1. Molecular Geometries and Bonding Chapter 9.4-9.8 Bonding Theory Valence Bond Theory Molecular Orbital Theory Complete Ch 9 problems # 29, 36, 38, 39, 42, 45, 49, 52, 55, 63, 75, 77, 85, 87

2. Molecular Geometries and Bonding Let’s Focus on Valence Bond Theory As we saw earlier, a single bond formed between two atoms is formed with orbital overlap.

3. Molecular Geometries and Bonding Let’s Focus on Valence Bond Theory Polyatomic molecules form via hybrid orbitals. Carbon, for example, yields four sp3 hybrid orbitals, allowing a molecule like CH 4 to have a tetrahedral shape.

4. Molecular Geometries and Bonding Hybrid Orbitals As we have discussed before, once you know the electron-domain geometry, you know the hybridization state of the atom.

5. Molecular Geometries and Bonding Valence Bond Theory designates two bond types arising from orbital overlap and hybrid orbitals. Sigma Bonds (σ) And Pi Bonds (π)

6. Molecular Geometries and Bonding Sigma (  ) Bonds Sigma bonds are characterized by  Head-to-head overlap.  Cylindrical symmetry of electron density about the internuclear axis. In other words, electron density concentrated between the two bonded nuclei.

7. Molecular Geometries and Bonding Pi (  ) Bonds Pi bonds are characterized by  Side-to-side overlap.  Electron density above and below the internuclear axis.

8. Molecular Geometries and Bonding Single Bonds Single bonds are always  bonds, because  overlap is greater, resulting in a stronger bond and more energy lowering.

9. Molecular Geometries and Bonding Multiple Bonds In a multiple bond one of the bonds is a  bond and the rest are  bonds.

10. Molecular Geometries and Bonding Multiple Bonds In a molecule like formaldehyde (shown at left) an sp 2 orbital on carbon overlaps in  fashion with the corresponding orbital on the oxygen. The unhybridized p orbitals overlap in  fashion.

11. Molecular Geometries and Bonding Multiple Bonds In triple bonds, as in acetylene, two sp orbitals form a  bond between the carbons, and two pairs of p orbitals overlap in  fashion to form the two  bonds.

12. Molecular Geometries and Bonding Delocalized Electrons: Resonance When writing Lewis structures for species like the nitrate ion, we draw resonance structures to more accurately reflect the structure of the molecule or ion.

13. Molecular Geometries and Bonding Delocalized Electrons: Resonance In reality, each of the four atoms in the nitrate ion has a p orbital. The p orbitals on all three oxygens overlap with the p orbital on the central nitrogen.

14. Molecular Geometries and Bonding Delocalized Electrons: Resonance This means the  electrons are not localized between the nitrogen and one of the oxygens, but rather are delocalized throughout the ion and thus accounting for the equal bond lengths observed throughout the structure.

15. Molecular Geometries and Bonding Resonance The organic molecule benzene has six  bonds and a p orbital on each carbon atom.

16. Molecular Geometries and Bonding Resonance In reality the  electrons in benzene are not localized, but delocalized. The even distribution of the  electrons in benzene makes the molecule unusually stable.

17. Molecular Geometries and Bonding Example Consider acetonitrile: a.Predict the bond angles around each carbon atom b.Give the hybridization at each of the carbon atoms c.Determine the number of σ and π bonds in the molecule

18. Molecular Geometries and Bonding Example Which of the following molecules or ions will exhibit delocalized bonding? SO 3, SO 3 2-, H 2 CO, O 3, NH 4 +

19. Molecular Geometries and Bonding Valence Bond Theory in a Nut Shell… 1.All covalent bonds are formed by the sharing of two or more electrons. All bonds will have at least one of these bond pair concentrated in the space between the two interacting nuclei forming a sigma bond. 2.The appropriate set of hybrid orbitals used to form these sigma bonds is determined by the geometry of the molecule. 3.Atoms that share more than one pair of electrons will do so in pi bonds, which lie above and below the nuclei. 4.Molecules with two or more resonance structures can have pi bonds that extend beyond the two bonded atoms, allowing electrons to become delocalized.

