1. The Periodic Table and Periodicity

3. Arrangement In order of increasing atomic number in specific columns and rows.

4. Groups- vertical columns of the PT The Periodic Table 123456789101112131415161718 1 2 3 4 5 6 7

5. Periods- horizontal row on the PT The Periodic Table 123456789101112131415161718 1 2 3 4 5 6 7

6. Groups are important on the PT Why?  The elements in a group have similar chemical and physical properties!

7. Alkali Metals – Group 1 123456789101112131415161718 1 H 2 Li 3 Na 4 K 5 Rb 6 Cs 7 Fr

8. Alkaline Earth Metals – Group 2 123456789101112131415161718 1 2 Be 3 Mg 4 Ca 5 Sr 6 Ba 7 Ra

9. Halogens – Group 17 123456789101112131415161718 1 2 F 3 Cl 4 Br 5 I 6 At 7

10. Noble Gases – Group 18 123456789101112131415161718 1 He 2 Ne 3 Ar 4 Kr 5 Xe 6 Rn 7 Uuo

11. Transition Metals – Groups 3 - 12 123456789101112131415161718 1 2 3 4 5 6 7

12. Inner Transition Metals 123456789101112131415161718 1 2 3 4 5 6 7 La Yb Ac No

13. Metals - Lustrous Good conductors of heat & electricity Malleable – can be pounded into thin sheets Ductile – can be drawn into thin wire

14. Metals on the PT 123456789101112131415161718 1 2 3 4 5 6 7

15. Nonmetals - Lack properties of metals 123456789101112131415161718 1 2 3 4 5 6 7

16. Metalloids (semi-metals)- have a mixture of metallic and nonmetallic properties 123456789101112131415161718 1 2 3 Si 4 GeAs 5 SbTe 6 PoAt 7

17. Diatomic Elements Most elements can be isolated to atomic elements – individual atoms 7 elements are too reactive to exist as individual atoms, instead, they are found as molecular elements – 2 atoms bonded together Hydrogen, H 2 Oxygen, O 2 Nitrogen, N 2 Chlorine, Cl 2 Bromine, Br 2 Iodine, I 2 Fluorine, F 2

18. Periodicity Atomic radius – defined as ½ the distance between the nuclei of two adjacent atoms of an element.

19. Periodicity First Ionization Energy – energy needed to remove an electron from an atom. Electronegativity – ability of an atom to attract electrons to itself