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 transcript:

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

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 minimise repulsion, making a LINEAR shape bond angle is 180 o eg’s H 2, HCl, CO 2, HI, O 2, CS 2, N 2, C 2 H 2 ©

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 minimise repulsion, making a TRIGONAL PLANAR shape With a bond angle is 120 o eg’s BCl 2 Br, BClBr 2, C 2 H 4, H 2 CO, COCl 2, SO 3 ©

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 minimise repulsion, making a TETRAHEDRAL shape With a bond angle of o egs SiH 4, CH 2 Br 2, CCl 3 H, SiCl 4, CF 4, CH 3 Br ©

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 1 lone pair of electrons around the central atom the bond angle of less than o (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 o) TRIGONAL PYRAMIDAL shape eg’s NF 3, PCl 3, AsH 3, NI 3, AsF 3, PF 3, ©

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 2 lone pairs of electrons around the central atom the bond angle of less than o (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 o) V-SHAPE or BENT eg’s H 2 O, OF 2, SCl 2, H 2 S, SF 2, NOCl ©

V-shaped 3 regions of electron density around the central atom, which is sulfur 2 bonding pairs of electrons around the central atom there is 1 lone pair of electrons around the central atom the bond angle of less than 120 o (the lone pair of electrons take up space as if they were a bond, so the arrangement is trigonal planar but because lone pairs repel more than bonding pairs, the bond angle is less than the expected angle of 120 o) V-SHAPE or BENT eg’s SO 2, O 3, GeF 2 ©