Question

each polar molecule is known as a dipole. the attraction between the positive end of one dipole and the negative end of another is called a dipole - dipole force

1. observe: turn on the show nonpolar molecules inset. what do you notice?

non - polar molecules have temporary charges due to electron distribution variations, leading to london dispersion forces.
even when the molecules are nonpolar, random variations in the distribution of electrons can cause parts of these molecules to become slightly charged. this imbalance leads to very tiny, short - lived attractions between molecules called london dispersion forces

1. experiment: turn off show polar molecule inset and show nonpolar molecule inset. drag two h₂o molecules into the simulation area, and click play. click pause (⏸) when you see an attraction (dotted line) form between molecules. sketch the molecules, partial charges, and the attraction between them in the space to the right.

why is a hydrogen atom in one h₂o molecule attracted to the oxygen atom in an adjacent h₂o molecule?
because oxygen is more electronegative, creating partial charges. the intermolecular force between h2o molecules is hydrogen bonding.
drag the h₂o - h₂o molecule combination into the correct bin on the right. which type of intermolecular force causes attraction between h₂o molecules?
(activity c continued on next page)

Explanation:

Non - polar molecules show temporary charges from electron distribution variations causing London dispersion forces. In water ($H_2O$), oxygen's high electronegativity creates partial charges, leading to hydrogen bonding between $H_2O$ molecules.

Answer:

1. Non - polar molecules have temporary charges due to electron distribution variations, leading to London dispersion forces.
2. Hydrogen bonding causes the attraction between $H_2O$ molecules.