Organizing the periodic table

1. Organizing the periodic table Ch. 5.1

3. Search for Order • 1750 • Only 17 elements • 1789 • Lavoisier grouped into • Metals, nonmetals, gases and earths • No good method yet found

4. Mendeleev's Periodic Table • 1860’s • 63 elements • Deck of cards arrangement for students • Periodic Table- arrangement of elements in columns based on a set of properties that repeat from row to row • Arranged elements into rows of increasing mass • Elements with similar properties were in the same column

6. Mendeleev Predictions Evidence • Used properties of elements near blanks to predict properties of undiscovered elements • Close match between his predictions and actual new elements showed how correct his table was

7. The modern Periodic Table Ch. 5.2

9. The Periodic Law • Elements are arranged by INCREASING atomic #(# of ______)

10. Periodic Law Periods Groups • Rows • # of elements per period varies due to orbitals • Columns • Same group= similar properties • Electron Configuration

12. Classes of Elements • State at room temperature • Solid, liquid or gas • Occurring Naturally or not • 1-92 natural • 93+ not natural • General properties • Metal, nonmetal, metalloid

13. Metals • Good conductors of electricity • Solid, except Hg • Malleable • Ductile- made into thin wire • Transition metals • Form compounds with distinctive colors

14. Nonmetals • Poor conductors of electricity • Gas at room temp • If not, very brittle • F most reactive • Group 18 least reactive

15. Metalloids • Mixture of properties • Metals, and nonmetals • Varies with temperature

16. Variation Across Periods

17. Representative groups Ch. 5.3

19. Valance Electrons • Lewis Dot Structure • Electron located in the highest energy level • Increase left to right • Elements in groups have similar properties due to same # of valance electrons

20. Groups/Families: • 8 Total- going down columns

21. Alkali Metals • Group 1A • 1 Valance Electron • VERY Reactive • Reactivity increases from top to bottom • Found in nature • Only as compounds

22. Alkaline Earth Metals • Group 2A • 2 Valance Electrons • Reactivity • How they react with water

23. Boron Family • Group 3A • 3 Valance Electrons • Al- most abundant metal on Earth

24. Carbon Family • Group 4A • 4 Valance Electrons • Contains • nonmetal- C • 2 metaloids – Si, Ge • 2 metals – Sn, Pb • Except for H2O, most compounds in the body contain C

25. Nitrogen Family • Group 5A • 5 Valance Electrons • Contains • 2 nonmetals – N, P • 2 metaloids – As, Sb • 1 metal – Bi

26. Oxygen Family • Group 6A • 6 Valance Electrons • Contains • 3 nonmetals – O, S, Se • 2 metaloids – Te, Po • O is most abundant element in Earths crust

27. Halogens • Group 7A • 7 Valance Electrons • Physical properties- different • Chemical Properties- similar • Highly reactive nonmetals • Fl is most reactive • React easily with metals

28. Noble Gases • Group 8A • 8 Valance Electrons, except He(2) • Odorless, extremely un-reactive

29. Transition Metals • able to put more than eight electrons in the shell that is one in from the outermost shell • Sc has a configuration of 2-8-9-2 • able to put up to 32 electrons in their second to last shell • Au has an organization of 2-8-18-32-18-1

30. Transition Metals Lanthanide Actinide • Rare Earth or inner transition • Found naturally in Earth • Reactive, ionic • Radioactive • Metals tarnish when met with air

31. Websites • http://www.funbrain.com/periodic/index.html • http://www.privatehand.com/flash/elements.html