Sept_24 - 2 Pairs: e.g. BeH2 - the molecule is LINEAR to...

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2 Pairs: e.g. BeH 2 - the molecule is LINEAR to maximize the distance between bond pairs. - H – Be – H bond angle is 180° H H H B 3 Pairs: e.g. BH 3 - the molecule is trigonal planar - the H – B – H bond angle is 120° H – Be – H
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4 Electron Pairs tetrahedral trigonal pyramidal bent
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Lone Pairs vs. Bond Pairs In a tetrahedron, the expected bond angles are 109.5° H – C – H bond angle = 109.5° H – N – H bond angle = 107° H – O – H bond angle = 104.5° The slight differences are explained by the lone pairs occupying more space than bond pairs around the central atoms
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Multiple Bonds E.g. CO 2 - for the purposes of VSEPR multiple bonds behave like single bonds - so the central carbon would have 2 bonding pairs of electrons around it - carbon dioxide is linear. ¨ ¨ C O O ¨ ¨
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Trigonal bipyramidal Octahedral 6 pairs – e.g. SF 6 5 pairs – e.g. PCl 5 Higher Coordination Geometries
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F F F Cl F F F What about ClF 3 ? Three distinct choices for the structure
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Sept_24 - 2 Pairs: e.g. BeH2 - the molecule is LINEAR to...

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