CHEM 110 Study Guide - Midterm Guide: Bond-Dissociation Energy, Valence Electron, Hypervalent Molecule
Document Summary
Beh2 (4 valence electrons) and bh3 (6 valence electrons) Rule 3: molecules or ions with atoms that have more than an octet of valence electrons electrons. Bond length: the distance between bonded nuclei. Bond order: the number of electron pairs shared (# of bonds) Bond strength: the energy needed to break a covalent bond (also known as bond dissociation energy) Rule 1: molecules or ions with odd numbers of electrons. Rule 2: molecules or ions with atoms that have fewer than an octet of. Must be from 3rd row of the periodic table or below. If you run into two or more lewis structures that are possible for the same arrangement of atoms, you need to calculate the formal charge on each atom in the molecule. Formal charge = number of valence electrons (isolated atom) number of electrons on the atom in lewis structure (nonbonding electrons + of bonding electron) *easier method: formal charge= valence electrons - (dots + lines)
