I’ve Got Nothin’ (2017) READING FOR Monday: Chapter 8 sections 1 – 5 HOMEWORK – DUE Monday 6/26/17 HW 6: CH 6 #’s 7, 9, 13, 15, 17, 25, 28, 35-43 odd, 59, 63-75 odd Chapter 6 Extra Credit: DUE Monday 6/26 HW 11: CH 11 #’s 36, 45, 47, 49-52 (all), 59, 60, 63, 64, 65, 67, 99 No Extra Credit for CH 11 Lab Monday: Dry lab, no prelab Lecture Quiz Monday (stupid copier) Beacon with Chris Monday and Wednesday from 3:00 – 5:00 in LRC 107

Redox Reactions 3 Cl2(g) + 2 Al(s)  2 AlCl3(s) +3 –1 Gain Electrons REDUCED oxidizing agent 3 Cl2(g) + 2 Al(s)  2 AlCl3(s) reducing agent Lost Electrons OXIDIZED

Types of reactions Decomposition One thing  more than one thing A  B + C… H2CO3(aq)  H2O(l) + CO2(g) C3H5(NO3)3(l)  CO2(g) + H2O(g) + N2(g) + O2(g) Look for one reactant and multiple products

Types of reactions Predictable decompositions: metal hydrogen carbonates with heat metal hydrogen carbonate metal hydrogen carbonate metal hydrogen carbonate metal hydrogen carbonate metal carbonate + carbon dioxide + water metal carbonate metal carbonate + carbon dioxide metal carbonate + carbon dioxide + water metal carbonate + carbon dioxide + water metal carbonate + carbon dioxide + water metal carbonate + carbon dioxide + water Ca(HCO3)2(s) Ca(HCO3)2(s) Ca(HCO3)2(s) Ca(HCO3)2(s) CaCO3(s) + CO2(g) + H2O(g) CaCO3(s) + CO2(g) + H2O(g) CaCO3(s) + CO2(g) + H2O(g) CaCO3(s) + CO2(g) + H2O(g) CaCO3(s) + CO2(g) + H2O(g) calcium hydrogen carbonate is heated and decomposes in to calcium carbonate, carbon dioxide, and water calcium hydrogen carbonate is heated and decomposes in to calcium carbonate, carbon dioxide, and water calcium hydrogen carbonate is heated and decomposes in to calcium carbonate, carbon dioxide, and water calcium hydrogen carbonate is heated and decomposes in to calcium carbonate, carbon dioxide, and water calcium hydrogen carbonate is heated and decomposes in to calcium carbonate, carbon dioxide, and water calcium hydrogen carbonate is heated and decomposes in to calcium carbonate, carbon dioxide, and water calcium hydrogen carbonate is heated and decomposes in to calcium carbonate, carbon dioxide, and water calcium hydrogen carbonate is heated and decomposes in to calcium carbonate, carbon dioxide, and water

Types of reactions Predictable decompositions: metal carbonates with heat metal carbonate metal carbonate metal carbonate metal oxide + carbon dioxide metal oxide metal oxide + carbon dioxide metal oxide + carbon dioxide metal oxide + carbon dioxide Al2(CO3)3(s) Al2(CO3)3(s) Al2(CO3)3(s) Al2O3 + 3 CO2(g) Al2O3 + 3 CO2(g) Al2O3 + 3 CO2(g) Al2O3 + 3 CO2(g) aluminum carbonate is heated and decomposes in to aluminum oxide and carbon dioxide aluminum carbonate is heated and decomposes in to aluminum oxide and carbon dioxide aluminum carbonate is heated and decomposes in to aluminum oxide and carbon dioxide aluminum carbonate is heated and decomposes in to aluminum oxide and carbon dioxide aluminum carbonate is heated and decomposes in to aluminum oxide and carbon dioxide aluminum carbonate is heated and decomposes in to aluminum oxide and carbon dioxide aluminum carbonate is heated and decomposes in to aluminum oxide and carbon dioxide

Types of reactions Unpredictable decomposition reactions: metal oxides with heat metal oxide metal(?) + O2(g) Fe2O3(s) Fe(s) + O2(g) Fe2O3(s) FeO(s) + O2(g)

