CHEM 120 Lecture Notes - Lecture 14: Linus Pauling, Electronegativity, Chemical Polarity
Document Summary
Lewis bonding theory: emphasizes valence electrons to explain bonding: predicts properties such as: molecular stability, shape, size, and polarity, bonds between atoms are classified based on types of atoms that are bonded together. Polar covalent bonds: the electrons are not always shared equally, but sometimes are, f2 (electrons are shared equally, hf -> h + f - (arrow points towards more negative) a. b. Fluorine pulls harder on the electrons it shares with hydrogen. Polar covalent bond: electrons are shared unequally: electronegativity: the ability of an atom in a molecule to attract bonding electrons to, developed by american chemist, linus pauling. Electronegativity increases across a period (left to right), and decreases: fluorine is the most electronegative element, noble gas atoms are not assigned en values, opposite of atomic size trend. O=o-o o-o=o: resonance hybrids: combination of resonance form (dotted line for bond, extensions of lewis theory suggest that there is some degree of delocalized of electrons.
