Periodic Table Basics

A quick intro to the basics covered in Science 9 and Science 10 on the Periodic Table in Nova Scotia.

1. The Periodic Table M. Peverill

2. History of the Periodic Table 1817 - Johann Dobereiner, Law of Triads 1862 - A. E. Beguyer de C h ancourtois , First attempt at a periodic table 1863 - John Newlands, Law of Octaves 1864 - Lother Meyer, abbreviated version of Periodic Table. He published the extended version in 1870. Unfortunately for him…

3. Published his Periodic Table in 1869. More easily predicted new or missing elements. Mendeleev predicted 10 new elements, 7 of which existed . Dmitri Mendeleev

4. Columns = Groups Rows = Periods

5. Group = Number of valence electrons Period = Number of orbitals

6. Metals

7. Propertie s of Metals Form cations (positive ions) Good conductors Lustrous (shiny) Malleable Solid at room temp. (except for m ercury )

8. Non-Metals

9. Propertie s of Non-Metals Form anions (negative ions) Poor conductors Solid forms are brittle, group 17 and 18 are gases at room temp. (except for b romine )

10. Metalloids

11. Propertie s of Metalloids “Staircase” elements Appear metallic but are brittle Semi-conductors

12. Metal + Metal = Alloy Metal + Non-Metal = Ionic Compound (salt) Non-Metal + Non-Metal = Molecular Compound

13. Alkali Metals

14. Alkali Metals Group 1 = 1 valence electron Form cations with +1 charge Most reactive metals Do not exist purely in nature

15. Alkaline Earth Metals

16. Alkaline Earth Metals Group 2 = 2 valence electrons Form cations with +2 charge Less reactive than Group 1 metals Found as salts in nature (metal + halogen)

17. Transition Metals

18. Transition Metals Form cations just like other metals, but have multiple oxidation states (can have different charges). Exceptions: Ag and Zn

19. Halogens

20. Halogens Group 17 = 7 valence electrons Form anions with -1 charge Most reactive elements

21. Noble Gases

22. Noble Gases Group 18 = 8 valence electrons Full valence shell (stable octet), therefore they do not react Gases at room temp.

23. Atomic Number (# of protons) Element Symbol Element Name Atomic Mass (average mass of isotopes)

24. References Searle, S. (2011) Nova Scotia Science 10. McGraw-Hill Ryerson http://www.wou.edu/las/physci/ch412/ perhist.htm