CHMB31H3 Chapter 2: CHMB31 Chapter 2
Document Summary
Single bond: a shared electron pair, denoted a-b: covalent bond: formed when two neighboring atoms share an electron pair, double bond: two shared electron pairs, denoted a=b. Triple bond: three shared electron pairs, denoted a b. Lewis structure: diagram that shows pattern of bonds and lone pairs in a molecule. electrons. Decide on the number of electrons that are to be included in the structure by adding together the numbers of all the valence electrons provided by the atoms. Write the chemical symbols of the atoms in the arrangement that shows which atoms are bonded together. Stereochemically inert: lone pairs that do not influence the molecular geometry and are usually in the non-directional s orbitals. molecule. Lone pairs repel other pairs more strongly than bonding pairs do. o. Valence bond theory: valence bond theory (vb theory): considers the interaction of atomic orbitals on separate atoms as they are brought together to form a molecule.
