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_VSEPR Theory.pptx
- 1.
- 2. explain the shapesof, and bond angles in, molecules by using the qualitative model of electron-pair repulsion (including lone pairs), using as simple examples BF3 (trigonal planar), CO2 (linear), CH4 (tetrahedral), NH3 (pyramidal), H2O (non-linear), SF6 (octahedral), PF5 (trigonal bipyramidal)
- 3. What does theVSEPR states
- 4. VSEPR - Valanceshell electron pair repulsion Electrons pair are arranged around the central atom in such a way to minimise the repulsion between them
- 5.
- 6. Linear planar 180 degrees bondedby 2 electron pairs CO2, CS2 , HCN, BeF2
- 7.
- 8. Trigonal planar 120 degrees bondedby 3 electron pairs BF3 , AlCl3 , SO3 , NO3 -, CO3 2-
- 9.
- 10. Tetrahedral 109.5 degrees bonded by4 electron pairs SiCl4 , SO4 2-, ClO4 -, NH4+ NH4+ L.P of electron got changed to bond pair so repulsion decreases so angle slighty increase NH3 + H+ → NH4+ 107 109.5
- 11.
- 12. Trigonal Bipyramidal 120 and90 degrees bonded by 5 electron pairs PCl5
- 13.
- 14. Octahedral 90 degrees bonded by6 electron pairs SF6
- 15.
- 16. Trigonal pyramidal 107 degrees bondedby 3 electron pairs and one lone pair SiCl4 , SO4 2-, ClO4 -, NH4+ Due to high repulsion between the L.P and B.P electrons, the bond angle slighty decreases to 107 degrees
- 17.
- 18. Bent/V-shape/Angular 104.5 degrees bonded by2 electron pairs and 2 lone pair OCl2 , H2S, OF2 , SCl2, H3O+, SO2 Since there are 2 L.P, so the maxi repulsion taken place between the L.P & L.P and L.P & B.P so angle is reduced to 104.5