CHM136H1 Lecture Notes - Lecture 2: Valence Electron, Bond Energy, Lone Pair
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CHM136H1 Full Course Notes
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Promoting an electron requires energy excited state. Carbon always has 4 bonds (kekule and couper) The 4 bonds have specific spatial directions (vant hoff & le bel) Covalent bonds are formed from sharing electrons (lewis) Indicating covalent bonds: (lewis structures with dots: h has one dot (1s2, c has 4 dots (1s2, 2s2) (kekule structures lines are drawn for covalent bonds) dots used to indicate a lone pair of electrons. A stable molecule results at a completed shell octet rule. Octet rule: 8 dots for main group atoms 2 dots for hydrogen (more than 8 electrons usage of d orbitals bonding) Atoms with 1/2/3 electrons it forms 1/2/3 bonds. Atoms with 4+ electrons it forms as many bonds as they need electrons to fulfill the octet rule reaching a stable octet. Example: carbon has 4 valence electrons thus it forms 4 bonds. Example: nitrogen has 5 valence electrons and forms 3 bonds one lone pair.
