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What is the general rule?
Metal reactivity increases to the bottom left of the periodic table, with Francium (Fr) being the most reactive.
Metal reactivity:
Metals with the first low ionisation energy are more reactive, meaning that metals in Group 1 metals are the most reactive.
Transition metals have larger nuclear attraction and are generally less reactive.
Metal + Water → Metal oxide/Metal hydroxide + Hydrogen Gas
K, Na, CL → reacts with cold water
Mg → reacts with hot water
Al, Zn, Fe → reacts with steam when red hot
Pb, Sn, Cu,Hg, Ag, Au → no reaction
Water & metal reactivity
Water of higher temperatures provide more energy to ionise metals allowing for reaction, with lower element groups being more reactive.
Water temperature for reaction helps predict metal reactivity
Metal + dilute acid → salt + hydrogen gas
K, Na, Ca → bubbles rapidly and hydrogen gas formed may spontaneously combust
Mg → bubbles rapidly & releases hydrogen
Al, Zn, Fe → Bubbles very slowly to moderately, reacts faster in warm acid
Pb, Sn, Cu, Hg, Ag, Au → no reaction
Metal + oxide → metal oxide
K, Na, Ca → burn rapidly to form oxides or peroxides, combusts spontaneously in air
Mg → Burn readily of powders or as fine fibres to form oxides
Al, Zn, Fe, Pb, Sn, Cu, Hg → becomes coated with oxide layers which prevent further oxidisation
Ag, Au → no reaction
Metal and metal ions
Less reactive metal solutions ionise more reactive metals
Less reactive metal ions deposit out of solution