Types of reactions Unpredictable decomposition reactions: metal ___ates with heat metal ___ate something + something else KClO3(s) KCl + O2(g) Mg(NO3)2(s) Mg(NO2)2(s) + O2(g) Al2(SO4)3(s) Al2O3(s) + SO3(g)

Types of reactions Combination reactions Two things to one thing A + B…  C N2(g) + 3 H2(g)  2 NH3(l) Look for multiple reactants and a single product

Types of reactions Predictable combination reactions: non–VOS metals and non–metals Li(s) + S(s) Li2S(s) Ba(s) + P(s) Ba3P2(s)

Types of reactions Unpredictable combination reactions: VOS metals and non–metals Pb(s) + Se(s) PbSe(s) Pb(s) + Se(s) PbSe2(s)

Types of reactions Unpredictable combination reactions: non–metals and non–metals N2(g) + O2(g) N2O3(g) N2(g) + O2(g) NO2(g) N2(g) + O2(g) N3O2(g)

Types of reactions Combustion reactions A + O2(g)  H2O(g) + CO2(g) C5H12(l) + O2(g)  H2O(g) + CO2(g) Look for O2(g) as a reactant and H2O(g) and CO2(g) as products!!

Types of reactions Single replacement reactions A + BX  B + AX Ca(s) + HCl(aq)  H2(g) + CaCl2(aq) Look for one element and one compound or ion as reactants There tends to be a transfer of electrons in a single replacement reaction These are NOT NOT NOT ions!!!!!!

Activity Series Mg(s) + CdCl2(aq)  MgCl2(aq) + Cd (s) Li > K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn > Fe > Cd > Co > Ni > Sn > Pb > (H) > Cu > Ag > Hg > Au The activity series is used ONLY FOR SINGLE REPLACEMENT REACTIONS The more reactive metal will “want” to be the ion. Mg(s) + CdCl2(aq)  MgCl2(aq) + Cd (s) Mg > Cd so it WILL react! neutral atom +2 ion The MORE reactive metal will always be an ion or in a compound!!

Activity Series AuNO3(aq) + Ag(s)  AgNO3(aq) + Au(s) Li > K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn > Fe > Cd > Co > Ni > Sn > Pb > (H) > Cu > Ag > Hg > Au The activity series is used ONLY FOR SINGLE REPLACEMENT REACTIONS The more reactive metal will “want” to be the ion. AuNO3(aq) + Ag(s)  AgNO3(aq) + Au(s) Ag > Au so it WILL react! +1 ion neutral atom The MORE reactive metal will always be an ion or in a compound!!

Activity Series Al(s) + Sr(ClO3)2(s)  N.R. Li > K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn > Fe > Cd > Co > Ni > Sn > Pb > (H) > Cu > Ag > Hg > Au The activity series is used ONLY FOR SINGLE REPLACEMENT REACTIONS The more reactive metal will “want” to be the ion. Al(s) + Sr(ClO3)2(s)  N.R. Sr > Al so NO REACTION! neutral atom +2 ion The MORE reactive metal will always be an ion or in a compound!!

Activity Series Cu(s) + HBr(aq)  N.R. means in acid Li > K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn > Fe > Cd > Co > Ni > Sn > Pb > (H) > Cu > Ag > Hg > Au The activity series is used ONLY FOR SINGLE REPLACEMENT REACTIONS The more reactive metal will “want” to be the ion. Cu(s) + HBr(aq)  N.R. H > Cu so NO REACTION! neutral atom +1 ion The MORE reactive metal will always be an ion or in a compound!!

Activity Series HCl(aq) + Zn(s)  ZnCl2(aq) + H2(g) Li > K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn > Fe > Cd > Co > Ni > Sn > Pb > (H) > Cu > Ag > Hg > Au The activity series is used ONLY FOR SINGLE REPLACEMENT REACTIONS The more reactive metal will “want” to be the ion. HCl(aq) + Zn(s)  ZnCl2(aq) + H2(g) Zn > H so it WILL react! +1 ion neutral atom The MORE reactive metal will always be an ion or in a compound!!

