Relative Magnitudes of Forces The types of bonding forces vary in their strength as measured by average bond energy. Strongest Covalent bonds (400 kcal/mol) Hydrogen bonding (12 -16 kcal/mol ) Dipole-dipole interactions (2 -0. 5 kcal/mol) Weakest London forces (less than 1 kcal/mol)
Hydrogen Bonding between hydrogen and more electronegative neighboring atoms such as oxygen and nitrogen Hydrogen bonding between ammonia and water
Hydrogen Bonding in DNA Thymine hydrogen bonds to Adenine T A
Hydrogen Bonding in DNA Cytosine hydrogen bonds to Guanine C G
Dipole Related Forces Between Ion - Dipole Ion charge and dipole charge H - bonding Dipole - Dipole Ion – induced dipole Dipole – induced dipole Decreasing Strength Type Polar bonded hydrogen and dipole charge Dipole charge and dipole charge Ion charge and polarizable e- cloud Dipole charge and polarizable e- cloud Stronger than dipole-related forces: Ionic, metallic, and covalent bonding Weaker than dipole-related forces: London dispersion forces
London Dispersion Forces The temporary separations of charge that lead to the London force attractions are what attract one nonpolar molecule to its neighbors. Fritz London 1900 -1954 London forces increase with the size of the molecules. Synonyms: “London forces”, “dispersion forces”, and “dispersion-interaction forces”
London Dispersion Forces
London Forces in Hydrocarbons
Boiling point as a measure of intermolecular attractive forces