Periodic Table Review Sheet
Elements of the modern periodic table are in order of atomic number
Elements in the same group are chemically similar and have the same number of valence electrons
Element in the same period have the same number of principal energy levels
Atomic radius goes up from top to bottom in a group due to more energy levels
Atomic radius goes down from left to right across a period due to greater number of protons (nuclear charge)
Metals ions have a smaller atomic radius than their atoms
Non-metals have a larger atomic radius than their atoms
Electronegativity is attraction for electrons
Ionization energy is the amount of energy to remove the most loosely held electron
Electronegativity goes up from left to right because metals want to lose electrons and non-metals want to gain them
Electronegativity goes down from top to bottom in a group because of greater distance from nucleus
Ionization energy goes up from left to right across a period because metals want to loose electrons and non-metals want to gain them
Ionization energy goes down from top to bottom in a group because of greater distance from nucleus and shielding or screening effect
Metallic properties increase from right to left and top to bottom because it is easier to loose an electron
Non-metallic properties go up from left to right and bottom to top because of a greater desire to gain an electron
Bromine (non metal) and Mercury (metal) are the two liquids on the periodic table
Group 17 (halogens) have two gases, one liquid, and two solids at STP and are diatomic
Group 18 have full shells and are monatomic
Metalloids have properties of both metals and non-metals and are Boron Silicon Arsenic Germanium, Antimony and Tellurium
Metals are good conductors, ductile, malleable, and lustrous
Non Metals are brittle, nonconductors and not lustrous
Metallic properties are due to loosely held electrons
Group 1 and 2 elements are highly reactive and never found alone in nature
Of the Noble gases only Krypton, Xenon and Radon will react with Fluorine and Oxygen
Transition elements (groups 3-12) can lose electrons from two outer shells and form colored solutions and compounds.