Activity Series Ba(s) + H2O(l)  Ba(OH)2(aq) + H2(g) ^ Li > K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn > Fe > Cd > Co > Ni > Sn > Pb > (H) > Cu > Ag > Hg > Au The activity series is used ONLY FOR SINGLE REPLACEMENT REACTIONS The more reactive metal will “want” to be the ion. Ba(s) + H2O(l)  Ba(OH)2(aq) + H2(g) Ba > H2O so it WILL react! neutral atom The MORE reactive metal will always be an ion or in a compound!!

Activity Series Mn(s) + H2O(l)  N.R. ^ Li > K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn > Fe > Cd > Co > Ni > Sn > Pb > (H) > Cu > Ag > Hg > Au The activity series is used ONLY FOR SINGLE REPLACEMENT REACTIONS The more reactive metal will “want” to be the ion. Mn(s) + H2O(l)  N.R. H2O > Mn so NO REACTION! neutral atom The MORE reactive metal will always be an ion or in a compound!!

Activity Series H2SO4 + Hg  NR Ca + HOH  Ca(OH)2(aq) + H2(g) ^ H2O Li > K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn > Fe > Cd > Co > Ni > Sn > Pb > (H) > Cu > Ag > Hg > Au H2SO4 + Hg  NR H > Hg so it will NOT react! Ca + HOH  Ca(OH)2(aq) + H2(g) Ca > H2O so it WILL react! Mn(ClO4)2 + Mg  Mg(ClO4)2(aq) + Mn(s) Mg > Mn so it WILL react!

Types of reactions Neutralization reactions bases have a hydroxide – OH – in them NaOH(aq) – Ca(OH)2(aq) HA(aq) + BOH  BA + HOH(l) H2S(aq) + Sr(OH)2(aq)  SrS(aq) + HOH(l) look for an acid and a base

Types of reactions Double Replacement (look for 2 ionic compounds as reactants) AX + BY  AY + BX Fe2(SO4)3(aq) + Li3AsO4(aq)  FeAsO4(s) + Li2SO4(aq) Look for two ionic compounds or an ionic compound and an acid as reactants

Solubility Rules All ammonium and group 1 metal salts are SOLUBLE NO EXCEPTIONS All nitrate, chlorate, perchlorate, and acetate salts are SOLUBLE Most chloride, bromide, and iodide salts are SOLUBLE EXCEPTIONS! Compound containing silver, mercury (I), and lead (II) Most fluoride salts are SOLUBLE EXCEPTIONS! Compounds containing magnesium, calcium, strontium, barium, and lead (II) Most sulfate salts are SOLUBLE EXCEPTIONS! Compounds containing strontium, barium, mercury (I), and lead (II) Most sulfide, oxide, and hydroxide salts are INSOLUBLE EXCEPTIONS! Compounds containing calcium, strontium, and barium Most sulfite, carbonate, phosphate, oxalate, and chromate salts are INSOLUBLE

