Periodic Trends Chapter 6 Section 3

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

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

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

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

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

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

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

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

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

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