1. Periodic Trends/Patterns

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 Properties 02
Atomic Radii 02:

5. Ions and Ionic Radii
Chapter 06

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 Zeff(effective nuclear charge) increases, while the more negative an ion, the larger it is because Zeff 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 Ei, it has units of kJ/mol. IE

12. Successive ionization energy

13. Ionization Energy
Minor irregularities in the Ei 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 Zeff .
Zeff

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

16. Electron Affinity 02
EA Trend

17. Chemical recativity
(group 1 reactivity)
(halogen reactivity)

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.