1. IIIIII 6.3 Periodic Trends (p. 187-194) Ch. 6 - The Periodic Table

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

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

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

5. B. Chemical Reactivity

6. 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

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

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

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

10. zWhich atom has the larger radius? yBe orBa yCa orBr Ba Ca Examples

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

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

13. 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

14. zSuccessive Ionization Energies yMg1st 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

15. yAl1st 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

16. zWhich atom has the higher 1st I.E.? yNorBi yBa orNe N Ne Examples

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

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

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

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

21. H. Electronegativity z Ability of an atom to attract an electron Fluorine attracts the electron more than Hydrogen

22. Electronegativity Trends yIn groups, electronegativity decreases when atomic number increases yIn periods, electronegativity increases with atomic number

23. Example z Compare the Ionization Energies of metals and nonmetals. z Metals have low IE and Nonmetals have high IE. z Compare the Electronegativies of metals and nonmetals. z Metals have low EN and Nonmetals have high EN.

24. Summary of Periodic Table Trends zMoving Left --> Right yAtomic Radius Decreases yIonization Energy Increases yElectronegativity Increases zMoving Top --> Bottom yAtomic Radius Increases yIonization Energy Decreases yElectronegativity Decreases