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Thermochemical principals and properties (Shapes of Molecules (AB3…

- - - - Order of the levels: 1s 2s 2p 3s 3p 4s 3d 4p
        
        1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6
        
        [Ne]=1s2 2s2 2p6 [Ar]=1s2 2s2 2p6 3s2 3p6
  - - - AB2 linear 180 bent 120(one lone pair, 3 regions) bent 109(two lone pairs, 4 regions).
        AB3 trigonal planar 120 trigonal pyramid 109(one lone pair, 4 regions) T-shaped 90(two lone pairs, 5 regions).
        AB4 tetrahedral 109 see-saw(90 and 120, one lone pair, five regions) square planar 90(two lone pairs, six regions).
        AB5 trigonal bipyramidal 90 and 120 square pyramid 90(one lone pair, six regions).
        AB6 octahedral 90
      - ClF3 has 5 regions of negative charge around the central Cl atom. these regions repel for largest separation into a trigonal bipyramidal shape with bond angles of approximately 90 and 120
        there are three bonding regions and two lone pairs, therefore the shape of ClF3 is T-shaped. there are three polar Cl-F bonds. the Cl atom is the most electronegative. the ClF3 molecule is not symmetrical, so the effect of the bond dipoles will not cancel(out). ClF3 has a molecular dipole, and is therefore a polar molecule.