Happy Birthday Johannes Diderik van der Waals (1837) Mastering Chemistry New assignment will be posted later today Due Tuesday by 11:59PM Reading Chapter 7, sections 1-4

You analyze a 73.8241g sample of 18-crown-6 (a specific crown either) and find that there are 40.2489g of carbon and 26.8055g of oxygen in the sample with the rest being hydrogen. a) What are the percents of carbon and oxygen in the sample of 18-crown-6? What is the percent of hydrogen in 18-crown-6? What is the empirical formula of 18-crown-6? 18-crown-6 has a molar mass of 264.32 g/mol. What is the molecular formula?

You analyze a 73.8241g sample of 18-crown-6 (a specific crown either) and find that there are 40.2489g of carbon and 26.8055g of oxygen in the sample.

You analyze a 73.8241g sample of 18-crown-6 (a specific crown either) and find that there are 40.2489g of carbon and 26.8055g of oxygen in the sample. Empirical formula  C2H4O

You analyze a 73.8241g sample of 18-crown-6 (a specific crown either) and find that there are 40.2489g of carbon and 26.8055g of oxygen in the sample. 18-crown-6 has a molar mass of 264.32 g/mol C2H4O = 44.06 g/mol C2H4O 6(C2H4O)  C12H24O6 molecular formula = C12H24O6

States of Matter Solid – (s)  Fe(s) Solid – (s) Solid Liquid – (l) Liquid – (l)  H2O(l) Liquid Gas – (g) Gas – (g)  CO2(g) Gas Aqueous – (aq)  NaCl(aq) Aqueous – (aq) Aqueous Aqueous means “dissolved in water”

Balancing Chemical Equations Step 1: Translate from words to symbols sodium chloride is reacted with silver nitrate to form sodium nitrate and silver chloride sodium chloride is reacted with silver nitrate to form sodium nitrate and silver chloride sodium chloride is reacted with silver nitrate to form sodium nitrate and silver chloride sodium chloride is reacted with silver nitrate to form sodium nitrate and silver chloride sodium chloride is reacted with silver nitrate to form sodium nitrate and silver chloride sodium chloride is reacted with silver nitrate to form sodium nitrate and silver chloride NaCl(aq) NaCl(aq) + AgNO3(aq) NaCl(aq) + AgNO3(aq)  NaCl(aq) + AgNO3(aq)  NaNO3(aq) NaCl(aq) + AgNO3(aq)  NaNO3(aq) + AgCl(s)

Balancing Chemical Equations Step 1: Translate from words to symbols sodium chloride is reacted with silver nitrate to form sodium nitrate and silver chloride NaCl(aq) + AgNO3(aq)  NaNO3(aq) + AgCl(s) Step 2: Balance equation using coefficients Na 1 Na 1 Cl 1 Cl 1 Ag 1 Ag 1 NO3 1 NO3 1

Balancing Chemical Equations Step 1: Translate from words to symbols calcium bromate is added to lithium carbonate to form calcium carbonate and lithium bromate calcium bromate is added to lithium carbonate to form calcium carbonate and lithium bromate calcium bromate is added to lithium carbonate to form calcium carbonate and lithium bromate calcium bromate is added to lithium carbonate to form calcium carbonate and lithium bromate calcium bromate is added to lithium carbonate to form calcium carbonate and lithium bromate calcium bromate is added to lithium carbonate to form calcium carbonate and lithium bromate Ca(BrO3)2(aq) Ca(BrO3)2(aq) + Li2CO3(aq) Ca(BrO3)2(aq) + Li2CO3(aq)  CaCO3(s) + LiBrO3(aq) Ca(BrO3)2(aq) + Li2CO3(aq)  Ca(BrO3)2(aq) + Li2CO3(aq)  CaCO3(s)

