1. Module A-4 Molecular Electronics

2. Bohr Atomic Model

3. Hydrogen Emission Spectra Principal Quantum Number

4. Principal Quantum Numbers Orbital Quantum Number l = 0 to l = (n–1)

5. Quantum Energy States

6. Principal Quantum Numbers

7. Molecular Orbital Considerations H  H-H  H-H-H  H-H-H-H (1s electrons) Li  Li-Li  Li-Li-Li  Li-Li-Li-Li (2s electrons) (Li–Li = 2.67 A, H–H = 0.75 A)

8. Molecular  -Bonding and  * Bonding States

9.  bonds Electrons in chemical bonds ( e.g. H-H and C-H bonds) are generally quite localized and non-co nducting. These bonds are  bonds.Electrons in chemical bonds ( e.g. H-H and C-H bonds) are generally quite localized and non-co nducting. These bonds are  bonds.

10. Alkyl Chains and Aliphatic molecular Insulators   type orbits lie in the molecular plane and are insulating

11. Formulation of Large Molecular Chains

12. Formation of Energy Bands from Constituent Atoms

13. Energy Bands for metals, semiconductors and Insulators

14. Bandgap vs. Chain Length Poly(thiophene)

15. Saturation Effect All properties approach a saturation value.

16. Bandgap vs. conjugation length Increased conjugation length  smaller bandgap

17. Genesis of Nanotechnology 00 Chemistry 96 Chemistry 86 Physics 56 Physics 97 chemistry (Mitre 96)

18. Single Electron Transistors

20. Molecular Break junction SET

21. STM in Molecular Electronic Research Semiconducting