2. There is a decrease in ionisation energy as you go down the group. Beryllium to Magnesium

3. More Shielding Increase in Distance from the nucleus electrons removed easily

6. 31 P 15 32 S 16 1s 2s 2p3s3p

10. Subsequent ionisation energies and their relationship to electron shells 2 nd and 3 rd ionisation energy. X + (g)  X2 + (g) +e- X2 + (g)  X3 + (g) +e- Successive ionization energy can give information about an element. Such as the number of electrons in outer shell.

11. Sodium Electrons Protons Charge

12. Sodium Electrons Protons Charge

13. Sodium Electrons Protons Charge

14. Sodium Electrons Protons Charge

15. Sodium Electrons Protons Charge

17. SUCCESSIVE IONISATION ENERGIES Defining second ionization energy Second ionization energy is defined by the equation: It is the energy needed to remove a second electron from each ion in 1 mole of gaseous 1+ ions to give gaseous 2+ ions.

18. 2nd I.E. = 1820kJ mol -1 3rd I.E. = 2740 kJ mol -1 4th I.E. = 11600 kJ ol -1 1 st I.E. = 577kJ mol -1

19. Why do successive ionization energies get larger? Why is the fourth ionization energy of aluminum so large? 1s 2 2s 2 2p 6 3s 2 3p x 1.

20. Using ionization energies to work out which group an element is in Magnesium (1s 2 2s 2 2p 6 3s 2 ) is in group 2 of the Periodic Table and has successive ionization energies: ).

21. Silicon (1s 2 2s 2 2p 6 3s 2 3p x 1 3p y 1 ) is in group 4 of the Periodic Table and has successive ionization energies:

22. Chlorine has the electronic structure 1s 2 2s 2 2p 6 3s 2 3p x 2 3p y 2 3p z 1.