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Types of Chemical Reactions Most chemical reactions can be grouped into four categories. synthesis decomposition single displacement double displacement Understanding these types of reactions, we can predict products of unknown reactions. Synthesis Reaction: two or more reactants combine to produce a new product. (put together) A + B AB + e.g. 2H2 + O2 2H2O HCl + NH3 NH4Cl Decomposition Reactions: splitting of a large compound into elements or smaller compounds. (take apart) AB A + B + e.g. 2H2O 2H2 + O2 NH4NO3 N2O + 2H2O Decompositions can be thought of as the opposite to a synthesis reaction. Single Displacement Reactions: one element displaces another element from a compound. There are two general formulas: Z + AB A + ZB AB + Y AY + B + e.g. Mg + 2AgNO3 2Ag + Mg(NO3)2 (metals replacing metals) CaI2 + Br2 CaBr2 + I2 (non-metals replacing non-metals) + Double Displacement Reactions: elements in different compounds displace each other or exchange places. AB + XY AY + XB Where A and X are cations and B and Y are anions. B and Y simply change places. + e.g. Pb(NO3)2 + 2KI PbI2 + 2KNO3 + Everyday examples: Balance each equation and write the type of reaction on the line rusting of iron metal ____Fe + ____O2 ____Fe2O3 ___________________ hearing aid battery reaction ____HgO + ____Zn ___ ZnO + ____ Hg ___________________ electrolysis of water to make hydrogen fuel ____H2O ____ H2 + ____ O2 ___________________ plating silver on copper ___AgNO3 + ___Cu ___Cu(NO3)2 + ___Ag ___________________ carbon dioxide in atmosphere dissolving in oceans and changing to carbonic acid ____CO2 + ____ H2O ____H2CO3 ___________________ hydrochloric acid neutralized using a base sodium hydroxide (acid-base reaction) ____HCl + ____ NaOH ____NaCl + ____ H2O ___________________ PRACTICE: REACTION TYPES For each of the following chemical reactions a) balance the skeleton equation; b) classify by writing synthesis , decomposition, single displacement or double displacement on the line 1. Fe + O2 Fe2O3 _____________________ 2. H2 + O2 H2O _____________________ 3. Zn + HCl H2 4. Ca + HBr 5. Mg(ClO3)2 6. CaO + 7. N2O5 + 8. NH4ClO4 9. Al 10. Na2S + + H2O + ZnCl _____________________ CaBr2 + H2 _____________________ MgCl2 O2 _____________________ + Ca(OH)2 H2O _____________________ HNO3 _____________________ N2 + Cl2 + O2 + H2O CuSO4 HBr Al2(SO4)3 + Cu NaBr + H2S _____________________ _____________________ _____________________ A. Write a skeleton equation. B. Balance the skeleton equation. C. Identify the type of reaction. 1. Solid iron reacts with aqueous copper (I) nitrate to produce solid copper and aqueous iron (II) nitrate. 2. Aqueous potassium iodide reacts with chlorine gas to produce aqueous potassium chloride and iodine gas. 3. Solid aluminum reacts with solid sulfur to produce solid aluminum sulfide. 4. Solid potassium chlorate (KClO3) decomposes to form potassium chloride and oxygen gas.