1. IIIIII Periodic Trends 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. 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 B. Periodic Properties

4. zElectronegativity yA measure of an atom’s attraction for another atom’s electrons. zChemical Reactivity yHow likely or vigorously an atom reacts with other substances.

5. zAtomic Radius C. Atomic Radius Li Ar Ne K Na

6. zAtomic Radius yIncreases to the LEFT and DOWN C. Atomic Radius

8. 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 C. Atomic Radius

9. zFirst Ionization Energy D. Ionization Energy K Na Li Ar Ne He

10. D. Ionization Energy zEnergy required to overcome the attraction of the nuclear charge and remove an electron from a gaseous atom z1 st ionization energy – energy required to remove the 1 st outermost electron zIonization energy increases greatly when we try to remove core electrons

11. zFirst Ionization Energy yIncreases UP and to the RIGHT D. Ionization Energy

12. 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 - D. Ionization Energy

13. zSuccessive Ionization Energies yMg1st I.E.736 kJ 2nd I.E.1,445 kJ Core e - 3rd I.E.7,730 kJ 1s 2 2s 2 2p 6 3s 2 yLarge jump in I.E. occurs when a CORE e - is removed. D. Ionization Energy

14. 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 1s 2 2s 2 2p 6 3s 2 3p 1 zSuccessive Ionization Energies yLarge jump in I.E. occurs when a CORE e - is removed. D. Ionization Energy

15. zMelting/Boiling Point yHighest in the middle of a period. E. Melting/Boiling Point

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

17. G. Electronegativity zElectronegativity is a measure of an atom’s attraction for another atom’s electrons. zIt is an arbitrary scale that ranges from 0 to 4. zGenerally, metals are electron givers and have low electronegativities. zNonmetals are are electron takers and have high electronegativities. zWhat about the noble gases?

18. G. Electronegativity zAs you go across a period from left to right electronegativity of the representative elements increases zElectronegativity decreases as you move down a group zTrends among transition metals are not so regular

19. G. Electronegativity zFlourine is the most electronegative element-attracts electrons from the element it is bonded to form a negative ion. zCesium is the least electronegative element-doesn’t attract electrons-most likely will give away it’s outmost electron

20. G. Electronegativty

21. H. Chemical Reactivity zHow likely or vigorously an atom reacts with other substances zDetermined by how easily an electron can be removed (ionization energy) and how badly an atom wants to take another atom’s electrons (electronegativity)

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

23. H. Chemical Reactivity zAlkali Metals zAlkaline Earth Metals zTransition Metals zHalogens zNoble Gases

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

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

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

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

28. zWhich element is more electronegative? yCl or Fl yAs or Ca Fl As