20. Molecular Geometries and Bonding Molecular Orbital (MO) Theory Though valence bond theory effectively conveys most observed properties of ions and molecules, there are some concepts better represented by molecular orbitals.

21. Molecular Geometries and Bonding Molecular Orbital (MO) Theory In MO theory, we invoke the wave nature of electrons. If waves interact constructively, the resulting orbital is lower in energy: a bonding molecular orbital.

22. Molecular Geometries and Bonding Molecular Orbital (MO) Theory If waves interact destructively, the resulting orbital is higher in energy: an antibonding molecular orbital.

23. Molecular Geometries and Bonding MO Theory MO Theory begins with the construction of molecular orbitals. Whenever two atomic orbitals overlap, two molecular orbitals form. Let’s consider H 2. Notice, two orbitals will overlap, and thus, two molecular orbitals formed.

24. Molecular Geometries and Bonding Let’s turn this into a diagram…

25. Molecular Geometries and Bonding MO Theory In H 2 the two electrons go into the bonding molecular orbital. The bond order is one half the difference between the number of bonding and antibonding electrons. Recall, bond order indicates the stability of the bond formed.

26. Molecular Geometries and Bonding MO Theory For hydrogen, with two electrons in the bonding MO and none in the antibonding MO, the bond order is 1212 (2 - 0) = 1

27. Molecular Geometries and Bonding MO Theory In the case of He 2, the bond order would be 1212 (2 - 2) = 0 Therefore, He 2 does not exist.

28. Molecular Geometries and Bonding Example Write the electron configuration in terms of MOs and determine the bond order of H 2 - and H 2 +.

29. Molecular Geometries and Bonding Example According to molecular orbital theory, would either Be 2 or Be 2 + be expected to exist? Explain.

30. Molecular Geometries and Bonding MO Theory For atoms with both s and p orbitals, there are two types of interactions:  The s and the p orbitals that face each other overlap in  fashion.  The other two sets of p orbitals overlap in  fashion.

31. Molecular Geometries and Bonding MO Theory The resulting MO diagram looks like this. There are both  and  bonding molecular orbitals and  * and  * antibonding molecular orbitals.

32. Molecular Geometries and Bonding MO Theory The smaller p-block elements in the second period have a sizeable interaction between the s and p orbitals. This flips the order of the s and p molecular orbitals in these elements.

33. Molecular Geometries and Bonding Second-Row MO Diagrams

34. Molecular Geometries and Bonding Paramagnetism vs. Diamagnetism Molecular orbital theory allows one to predict the behavior of a substance in the presence of a magnetic field. Molecules with one or more unpaired electrons are attracted into a magnetic field. This behavior is called paramagnetism. Substances with no unpaired electrons are weakly repelled from a magnetic field…they exhibit diamagnetism.

35. Molecular Geometries and Bonding Example Predict the magnetic properties and bond order of the peroxide ion, O 2 2- and the acetylide ion, C 2 2-.

36. Molecular Geometries and Bonding Molecular Orbital Theory This model represents electrons in allowed energy states called molecular orbitals which can spread out across all the atoms of a molecule. MO diagrams represent the combination and relative energies of molecular orbitals. The diagrams allow for easy calculation of bond order, indicating the stability of the bond formed. Bonding and antibonding MOs formed by the combination of s orbitals are called sigma molecular orbitals while the combination of p orbitals are called pi molecular orbitals. The MO model correctly predicts properties like paramagnetism and diamagnetism.

37. Molecular Geometries and Bonding (a) With respect to electronic structure, which element in the second row of the periodic table is most similar to sulfur? (b) Use the VSEPR model to predict the S—S—S bond angles in S 8 and the hybridization at S in S 8. (c) Use MO theory to predict the sulfur–sulfur bond order in S 2. Is the molecule expected to be diamagnetic or paramagnetic? (d) Use average bond enthalpies (Table 8.4) to estimate the enthalpy change for the reaction just described. Is the reaction exothermic or endothermic? SAMPLE INTEGRATIVE EXERCISE Putting Concepts Together Elemental sulfur is a yellow solid that consists of S 8 molecules. The structure of the S 8 molecule is a puckered eight-membered ring (Figure 7.30). Heating elemental sulfur to high temperatures produces gaseous S 2 molecules: