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p. 3 Balancing Chemical Equations –Coefficients: Numbers in front of each chemical formula 1) 1, 3, 2 2) 2, 2, 3 3) 2, 1, 2, 1 4) 2, 1, 2 5) 2, 1, 2, 1 6) 2, 3, 6, 1 7) 1, 2, 1, 2 8) 1, 5, 3, 4 9) 2, 25, 16, 18 10) 1, 3, 1, 3 11) 4, 5, 2 12) 2, 2, 2, 1 13) 2, 4, 1 14) 1, 12, 8 15) 6, 6, 1, 6 16) 2, 1, 2, 1 17) 2, 1, 1, 1, 1 Notes of Chemical Reactions’ Abbreviations Nov 18th, 2014 Hof Brincl: diatomic molecules/in pairs also gaseous (g) H2, O2, F2, Br2, I2, N2, Cl2 aqueous: dissolved in water, in solution (aq) liquid: pure covalent compound Ex: H2O(l) **pure metallic element: uncharged and solid Ex: Cu(s) CuSO4 : ionic and Cu2+ (aq) (charged) pure copper sprinkles: Cu (s) (uncharged) p. 4 Word Equations: Watch for Hof Brincl!! 1) Zn + Pb(NO3)2 Zn(NO3)2 + Pb 2) 2AlBr3 + 3Cl2 2AlCl3 + 3Br2 3) 2Na3PO4 + 3CaCl2 6NaCl + Ca3(PO4)2 4) 2KClO3 2KCl + 3O2 5) 2Al + 6HCl 2AlCl3 + 3H2 6) 3Ca(OH)2 + 2H3PO4 Ca3(PO4)2 + 6H2O 7) Cu + 2H2SO4 CuSO4 + 2H2O + SO2 8) 2H2 + 2NO 2H2O + N2 p. 5 Word Equations (Hof Brincl) 1) 2AlBr3 + 3Cl2 2AlCl3 + 3Br2 2) 2H2 + O2 2H2O 3) N2 + 3H2 2NH3 4) HCl + NaF NaCl + HF 5) Fe + PbS FeS + Pb 6) H2SO4 SO3 + H2O 7) 2Na2O + 2F2 4NaF + O2 8) 2KI + Br2 2KBr + I2 9) 3Zn + 2FeCl3 3ZnCl2 + 2Fe 10) 4Al + 3O2 2Al2O3 11) 2N2 + 5O2 2N2O5 p.6 More Word Equations (Include the states: s, l, aq, g) 1) 2O2(g) + N2(g) 2NO2(g) 2) 2BeI2(aq) + Sn(NO3)4(aq) 2Be(NO3)2(aq) + SnI4(s) 3) 2Fe(s) + 3F2(g) 2FeF3(s) 4) 2HCl(aq) + Mg(OH)2(aq) MgCl2(aq) + 2H2O(l) 5) 2(NH4)3N(aq) + 3Pb(ClO3)2(aq) 6NH4ClO3(aq) + Pb3N2(s) 6) H2CO3(aq) CO2(g) + H2O(l) 7) 2Na3PO4(aq) + 3CuSO4(aq) 3Na2SO4(aq) + Cu3(PO4)2(s) 8) H2O(l) + CO(g) H2(g) + CO2(g) p.7 Concept Attainment-Classifying Chemical Rxns Examples of synthesis: b, c use a highlighter Synthesis: 2 compounds combining to form a larger substance. p.8 Examples of single replacement: a, d use a highlighter Single replacement: One element replaces another element in a compound. Examples of decomposition: b, e use a highlighter Decomposition: Large substance is breaking down into smaller compounds. Examples of double replacement: c, d use a highlighter Double replacement: An ion of a compound is switched with another metal or non metal to form another compound. p.9 Examples of combustion: a, d, e use a highlighter Combustion: Reaction with oxygen as a reactant. Examples of neutralization: a, d use a highlighter Neutralization: An acid(H-) is reacting with a base(-OH) to produce a salt(cation + anion) and water. p. 10 Classification of Chemical Reactions 1) synthesis 2) decomposition 3) single replacement 4) synthesis, combustion 5) decomposition 6) single replacement 7) synthesis 8) double replacement 9) decomposition 10)neutralization(special type of DR) p.11 Classifying Reactions Practice 1) combustion 2) single replacement 3) double replacement 4) decomposition 5) synthesis 6) single replacement 7) neutralization (DR) 9) decomposition 11) single replacement 13) single replacement 15) neutralization (DR) 8) synthesis, combustion 10) combustion 12) decomposition 14) single replacement **T** p.12 Predicting Products of Chemical Reactions 1) MgBr2 + Cl2 MgCl2 + Br2 single replacement 2) 2Al + Fe2O3 2Fe + Al2O3 single replacement 3) 2AgNO3 + ZnCl2 2AgCl + Zn(NO3)2 double replacement MnO2 (catalyst) 4) 2H2O2 --- 2H2O + O2 decomposition elephant toothpaste demo 5) Zn + 2HCl ZnCl2 + H 2 single replacement 6) H2SO4 + 2NaOH Na2SO4 + 2H2O neutralization 7) 2Na + H2 2NaH synthesis 8) 2CH3COOH + Cu NR s(no reaction) **T** p. 13 Balancing Equations and Classifying Rxns All the rxns below are single replacement rxns i) Zn + MgSO4 NR (Zn is below Mg) ii) 2Al(s) + Fe2O3(aq) Al2O3(aq) + 2Fe(s) (Al is above Fe) iii) Pb + KNO3 NR (Pb is below K) iv) Ni + FeSO4 NR (Ni is below Fe) v) Zn(s) + CuCl2(aq) ZnCl2(aq) + Cu(s) (Zn is above Cu) vi) F2(g) + 2KCl(aq) 2KF(aq) + Cl2(g) (F2 is above Cl2) vii) I2 + FeBr3 NR (I2 is below Br2) viii) 3Zn(s) + 2H3PO4(aq) Zn3(PO4)2(aq) + 3H2(g) (Zn is above H2)