CHMA10H3 Chapter 9: Chapter 9 - Chemical Bonding I Lewis Theory

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CHMA10H3 Full Course Notes
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Chemical bonds form because they lower the potential energy between charged particles (potential energy of bonded atoms < potential energy of separate atoms. Chemical bonds: interactions between atoms (from elements to molecules. Ionic bond: between metal and nonmetal, electron transferred. Covalent bond: between nonmetal and nonmetal, electrons shared. Metallic bond: between metal and metal, electrons pooled. Valence electrons: electrons in all sublevels with highest principal energy shell, very important in bonding. Core electrons: electrons in lower energy shells. Lewis structure of atoms: represent the valence electrons surrounding the symbol of the element, use symbol of element to represent nucleus and inner electrons. Octet rule: stable configuration of 8 electrons in outermost shell, ns2np6. 9. 4 ionic bonding: lewis structures and lattice energies. Atoms bond because it result in a more stable electron configuration (lower potential energy) Electrons are transferred until metal loses all valence electrons and nonmetal has octet.

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