2. Periodic Properties

4. Periodic Table with f-block included A.Electron Configurations

5. II. The Modern Periodic Table Arises from Periodic Law: A. Includes: 1. periods/rows 2. groups/families There are 4 categories of groups: 1.Representative (also Main Group Elements) 2.Transition elements 3.Inner transition (also Lanthanide and Actinide) 4.Noble Gases Some groups have special names: –1A (Alkali Metals) –2A (Alkaline Earth Metals) –7A (Halogens) –8A I (Noble Gases) The letters A and B in the group distinguish families –A = representative –B = transition

6. Groups The group # is the number assigned to a vertical column on the periodic table. Another name is a Family. 18 groups in the periodic table. Groups 1, 2, 13 – 18 are representative (A) Groups 3 – 12 are transition (B) Some label periodic tables label these groups.

8. Periods 1. The period number is the number assigned to a horizontal row on the periodic table. 2. The number of protons increase from left to right across a period. 3. This number is the atomic number. The period number indicates how many energy levels (rings) each atom has.

9. alkali Alkaline earth halogenshalogens NoblegasNoblegas

11. METALS shiny-luster solids (except Hg) malleable ductile (stretch to wire) conduct heat & electricity most elements are metals

12. NONMETALS solids, liquids & gases luster-dull brittle poor conductors upper-right hand corner (& H)

13. Metalliods along stairstep line – between B & Al (Al is not a metalloid!) classified as nonmetals but conduct heat and electricity under certain conditions some metal & nonmetal properties

14. Group 1 - Alkali Metals soft, shiny reacts violently with water VERY reactive, one valence e- to lose; cation

15. Alkali metals http://www.youtube.com/watch?v=m55kgy ApYrY&safety_mode=true&persist_safety_ mode=1http://www.youtube.com/watch?v=m55kgy ApYrY&safety_mode=true&persist_safety_ mode=1

16. Group 2 - Alkaline Earth Metals 2 valence e-; cation reactive

17. http://www.youtube.com/watch?v=m55kgy ApYrY&safety_mode=true&persist_safety_ mode=1http://www.youtube.com/watch?v=m55kgy ApYrY&safety_mode=true&persist_safety_ mode=1

18. Transition Metals Elements in groups 3-12 Less reactive harder metals Includes metals used in jewelry and construction. Metals used “as metal.”

19. Transition Metals Groups 3-12 Ions change – changes properties NOT REPRESENTATIVE!

20. Halogens Elements in group 17 Very reactive, volatile, diatomic, nonmetals Always found combined with other element in nature. Used as disinfectants and to strengthen teeth.

21. Halogens -Group 17 -1 ions, highly reactive 7 valence e-

22. Noble Gases Elements in Group 18 Noble gases are usually unreactive. This is because they have full valence shells. Elements with full valence shells do not easily gain or lose electrons.

23. Noble Gas Stability Atoms want to gain stability, like the noble gases. Atoms will try to gain or lose electrons to have a full valence shell.

24. Phases of Elements 1. Liquids: You must know: Hg and Br 2. Gases: Don’t memorize, but you need to know their general location. Gases are towards the right side of the periodic table. 3. Solids: All metals, except Hg - mercury

26. Periodic Trends

27. MetallicCharacter – elements having properties of metals i)L to R: metals to nonmetals ii) Nonmetals are at the right of the Table. They tend to be insulators and react easily with metals. iii) Metalloids separate the metals and nonmetals and have intermediate properties iv) Noble Gases exist at the extreme right, are chemically stable and have full valence shells

28. Atomic Radius –Atomic radius – size of a neutral atom Shielding effect – inner energy levels ‘shield’ the outermost electrons from the positive charge pull of the nucleus –Atomic radius increases as you move down the groups Great distance (adding energy levels) from nucleus = less pull towards center –Decreases as you move left to right More pull from nucleus (more protons), but no new distance –EXCEPTION: Noble Gases – much bigger than group 17 – full outer shell

29. Atomic Radii

31. Ionic Size (Radius) –Ionic Radius - size of an ion –Cations (+) are always SMALLER than neutral atom Nuclear charge the same, less e - = strong pull inwards –Anions (-) are always LARGER than neutral atom Nuclear charge the same, MORE e - = less pull inwards –Increases as you go down a group –Decreases from left to right

32. Ionic Radii

33. Ionization Energy –Ionization energy – the energy that is required to remove an e - from an atom –Ion – atom which has gained or lost electrons Cation – (+) charged ion (lost e - ) Anion – (-) charged ion (gained e - ) –Decreases as you move down the periodic table Outermost electron gets further from nucleus, easier to pull off –Increases as you move across a period No more distance from nucleus, but higher charge = held more tightly

34. Ionization Energy

35. Electronegativity Elements relative ability of its atoms to attract electrons in a chemical bond Fluorine – Most electronegative Francium – Least electronegative Nobel Gases are left out because they form very few compounds Increase across a period Decrease down a group

36. Electronegativity