1. Lecture 2.0 Bonds Between Atoms
Famous Physicists’ Lecture

2. Electronic Structure in Atoms
Max Planck
Electron (1897) has duality,
Wave E=hc/λ = h,
λ =wavelength of electron
 =frequency
Particle of mass, me

3. Bohr Atom Only specific orbits = Atomic Orbitals
Circumference of orbit = n*λ
for Hydrogen, Z=1, R1= nm
Z= number of protons

5. Electronic Structure in Atoms
Ionization energy = transition from n
Emission Radiation (Light and X-rays)
transition nanb gives off Photon with energy
Bonding in Molecules – Ionic and Covalent
Louis Victor Pierre Raymond duc de Broglie

6. EN Not correct due to charge screening and QM

7. Emission Line Spectra

8. Energy Level Diagrams, Hydrogen4
-1.51 eV 3 L
-3.40 eV 2 K
-13.6 eV 1

9. Periodic Table of Element
Chemical Properties

10. Heisenberg Uncertainty Principle
(me v) x  h/(2π)
Cannot specify both momentum (or velocity) and location of an electron at same time
Electrons are smeared in space
Probability of finding an electron at a location is best way to describe and electron

11. Schrodinger Wave Equation (time independent)
Wave Function, ψ=f(r,θ,φ)
Probability of finding an electron=
| ψ|2 = ψ* ψ i.e. complex conjugate

12. Pauli’s Exclusion Principle -Only one electron in each location accounting for spin
Principle Q# Orbital Q# Magnetic Q# Spin Q#

13. Zeeman Effect = Splitting or emission lines if in B field

14. Shape of Orbitals

15. Bonding in Molecules Ionic - electrons stolen
Covalent - electrons shared
Metal
hybridization, sp, sp2, sp3
Molecular Orbitals for shared electrons = covalent bonds

16. Atoms in Solids Ionic Bonding, NaCl Covalent Bonding Metals
Hetero Atoms = Ceramics, e.g. MgO

17. Electrostatic forces in Ionic Solids
Many Atoms at various separations
Maudelin Constant, Md
NaCl, ao=0.281 nm and Elatttice=8.95 eV.

18. Repulsive Force at small r
Total Force = Coulomb Force + Repulsive Force

19. Metallic Bonding Electrons Free to move among all atoms Determines
Electron Gas
Determines
Electrical Conduction
Thermal Conduction

20. In Covalent Crystalline Solids, what happens to the atomic orbitals?

21. Molecular Orbitals New Energy New Shapes to Orbitals if hybridization• •
New Energy
Bonding
Anti Bonding
New Shapes to Orbitals if hybridization 1s • •

22. Bonds Between Molecules
Hydrogen Bonding
Van der Waals Forces
Dipole-Dipole interactions
Dipole Moment = Charge * separation
Permanent
Instantaneous

23. Melting Point Molecular Solids Metals Ionic Solids Covalent Solids
Strength of
Inter-Molecular
Bonds
Melting Point

24. Melting Point