VIIIA Structure and Bonding A

VIIIA Structure and Bonding A - VII Structure and Bonding...

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VII Structure and Bonding
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Lewis Structures Electronic symbols (Lewis symbols) pictorial representation of the outer shell (valence) electrons H(1e) He(2e) H• He : Li(Grp 1) Be(Grp 2) B(Grp 13) C(Grp 14) Li• •Be• • B • • C • N(Grp 15) O(Grp 16) F(Grp 17) Ne(Grp 18) • • • N • • • • O • • • • • • F • • • • • • Ne • • •
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Lewis Structures are combinations of electronic symbols to represent the chemical bonds Terms and Symbols Octet - 8 electrons around an atom Duet - 2 electrons around H - indicates 2 electrons Valence electrons - outer shell electrons Sigma bond ( σ ) - first bond between any 2 atoms Pi bond ( π ) - 2nd and 3rd bond between the same two atoms Lone Pair Electrons - pair of electrons on a atom, not involved in a bond
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Drawing Lewis Structures 1) Count the valence electrons 2) Determine the central atom (least electronegative) 3) Attach atoms to the central atom with sigma bonds 4) Complete octets on all the attached atoms if possible 5) Put extra electrons (if any) on the central atom 6) If not enough electrons to complete octet of the central, form π bonds 7) Determine VSEPR notation
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Determining VSEPR notation VSEPR = Valence Shell Electron Pair Repulsion E = lone pair ( non bonding electrons) on the central atom A = central atom X = attached atom
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Determining Lewis Structures CO 2 (16) O C O O C O AX 2 SO 3 (24) O O S O O O S O O O S O O O S O Resonance forms AX 3
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Resonance forms - different forms of a Lewis structure Differ only in the placement of electrons.
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  • Spring '08
  • Kramer
  • Chemistry, Electron, Valence, Lewis Structure, Chemical bond, Geometry Molecular Geometry, Electron Pair Geometry Linear Trigonal Planar Trigonal Planar Tetrahedral Tetrahedral Tetrahedral Trigonal Bipyramid Trigonal Bipyramid Trigonal Bipyramid Trigonal Bipyramid Octahedral Octahedral Octahedral Molecular Geometry Linear Trigonal Planar Bent T, Molecular Geometry Polarity

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