2. Periodicity

3. Periodic Properties Also called periodicity Properties associated with the periodic table Repetitious over the table Have a pattern across the table associated with them

4. Effective Nuclear Charge (Zeff)

5. +Z INNER SHELL OR CORE ELECTRONS OUTER SHELL OR VALENCE ELECTRONS OUTERMOST s ELECTRONS PARTIALLY FILLED SUBLEVELS FOR MAIN GROUP.....THE ns AND np ELECTRONSFOR MAIN GROUP..... THE GROUP NUMBER PERIODICITY OF CHEMICAL PROPERTIES RESULT FROM PERIODICITY OF VALENCE ELECTRONS FILLED ORBITALS

6. Be +4 VALENCE ELECTRONS DO NOT EXPERIENCE FULL POSITIVE CHARGE ARE SHEILDED Z eff = Z -  EnEn INCREASE INCINC ORBITAL E LOWER IN ATOMS WITH HIGH Z eff

7. Periodic Properties 1. Ionization Energy 2. Atomic Radius 3. Electron Affinity 4. Electronegativity

8. Ionization Energy Energy required to remove an electron from an atom If removing valence electrons: 1 st ionization energy

9. IONIZATION ENERGY E REQUIRED TO REMOVE THE OUTERMOST ELECTRON FROM AN ATOM OR ION IN ITS GASEOUS STATE Z eff INCREASE n IE DECDEC INCREASE IE 1 < IE 2 < IE 3, ETC LOWER IE: MORE EASILY ATOM FORMS CATIONS MORE METALLIC CHARACTER FOR ELEMENT

10. Atomic Radius Size of the radius of the atom Comparison vs. Ionic radius –Metals: AR is greater than IR (loss of e-) –Non-metals: IR is greater than AR (gain of e-)

11. ATOMIC RADII DEFINED BY SIZE OF OUTERMOST ORBITALS Z eff INCREASE n r INCINC DECREASE oooooooo o o o o o o oo o o o o o o CATION < ATOM ANION > ATOM

12. Electron Affinity Tendency of a non-bonded atom to attract electrons to itself Non-metals have higher electron affinities because of their valence electrons

13. Electonegativity Tendency of elements who are bonded to attract electrons to themselves

14. ELECTRONEGATIVITY A MEASURE OF THE POWER OF AN ATOM TO ATTRACT ELECTRONS TO ITSELF HIGH , LARGE Z eff, LOW n UNFILLED ORBITAL....NON-METALS Z eff INCREASE n  DECDEC HIGH  : MORE EASILY ATOM FORMS ANIONS MORE NON-METALLIC CHARACTER TO ELEMENT

15. MAGNETIC PROPERTIES MAGNETIC FIELDS CAUSED BY SPINNING ELECTRONS DIAMAGNETIC: PARAMAGNETIC: NO UNPAIRED ELECTRONS NO ATTRACTION TO APPLIED MAGNETIC FIELD UNPAIRED ELECTRONS ATTRACTED TO APPLIED MAGNETIC FIELD

16. ARRANGE THE FOLLOWING IN INCREASING ORDER: Si, P, S ATOMIC RADIUS IONIZATION ENERGY ELECTRONEGATIVITY < Na, K, Cl ATOMIC RADIUS IONIZATION ENERGY ELECTRONEGATIVITY < Cs, Fe, S ATOMIC RADIUS IONIZATION ENERGY ELECTRONEGATIVITY < S P Si Si P S Si P S Cl Na K K Na Cl K Na Cl S Fe Cs Cs Fe S

17. ENERGYENERGY A B C ARRANGE IN ORDER OF: INCREASING IONIZATION ENERGY DECREASING ELECTRONEGATIVITY WHICH IS DIAMAGNETIC AND WHICH IS PARAMAGNETIC? C IS PARAMAGNETIC C < A < B C > A > B