Main Group

Alkali Metals

ns1 configurgation

Flame colors

Malleable

Low Density

Low Melting Point

Easily oxidized

Hydrogen

Most abundant

Colorless / Odorless

Liquid at 20K

Tasteless

Oxide

-2

Peroxide

-1

Superoxide

-1/2

Alkali Earth Metals

ns2 configuration

insoluable

Don’t decompose well

Low densities

Low mps

Low Bps

Generally produced by Reduction or electrolysis

Beryllium

• Higher mp

• Harder

• Unreactive towards air and water

• Smaller size • High ionization energy

• Tends to be covalent rather than ionic

• chloride has a unique structure where the chlorine atoms of subsequent units are on perpendicular planes.

Hardwater

Ions precipitate outside , CaCO3 MgCo3

Can be removed via ion exchange

Isocogens

s2p1

relatively soft and reactive

Good conductors

Form Dimers

+1, +3 (IP)

Dimers

Where two identical compounds bond together

Aluminium

Most abundant metal in the Earth’s crust (8.1%)

Strong Light Metal

Formed by electroylsis

Reducing Agent

Gallium

Obtained by smelting

High Density liquid state

Attacks metals by diffusing into their crystal lattice

Applications: electronics, LEDs, transistors, semiconductors, amplifiers, solar cells

Indium

Squeals when bent

Can be a strong oxidizing or reducing agent depending on ox. state

Thallium

Greek word twig

Very toxic

Inert Pair effect

Occurs for metals and semi metals of groups 13,14,15, and 16, Can keep the s electrons and lose the p electron, only occurs with full d block

Tetregens

s2p2

Formed by roasting and reduction

+2 +4 (IP)

Tin Functions

storing food, solder, pewter (alloy)

Lead Functions

Batteries, Ammunition, pipes