1. 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