Solubility and Reactions Na2C2O4(aq) + CaCl2(aq)  2 NaCl(aq) + CaC2O4(s) Na2C2O4(aq) + CaCl2(aq)  2 NaCl(aq) + CaC2O4(s) Na2C2O4(aq) + CaCl2(aq)  2 NaCl(aq) + CaC2O4(s) Na2C2O4(aq) + CaCl2(aq)  2 NaCl(aq) + CaC2O4(s) Na2C2O4(aq) + CaCl2(aq)  2 NaCl(aq) + CaC2O4(s) 3 H2SO4(aq) + 2 Fe(OH)3(s)  Fe2(SO4)3(aq) + 6 H2O(l) 3 H2SO4(aq) + 2 Fe(OH)3(s)  Fe2(SO4)3(aq) + 6 H2O(l) 3 H2SO4(aq) + 2 Fe(OH)3(s)  Fe2(SO4)3(aq) + 6 H2O(l) 3 H2SO4(aq) + 2 Fe(OH)3(s)  Fe2(SO4)3(aq) + 6 H2O(l) 3 H2SO4(aq) + 2 Fe(OH)3(s)  Fe2(SO4)3(aq) + 6 H2O(l) 2 LiCl(aq) + Hg2(C2H3O2)2(aq)  2 LiC2H3O2(aq) + Hg2Cl2(s) 2 LiCl(aq) + Hg2(C2H3O2)2(aq)  2 LiC2H3O2(aq) + Hg2Cl2(s) 2 LiCl(aq) + Hg2(C2H3O2)2(aq)  2 LiC2H3O2(aq) + Hg2Cl2(s) 2 LiCl(aq) + Hg2(C2H3O2)2(aq)  2 LiC2H3O2(aq) + Hg2Cl2(s) 2 LiCl(aq) + Hg2(C2H3O2)2(aq)  2 LiC2H3O2(aq) + Hg2Cl2(s) 2 HF(aq) + Ba(OH)2(aq)  BaF2(s) + 2 H2O(l) 2 HF(aq) + Ba(OH)2(aq)  BaF2(s) + 2 H2O(l) 2 HF(aq) + Ba(OH)2(aq)  BaF2(s) + 2 H2O(l) 2 HF(aq) + Ba(OH)2(aq)  BaF2(s) + 2 H2O(l) 2 HF(aq) + Ba(OH)2(aq)  BaF2(s) + 2 H2O(l) K2CO3(aq) + 2 HClO4(aq)  2 KClO4(aq) + H2O(l) + CO2(g) K2CO3(aq) + 2 HClO4(aq)  2 KClO4(aq) + H2O(l) + CO2(g) K2CO3(aq) + 2 HClO4(aq)  2 KClO4(aq) + H2O(l) + CO2(g) K2CO3(aq) + 2 HClO4(aq)  2 KClO4(aq) + H2O(l) + CO2(g) K2CO3(aq) + 2 HClO4(aq)  2 KClO4(aq) + H2O(l) + CO2(g) K2CO3(aq) + 2 HClO4(aq)  2 KClO4(aq) + H2O(l) + CO2(g) 2 NaNO3(aq) + Mg(ClO3)2(aq)  2 NaClO3(aq) + Mg(NO3)2(aq) 2 NaNO3(aq) + Mg(ClO3)2(aq)  2 NaClO3(aq) + Mg(NO3)2(aq) 2 NaNO3(aq) + Mg(ClO3)2(aq)  2 NaClO3(aq) + Mg(NO3)2(aq) 2 NaNO3(aq) + Mg(ClO3)2(aq)  2 NaClO3(aq) + Mg(NO3)2(aq) 2 NaNO3(aq) + Mg(ClO3)2(aq)  2 NaClO3(aq) + Mg(NO3)2(aq)

Predicting Reaction Products

Predicting Reactions – Double Replacement Step 1: Write ONE of each ion directly above the reactants Write the balanced chemical reaction for the reaction of aluminum chloride and magnesium sulfate. Al+3 Cl–1 Mg+2 SO42– Step 1: AlCl3 + MgSO4 

Predicting Reactions – Double Replacement Step 1: Write ONE of each ion directly above the reactants Step 2: Copy ONE of each ion above the products, but swap the anions Write the balanced chemical reaction for the reaction of aluminum chloride and magnesium sulfate. Al+3 Cl–1 Mg+2 SO42– Al3+ SO42– + Mg2+ Cl–1 Step 2: Step 1: AlCl3 + MgSO4 

Predicting Reactions – Double Replacement Step 1: Write ONE of each ion directly above the reactants Step 2: Copy ONE of each ion above the products, but swap the anions Step 3: Combine cations and anions to form neutral compounds Write the balanced chemical reaction for the reaction of aluminum chloride and magnesium sulfate. Al+3 Cl–1 Mg+2 SO42– Al3+ SO42– + Mg2+ Cl–1 Step 3: Step 2: AlCl3 + MgSO4  Al2(SO4)3 + MgCl2

Predicting Reactions – Double Replacement Step 1: Write ONE of each ion directly above the reactants Step 2: Copy ONE of each ion above the products, but swap the anions Step 3: Combine cations and anions to form neutral compounds Write the balanced chemical reaction for the reaction of calcium oxalate with nickel (III) acetate Ca+2 C2O4–2 Ni+3 C2H3O2–1 Ca2+ C2H3O2–1 + Ni3+ C2O4–2 Step 2: Step 1: Step 3: CaC2O4 + Ni(C2H3O2)3  Ca(C2H3O2)2 + Ni2(C2O4)3