Chapter 10 (Chemical Bonding): Types of Bonding: • Ionic (full transfer of electrons to achieve full octets in all atoms) • A molecule of an ionic compound is referred to as a “formula unit”, as there is no way to distinguish between the end of one unit and the beginning of another within an ionic crystal. o Ionic crystal: (boundless; no molecular boundaries) • Lewis Diagrams of Ionic Molecules: Covalent (sharing of electrons within a single bond to claim full octets around both atoms)o Diatomic elements There are seven naturally-occurring diatomic elements: o Multiple covalent bonds• Predicting # of covalent bonds around common main group atoms ! Carbon: typically 4 covalent bonds, no lone electron pairs ! Nitrogen: typically 3 covalent bonds, 1 lone electron pair ! Oxygen: typically 2 covalent bonds, 2 lone electron pairs ! Any Halogen: typically 1 covalent bond, 3 lone electron pairs • Polar covalent bonds vs. non-polar covalent bonds (Electronegativity) ! The more polar the bond, the more “ionic character” it has• Electronegativity • Lewis Diagrams of covalent molecules:• Exceptions to the octet rule ! Compounds with an odd # of electrons (Oxides of nitrogen) ! Compounds having <4 valence electrons (Be & B) ! Compounds whose central atom is within or above the 3rd row in the periodic table allowing for more than 4 electron pairs.(d-orbital assistance). • Metallic Bonding (delocalized sharing of electrons within a network of atoms)Molecular shape: • Valence Shell Electron Pair Repulsion (VSEPR) • 3 types of Electron Geometry: Linear, Trigonal Planar, Tetrahedral • Types of Molecular Geometry: o Linear, Trigonal Planar, Tetrahedral, Trigonal Pyramidal, Bent.Polar Molecules: Based upon additive contributions of all dipole moments of individual bonds within a