Bonding

• Effective nuclear charge is the electrostatic attraction valence electrons experience towards the nucleus.
• Ionization energy is the amount of energy required to remove an electron from a gaseous atom.
• Electron affinity is the change in energy of a gaseous atom when an electron is added to the atom, forming an anion.
• Effective nuclear charge = Total number of protons - Total number of shielding electrons
• Covalent bonding is the electrostatic attraction between a shared pair of electrons and a positively charged nuclei.
• Ionic bonding is the electrostatic attraction between a lattice of cations and anions
• Metallic bonding is the electrostatic attraction between a lattice of cations and a sea of delocalized electrons
• London dispersion force occurs when there is a temporary electrostatic attraction between molecules due to an instantaneous dipole.
• Dipole-dipole forces occurs when there is an electrostatic attraction between polar molecules and their permanent dipoles.
• Hydrogen bonding (intermolecular force) occurs when a hydrogen is bonded to oxygen, nitrogen, or fluorine due to their extreme electronegativity.
• Intramolecular force describes the forces within a molecule while intermolecular force describes the forces between molecules.

  
• Relationship between intramolecular and intermolecular

  
• Strength of Intermolecular forces from least to greatest

  London dispersion < Dipole-dipole < Hydrogen bonding
• Bond polarity & differences in electronegativity

  
• Bond polarity diagrams

  
• A molecule may have polar bonds present but the symmetry of the molecule may prevent the molecule as a whole being polar if the dipole moments of the individual bonds cancel out.

  
• Polar molecules will dissolve in polar solvents, such as water.
• Non-polar molecules will dissolve in non-polar solvents, such as hexane.