The Periodic Table

1. Chemistry Dr. Davis The Periodic Table

3. Periodic Table • Group – Vertical columns on PT • Period – Horizontal rows on PT

4. Main-Group Elements • Groups 1, 2, and 13-18

5. Main-Group Elements • The chemical properties of the main-group elements depends on their number of valence electrons • Valence electrons are the outermost electrons involved in chemical bonding

6. Valence Electrons & Chemical Properties • Each group of the main-group elements has the same number of valence electrons • Each element wants to be as stable as possible • All main-group elements want a full shell of electrons, which is 8 valence electrons

7. Valence Electrons & Chemical Properties • Each group forms ions based on the easiest way to obtain this full shell • Also known as the octet rule

8. Family Groups • Noble Gases (Group 18) • Examples: Ne, Xe • Description: stable, unreactive group of gases • Number of Valence Electrons: 8 • Forms NO ions

9. Family Groups • Halogens (Group 17) • Examples: F, Cl • Description: Highly reactive group of gases • Number of Valence Electrons: 7 • Forms 1- ions

10. Family Groups • Alkali Metals (Group 1) • Examples: Na, K (not H) • Description: Highly reactive group of metals • Number of Valence Electrons: 1 • Forms 1+ ions

11. Brainiac Movie

12. Family Groups • Alkaline-Earth Metals (Group 2) • Examples: Be, Mg • Description: Slightly less reactive group than alkali metals • Number of Valence Electrons: 2 • Forms 2+ ions

13. Family Groups • Transition Metals (Group 3 – 12) • Examples: Fe, Au, Ag • Description: Fairly stable group of metals • Forms multiple ions

14. Family Groups • Lanthanides & Actinides • Location: Bottom 2 periods of PT • Description: Heavy metals, synthetics, radioactive

15. States of Matter • Metals and Nonmetals (Staircase)