What you’ll learn4 learning objectivesChoose one objective for a focused lesson, or study the complete topic.3.6.1Hydrogen bonding• Ammonia and water as simple examples- (a) describe hydrogen bonding, limited to molecules containing N–H and O–H groups, including- (b) use the concept of hydrogen bonding to explain the anomalous properties of H₂O (ice and water):- its relatively high melting and boiling points- its relatively high surface tension- the density of solid ice compared with liquid waterSyllabus objective3.6.2Electronegativity and bond polarity• Use the concept of electronegativity to explain bond polarity and dipole moments of moleculesSyllabus objective3.6.3Van der Waals’ forces as the intermolecular• Those due to bond formation, and use the term van der Waals’ forces as a generic term to describe all intermolecular forces- (a) describe van der Waals’ forces as the intermolecular forces between molecular entities other than- (b) describe the types of van der Waals’ forces:- instantaneous dipole–induced dipole (id-id) forces, also called London dispersion forces- permanent dipole–permanent dipole (pd-pd) forces, including hydrogen bonding- (c) describe hydrogen bonding and understand that hydrogen bonding is a special case of permanent dipole–permanent dipole forces between molecules where hydrogen is bonded to a highly electronegative atomSyllabus objective3.6.4That, in general, ionic, covalent and metallic• State that, in general, ionic, covalent and metallic bonding are stronger than intermolecular forcesSyllabus objective