Electron Configuration examples, Chemistry I.pptx

Presentation contains examples and introduction to electron configuration.

1. Periodic Properties

2. Z IE 1 (MJ/mol) Z IE 1 (MJ/mol) 1 H 1.31 11 Na 0.50 2 He 2.37 12 Mg 0.74 3 Li 0.52 13 Al 0.58 4 Be 0.90 14 Si 0.79 5 B 0.80 15 P 1.01 6 C 1.09 16 S 1.00 7 N 1.40 17 Cl 1.25 8 O 1.31 18 Ar 1.52 9 F 1.68 19 K 0.42 10 Ne 2.08 20 Ca 0.59 Table 1: First ionization energy for selected elements Graph 1 : First Ionization Energies

3. Outermost subshell being filled with electrons

4. H He Li Be B C N 1s 2s 2p 1s 2s 2p 1s 2s 2p 1s 2s 2p 1s 2s 2p 1s 2s 2p 1s 2s 2p

5. O F Ne Na Si Cl Ar 1s 2s 2p 1s 2s 2p 1s 2s 2p 1s 2s 2p 1s 2s 2p 1s 2s 2p 1s 2s 2p 3s 3p 3s 3p 3s 3p 3s 3p

6. s orbitals

7. p orbitals

8. d orbitals

9. Order of orbitals (filling) in multi-electron atom 1s < 2s < 2p < 3s < 3p < 4s < 3d < 4p < 5s < 4d < 5p < 6s

10. General Trend in First Ionization Energies Increasing First Ionization Energy Increasing First Ionization Energy

11. Effective Nuclear Charge

12. Outermost subshell being filled with electrons

13. +1 +2 +3 -1 -2 -3 Cations and Anions Of Representative Elements

14. H F F H electron rich region electron poor region e - rich e - poor d + d - Electronegativity is the ability of an atom to attract toward itself the electrons in a chemical bond.

15. Electronegativity is the ability of an atom to attract toward itself the electrons in a chemical bond. Electron Affinity - measurable , Cl is highest Electronegativity - relative , F is highest X ( g) + e - X - ( g)