1. VSEPR. The familiar VSEPR (Valence Shell Electron Pair Repulsion) approach to molecular structure was developed by Ronald Gillespie. The basic idea is that lone pairs of electrons occupy space around a central atom in much the same way as do atoms that are bonded to the central atom. The lone pairs and bonded atoms then assume that geometry that minimizes electrostatic repulsion between them. Ronald Gillespie.

2. Electron domains and molecular geometry: Lewis dot diagram of ammonia each lone pair of electrons plus each atom bonded to the central atom constitute an electron ‘domain’ Ammonia trigonal pyramidal (derived from tetrahedral geometry) lone pair of electrons observed geometry is that where the electron domains are as far apart as possible H H H N

3. Using VSEPR In order to use VSEPR to predict molecular structure: 1)Draw up Lewis dot diagram for the molecule or ion. The first atom (e.g. Br in BrF 5 ) is always the central atom. Place the other atoms around the central atom. If these are single bonds, contribute one electron per attached atom. Then add the valence electrons for the central atom = 7 for Br. 2) Work out number of electron domains = valence electron pairs (‘n’) plus attached atoms on central atom. For BrF 5 n = 6. 3) Relate n to the type of structure predicted for that value of n. n = 6 = octahedral. 4) Place lone pairs in expected positions, maximizing separation of lone pairs. For BrF 5, there is one lone pair, so mol. structure = square pyramidal. red = 7 valence electrons for Br place 5 F atoms around central Br

4. The structure of BrF 5 from VSEPR: Lewis dot diagram n = 6 from five attached atoms plus one electron pair n = 6, parent structure = octahedral, but one site occupied by a lone pair molecular or final structure – disregard the lone pair molecular structure = square pyramidal parent structure lone pair

5. Parent shapes for EX n molecules (n = 2-5) Formula n shapeshapes of structures EX 2 2 linear EX 3 3 trigonal planar EX 4 4 tetrahedral EX 5 5 trigonal bipyramidal

6. Parent shapes for EX n molecules (n = 6-8) Formula n shapeshapes of structures EX 6 6 octahedral EX 7 7 pentagonal bipyramidal EX 8 8 square antiprismatic

7. Final structures for VSEPR theory.

8. More final structures for VSEPR.

9. A series of derivatives of the EX 4 geometry (all with n = 4) but with increasing numbers of lone pairs: Methane ammonia water hydrogen fluoride Tetrahedral trigonal pyramid bent linear diatomic lone pairs

10. Structures derived from trigonal geometry (n = 3): boron trifluoride nitrite anion, NO 2 - trigonal planar bent lone pair

11. Ozone – a bent molecule: The structure of the O 3 (ozone) molecule can be predicted using VSEPR. First draw up the Lewis dot diagram: Central atom (red valence electrons) For the valence shell of the central oxygen atom n = 3, so parent geometry = trigonal. The final structure is thus two-coordinate bent, as seen for the ozone molecule below: Structure of the ozone molecule (oxygens = red atoms) ozone Note that two pairs of e’s still count as only one electron domain = one attached O-atom

12. Structures derived from TBP (n = 5): ( Note: Lone pairs go in the plane:)

13. Structures derived from the octahedron (n = 6):

14. Structures derived from the pentagonal bipyramid (n = 7) (Note: lone pairs go axial)

15. Example: Note: The way the number of valence electrons (= 12) on the iodine is derived is from the seven valence electrons for iodine (group 7 in the periodic table), plus one each from the F-atoms, and one from the negative charge on the complex. Negative charge adds a valence electron to iodine.

16. Example: Chlorine trifluoride NOTE: in structures derived from a TBP parent structure, the lone pairs always lie in the plane, as seen here for the T-shaped structure of ClF 3.

17. The structure of [IF 5 (C 6 H 5 )] -: Note: an aliphatic or aromatic group is equivalent to an F. S.Hoyer, K.Seppelt (2004) J. Fluorine Chem.,125, 989 iodine phenyl group fluorine

18. Diphenyl(acetato)iodine(V)oxide carbon atoms from phenyls oxygen from acetato group two pairs of electrons = double bond oxide oxygen phenyl group iodine

19. The structure of bis(pentafluorophenyl)xenon. VSEPR explains this type of structure, which is linear like XeF 2. (explain the latter in terms of VSEPR) H.Bock, D.Hinz-Hubner, U.Ruschewitz, D.Naumann (2002) Angew.Chem.,Int.Ed., 41, 448 xenon pentafluoro phenyl group

20. The [I(C 6 H 5 ) 2 ] + cation: phenyl group iodine

21. Bis(trifluoroacetato)phenyl-iodine(III) iodine phenyl group trifluoroacetate group

22. The effect of lone pairs on bond angles: In VSEPR the lone pairs appear to occupy more space than electron pairs in bonds, with the result that bond angles are compressed away from the lone pairs. For example, in structures derived from tetrahedral parent geometry, such as water or ammonia, the H-O-H and H-N-H angles are compressed to be less than the 109.5º expected for a regular tetrahedron: lone pairs water ammonia

23. Effects of lone pairs on bond angles in ClF 3 and ClF 5. chlorine trifuoride chlorine pentafluoride 86.0 o 87.5 o