Groups in the Periodic Table

Hard, strong, shiny, malleable, good conductors of heat and electricity, high melting points, high densities, catalysts, form colourful compounds

Positive ions are surrounded by delocalised electrons and form strong bonds

They have delocalised electrons that can carry a charge

There are strong bonds between negative electrons and positive ions

Metals have layers of atoms in sheets that can slide over each other easily, so it can bend. Adding another element that has atoms of different sizes disrupts these sheets, so they cannot slide

Some are only two dimensional, rather than three in real life Ions and particles are very large, while in real life they would be small, with lots of empty space between them

Lithium - Li Sodium - Na Potassium - K Rubidium - Rb Caesium - Cs Francium - Fr

There are more electron shells, so the outermost electron is further from the nucleus, so the attraction force is weaker, so it can be lost more easily

Soft, low melting and boiling points, float on water - low densities, very reactive with water, form an alkali in water

They float, move around and fizz. Over time they disappeared as they turned into hydroxide and let off hydrogen gas. Potassium produced a purple flame Rubidium and caesium explode

e.g. Lithium + water –> lithium hydroxide + hydrogen 2Li + 2H2O –> 2LiOH + H2

Hold a test tube over it and hold a lit splint over it. If it makes a squeaky pop sound, hydrogen gas is present

They need to form a covalent bond to have a full outer shell. This is called diatomic, as opposed to monotomic

Fluorine - F Chlorine - Cl Bromine - Br Iodine - I Astatine - At

Fluorine - gas - pale yellow Chlorine - gas - green Bromine - liquid - red Iodine - solid - grey, purple vapour Astatine - solid - black

Chlorine turns damp blue litmus paper red, then bleach it white

They react vigorously with some to form salts called metal halides Sodium + chlorine –> sodium chloride 2Na + Cl2 –> 2NaCl

They react to form soluble hydrogen halides Hydrogen + chlorine –> hydrogen chloride H2 + Cl2 –> 2HCl

There is less of a force to attract an electron to the nucleus, so it gets harder to attract the extra electron to fill the outer shell

The halogens lose electrons (oxidation) Halide ions gain electrons (reduction) Cl2 + 2KBr –> Br2 + 2KCl Oxidised Reduced

Helium - He Neon - Ne Argon - Ar Krypton - Kr Xenon - Xe Radon - Rn

They have a full outer shell, so they don’t easily give up or gain electrons

Colourless, gases at room temperature, inert, non-flammable, hard to observe

Providing an inert atmosphere, light bulbs and welding (to stop metals from burning or being oxidised), and airships and balloons (low densities and inert)