1. Electron Configuration

2. The way electrons are arranged around the nucleus.

3. Quantum Mechanical Model 1920’s Werner Heisenberg (Uncertainty Principle) Louis de Broglie (electron has wave properties) Erwin Schrodinger (mathematical equations using probability, quantum numbers)

4. Principal Quantum Number, n Indicates main energy levels n = 1, 2, 3, 4… Each main energy level has sub-levels

5. Energy Sublevels s p d fg

6. The principle quantum number, n, determines the number of sublevels within the principle energy level.

7. Orbital Quantum Number, ℓ (Angular Momentum Quantum Number) Indicates shape of orbital sublevels ℓ = n-1 ℓsublevel 0 s 1 p 2 d 3 f 4 g

8. Orbital The space where there is a high probability that it is occupied by a pair of electrons. Orbitals are solutions of Schrodinger’s equations.

9. Orbitals in Sublevels Sublevel # Orbitals # electrons s12 p36 d510 f714 g918

10. Three rules are used to build the electron configuration: Aufbau principle Pauli Exclusion Principle Hund’s Rule

11. Aufbau Principle Electrons occupy orbitals of lower energy first.

12. Aufbau Diagram

13. -Pauli Exclusion Principle (Wolfgang Pauli, Austria, 1900-1958) -Electron Spin Quantum Number An orbital can hold only two electrons and they must have opposite spin. Electron Spin Quantum Number (m s ): +1/2, -1/2

14. Hund’s Rule In a set of orbitals, the electrons will fill the orbitals in a way that would give the maximum number of parallel spins (maximum number of unpaired electrons). Analogy: Students could fill each seat of a school bus, one person at a time, before doubling up.

15. Aufbau Diagram for Hydrogen

16. Aufbau Diagram for Helium

17. Aufbau Diagram for Lithium

18. Aufbau Diagram for Beryllium

19. Aufbau Diagram for Boron

20. Aufbau Diagram for Carbon

21. Aufbau Diagram for Nitrogen

22. Aufbau Diagram

23. Notations of Electron Configurations Standard Shorthand

24. Aufbau Diagram for Fluorine

25. Standard Notation of Fluorine Main Energy Level Numbers 1, 2, 2 Sublevels Number of electrons in the sub level 2,2,5 1s 2 2s 2 2p 5

26. Shorthand Notation Use the last noble gas that is located in the periodic table right before the element. Write the symbol of the noble gas in brackets. Write the remaining configuration after the brackets. Ex: Fluorine: [He] 2s 2 2p 5

27. Blocks in the Periodic Table 1 18 2 13 14 15 16 17 s p d f 3 4 5 6 7 8 9 10 11 12

28. Unit 3 review Atomic scientists what did they do? Atomic theory, Dalton vs modern Law of def prop, law of cons of mass, law of multiple proportions Periodic table Trends- what is it, describe it Groups of elements and traits How to read it Know how to determine what is in an atom Ion vs isotope Electomagnetic spectrum- what is it why important Wavelength, frequency, amplitude Calculations Photons, quantum, plank Line emission, photoelectric effect excited state vs. Sublevels- orbital shapes electrons at each level Electron configuration

29. Unit 3 review Atomic scientists what did they do? Atomic theory, Dalton vs modern Law of def prop, law of cons of mass, law of multiple proportions Periodic table Trends- what is it, describe it Groups of elements and traits How to read it Know how to determine what is in an atom Ion vs isotope Electomagnetic spectrum- what is it why important Wavelength, frequency, amplitude Calculations Photons, quantum, plank Line emission, photoelectric effect excited state vs. Sublevels- orbital shapes electrons at each level Electron configuration

30. Unit 3 review Atomic scientists what did they do? Atomic theory, Dalton vs modern Law of def prop, law of cons of mass, law of multiple proportions Periodic table Trends- what is it, describe it Groups of elements and traits How to read it Know how to determine what is in an atom Ion vs isotope Electomagnetic spectrum- what is it why important Wavelength, frequency, amplitude Calculations Photons, quantum, plank Line emission, photoelectric effect excited state vs. Sublevels- orbital shapes electrons at each level Electron configuration

31. Unit 3 review Atomic scientists what did they do? Atomic theory, Dalton vs modern Law of def prop, law of cons of mass, law of multiple proportions Periodic table Trends- what is it, describe it Groups of elements and traits How to read it Know how to determine what is in an atom Ion vs isotope Electomagnetic spectrum- what is it why important Wavelength, frequency, amplitude Calculations Photons, quantum, plank Line emission, photoelectric effect excited state vs. Sublevels- orbital shapes electrons at each level Electron configuration