1. Dipole Forces Main Concept:
Dipole forces result from the attraction among the positive ends and negative ends of polar molecules. Hydrogen bonding is a strong type of dipole-dipole force that exists when very electronegative atoms (N, O, and F) are involved.

2. Dipole Forces Dipoles Definition Causes
Polar vs. Nonpolar Interactions
Types of Dipoles
Dipole-Dipole
Dipole-Induced Dipole
Hydrogen Bonding
Definition
Causes

3. - Dipole: an atom or molecule which has slight negative and positive ends caused by an uneven distribution of electrons
- Electronegativity differences are responsible for uneven distributions of electrons between atoms

4. vs
- Molecules with dipole moments experience Coulombic interactions resulting in net attractive interaction when near each other
Intermolecular dipole-dipole forces are weaker than ionic forces/covalent bonds
Interactions between polar molecules are typically greater than between nonpolar molecules of comparable size because interactions act in addition to London dispersion forces

5. (from previous)
Dipole-dipole attractions  represented by diagrams showing positive and negative ends of polar molecules maximizing attractions and minimizing repulsions as a liquid or solid
Dipole-induced dipole interactions  between polar and nonpolar molecules; strength of these forces increases with magnitude of dipole of polar molecule and with polarizability of nonpolar molecule

6. Question:
Order the following in terms of which would have a greater magnitude of dipole and explain why you think this.
HF vs H2O vs NH3

7. - Hydrogen bonding  a relatively strong type of intermolecular interaction
- Between hydrogen atoms covalently bonded to highly electronegative atoms (N, O, and F) attracted to negative ends of a dipole formed by electronegative atoms (N, O, and F) in a different molecule, or different part of same molecule
- When hydrogen bonding is present, small molecules may have strong intermolecular attractions

9. - Representations of hydrogen bonding b/w molecules, or b/w different parts of single molecule (DNA, proteins), show diagrams of molecules with hydrogen bonding and location of hydrogen bonds

10. - Ionic interactions with dipoles are important in solubility of ionic compounds in polar solvents