CHEM 001 Lecture Notes - Lecture 12: Lewis Structure, Formal Charge, Sulfur Dioxide

• School: College of The Sequoias
• Department: Chemistry (CHEM)
• Course: CHEM 001
• Professor: guerra

Document Summary

Lec4 resonance: some lewis structures have multiple bonds in different equivalent locations. Formal charge of an atom decides gain or loss of e- while forming a covalent bond to assign formal charge: Determine number of valence electrons per atom. Compare s and l with number of valence electrons of free atom. Anything after group 3 row 3 has extra orbitals they can use to accommodate electrons (ex: p, s, cl) these compounds can form expanded octets radical: compound with unpaired e- More charges+lewis acids and bases they react with almost anything, including dna remember that formal charge: fc=v-(l+b) P, s, and cl can accommodate more than 8 valence electrons (expanded octet) Why? atoms in period 3 or higher have d-orbitals in valence shell that accommodate additional e- Remember that the octet has 8 e- in s2p6 the 3d state here can be used in this case.