Explain briefly how instantaneous dipole - induced dipole bonds form.

(ASSISTED WITH DIAGRAMS)

The electrons of a molecule are constantly moving around it in charge clouds, meaning that at any one point in time, the molecule's electrons could be more likely on one side than the other. This creates a dipole in that molecule (a seperation of opposite electrical charges) where one end is positive, with no/little electrons, and the other end, where the electrons are gathered, are negative - this molecule now has a temporary polarity. As alike charges repel, if this molecule approaches a non-polar molecule, it will induce a dipole in this new molecule as the negative end (the electrons there) will repel the electrons in the charge cloud of 'Molecule B', inducing a dipole here. The negative end of Molecule A will have created a positive end in the closest side of Molecule B, and these opposite charges will now attract each other, creating an instaneous and relatively weak bond between the two molecules.