1. IIIIII The Periodic Trend

2. ysize of atom Atomic Radius

3. Atomic Radius - Groups zAtomic radius increases as you move down a group zWhy? zAtomic size increases because more electrons are added which results in more orbits.

4. Atomic Radius - Periods zAtomic radius decreases as you move across a period zWhy? zIncreased (+) nuclear charge pulls the (-) electrons closer to the nucleus zAtomic size decreases

5. zIncreases to the LEFT and DOWN Atomic Radius

6. IONIC RADIUS zIons are charged atoms, either +ve or –ve zCations are +ve and form when atoms lose electrons zAnions are -ve and form when atoms gain electrons

7. Ionic Radius – Cations Group zCations are smaller than their parent atoms. zWhy? zBy losing electrons they become shorter

8. Ionic Radius – Anions Groups zAnions are larger than their parent ions zWhy? zWhen extra (-) electrons are added, the size of atom becomes bigger.

9. ELECRTONEGATIVITY zAbility of an atom to attract electrons toward itself in a chemical bond. zThe difference between the electronegativities of two atoms determines what kind of bond they form.

10. Electronegativity - Periods zElectronegativity increases going left to right across the periodic table. zFluorine has the highest. zLithium has the lowest. LiBeBCNOF 1.01.52.02.53.03.54.0

11. Electronegativity - Groups zElectronegativity decreases going down a group zWHY?? zAs atoms get bigger the bonding electrons are far from the attraction of the nucleus. H 2.1 Li 1.0 Na 0.9 K 0.8 Rb 0.8 Cs 0.7 Fr 0.7

12. Ionization Energy zFirst Ionization Energy zIncreases UP and to the RIGHT

13. zMelting/Boiling Point yHighest in the middle of a period. Melting/Boiling Point

14. zWhich atom has the larger radius? yBeorBa yCaorBr Ba Ca Examples

15. zWhich atom has the higher melting/boiling point? yLiorC yCrorKr C Cr Examples

16. zWhich particle has the larger radius? ySorS 2- yAlorAl 3+ S 2- Al Examples