CHEM 101 Chapter Notes - Chapter 7: Chemical Polarity, Lone Pair, Bond Length
Document Summary
Bond length - optimum distance between nuclei; minimum energy , maximum stability. Nucleus-electron attractions are greater than the nucleus-nucleus repulsions, resulting in a net attractive force binding atoms together. (higher energy) h+h h - h (lower energy) Bond dissociation energy - amount of energy that must be supplied to break a chemical bond in a molecule (always positive) Bond order - number of electron pairs shared between atoms. Electrostatic potential maps - use color to portray calculated electron distribution. Bond polarity is due to differences in electronegativity. Increased bond polarity leads to increased bond strength. Bonds exist within molecules but not between molecules. Intermolecular forces - attractive forces between molecules; weaker than covalent bonds. Octet rule - each atom wants 8 valence electrons. Lone pairs - pairs of nonbonding electrons. Bonding pairs - pairs of shared electrons. Double and triple bonds - share two and three pairs of electrons.
