1. Trends On the Periodic Table (it’s positively all about the Protons)

2. Rows (periods) Columns (groups  Atomic number- protons – increases as you move across a row  Number of energy levels increases as you move down a group

3. Blocks- s, d,p,f  S- group 1,2 valence electrons in s orbital  D- middle of table valence electrons in d orbital  P- last six groups- valence electrons in p orbital  F- two pull out rows valence electrons in f orbital

4. Atomic Radii- radius of the atom  Period- decrease  Group- increase  Why??? Remember the protons

5. Ionization Energy: amount of energy needed to remove an electron  Period- increase  Group- decrease  Why??? Remember the protons

6. Electronegativity: measure of the ability to attract electrons from nearby atoms  Period- increase  Group- decrease  Why??? Remember the protons

7. Ionic Radii: radius of ions cations (+) anions (-)  Cations: loss of electrons Left side of table…….metals Ionic radius- shrinks  Annions: Gain of electrons: Upper right table…. Nonmetal Ionic radius- increases Why??? Remember the protons

8. Why do we care????  Periodic Law: Elements physical and chemical properties can be predicted by location on the periodic table. All elements in the same group behave in a similar manner