2 Synthesis Reaction2 or more substances combining to form a single compoundA + B → ABN2(g) + 3H2(g) → 2NH3(g)
3 Decomposition Reaction A single reactant breaks down into simpler substances.CD → C + D2H2O2(l) → 2H2O(l) + O2(g)
4 Single- replacement Reaction An element replaces another in an ionic compound.E + FG → F + EGL + JK → K + JL2Na(s) + MgCl2(aq) → Mg(s) + 2NaCl(aq)2F2(g) + 2FeBr3(aq) → 3Br2(l) + 2FeF2(aq)
5 Single- replacement Reactions Only occur if the element doing the replacing is more active (reactive) than the other element!
6 Each element can replace all the other elements below it! Activity Series of the ElementsActivity Series of the ElementsMETALS NON-METALS (halogens)Lithium FluorinePotassium ChlorineCalcium BromineSodium IodineMagnesiumAluminumZincChromiumIronNickelTinLead“Hydrogen”CopperMercurySilverPlatinumEach element can replace all the other elements below it!
7 Double- replacement Reactions The cations of 2 ionic compounds exchange anions.QR + ST → QT + SRBaBr2(aq) + 2AgNO3(aq) → Ba(NO3)2(aq) + 2AgBr(s)
8 Combustion ReactionA hydrocarbon is burned with oxygen to produce carbon dioxide, water and light/ heat.CxHy + O2(g) → CO2(g) + H2O(g)2C4H10(l) + 13O2(g) → 8CO2(g) + 10H2O(g)2C2H5OH(l) + 7O2(g) → 4CO2(g) + 6H2O(g)
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