1. The Periodic Table The most important tool in chemistry

2. Periodic Table organization? The periodic table will be your most useful tool; it is organized in two specific ways: 1) increasing atomic number, and 2) similar chemical properties. family – vertical column in PT. -> elements in the same family exhibit similar chemical and physical properties

3. Blocks of the Periodic Table

4. Procedure: 1.Number the columns 1-18 across the top 2.Number the rows down the left-side 3.Fill-in 5-10 elements that you work with 4.Label the following families: alkali metal, alkaline-earth metal, transition metal, halogen, noble gas Periodic Table Activity

5. Periodic Table Period – rows numbered 1 to 7. Group – columns numbered 1 to 18; also called Families. Group   Period

6. Periodic Table The periodic table can be most easily be separated into three sections:Metals, non-metals, and metalloids Metals  non-metals metalloids Noble gases

7. Characteristics of Metals 1)lustrous appearance. 2) mostly solids that are malleable (shapeable). 3)excellent electrical and thermal conductors. 4)tend to form (+) ions in ionic compounds → give up electrons

8. Charact. of non-Metals 1)dull appearance. 2)wide diversity in physical states with solids being brittle or soft. 3)poor electrical and thermal conductors (great insulators!). 4)tend to form (-) ions in ionic compounds → gain electrons

9. Periodic Table Alkali metals – Group 1 Alkaline Earth metals – Group 2 Halogens – Group 17 Noble Gases – Group 18

10. Periodic Table Transition metals – Groups 3-12 Inner Transition metals

11. Periodic Table Practice SymbolAt.#Family #Family Name Na111 He218 Li31 Be42 B513 H1 Alkali metal Noble gas Alkali metal Alkaline earth metal Metalloid Family by itself

12. Diatomic Molecules Di = 2 Famous German scientist discovered: Cl I F Br O H N 222 222 2 Molecules always want to be in pairs and NOT alone

13. Atomic Radii

14. Periodic Trends Atomic Size The trend down a group is that atomic size increases as number of the valence shell increases

15. Periodic Trends Atomic Size The trend across a period is that atomic size decreases because the number of protons increases but no additional energy levels are added. The more + nucleus can draw e- closer

16. Periodic Trends 1 st Ionization Energy The removal of electrons from an atom can occur two ways: 1) transfer to another atom. 2) “artificially” with external energy. M + Energy  M + + e - Energy = Ionization Energy (IE)

17. Ionization Energies

18. Periodic Trends 1 st Ionization Energy Trends in IE are the reverse of atomic size trends. smallest atomic radius highest IE largest atomic radius lowest IE

19. Periodic Trends Electron Affinity Electron affinity is the attraction of an atom (in the gas phase) for additional electrons. A(g) + e -  A - (g) + Energy (exotherm) The electron obtained always goes into the lowest energy subshell in which there is space available!

20. Electron Affinity

21. Periodic Trends Electron Affinity Think of the electron being in a hole and the electron affinity is related to how deep the hole is! smallest anion radius highest EA largest anion radius lowest EA

22. Periodic Trends Electronegativity The ability for an atom to attract electrons from a neighboring atom smallest atomic radius has highest electronegativity - fluorine 4.0 largest atomic radius lowest electronegativity – Francium 0.7

23. Electronegativities

24. Periodic Trends Ion Size Cations are always smaller than the atom - fewer electrons so each one is held just a little bit tighter. Cation Charge Size Fe(145 pm); Fe 2+ (74 pm); Fe 3+ (64 pm)

25. Periodic Trends Ion Size Anions are always larger than the atom - more electrons than protons in the nucleus so the charge felt per electron goes down. Anion Charge Size