in a connection. As seen above, the arrow points from the less electronegative element toward the more electronegative one.
- London Dispersion are the least strong intramolecular interactions, and they take place as an electrostatic interaction of transient dipole moments created in the molecule just when they approach each other sufficiently close.
- A hydrogen atom bound to an electronegative atom like O, N, or F experiences yet another sort of intermolecular electrostatic interaction, called hydrogen bonding.
Which of these forces is present or predominates in a specific compound depends on its functional groups. They are all electrostatic interactions, meaning they all come from the attraction of opposite charges.
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