2.  1. Atomic Radius/Ionic Radius  2. Metallic Character  3. Ionization Energy  4. Electronegativity

3.  What is it? The distance from the nucleus to the outer/valence energy level. Small atomic radius Large atomic radius

4. Increases

5.  As you go from left to right the atomic radius gets smaller. BUT WHY?  The nuclear charge (# of p+ inside the nucleus) increases. This increase in positive charge pulls the e- cloud closer to the nucleus; therefore decreasing the atomic radius!

6.  ANIONS: (- charge) become LARGER than the parent neutral atom. They are gaining electrons, the e- spread out a little making the ion formed a little larger. [NONMETALS]  CATIONS: (+ charge) become SMALLER than the parent neutral atom. They are losing electrons from the valence shell. [METALS]

7. Anions: Get Larger Cations: Get Smaller

8. Remember where metals and nonmetals are located on the periodic table. That makes this trend one of the easiest to remember!

9. THE TREND

10.  What is that???  It is the energy required to remove the most loosely held electron from the valence shell of the atom in the gaseous phase.  Abbreviated IE

11. Within a PERIOD, the IE increases with atomic #. The larger the atomic #, the larger the positive charge in the nucleus which means a stronger hold on the e- s; more energy to remove it. Within a GROUP, the IE decreases as you go down the group. Electrons are further away from the nucleus AND the shielding effect.

13.  What is it???  It is a measure of the ability of an atom to attract electrons to itself.  Arbitrary scale - values range from 0.7 to 4.0  Fluorine has the highest electronegativity (4.0).  Noble gases are excluded since they are already stable and don’t want to attract any electrons.

14. FOXY Fluorine ! FREAKY Franciu m

15. INCREASES

16. THAT’S ALL FOLKS!!