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Warm-up April 5th Write the balanced chemical equation for: Balance each chemical equation Ba(ClO3)2 BaCl2 + O2 Mg(NO3)2 + KCl MgCl2 + KNO3 Types of Reactions A. Combustion Hydrocarbon + oxygen carbon dioxide and water CH4 + 2O2 CO2 + 2H2O 2C8H18 + 25O2 16CO2 + 18H2O B. Synthesis the combination of 2 or more substances to form a compound only one product A + B AB B. Synthesis H2 + Cl2 2 HCl C. Decomposition a compound breaks down into 2 or more simpler substances only one reactant AB A + B C. Decomposition 2 H 2O 2 H 2 + O 2 D. Single Replacement one element replaces another in a compound metal replaces metal (+) nonmetal replaces nonmetal (-) A + BC B + AC D. Single Replacement Cu + 2AgNO3 Cu(NO3)2 + 2Ag E. Double Replacement ions in two compounds “change partners” cation of one compound combines with anion of the other AB + CD AD + CB E. Double Replacement Pb(NO3)2 + K2CrO4 PbCrO4 + 2KNO3 Warm-up November 16th Balance each chemical equation Ba(ClO3)2 BaCl2 + O2 Mg(NO3)2 + KCl MgCl2 + KNO3 Reactions in aqueous solutions Many reactions happen in solution Makes it so the ions separate so they can interact. Solids, liquids, and gases are not separated, only aqueous Complete ionic equations: Every aqueous compound is written as separate ions Solids, liquids and gases as whole compounds MgCl2(aq) + PbSO4(aq) → MgSO4(aq) + PbCl2(s) Complete net ionic equation: Mg2+(aq) + Cl-(aq) + Pb2+(aq) + SO4(aq) → Mg2+(aq) + SO4(aq) + PbCl2(s) FeBr3(aq) + 3KOH(aq) 3KBr(aq) + Fe(OH)3(s) Fe3+(aq)+ Br-(aq) + 3K+(aq) +3OH-(aq) →3K+(aq) +3Br-(aq) + Fe(OH)3(s) K+ and Br- do not change, they are spectator ions Fe3+(aq) +3OH-(aq) →Fe(OH)3(s) This is what really happens in the reaction! Net Ionic Equations Shows only those particles that change before and after. Eliminate spectator ions Needs to be balanced in terms of both mass and charge Fe3+(aq) +3 OH-(aq) →Fe(OH)3(s) Write the Net Ionic Equation for: HCl (aq) + Ba(OH)2 (aq) → BaCl2(s) + HOH (l) Al(s) + FeSO4(aq) → Al2(SO4)3(aq) + Fe(s) K2CO3(aq) + MgI2(aq) →MgCO3(s) + KI(aq) Predicting precipitates Precipitate-Solid formed from aqueous solution. You can predict them if you know some general rules for solubility. Look at your Reference Tables! Is it soluble? LiBr Ba(NO3)2 CaSO4 PbCl2 CaCO3 K2CO3 Cd(ClO3)2 Is there a reaction? For double replacement- has to make gas, solid or water. Water from an acid- H+ and a hydroxide- OH- makes HOH Solids- from solubility rules Exchange ions and see if something is insoluble Predict the products and write the net ionic equations for each: MgSO4 + NaOH → H2SO4 + KOH → K3PO4 + FeF3→