Balancing Chemical Equations Step 1: Translate from words to symbols calcium bromate is added to lithium carbonate to form calcium carbonate and lithium bromate Ca(BrO3)2(aq) + Li2CO3(aq)  CaCO3(s) + 2 LiBrO3(aq) Ca(BrO3)2(aq) + Li2CO3(aq)  CaCO3(s) + 2 LiBrO3(aq) Ca(BrO3)2(aq) + Li2CO3(aq)  CaCO3(s) + 2 LiBrO3(aq) Ca(BrO3)2(aq) + Li2CO3(aq)  CaCO3(s) + 2 LiBrO3(aq) Ca(BrO3)2(aq) + Li2CO3(aq)  CaCO3(s) + 2 LiBrO3(aq) Ca(BrO3)2(aq) + Li2CO3(aq)  CaCO3(s) + LiBrO3(aq) Ca(BrO3)2(aq) + Li2CO3(aq)  CaCO3(s) + 2 LiBrO3(aq) Ca(BrO3)2(aq) + Li2CO3(aq)  CaCO3(s) + LiBrO3(aq) Ca(BrO3)2(aq) + Li2CO3(aq)  CaCO3(s) + 2 LiBrO3(aq) Ca(BrO3)2(aq) + Li2CO3(aq)  CaCO3(s) + LiBrO3(aq) Ca(BrO3)2(aq) + Li2CO3(aq)  CaCO3(s) + LiBrO3(aq) Ca(BrO3)2(aq) + Li2CO3(aq)  CaCO3(s) + LiBrO3(aq) Ca(BrO3)2(aq) + Li2CO3(aq)  CaCO3(s) + LiBrO3(aq) Ca(BrO3)2(aq) + Li2CO3(aq)  CaCO3(s) + LiBrO3(aq) Ca(BrO3)2(aq) + Li2CO3(aq)  CaCO3(s) + LiBrO3(aq) Ca(BrO3)2(aq) + Li2CO3(aq)  CaCO3(s) + 2 LiBrO3(aq) Ca(BrO3)2(aq) + Li2CO3(aq)  CaCO3(s) + 2 LiBrO3(aq) Ca(BrO3)2(aq) + Li2CO3(aq)  CaCO3(s) + 2 LiBrO3(aq) Ca(BrO3)2(aq) + Li2CO3(aq)  CaCO3(s) + LiBrO3(aq) Step 2: Balance equation using coefficients Ca 1 1 Ca 1 1 BrO3 2 2 BrO3 1 2 Li 2 2 Li 1 2 CO3 1 1 CO3 1 1

Balancing Chemical Equations copper (I) iodide and lead (II) acetate react to form copper (I) acetate and lead (II) iodide copper (I) iodide and lead (II) acetate react to form copper (I) acetate and lead (II) iodide copper (I) iodide and lead (II) acetate react to form copper (I) acetate and lead (II) iodide copper (I) iodide and lead (II) acetate react to form copper (I) acetate and lead (II) iodide copper (I) iodide and lead (II) acetate react to form copper (I) acetate and lead (II) iodide CuI(aq) CuI(aq) + Pb(C2H3O2)2(aq)  CuC2H3O2(aq) CuI(aq) + Pb(C2H3O2)2(aq) CuI(aq) + Pb(C2H3O2)2(aq)  CuC2H3O2(aq) + PbI2(s)

Balancing Chemical Equations copper (I) iodide and lead (II) acetate react to form copper (I) acetate and lead (II) iodide 2 CuI(aq) + Pb(C2H3O2)2(aq)  CuC2H3O2(aq) + PbI2(s) 2 CuI(aq) + Pb(C2H3O2)2(aq)  CuC2H3O2(aq) + PbI2(s) 2 CuI(aq) + Pb(C2H3O2)2(aq)  2 CuC2H3O2(aq) + PbI2(s) 2 CuI(aq) + Pb(C2H3O2)2(aq)  CuC2H3O2(aq) + PbI2(s) 2 CuI(aq) + Pb(C2H3O2)2(aq)  CuC2H3O2(aq) + PbI2(s) 2 CuI(aq) + Pb(C2H3O2)2(aq)  CuC2H3O2(aq) + PbI2(s) 2 CuI(aq) + Pb(C2H3O2)2(aq)  CuC2H3O2(aq) + PbI2(s) 2 CuI(aq) + Pb(C2H3O2)2(aq)  CuC2H3O2(aq) + PbI2(s) 2 CuI(aq) + Pb(C2H3O2)2(aq)  2 CuC2H3O2(aq) + PbI2(s) 2 CuI(aq) + Pb(C2H3O2)2(aq)  CuC2H3O2(aq) + PbI2(s) 2 CuI(aq) + Pb(C2H3O2)2(aq)  2 CuC2H3O2(aq) + PbI2(s) 2 CuI(aq) + Pb(C2H3O2)2(aq)  CuC2H3O2(aq) + PbI2(s) 2 CuI(aq) + Pb(C2H3O2)2(aq)  2 CuC2H3O2(aq) + PbI2(s) 2 CuI(aq) + Pb(C2H3O2)2(aq)  2 CuC2H3O2(aq) + PbI2(s) 2 CuI(aq) + Pb(C2H3O2)2(aq)  CuC2H3O2(aq) + PbI2(s) 2 CuI(aq) + Pb(C2H3O2)2(aq)  2 CuC2H3O2(aq) + PbI2(s) 2 CuI(aq) + Pb(C2H3O2)2(aq)  2 CuC2H3O2(aq) + PbI2(s) 2 CuI(aq) + Pb(C2H3O2)2(aq)  2 CuC2H3O2(aq) + PbI2(s) 2 CuI(aq) + Pb(C2H3O2)2(aq)  2 CuC2H3O2(aq) + PbI2(s) 2 CuI(aq) + Pb(C2H3O2)2(aq)  2 CuC2H3O2(aq) + PbI2(s) CuI(aq) + Pb(C2H3O2)2(aq)  CuC2H3O2(aq) + PbI2(s) CuI(aq) + Pb(C2H3O2)2(aq)  CuC2H3O2(aq) + PbI2(s) CuI(aq) + Pb(C2H3O2)2(aq)  CuC2H3O2(aq) + PbI2(s) CuI(aq) + Pb(C2H3O2)2(aq)  CuC2H3O2(aq) + PbI2(s) CuI(aq) + Pb(C2H3O2)2(aq)  CuC2H3O2(aq) + PbI2(s) CuI(aq) + Pb(C2H3O2)2(aq)  CuC2H3O2(aq) + PbI2(s) CuI(aq) + Pb(C2H3O2)2(aq)  CuC2H3O2(aq) + PbI2(s) CuI(aq) + Pb(C2H3O2)2(aq)  CuC2H3O2(aq) + PbI2(s) CuI(aq) + Pb(C2H3O2)2(aq)  CuC2H3O2(aq) + PbI2(s) Cu 1 2 2 Cu 1 1 2 I 1 2 2 I 2 2 2 Pb 1 1 1 Pb 1 1 1 C2H3O2 2 2 2 C2H3O2 1 1 2

