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Shapes of molecules 1) sketch the Lewis structure 2) locate the central atom 3) count regions of electron density around the central atom double/triple.

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Presentation on theme: "Shapes of molecules 1) sketch the Lewis structure 2) locate the central atom 3) count regions of electron density around the central atom double/triple."— Presentation transcript:

1 Shapes of molecules 1) sketch the Lewis structure 2) locate the central atom 3) count regions of electron density around the central atom double/triple bonds and lone pairs count as ONE region of electron density 4) determine shape and angle bearing in mind that repulsion varies… lone pair-lone pair > lone pair-bonding pair > bonding pair-bonding pair ©

2 Linear 2 regions of electron density around the central atom, which is Beryllium 2 bonding pairs of electrons around the central atom there are no lone pairs of electrons around the central atom the regions of electron density are arranged as far as possible from each other, in order to maximise repulsion, making a LINEAR shape bond angle is 180o eg’s H2, HCl, CO2, O2, CS2, N2, HOCl, BeCl2 ©

3 Trigonal planar 3 regions of electron density around the central atom, which is Boron 3 bonding pairs of electrons, around the central atom there are no lone pairs of electrons, around the central atom the regions of electron density are arranged as far as possible from each other, in order to maximise repulsion, making a TRIGONAL PLANAR shape With a bond angle is 120o eg’s BCl3, BCl2Br, BClBr2, H2CO, COCl2, SO3 ©

4 Tetrahedral 4 regions of electron density around the central atom, which is carbon 4 bonding pairs of electrons around the central atom there are no lone pairs of electrons around the central atom the regions of electron density are arranged as far as possible from each other, in order to maximise repulsion, making a TETRAHEDRAL shape eg’s SiH4, CH2Br2, SO42-, PO43-, SiCl4, CF4 ©

5 Trigonal pyramidal 4 regions of electron density around the central atom, which is Nitrogen 3 bonding pairs of electrons around the central atom there is one lone pair of electrons around the central atom the bond angle of 107o (the lone pair of electrons takes up space as if they were a bond, so the arrangement is tetrahedral but because lone pairs repel more than bonding pairs, the bond angle is less than the expected angle of 109o) Trigonal pyramidal shape eg’s NH3, NF3, PCl3, AsH3, AsF3, PF3 ©

6 V-shaped 4 regions of electron density around the central atom, which is Oxygen 2 bonding pairs of electrons around the central atom there are two lone pairs of electrons around the central atom the bond angle of 104o (the two lone pairs of electrons take up space as if they were a bond, so the arrangement is tetrahedral but because lone pairs repel more than bonding pairs, the bond angle is less than the expected angle of 109o) V-shape or bent eg’s H2O, OF2, SCl2 ©

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