Periodic Properties properties electron configurations nuclear charge hydrogen

Periodic Properties properties electron configurations nuclear charge hydrogen atom 1 electron 1 s 1 Z=1 E = - RH Z 2 1 nf 2 - 1 ni 2 to remove e- nf = ∞ from ground state ni = 1 E =2. 178 x 10 -18 J x 6. 022 x 1023 atoms = 1311 k. J atom mol Ionization Energy, I

H 1 s 1 Z = +1 E = 1311 k. J/mol He+ 1 s 1 Z = +2 E = 5250 k. J/mol - - + E = - RH 2+ Z 2 1 nf 2 - 1 ni 2 = 5250 k. J/mol higher nuclear charge lowers orbital energy stabilizes systems with more than 1 electron studied experimentally ionization reactions

1. Effect of 2 electrons in same orbital He+ 1 s 1 E = 5250 k. J/mol He 1 s 2 E = 2372 k. J/mol Z = +2 same nuclear charge - 2+ - orbital energy higher e- e- repulsion less stable easier to remove e-

2. Effect of electrons in different orbital Li ground state 1 s 2 2 s 1 E = 520 k. J/mol Li 2+ excited state 2 s 1 E = 2954 k. J/mol Z = +3 same nuclear charge 2 s 2 s 1 s 1 s - 3+ - - - 3+ inner electrons shielding charge Zeff < Z

3. Effect of orbital shape Li ground state 1 s 2 2 s 1 E = 520 k. J/mol Li excited state 1 s 2 2 p 1 E = 341 k. J/mol Z = +3 same nuclear charge 2 s 2 p 1 s - - 3+ - 1 s - 3+ - - s orbitals penetrating lower energy

Potential Energy determines orbital energies 1. Greater nuclear charge (Z) lowers energy electrons more difficult to remove 2. Electron-electron repulsion raise energy electrons easier to remove electrons shield Z inner electrons shield better 3. Orbitals with more penetration lower energy electrons more difficult to remove s<p<d<f

I 1 increase Z increases shielding stays same adding valence ecore e- unchanged I 1 decrease Zeff decreases more shielding ecore e-

2 p 2 s 2 p - - 2 s 1 s 1 s - - - 5+ 10+ - - B - Ne

2 p 2 s 2 s 1 s 1 s - - 4+ 5+ - - - B Be N O e- e- repulsion

Second Ionization Energy I 1 Na I 2 I 3 I 4 I 5 I 6 I 7 495 4560 Mg 735 Al 580 Si 780 P 1060 S 1005 1445 7730 1815 11, 600 1575 16, 100 1890 21, 200 2260 27, 000 very difficult to remove Cl 1255 2295 core electrons Ar 1527 2665

Atomic Radius increase in size n dominates decrease in size Zeff dominates

Electron Affinity Energy given off when a gas phase atom gains e. Cl (g) + e- Cl- (g) Increases Zeff increases Noble gases – no tendency to gain e-

Summary atomic radius decreases ionization energy increases electron affinity increases Zeff atomic radius increases n ionization energy decreases metals lose e- non-metals gain e-