1. Molecular Shape and Polarity The Importance of Geometry in Determining Physical Properties

2. Structure Determines Properties It is important to understand structure in order to predict properties Structure can be predicted Predicting molecular structure begins with Lewis Dot Diagrams

3. Drawing Lewis Dot Structures First step: decide what atoms are bonded together – This is not always an easy choice For most binary covalent compounds and polyatomic ions the central atom will be the atom that occurs only once in the formula. When in doubt use the most symmetrical atom arrangement. Using CH 4 and CO 3 2- as examples H O O H C H and C H O

4. Lewis Dot Structures- Step 2 2. Count the total number of valence electrons in the ion or molecule – CH 4 has 8 valence electrons, 4 from Carbon and 1 from each of the four H atoms – CO 3 2- has 24 valence electrons, 4 from Carbon, 6 from each of the three Oxygen, plus 2 added to give the ion a charge of 2-

5. Lewis Dot Structures- Step 3 Place a pair of electrons (dots) between the central atom and each of the other atoms. H O O H C H and C H O

6. Lewis Dot Structures- Step 4 Distribute the remaining outer electrons so that each atom has a filled outer energy level, a filled octet (exceptions H only 2, B only 6) A complete Structure This structure does not work it needs 2e-

7. Lewis Dot Structures- Step 5 When there are not enough electrons to satisfy the octet rule, make double or triple bonds When there are extra electrons, place these on the central atom.

8. Check up from the Neck Up! Draw Lewis Structures for each of the following. 1.H 2 S 2.NH 4 + 3.NO 3 - 4.CO 5.CCl 4 6.HCOOH (one H bonds to C, One to O)

9. Answers

10. Outer Level Electron Pair Repulsion Outer level electron pair charge clouds repel each other The electron pairs stay as far away from each other as possible to minimize repulsion This theory explains many of the shapes of molecules.

12. Multiple Bond Molecular Shapes Carbon atom can form 4 chemical bonds with several arrangements – These can be single bonds in a tetrahedral arrangement – Can form 1 double bond and 2 single bonds having trigonal planar geometry – 2 double bonds are arranged in a linear molecule – Carbon can also form 1 single bond and 1 triple bond

13. Polarity Most chemical bonds are not 100% ionic nor 100% covalent because of differing electronegativities. Unequal sharing creates polar molecules or polar covalent bonds – H-Cl is a polar bond H Cl an arrow is used to represent a polar bond, pointing toward the more electronegative element. – Not all polar bonds create polar molecules, geometry plays a role Symmetrical arrangement of polar bonds can cancel polar effect. Unsymmetrical arrangements can produce polar molecules

14. Polarity Unsymmetrical arrangements occur in water, creating a polar molecule Many Physical properties, such as melting and boiling points and solubility are affected by degree of polarity of molecules

15. Apply what we’ve learned about polarity. Determine the polarity of HCN and SOCl 2 – First draw the Lewis structures and identify the geometry – Then use electronegativity to determine polarity (pg302) – Draw the appropriate arrows and geometry

16. Answers H  C  N en H=2.1, en C=2.5, en N=3.0 Linear O  S  Cl en S=2.5, en Cl= 3.0, en O=3.5 Cl trigonal pyramid

17. Geometry and Polarity Determine Physical Properties