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Chem-To-Go Lesson 19 Unit 4 COVALENT BONDING – VSEPR THEORY

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THREE-DIMENSIONAL Actual bond angles = 109.5˚ Valence Shell Electron Pair Repulsion Theory Areas of electron density repel each other and spread out as far as possible in 3-dimensions

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PREDICTING 3-D SHAPE & ANGLES # regions of high electron density molecular shapebond angle 2linear180° 3trigonal planar120° 4bent <109.5° 4tetrahedral109.5° 4trigonal pyramidal<109.5°

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Example #1: SiO 2 # regions of high electron density molecular shape bond angle 2linear180° 3 trigonal planar 120° 4bent <109.5° 4tetrahedral109.5° 4 trigonal pyramidal <109.5°

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Example #2: SO 3 # regions of high electron density molecular shape bond angle 2linear180° 3 trigonal planar 120° 4bent <109.5° 4tetrahedral109.5° 4 trigonal pyramidal <109.5°

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Example #3: H 2 O # regions of high electron density molecular shape bond angle 2linear180° 3 trigonal planar 120° 4bent <109.5° 4tetrahedral109.5° 4 trigonal pyramidal <109.5°

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Example #4: CCl 4 # regions of high electron density molecular shape bond angle 2linear180° 3 trigonal planar 120° 4bent <109.5° 4tetrahedral109.5° 4 trigonal pyramidal <109.5°

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Example #5: PCl 3 # regions of high electron density molecular shape bond angle 2linear180° 3 trigonal planar 120° 4bent <109.5° 4tetrahedral109.5° 4 trigonal pyramidal <109.5°

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