Balancing Chemical Equations Al2(SO4)3(aq) + BaCl2(aq)  2 AlCl3(aq) + 3 BaSO4(s) Al2(SO4)3(aq) + BaCl2(aq)  2 AlCl3(aq) + BaSO4(s) Al2(SO4)3(aq) + 3 BaCl2(aq)  2 AlCl3(aq) + 3 BaSO4(s) Al2(SO4)3(aq) + BaCl2(aq)  AlCl3(aq) + BaSO4(s) Al 2 2 2 2 Al 1 2 2 2 SO4 3 3 3 3 SO4 1 1 3 3 Ba 1 1 1 3 Ba 1 1 3 3 Cl 2 2 2 6 Cl 3 6 6 6

Diatomic Elements Elements the exist as diatomic molecules when UNCOMBINED (meaning not in a compound with other elements). H2, N2, O2, F2, Cl2, Br2, I2 NaCl, AlI3, BiF5, TiBr4, K3N

Balancing Chemical Equations 4 12 10 6 2 C3H5(NO3)3(l)  CO2(g) + H2O(l) + 3 N2(g) + O2(g) 2 C3H5(NO3)3(l)  6 CO2(g) + H2O(l) + 3 N2(g) + O2(g) 2 C3H5(NO3)3(l)  6 CO2(g) + 5 H2O(l) + 3 N2(g) + O2(g) 4 C3H5(NO3)3(l)  12 CO2(g) + 10 H2O(l) + 6 N2(g) + O2(g) C3H5(NO3)3(l)  CO2(g) + H2O(l) + N2(g) + O2(g) C 3 6 6 6 12 C 1 1 6 6 12 N 3 6 6 6 12 N 2 6 6 6 12 H 5 10 10 10 20 H 2 2 2 10 20 O 9 18 18 18 36 O 5 5 15 19 36

Types of reactions Decomposition Synthesis One thing  more than one thing A  B + C… H2CO3(aq)  H2O(l) + CO2(g) Synthesis Two things to one thing A + B…  C N2(g) + 3 H2(g)  2 NH3(l)

Types of reactions Single Displacement Combustion A + BX  B + AX Ca(s) + 2 HCl(aq)  H2(g) + CaCl2(aq) Combustion A + O2(g)  H2O(l) + CO2(g) C5H12(l) + 7 O2(g)  6 H2O(l) + 4 CO2(g) Double Displacement (look for 2 ionic compounds on the reactant side) AX + BY  AY + BX 3 Fe2(SO4)3(aq) + 2 Li3AsO4(aq)  2 FeAsO4(s) + 3 Li2SO4(aq)

Types of reactions Neutralization look for an acid and a base bases have a hydroxide – OH – in them NaOH(aq) Ba(OH)2(aq) NH3(aq) HA(aq) + BOH  BA + H2O(l) H2S(aq) + Sr(OH)2(aq)  SrS(aq) + 2 H2O(l)

