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