Based on electron shift Dispersion Dipole-Dipole Ion-Dipole Hydrogen Bonding Description: Weakest of all molecular interactions, caused by the movement of electrons. Electrical charge can be unbalanced when caused by movement of electrons. Description: cations attracted to negative dipole end dissolves anion attracted to positive dipole end in polar solvents Description: the attraction interacting a hydrogen atom with an electro negative atom between H2, N2, O2, F2 Description: The attraction of the positive end of one molecule to another Si Cl C F δ+ δ- Based on electron shift P F C H Cl O H N O H Sr2+ Types of molecules: Polar Molecules Relative Strength: are similar but is the 2nd weakest ionic bond Effect on Properties: raises boiling and melting point, dissolves in polar substances Real Life Example: Polar and non-polar don’t mix Other important Facts: Vander Waals Forces Types of Molecules: must contain hydrogen Relative Strength: Second Strongest Effects on Properties: makes boiling and melting points higher Real Life Examples: Water, methanol Other Important Facts: Forces not chemical bonds Types of Molecules: All molecules and atoms Types of Molecules: Polar Molecules ionic Relative Strength: Strongest Effect on Properties: dissolves in polar molecules Real Life Examples: H2o, Salt water Other Important Facts: most commonly found in ionic solutions Relative Strength: Weakest intermolecular force Effect on Properties: As molar mass increases it causes higher melting and boiling points. The shape of the property is also effected. Real Life Example: as molar mass of noble gases increase the boiling point increases Website: chemed.chem.purdue.edu/genchem/.../bp/.../intermol.html Other important information: Dispersion forces are also known as London dispersion forces BY: Brian and group