Periodic Table Organization

Main Block Elements (RepresentaTive Elements) Valance electrons are s and p orbitals The A group or 1-2 and 13-18

(Outer) transition metals Group B Valence electrons are in the d orbital Common metals fall into this group

Inner Transition Metals Group B Valence electrons are f orbitals Rare earth metals, less common

Alkali Metals Group 1A (Hydrogen not included) Metallic, the softest of metals, lowest density of metals, low melting points, very reactive s orbital , 1 valence electron

Alkaline earth Metals Group 2A Reactive, but not as much as Alkali metals, low density, soft S orbital, 2 valence electrons

Transition metals (in the middle) Common metals Generally hard, high melting and boiling points, high density Reactivity varies d orbital valence electrons

Inner transition:lanthanides and actinides Lanthanides have similar properties to the alkaline earth metals, used in small quantities in some industry Actinides are similar to alkaline earth metals, but are very dense with high melting points. Many are man made and radioactive. f orbital valance electrons

Noble Gases Group 18 or 8A; Very stable, with a full outer shell of valence electrons (8), following the octet rule.

Halogens Group 7A or 17 7 valence electrons in the p orbital, 1 short of full shell Very reactive and very useful

Pnictogens and chalcogens and others Pnictogens, group 15 (5A), chalcogens, group 16(6A), and group 13-14(3A and 4A) are made of metals, non-metals and metalloids. They have a variety of properties The number in front of the A indicate number of valence electrons

Hydrogen Under 1A, but it is its own group. Gains and loses electrons, but not as reactive a alkali metals or halogens Very useful and abundant element.

Metals On the wall they are blue Most elements Silver-ish, except copper and gold Solid at room temperature, except mercury which is a liquid Lustrous or shiny Malleable, ductile Conduct heat and electricity High melting point, dense and react with acids

Non-metals Near the Noble Gases On the wall, they are orange, yellow and Hydrogen Dull in appearance Brittle Poor conductors of heat and electricity Not too reactive with acids Low melting points Solids, liquids or gases at room temperature

Metalloids or semi-metals On the wall, they are green Zigzag on the Periodic Table Properties of both metals and non-metals May or may not conduct electricity, conduct best when mixed with other elements.

Solids, Liquids, and Gases (room Temp.) Solids: Most elements Liquids: Mercury and Bromine(Br2) Gases: Nobles, H2, N2,O2, F2, Cl2 last diatomic solid I2; The 7 Diatomics have to bond with themselves to exist in nature, so the 2 subscript

Valence electrons Outermost electrons in an orbital of an element These are responsible for reactions and bonding; They are shared or transferred (given/taken)

Electron configuration How electrons orbit the nucleus of an atom, with s,p,d and f indicating general shape of orbital These will be represented in various distances or levels from the nucleus The outermost electrons are called valence electrons

Octet Rule The outer shells of elements will react or bond until they have a full valence shell like the noble gases This is usually 8 valence electrons obtained from sharing or transferring of electrons in bonding