1. Periodic Trends
Chapter 6 Section 3

2. 1. Shirt and pants
Oxygen + Einsteinium + Chlorine + Thorium
2. A small angle
Uranium + Actinium + Tellurium
3. A bone in your leg
Boron + Uranium + Iodine + Lanthanum + Fluorine
4. A place full of silicon dioxide
Actinium + Beryllium +Hydrogen

3. Periodic Table Rows  Periods Columns  Groups/Families
Remember Valence Electron Trends

4. Atomic Radius Increases moving down a group or family
Increases moving towards group 1

5. Practice – Put in order of decreasing radii
Al, Na, P, S
Br, Ca, Cl, K
Al, Ga, In
As, Ge, Ga

6. Ionic Radius
Ion – an atom or a bonded group of atoms that has a positive or negative charge
Na+ is a cation
Smaller than parent atom
Cl- is an anion
Larger than parent ion
Increases moving down a group or family
Ionic Radius decreases along an isoelectronic series
Isoelectronic series – group of atoms that have the same electron value

8. Practice – Rank in increasing ionic radii
Br- , Cl- , F-
Be2+, Ca2+, Mg2+
Ca2+, Ga3+, K+

9. Ionization Energy
The energy required to remove an electron from a gaseous atom
Atoms with large ionization energy are less likely to form positive ions(cations)
Octet Rule – atoms gain, lose, and share electrons to acquire a full set of eight electrons
Generally increases as you move to the right
Generally decreases as you move down a group

11. Practice – List in increasing order
S, Mg, Si
O, Cs, K

12. Electron Affinity
Of an element indicates the relative ability of its atoms to attract electrons in a chemical bond
Fluorine is the most electronegative
Noble gases rarely form compounds so they have no electronegativity
Increases to the right
Decreases going down

14. Practice – List in decreasing order
Na, Li, K
K, Sc, Ca
As, Sn, S