Balancing Chemical Equations Write the balanced equation for the burning of heptane, C7H16(l) COMBUSTION!!!!! C7H16(l) + O2(g)  H2O(g) + 7 CO2(g) C7H16(l) + O2(g)  8 H2O(g) + 7 CO2(g) C7H16(l) + O2(g) C7H16(l) C7H16(l) + O2(g)  H2O(g) + CO2(g) C7H16(l) + O2(g)  H2O(g) C7H16(l) + 11 O2(g)  8 H2O(g) + 7 CO2(g) C 7 7 7 7 C 1 7 7 7 H 16 16 16 16 H 2 2 16 16 O 2 2 2 22 O 3 15 22 22

Balancing Chemical Equations Write the balanced equation for the burning of nonene, C9H18(l) TYPO!!!!!! 2 C9H18(l) + O2(g)  18 H2O(g) + 18 CO2(g) 2 C9H18(l) + 27 O2(g)  18 H2O(g) + 18 CO2(g) C9H18(l) C9H18(l) + O2(g)  H2O(g) C9H18(l) + O2(g) C9H18(l) + O2(g)  H2O(g) + 9 CO2(g) C9H18(l) + O2(g)  H2O(g) + CO2(g) C9H18(l) + O2(g)  9 H2O(g) + 9 CO2(g) even number of oxygen odd number of oxygen double EVERYTHING other than O2 C 9 18 18 C 1 9 9 18 H 18 36 36 H 2 2 18 36 O 2 2 54 O 3 19 27 54

Solubility Rules All ammonium and group 1 metal salts are SOLUBLE (no exceptions) All nitrate, chlorate, perchlorate, and acetate salts are SOLUBLE (no exceptions) 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 and hydroxide salts are INSOLUBLE. EXCEPTIONS! Compounds containing calcium, strontium, and barium Most 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 Na2C2O4(aq) + CaCl2(aq)  2 NaCl + CaC2O4 Na2C2O4(aq) + CaCl2  2 NaCl + CaC2O4 Na2C2O4 + CaCl2  2 NaCl + CaC2O4 3 H2SO4(aq) + 2 Fe(OH)3(s)  Fe2(SO4)3(aq) + 6 H2O 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 + 6 H2O 3 H2SO4(aq) + 2 Fe(OH)3  Fe2(SO4)3 + 6 H2O 3 H2SO4 + 2 Fe(OH)3  Fe2(SO4)3 + 6 H2O 2 LiCl(aq) + Hg2(C2H3O2)2(aq)  2 LiC2H3O2(aq) + Hg2Cl2(s) 2 LiCl(aq) + Hg2(C2H3O2)2(aq)  2 LiC2H3O2(aq) + Hg2Cl2 2 LiCl(aq) + Hg2(C2H3O2)2(aq)  2 LiC2H3O2 + Hg2Cl2 2 LiCl(aq) + Hg2(C2H3O2)2  2 LiC2H3O2 + Hg2Cl2 2 LiCl + Hg2(C2H3O2)2  2 LiC2H3O2 + Hg2Cl2 K2CO3(aq) + 2 HClO4(aq)  2 KClO4(aq) + H2O(l) + CO2(g) K2CO3(aq) + 2 HClO4(aq)  2 KClO4(aq) + H2O(l) + CO2 K2CO3(aq) + 2 HClO4(aq)  2 KClO4(aq) + H2O + CO2 K2CO3(aq) + 2 HClO4(aq)  2 KClO4 + H2O + CO2 K2CO3 + 2 HClO4  2 KClO4 + H2CO3 K2CO3(aq) + 2 HClO4  2 KClO4 + H2O + CO2 K2CO3 + 2 HClO4  2 KClO4 + H2O + CO2 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 2 NaNO3(aq) + Mg(ClO3)2(aq)  2 NaClO3 + Mg(NO3)2 2 NaNO3(aq) + Mg(ClO3)2  2 NaClO3 + Mg(NO3)2 2 NaNO3 + Mg(ClO3)2  2 NaClO3 + Mg(NO3)2

Electrolytes What are they? Three types of electrolytes: Non-electrolytes Molecular compounds Insoluble salts (insoluble ionic compounds) Do NOT form ions in water Weak electrolytes Weak acids Form very VERY few ions in water

Electrolytes What are they? Three types of electrolytes: Strong electrolytes Strong acids Soluble salts (soluble ionic compounds) Completely break apart into ions Called ionization when talking about acids Called disassociation when talking about salts

Electrolytes Strong acids? HCl(aq) HBr(aq) HI(aq) HNO3(aq) HClO4(aq) H2SO4(aq) ANY other acid is a weak acid (which makes it a weak electrolyte