THE PERIODIC TABLE
Periodic table used for:
-classifying elements
-predicting propertise of elements
-info about elements; atomic #, relative atomic mass, symbol

Periods-horizontal lines of PT, same period = same e- shell filled
Acidity; left > basic > amphoteric > acidic oxides > right
Metallic nature; left > metallic > non-metallic > right
# of valence electrons: left > increases > right

Groups-vertical columns of PT, 8 groups
Group = valence e-s
Metallic nature; up > more metallic > down
Melting and boiling pts; non-metals : up > increases > down, metals: up > decreases > down

GROUP I (ALKALI METALS)
-alkali metals: from the group > soluble bases, alkalis
up > more reactive > down (bigger atoms, less attractive force on outer e-s > more easily lost > more reactive)
group I metals + H₂O metal hydroxide + H₂ (g)
Displacement: Metal + metal ion metal ion + metal (more reactive metal changes to ion)

GROUP VII (HALOGENS)
Up > less reactive > down (bigger atoms, more difficult to attract e-s)
Halides: ions of halogens
Displacement: Halogens + Halides Halides + Halogens (more reactive halogen changes to ion)

GROUP VIII or 0 (NOBLE GASES)
Unreactive: stable e- config
Argon in lamps: prevents filament form oxidising as it doesnt react w/ it
Helium in balloons: lighter than air, non-combustible

TRANSITION METALS(TYPICAL METALS)
-conduct elec + heat
-high density, low volatility
-coloured compounds; Fe+2-green, Fe+3-brown
-variable oxidation states; Fe+2, Fe+3
-used as catalysts; iron used as catalyst in ammonia productions

Group	I	II	III	VI	V	VI	VII	VIII
Oxidation state	+1	+2	+3	±4	-3/+5	-2/+6	-1/+7	0

Metals
Organic Chemistry
Non-metals
The Particulature Natrue of Matter
Experimental Techniques
Atoms, Elements and Compounds
Stoichiometry + Mole Concept
Acids + Bases
Chemical Reactions + Electrolysis
Rate and Heat of Reactions + Reversible Reactions

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