1. Molecular Geometry 2-2 Ch. 6 – Molecular shape

2. Molecules are three-dimensional objects that occupy a three- dimensional world; In general, only the smallest molecules can be said to have a fixed geometrical shape; the icosahedral C 60 “soccer ball” is a rare exception.

3. VSEPR Theory Valence Shell Electron Pair Repulsion Theory - focuses on the bonding and nonbonding electron pairs present in the outermost (“valence”) shell of an atom to which are connected two or more other atoms. Electron pairs orient themselves in order to minimize repulsive forces.

4. VSEPR Theory Types of e - Pairs –Bonding pairs - form bonds –Lone pairs - nonbonding e - Lone pairs repel more strongly than bonding pairs!!!

5. Draw the Lewis Diagram. Shape is determined by the # of bonding pairs and lone pairs. Know the 5 common shapes ! Determining Molecular Shape

6. 1. Common Molecular Shapes 2 bond 0 lone LINEAR 180° AB 2

7. Linear molecules: AB 2 Ex: BeCl 2 and CO 2. -If you write out the electron dot formula for carbon dioxide, you will see that the C- O bonds are double bonds. Double bonds are treated like single bonds when shape is determined!!!!!!

8. Be 180° Be 90° 270° The shape of BeCl 2 is linear. BeCl 2 TWO ELECTRON PAIRS AROUND BERYLLIUM ATOM ClBeCl THE MOLECULAR SHAPE IS BASED ON THE POSITION OF THE ATOMS!

9. CO 2 O C O 2 bond 0 lone LINEAR 180°

10. 3 bond 0 lone TRIGONAL PLANAR 120° AB 3 2. Common Molecular Shapes

11. Trigonal planar: AB 3 In the molecule BF 3, there are three regions of electron density extending out from the central boron atom. The repulsion between these will be at a minimum when the angle between any two is 120°. This requires that all four atoms be in the same plane; the resulting shape is called trigonal planar.

12. B 120° FF F B THE SHAPE OF BF 3 IS TRIGONAL PLANAR. BF 3 NO OCTET ON B ! THREE ELECTRON PAIRS AROUND THE BORON ATOM. MOLECULAR SHAPE FBF F ATTACH FLOURINES TO EPG.

13. 3. Common Molecular Shapes 2 bond 1 lone BENT <120° AB 2 EAB 2 E 2

14. Shape with lone pairs: AB 2 E 2 2 bonding electrons and 2 lone pairs or AB 2 E, 2 bonding electrons and 1 lone pair Bent: The nonbonding electrons are also in orbitals that occupy space and repel the other orbitals.

15. OSeO SeO 2 SeO 2 IS V-SHAPED, OR BENT Se OO VSEPR treats double bonds like a single bond

16. Se OO OO RESONANCE!

17. 2 bond 2 lone BENT 104.5° H2OH2O Common Molecular Shapes

18. 4 bond 0 lone TETRAHEDRAL 109.5° AB 4 4. Common Molecular Shapes

19. Tetrahedral: AB 4 Methane, CH 4, contains a carbon atom to which are connected four hydrogens. Consequently, the four equivalent bonds will point in four equivalent directions in three dimensions.

20. CH 4 HCH H H There are four electron pairs around the carbon atom. 90° C BUT……….

21. There is a better arrangement for four electron pairs: 109.5° C TETRAHEDRAL The angle is….. Put on the H-atoms…….

22. There is a better arrangement for four electron pairs: TETRAHEDRAL 4 electron pairs tetrahedral EPG C H H H H The shape of CH 4 is tetrahedral.

23. 3 bond 1 lone TRIGONAL PYRAMIDAL 107° AB 3 E 5. Common Molecular Shapes

24. PF 3 3 bond 1 lone TRIGONAL PYRAMIDAL 107° F P F F

25. Polyatomic ions The charge will dictate how many less or extra electrons will be added to the lewis dot diagrams. NO 3 - the negative charge tells you that you need to add one more electron to the diagram. 5 + 3(6) + 1 = 24 Polyatomic ions

26. Nitrate anion N OO O VSEPR treats multiple bonds as effective single electron pairs. Trigonal planar is the shape