1. IIIIII C. Johannesson III. Periodic Trends (p. 140 - 154) Ch. 5 - The Periodic Table

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

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

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

5. C. Johannesson 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

6. C. Johannesson zAtomic Radius D. Atomic Radius Li Ar Ne K Na

7. C. Johannesson zAtomic Radius yIncreases to the LEFT and DOWN D. Atomic Radius

8. C. Johannesson 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

9. C. Johannesson zFirst Ionization Energy E. Ionization Energy K Na Li Ar Ne He

10. C. Johannesson zFirst Ionization Energy yIncreases UP and to the RIGHT E. Ionization Energy

11. C. Johannesson 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

12. C. Johannesson 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

13. C. Johannesson 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

14. C. Johannesson zMelting/Boiling Point yHighest in the middle of a period. F. Melting/Boiling Point

15. C. Johannesson

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

17. C. Johannesson

18. Ionic Radius zIncreases right to left - atoms lose e-; they become smaller because they may drop energy level or because outer shell has less electrons so less attraction to nucleus zIncreases top to bottom -higher energy level means that valence electrons are further away so increase in size. C. Johannesson

20. zWhich atom has the larger radius? yBeorBa yCaorBr Ba Ca Examples

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

22. Electronegativity zAbility to attract electrons in a bond *doesn’t apply to Noble gases- Why? Related to ionization energy. -low electronegativity is because the nuclei don’t exert a strong attractive force -Group- as atmoic # increases- increased distance between valence e- and nucleus. **SO: decreases down group, decreases right to left across period. C. Johannesson

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

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