CHEMISTRY. Data Booklet revised 2008

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1 CHEMISTRY Data Booklet revised 2008

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3 Legend for Elements Atomic number Electronegativity Symbol Name 1.8 Fe iron Key , 2+ Atomic molar mass (g/mol)* Most stable ion charges 2.0 B boron Note: The legend denotes the physical state of the elements at exactly kpa and K C carbon Metallic solids Non-metallic solids N nitrogen Gases Liquids O oxygen F fluorine He helium Ne neon , 1.9 Ni nickel , 2.2 Pd palladium , Pt platinum 110 (271) Ds darmstadtium 12 * Based on 6 C ( ) Indicates mass of the most stable isotope , Cu copper Ag silver , Au gold 111 (272) Rg roentgenium Zn zinc Cd cadmium , Hg mercury Al aluminium Ga gallium In indium , 1.8 Tl thallium Si silicon Ge germanium , Sn tin * 2+, Pb lead P phosphorus As arsenic , Sb antimony , Bi bismuth S sulfur Se selenium Te tellurium 84 (209) 2+, Po polonium Cl chlorine Br bromine I iodine 85 (210) 2.2 At astatine Ar argon Kr krypton Xe xenon 86 (222) Rn radon * The isotopic mix of naturally occurring lead is more variable than other elements, preventing precision to greater than tenths of a gram per mole Eu europium, Gd gadolinium Tb terbium Dy dysprosium Ho holmium Er erbium Tm thulium Yb ytterbium, Lu lutetium (243) Am, 4+ americium 96 (247) Cm curium 97 (247) Bk, 4+ berkelium 98 (251) Cf californium 99 (252) Es einsteinium 100 (257) Fm fermium 101 (258) Md 2+, mendelevium 102 (259) No nobelium 2+, 103 (262) Lr lawrencium

4 Chemistry Notation Symbol Term Unit(s) c specific heat capacity J/(g ºC) or J/(g K) C heat capacity J/ºC or J/K E electrical potential V or J/C E k kinetic energy kj E p potential energy kj H enthalpy (heat) kj f Hº standard molar enthalpy of formation kj/mol I current A or C/s K c equilibrium constant K a acid ionization (dissociation) constant K b base ionization (dissociation) constant M molar mass g/mol m mass g n amount of substance mol P pressure kpa Q charge C T temperature (absolute) K t temperature (Celsius) ºC t time s V volume L c amount concentration mol/l Symbol Term delta (change in) º standard [ ] amount concentration

5 Miscellaneous C... equivalent to K Specific heat capacity... c air = 1.01 J/(g C) (at K and kpa) c polystyrene foam cup = 1.01 J/(g C) Water autoionization constant... (Dissociation constant) c copper = J/(g C) c aluminium = J/(g C) c tin = J/(g C) c water = 4.19 J/(g C) K w = at K (for ion concentrations in mol/l) Faraday constant... F = C/mol e Quadratic formula... x = b ± b 2 4ac 2a Selected SI Prefixes Prefix Exponential Symbol Value tera T giga G 10 9 mega M 10 6 kilo k 10 3 milli m 10 3 micro µ 10 6 nano n 10 9 pico p 10 12

6 Standard Molar Enthalpies of Formation at K Name Formula Δ f H (kj/mol) aluminium oxide Al 2 O 3 (s) ammonia NH 3 (g) 45.9 ammonium chloride NH 4 Cl(s) ammonium nitrate NH 4 NO 3 (s) barium carbonate BaCO 3 (s) barium chloride BaCl 2 (s) barium hydroxide Ba(OH) 2 (s) barium oxide BaO(s) barium sulfate BaSO 4 (s) benzene C 6 H 6 (l) butane C 4 H 10 (g) calcium carbonate CaCO 3 (s) calcium chloride CaCl 2 (s) calcium hydroxide Ca(OH) 2 (s) calcium oxide CaO(s) calcium sulfate CaSO 4 (s) carbon dioxide CO 2 (g) carbon monoxide CO(g) chromium(iii) oxide Cr 2 O 3 (s) copper(i) oxide Cu 2 O(s) copper(ii) oxide CuO(s) copper(ii) sulfate CuSO 4 (s) copper(i) sulfide Cu 2 S(s) 79.5 copper(ii) sulfide CuS(s) 53.1 dinitrogen tetroxide N 2 O 4 (g) ethane C 2 H 6 (g) 84.0 ethanoic acid (acetic acid) CH 3 COOH(l) ethanol C 2 H 5 OH(l) ethene (ethylene) C 2 H 4 (g) ethyne (acetylene) C 2 H 2 (g) glucose C 6 H 12 O 6 (s) hydrogen bromide HBr(g) 36.3 hydrogen chloride HCl(g) 92.3 hydrogen fluoride HF(g) hydrogen iodide HI(g) hydrogen perchlorate HClO 4 (l) 40.6 hydrogen peroxide H 2 O 2 (l) hydrogen sulfide H 2 S(g) 20.6 iron(ii) oxide FeO(s) iron(iii) oxide Fe 2 O 3 (s) iron(ii,iii) oxide (magnetite) Fe 3 O 4 (s) lead(ii) bromide PbBr 2 (s) lead(ii) chloride PbCl 2 (s) lead(ii) oxide (red) PbO(s) lead(iv) oxide PbO 2 (s) magnesium carbonate MgCO 3 (s) magnesium chloride MgCl 2 (s)

