2. Periodic Trend Nuclear charge atomic size or radius ionization energy electron affinity electronegativity metallic character Reactivity bonding characteristics crystal configurations acidic properties densities

3. Atomic radius

4. Periodic Properties02 Atomic Radii 02:

5. Ions and Ionic Radii Chapter 065

8. Ions and Ionic Radii

10. Trend of ionic radii The cation of an atom decreases in size while the anion of an atom increases in size. The trend can not be made according to the periodic table, but by the isoelectronic series. The more positive an ion is the smaller it is because Z eff increases, while the more negative an ion, the larger it is because Z eff decreases.

11. Ionization Energy Defined as the amount of energy necessary to remove the outermost electron from an isolated neutral atom in the gaseous state to infinity. Abbreviation is E i, it has units of kJ/mol. IE

12. Successive ionization energy

13. Ionization Energy Minor irregularities in the E i values are explained by looking at the electron configurations. IE Trend

14. Ionization Energy Ionization energies vary periodically, which is explained by the changes in Z eff. Z eff

15. Electron Affinity Electron Energy: Energy change that occurs when an electron is added to an isolated atom in the gaseous state. Abbreviation is E ea, it has units of kJ/mol. Values are generally negative because energy is released. Value of E ea results from interplay of nucleus electron attraction, and electron–electron repulsion. EA

16. Electron Affinity02 EA Trend

17. Chemical recativity http://www.youtube.com/watch?feature=player_d etailpage&v=uixxJtJPVXk (group 1 reactivity) http://www.youtube.com/watch?feature=player_d etailpage&v=uixxJtJPVXk http://www.youtube.com/watch?v=u2ogMUDBaf4 &feature=player_detailpage (halogen reactivity) http://www.youtube.com/watch?v=u2ogMUDBaf4 &feature=player_detailpage

18. Metallic Character The metallic character of atoms can be related to the desire to loose electrons On the periodic table, the metallic character of the atoms increase down a family and decreases from left to right across a period.