CHEMISTRY 161 Chapter 7 Quantum Theory and Electronic Structure of the Atom

1. CHEMISTRY 161 Chapter 7 Quantum Theory and Electronic Structure of the Atom www.chem.hawaii.edu/Bil301/welcome.html

2. REVISION H = E  atomic orbital wave function of an electron in an atom 2 probability of finding an electron at a given location Schroedinger

3. ORBITALS AND QUANTUM NUMBERS • principle quantum number • 2. angular momentum quantum number • 3. magnetic quantum number • 4. spin quantum number n = 1, 2, 3, 4, 5… l = 0, 1, … (n-1) ml = -l, (-l +1), … 0…… (+l-1) +l ms = -1/2; + 1/2

4. ATOMIC ORBITALS (n, l, ml, ms)

5. Ψ(n, l, ml, ms) = Rn,l(r) Yml(Θ,Φ)

6. 4πr2[Rn,l(r)]2

7. Yml(Θ,Φ) z (x,y,z) r Θ Φ y x

8. 1s, 2s, 3s

9. 2pz

10. Yml(Θ,Φ)

11. Ψ1,0 = 1s probability of finding the electron within a sphere of a radius r r 90 % ‘boundary surfaces’

12. 1s, 2s, 3s 1s 2s 3s s orbitals do not depend on Φ or Θ

13. p orbitals + and – refers to Ψ, but the figure shows Ψ2

14. 2px, 3px, 4px 4px 2px 3px

15. d orbitals

16. 3s 3p 3d 2s 2p 1s E Orbital Energies energy level diagram H atom energy depends only on principal quantum number orbitals with same n but different l are degenerate

17. 4d 5s 4p 3d 4s 3p E 3s 2p 2s 1s MULTI-ELECTRON ATOM energy depends on n and ml orbitals with same n and different l are not degenerate

18. Orbital Energies

19. Homework Chapter 7, pages 267-271 problems