7 Standard Molar Enthalpies of Formation at K Name Formula Δ f H (kj/mol) magnesium hydroxide Mg(OH) 2 (s) magnesium oxide MgO(s) magnesium sulfate MgSO 4 (s) manganese(ii) oxide MnO(s) manganese(iv) oxide MnO 2 (s) mercury(ii) oxide (red) HgO(s) 90.8 mercury(ii) sulfide (red) HgS(s) 58.2 methanal (formaldehyde) CH 2 O(g) methane CH 4 (g) 74.6 methanoic acid (formic acid) HCOOH(l) methanol CH 3 OH(l) nickel(ii) oxide NiO(s) nitric acid HNO 3 (l) nitrogen dioxide NO 2 (g) nitrogen monoxide NO(g) octane C 8 H 18 (l) pentane C 5 H 12 (l) phosphorus pentachloride PCl 5 (s) phosphorus trichloride (liquid) PCl 3 (l) phosphorus trichloride (vapour) PCl 3 (g) potassium bromide KBr(s) potassium chlorate KClO 3 (s) potassium chloride KCl(s) potassium hydroxide KOH(s) propane C 3 H 8 (g) silicon dioxide (α-quartz) SiO 2 (s) silver bromide AgBr(s) silver chloride AgCl(s) silver iodide AgI(s) 61.8 sodium bromide NaBr(s) sodium chloride NaCl(s) sodium hydroxide NaOH(s) sodium iodide NaI(s) sucrose C 12 H 22 O 11 (s) sulfur dioxide SO 2 (g) sulfuric acid H 2 SO 4 (l) sulfur trioxide (liquid) SO 3 (l) sulfur trioxide (vapour) SO 3 (g) tin(ii) chloride SnCl 2 (s) tin(iv) chloride SnCl 4 (l) tin(ii) oxide SnO(s) tin(iv) oxide SnO 2 (s) water (liquid) H 2 O(l) water (vapour) H 2 O(g) zinc oxide ZnO(s) zinc sulfide (sphalerite) ZnS(s) cont d 5

8 Ion Solubility greater than or equal to 0.1 mol/l (very soluble) Solubility less than 0.1 mol/l (slightly soluble) Solubility of Some Common Ionic Compounds in Water at K H + Na + NH 4 +, NO 3 ClO 3, ClO 4 CH 3 COO F Cl Br I SO 4 most most most most RbClO 4 CsClO 4 AgCH 3 COO Hg 2 (CH 3 COO) 2 Li + Mg 2+ Ca 2+ Sr 2+ Ba 2+ Fe 2+ Hg 2 2+ Pb 2+ Cu + Ag + Hg 2 2+ Hg 2+ Pb 2+ 2 Ca 2+ Sr 2+ Ba 2+ Hg 2 2+ Pb 2+ Ag + CO 3 2 PO 4 3 SO 3 2 H + Na + K + NH 4 + most Exception: Li 2 CO 3 is soluble IO 3 OOCCOO 2 S 2 OH H + Na + K + + NH 4 Li + Ni 2+ Zn 2+ most Exceptions: Co(IO 3 ) 2 Fe 2 (C 2 O 4 ) 3 are soluble H + Na + K + + NH 4 Li + Mg 2+ Ca 2+ Note: This solubility table is only a guideline that is established using the K sp values. A concentration of 0.1 mol/l corresponds to approximately 10 g/l to 30 g/l depending on molar mass. most H + Na + K + + NH 4 Li + Sr 2+ Ca 2+ Ba 2+ most Flame Colour of Elements Element Symbol Colour lithium Li red sodium Na yellow potassium K violet rubidium Rb violet cesium Cs violet calcium Ca yellowish red strontium Sr scarlet red barium Ba yellowish green copper Cu blue to green boron B yellowish green lead Pb blue-white Note: The flame test can be used to determine the identity of a metal or a metal ion. Blue to green indicates a range of colours that might appear. 6

