1. IIIIII The Periodic Table I. History

2. A. Mendeleev zDmitri Mendeleev (1869, Russian) yOrganized elements by increasing atomic mass. yElements with similar properties were grouped together. yThere were some discrepancies.

3. A. Mendeleev zDmitri Mendeleev (1869, Russian) yPredicted properties of undiscovered elements.

4. B. Moseley zHenry Mosely (1913, British) yOrganized elements by increasing atomic number. yResolved discrepancies in Mendeleev’s arrangement.

5. IIIIII Do Periodic Law Activity The Periodic Table

6. IIIIII II. Organization of the Elements The Periodic Table

7. zMetals zNonmetals zMetalloids A. Metallic Character

8. IIIIII III. Periodic Trends The Periodic Table

9. A. Periodic Law zWhen elements are arranged in order of increasing atomic #, elements with similar properties appear at regular intervals.

10. B. Chemical Reactivity zFamilies ySimilar valence e - within a group result in similar chemical properties

11. B. Chemical Reactivity zAlkali Metals zAlkaline Earth Metals zTransition Metals zHalogens zNoble Gases

12. zAtomic Radius ysize of atom © 1998 LOGAL zFirst Ionization Energy yEnergy required to remove one e - from a neutral atom. © 1998 LOGAL zMelting/Boiling Point C. Other Properties

13. zAtomic Radius D. Atomic Radius Li Ar Ne K Na

14. zAtomic Radius yIncreases to the LEFT and DOWN D. Atomic Radius

15. zWhy larger going down? yHigher energy levels have larger orbitals yShielding - core e - block the attraction between the nucleus and the valence e - zWhy smaller to the right? yIncreased nuclear charge without additional shielding pulls e - in tighter D. Atomic Radius

16. zFirst Ionization Energy E. Ionization Energy K Na Li Ar Ne He

17. zFirst Ionization Energy yIncreases UP and to the RIGHT E. Ionization Energy

18. zWhy opposite of atomic radius? yIn small atoms, e - are close to the nucleus where the attraction is stronger zWhy small jumps within each group? yStable e - configurations don’t want to lose e - E. Ionization Energy

19. zSuccessive Ionization Energies  Mg 1st I.E.736 kJ 2nd I.E.1,445 kJ Core e - 3rd I.E.7,730 kJ yLarge jump in I.E. occurs when a CORE e - is removed. E. Ionization Energy

20.  Al 1st I.E.577 kJ 2nd I.E.1,815 kJ 3rd I.E.2,740 kJ Core e - 4th I.E.11,600 kJ zSuccessive Ionization Energies yLarge jump in I.E. occurs when a CORE e - is removed. E. Ionization Energy

21. zMelting/Boiling Point yHighest in the middle of a period. F. Melting/Boiling Point

22. zIonic Radius yCations (+) xlose e - xsmaller © 2002 Prentice-Hall, Inc. yAnions (–) xgain e - xlarger G. Ionic Radius

23. zWhich atom has the larger radius?  BeorBa yCaorBr Ba Ca Examples

24. zWhich atom has the higher 1st I.E.? yNorBi yBaorNe N Ne Examples

25. zWhich atom has the higher melting/boiling point? yLiorC yCrorKr C Cr Examples

26. zWhich particle has the larger radius? ySorS 2- yAlorAl 3+ S 2- Al Examples

27. The Periodic Table zDo Periodic Trends WS