Intermolecular Forces Graphic Organizer
Table of Contents:
1. Filled-out notes (Teacher’s guide)
2. Scaffolded notes (one box for each column is filled out as an example, and
the “Key Point” is included)
3. Blank notes (non-scaffolded version)
Notes:
This graphic organizer can be used as a guide for class notes: students can fill it
out as a class while the teacher lectures. This graphic organizer could also be used
as an independent activity: students can fill it out as they read their textbook.
Intermolecular Forces
Type of
Bond
Van der Waals Forces
Hydrogen Bonds
Dipole interactions
Dispersion forces
Definition
Oppositely charged regions of
polar molecules are attracted to
each other
Random electron motion on one
molecule affects the electron motion
on the other, and the oppositely
charged regions are attracted.
**These are the weakest interactions
between molecules.
A hydrogen covalently bonded to a
very electronegative atom is also
weakly bonded to an unshared
electron pair of another atom.
Examples
A polar molecule like ammonia
(NH3) experiences dipole forces.
Iodine is solid at room temperature
because its dispersion forces are
strong enough to hold molecules
close together.
Hydrogen bonds in water molecules
give water many of its unique
properties (like high surface
tension).
Picture
Key Point: Intermolecular attractions are weaker than either ionic or covalent bonds but they are still important!
They are the reason for many of the properties we observe in solids and liquids.
Intermolecular Forces
Type of
Bond
Van der Waals Forces
Dipole interactions
Dispersion forces
Hydrogen Bonds
Picture
Definition
Examples
Random electron motion on one
molecule affects the electron motion
on the other, and the oppositely
charged regions are attracted.
**These are the weakest interactions
between molecules.
Hydrogen bonds in water molecules
give water many of its unique
properties (like high surface
tension).
Key Point: Intermolecular attractions are weaker than either ionic or covalent bonds but they are still important!
They are the reason for many of the properties we observe in solids and liquids.
Intermolecular Forces
Type of
Bond
Van der Waals Forces
Dipole interactions
Dispersion forces
Picture
Definition
Examples
Key Point:
Hydrogen Bonds