1. Periodic Trends

2. Atomic Size (Radius) As you go down in a group on the periodic table, the atomic size increases. Bigger = More electron Shells

3. As you go across the periodic table, the atomic radius decreases. 3 p+ 9p+ 3 e - 9 e - Bigger – Less Attraction Smaller – More Attraction Atomic Radius is found on Table S of Reference Tables Li F 2

4. Ionization Energy Ionization Energy = the energy needed to remove a valence electron. Metals = giving Non-Metals = greedy

5. Electronegativity Electronegativity = the desire of an atom for an electron.

7. Valence Electrons As you go down a group, the valence electrons remain the same.

8. Valence Electrons Bonding: Group 11 + ionNa 1+ Group 22 + ionMg 2+ Group 14 four covalent bonds (carbon) Group 16 2 - ion w/ metal covalent w/nonmetal Group 171 - ion Group 18 no bondingstable octet

9. Reactivity Reactivity = how fast the element reacts. Metallic  gives electronsNa + ion Nonmetallic  gets electronsF - ion Semimetals  can give or get electrons Noble Gases  don’t react

10. Noble Gas: Don’t React

11. Transition Metals Sc  2-8-9-2Ti  2-8-10-2 Inner shells (lower energy level) fill before completing higher outer levels. (d-sublevel) Properties don’t change much as you go across. Make compounds with color. Some have multiple oxidation states Cr, Mn, Ti, V Electrons for bonding come from 2 outer shells.

12. Transition Metals

13. Radioactive Elements Elements beyond Bi (#84-114) Also Tc & Pm

14. Man Made Elements Not found in nature Unstable Beyond Uranium (#93-114 Also Tc & Pm