9 Table of Selected Standard Electrode Potentials* Reduction Half-Reaction Electrical Potential E (V) F 2 (g) + 2 e 2 F (aq) PbO 2 (s) + SO 2 4 (aq) + 4 H + (aq) + 2 e PbSO 4 (s) + 2 H 2 O(l) MnO 4 (aq) + 8 H + (aq) + 5 e Mn 2+ (aq) + 4 H 2 O(l) Au (aq) + 3 e Au(s) ClO 4 (aq) + 8 H + (aq) + 8 e Cl (aq) + 4 H 2 O(l) Cl 2 (g) + 2 e 2 Cl (aq) HNO 2 (aq) + 4 H + (aq) + 4 e N 2 O(g) + 3 H 2 O(l) Cr 2 O 2 7 (aq) + 14 H + (aq) + 6 e 2 Cr (aq) + 7 H 2 O(l) O 2 (g) + 4 H + (aq) + 4 e 2 H 2 O(l) MnO 2 (s) + 4 H + (aq) + 2 e Mn 2+ (aq) + 2 H 2 O(l) Br 2 (l) + 2 e 2 Br (aq) Hg 2+ (aq) + 2 e Hg(l) OCl (aq) + H 2 O(l) + 2 e Cl (aq) + 2 OH (aq) NO 3 (aq) + 4 H + (aq) + 2 e N 2 O 4 (g) + 2 H 2 O(l) Ag + (aq) + e Ag(s) Fe (aq) + e Fe 2+ (aq) O 2 (g) + 2 H + (aq) + 2 e H 2 O 2 (l) I 2 (s) + 2 e 2 I (aq) O 2 (g) + 2 H 2 O(l) + 4 e 4 OH (aq) Cu 2+ (aq) + 2 e Cu(s) SO 2 4 (aq) + 4 H + (aq) + 2 e H 2 SO 3 (aq) + H 2 O(l) Sn 4+ (aq) + 2 e Sn 2+ (aq) S(s) + 2 H + (aq) + 2 e H 2 S(aq) AgBr(s) + e Ag(s) + Br (aq) H + (aq) + 2 e H 2 (g) Pb 2+ (aq) + 2 e Pb(s) Sn 2+ (aq) + 2 e Sn(s) AgI(s) + e Ag(s) + I (aq) Ni 2+ (aq) + 2 e Ni(s) Co 2+ (aq) + 2 e Co(s) PbSO 4 (s) + 2 e Pb(s) + SO 2 4 (aq) Se(s) + 2 H + (aq) + 2 e H 2 Se(aq) Cd 2+ (aq) + 2 e Cd(s) Cr (aq) + e Cr 2+ (aq) Fe 2+ (aq) + 2 e Fe(s) NO 2 (aq) + H 2 O(l) + e NO(g) + 2 OH (aq) Ag 2 S(s) + 2 e 2 Ag(s) + S 2 (aq) Zn 2+ (aq) + 2 e Zn(s) H 2 O(l) + 2 e H 2 (g) + 2OH (aq) Cr 2+ (aq) + 2 e Cr(s) Se(s) + 2 e Se 2 (aq) SO 2 4 (aq) + H 2 O(l) + 2 e SO 2 3 (aq) + 2OH (aq) Al (aq) + 3 e Al(s) Mg 2+ (aq) + 2 e Mg(s) Na + (aq) + e Na(s) Ca 2+ (aq) + 2 e Ca(s) Ba 2+ (aq) + 2 e Ba(s) K + (aq) + e K(s) Li + (aq) + e Li(s) *For 1.0 mol/l solutions at K (25.00 C) and a pressure of kpa 7

10 Common Name IUPAC / Systematic Name perchloric acid aqueous hydrogen perchlorate hydroiodic acid aqueous hydrogen iodide hydrobromic acid aqueous hydrogen bromide hydrochloric acid aqueous hydrogen chloride sulfuric acid aqueous hydrogen sulfate nitric acid aqueous hydrogen nitrate Relative Strengths of Acids and Bases at K Acid Formula Conjugate Base Formula HClO 4 (aq) ClO 4 (aq) very large HI(aq) I (aq) very large HBr(aq) Br (aq) very large HCl(aq) Cl (aq) very large H 2 SO 4 (aq) HSO 4 (aq) very large HNO 3 (aq) NO 3 (aq) very large hydronium ion H 3 O + (aq) H 2 O(l) 1 oxalic acid HOOCCOOH(aq) HOOCCOO (aq) K a sulfurous acid aqueous hydrogen sulfite H 2 SO 3 (aq) HSO 3 (aq) hydrogen sulfate ion HSO 4 (aq) SO 4 2 (aq) phosphoric acid aqueous hydrogen phosphate citric acid 2-hydroxy-1,2,3-propanetricarboxylic acid hydrofluoric acid aqueous hydrogen fluoride nitrous acid aqueous hydrogen nitrite formic acid methanoic acid H 3 PO 4 (aq) H 2 PO 4 (aq) C 3 H 5 O(COOH) 3 (aq) C 3 H 5 O(COOH) 2 COO (aq) HF(aq) F (aq) HNO 2 (aq) NO 2 (aq) HCOOH(aq) HCOO (aq) hydrogen oxalate ion HOOCCOO (aq) OOCCOO 2 (aq) lactic acid 2-hydroxypropanoic acid ascorbic acid 2(1,2-dihydroxyethyl)-4,5-dihydroxy -furan-3-one benzoic acid benzenecarboxylic acid acetic acid ethanoic acid C 2 H 5 OCOOH(aq) C 2 H 5 OCOO (aq) H 2 C 6 H 6 O 6 (aq) HC 6 H 6 O 6 (aq) C 6 H 5 COOH(aq) C 6 H 5 COO (aq) CH 3 COOH(aq) CH 3 COO (aq)

