CH 104 Lecture Notes - Lecture 10: Electron Configuration, Nonmetal, Noble Gas
Document Summary
Joining of two atoms in a stable arrangement. Elements aim to reach the electron configuration of the noble gas closest to them on the periodic table. Number of bonds + number of lone pairs = 4 (except hydrogen) Formed between 2 nonmetals or a nonmetal and a metalloid. Unshared electron pairs are called lone pairs. Main group elements share electrons until they reach an octet. Hydrogen shares electrons until it reaches 2. Shows the location of all valence electrons. Use multiple bonds to fill octets: a double bond contains 4 electrons, a triple contains 6, triple bonds usually involve c,n and o. Total valence electrons- single electron bonds= number of lone pairs in structure. Elements in group 3a only need 6 electrons. Subtract one electron for every positive charge. Add one electron for every negative charge. Two lewis structures that have the same arrangement of atoms but a different arrangement of electrons.