1. Periodic Table Trends

3. Metallic character

4. Metallic Character Depends on how readily the element gives up their valence e-’s

5. Atomic Radius Same shell across the period Addition of one proton draws the electrons closer to the nucleus Additional shells

6. Graph of Atomic Radius

7. Electronegativity

8. The tendency of an atom to attract e-’s Fluorine is the most electronegative element in the table WHY? –Its empty valence shell is near the highly attractive (+) nucleus (note: has 9 protons) –No shielding effect from inner shells

9. Ionisation Energy

10. The amount of energy (kJ) required to remove the most loosely held e- from an atom to form a positive ion –Eg. K (g)  K + (g) + e- (IE = 500 kJ) –Eg. Ne (g)  Ne + (g) + e- (IE = 2000 kJ) –A higher IE would mean a higher attraction to the nucleus

11. Ionisation Energy Affected by: –Charge of the nucleus –Distance of the e- to the nucleus –The # of inner e- shells shielding or screening the outer e-’s –If e- is single or paired within the orbital

12. Reactivity