This document provides information about electron configurations and the filling of orbitals in atoms. It includes trends in ionization energies from the periodic table, evidence for electron sublevels, and rules for filling orbitals according to the Aufbau principle, Hund's rule, and the Pauli exclusion principle. The document poses practice problems in predicting ionization energies and writing electron configurations for various elements.

1. HL Atomic Structure Sketch the graph of first ionisation energies. What other evidence do we have for electron sub levels ? http://www.ptable.com/

2. Aims Show how successive ionization energy data is related to the electron configuration of an atom.

3. Trends in the PT

4. Sub Levels Evidence

5. Further Evidence

6. Problem Predict which element in each of the following pairs has the larger first ionization energy. (a) Na or Mg (b) Mg or Al (b) B or Al (c) F or Cl

7. Definitions Aufbau Lowest energy filled first Hund Same sub-shell – singly first Pauli no two electrons in the same atom can be in the same quantum state

8. s pdf shapes http://lincoln.pps.k12.or.us/lscheffler/OrbitalShapesOverheads.htm

9. Picturing Electrons

10. Filling Orbitals http://www.youtube.com/watch?v=fv-YeI4hcQ4&feature=fvw

11. Orbitals Rules :- Electrons are found in orbitals 2 electrons in each orbital – with opposite ‘spin’ They will pair up only when all empty orbitals are filled. S can hold 2 P can hold 6 ( px, py and pz ) D can hold 10 F can hold 14

12. Order of Filling of Orbitals

13. Order of Filling of Orbitals

14. Blocks in the PT

15. How To …. Use the Periodic Table to find the atomic number, and hence number of electrons. Fill up orbitals in the order 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p - until you run out of electrons. The 3d is the awkward one - remember that specially. Fill p and dorbitals singly as far as possible before pairing electrons up.

16. Task Write a ‘how to fill electronic orbitals help sheet’ Include 10 elements with their full electron configuration 3 from s block – 3 from p block and 4 from d block.

17. HL Atomic Theory Apply the Aufbau principle, Hund’s rule and the Pauli exclusion principle to write electron configurations for atoms and ions up to Z = 54.

18. What is electron configuration of Ca C Zn S

19. Cu and Cr Chromium and Copper have electron configurations [Ar] 3d5 4s1 and [Ar] 3d10 4s1 respectively

20. Ions Notation Sc - (Ar) 4s2 3d1 Ti - (Ar) 4s2 3d2 V - (Ar) 4s2 3d3 Cr - (Ar) 4s1 3d5 Mn - (Ar) 4s2 3d5 Fe - (Ar) 4s2 3d6 Co - (Ar) 4s2 3d7 Ni - (Ar) 4s2 3d8 Cu - (Ar) 4s1 3d10 Zn - (Ar) 4s2 3d10

21. Plenary Questions 58 - 60

22. Starter

23. Let’s Balloon