11 Relative Strengths of Acids and Bases at K Common Name IUPAC / Systematic Name Acid Formula Conjugate Base Formula K a dihydrogen citrate ion C 3 H 5 O(COOH) 2 COO (aq) C 3 H 5 OCOOH(COO) 2 2 (aq) butanoic acid C 3 H 7 COOH(aq) C 3 H 7 COO (aq) propanoic acid C 2 H 5 COOH(aq) C 2 H 5 COO (aq) carbonic acid (CO 2 + H 2 O) aqueous hydrogen carbonate H 2 CO 3 (aq) HCO 3 (aq) hydrogen citrate ion C 3 H 5 OCOOH(COO) 2 2 (aq) C 3 H 5 O(COO) 3 3 (aq) hydrosulfuric acid aqueous hydrogen sulfide H 2 S(aq) HS (aq) hydrogen sulfite ion HSO 3 (aq) SO 3 2 (aq) dihydrogen phosphate ion H 2 PO 4 (aq) HPO 4 2 (aq) hypochlorous acid aqueous hydrogen hypochlorite hydrocyanic acid aqueous hydrogen cyanide HOCl(aq) OCl (aq) HCN(aq) CN (aq) ammonium ion NH + 4 (aq) NH 3 (aq) hydrogen carbonate ion HCO 3 (aq) CO 2 3 (aq) hydrogen ascorbate ion HC 6 H 6 O 6 (aq) C 6 H 6 O 2 6 (aq) hydrogen phosphate ion HPO 2 4 (aq) PO 3 4 (aq) water H 2 O(l) OH (aq) Note: An approximation may be used instead of the quadratic formula when the concentration of H 3 O + produced is less than 5% of the original acid concentration (or the concentration of the acid is times greater than the K a ). The same approximation can also be used for weak bases. The formula of the carboxylic acids have been written so that the COOH group can be easily recognized. Either the common or IUPAC name is acceptable. 9

12 Indicator Acid Base Indicators at K Suggested Abbreviation(s) ph Range Colour Change as ph Increases methyl violet HMv(aq) / Mv (aq) yellow to blue ~ K a cresol red H 2 Cr(aq) / HCr (aq) HCr (aq) / Cr 2 (aq) red to yellow yellow to red ~ thymol blue H 2 Tb(aq) / HTb (aq) HTb (aq) / Tb 2 (aq) red to yellow yellow to blue orange IV HOr(aq) / Or (aq) red to yellow ~ methyl orange HMo(aq) / Mo (aq) red to yellow bromocresol green HBg(aq) / Bg (aq) yellow to blue methyl red HMr(aq) / Mr (aq) red to yellow chlorophenol red HCh(aq) / Ch (aq) yellow to red bromothymol blue HBb(aq) / Bb (aq) yellow to blue phenol red HPr(aq) / Pr (aq) yellow to red phenolphthalein HPh(aq) / Ph (aq) colourless to pink thymolphthalein HTh(aq) / Th (aq) colourless to blue alizarin yellow R HAy(aq) / Ay (aq) yellow to red indigo carmine HIc(aq) / Ic (aq) blue to yellow ~ ,3,5 trinitrobenzene HNb(aq) / Nb (aq) colourless to orange ~

13 Colours of Common Aqueous Ions Solution Concentration Ionic Species 1.0 mol/l mol/l chromate yellow pale yellow chromium(iii) blue-green green chromium(ii) dark blue pale blue cobalt(ii) red pink copper(i) blue-green pale blue-green copper(ii) blue pale blue dichromate orange pale orange iron(ii) lime green colourless iron(iii) orange-yellow pale yellow manganese(ii) pale pink colourless nickel(ii) blue-green pale blue-green permanganate deep purple purple-pink 11

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