CHEM 1201 February 24 Notes
CHEM 1201 February 24 Notes CHEM 1201
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This 1 page Class Notes was uploaded by Kelsie Carter on Saturday February 27, 2016. The Class Notes belongs to CHEM 1201 at University of Colorado Colorado Springs taught by Kristi Follett in Winter 2016. Since its upload, it has received 17 views. For similar materials see in Chemistry at University of Colorado Colorado Springs.
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Date Created: 02/27/16
III. Lewis Dot Structure A. electron Lewis dot structures show valence electrons B. molecular formula: shows the number and kinds of atoms C. structural formula: show the arrangement of the atoms D. shapes of molecules are determined by VSPER theory (valence electron pair repulsion) E. drawing molecules 1. Skeletal structure: rough picture, determine central atom (educated guess), often Carbon 2. Add up the valence electrons for all the elements 3. Place all electrons into pairs on the structure, forming octets 4. Exceptions: P, S, N, O, B, H 5. If you run out of valence electrons before completing octets double/triple bond may be present IV. Shapes of Molecules: molecular geometry Groups or lone pairs surrounding an atom A. Bent: two pairs shared electrons, 2 lone pairs B. Tetrahedral: four pairs of shared electrons C. Trigonal Pyramidal: three pairs of shared electrons, one lone pair (5A) D. Trigonal Planar: three pairs of shared electrons E. Linear: one or two pairs of shared electrons, like diatomics (flat surface) (makes a straight line) V. Electron Geometry- shape considering total number of electron pairs (shared + or – unshared) A. Linear: one or two pairs of electrons, O-C-O B. Trigonal Planar: three pairs of electrons C. Tetrahedral: four pairs of electrons VI. Polarity A. a molecule is polar if the center of positive and negative charge don’t coincide (unequal) B. a molecule is nonpolar if no polarity exists, or positive and negative cancel each other out
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