COO. chromate CH 3 NH 4. dichromate C 6 COO H 5. cyanide BO 3. hydroxide C 2. iodate CO 3. nitrate HCO 3. nitrite CIO 4.

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1 Data Booklet Data Booklet Updated 2010

2 Table of Common Polyatomic Ions ,1 H hydrogen Li lithium Na sodium K potassium Rb rubidium Cs cesium 87 (223) Fr francium References Be beryllium Mg magnesium Ca calcium Sr strontium Ba barium 88 (226) 0.9 Ra radium acetate (ethanoate) ammonium benzoate borate carbide carbonate hydrogen carbonate perchlorate chlorate chlorite hypochlorite Sc scandium Y yttrium CH 3 COO NH 4 + C 6 H 5 COO BO 3 3 C , 1.5 Ti titanium Zr zirconium CO 3 2 HCO 3 CIO 4 CIO 3 CIO La Hf lanthanum hafnium 89 (227) 104 (261) Ac actinium Lide, D.R CRC Handbook of Chemistry and Physics. 86 th ed. Boca Raton: CRC Press. Speight, James G Lange s Handbook of Chemistry. 16 th ed. New York: McGraw-Hill, Inc. IUPAC commission on atomic weights and isotopic abundances qmw.ac.uk/iupac/atwt/index.html. Rf rutherfordium OCl or CIO chromate dichromate cyanide hydroxide iodate nitrate nitrite oxalate hydrogen oxalate permanganate peroxide , V vanadium , 1.6 Nb niobium Ta tantalum 105 (262) Db dubnium persulfide , 1.7 Cr chromium Mo molybdenum W tungsten 106 (266) Sg seaborgium lanthanide and actinide series begin Ce Pr cerium praseodymium Th thorium , Pa protactinium Cr O 4 2 Cr 2 O 7 2 CN OH IO 3 NO 3 NO 2 OOCCOO 2 HOOCCOO MnO 4 O 2 2 S , Mn manganese 43 (98) Tc technetium Re rhenium 107 (264) Bh bohrium Nd neodymium , U uranium phosphate hydrogen phosphate dihydrogen phosphate silicate sulfate hydrogen sulfate sulfite hydrogen sulfite hydrogen sulfide thiocyanate thiosulfate , 1.8 Fe iron Ru ruthenium Os osmium 108 (277) Hs hassium 61 (145) Pm promethium 93 (237) Np neptunium PO 4 3 HPO 4 2 H 2 PO 4 SiO 3 2 SO 4 2 HSO 4 SO 3 2 HSO 3 HS SCN S 2 O , 1.9 Co cobalt Rh rhodium Ir iridium 109 (268) Mt meitnerium , 1.2 Sm samarium 94 (244) 4+, Pu plutonium

3 Legend for Elements Atomic number Electronegativity Symbol Name Key , 1.8 Fe iron Atomic molar mass (g/mol)* Most stable ion charges Note: The legend denotes the physical state of the elements at exactly kpa and K B boron Metallic solids Non-metallic solids C carbon N nitrogen Gases Liquids O oxygen F fluorine He helium Ne neon , 1.9 Ni nickel , 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 P silicon phosphorus Ge As germanium arsenic ,, Sn Sb tin antimony * , 4+, Pb Bi lead bismuth S sulfur Se selenium Te tellurium 84 (209), Po polonium Cl chlorine Br bromine I iodine 85 (210) 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 95 (243), 4+ Am americium 96 (247) Cm curium 97 (247), 4+ Bk berkelium 98 (251) Cf californium 99 (252) Es einsteinium 100 (257) Fm fermium 101 (258), Md mendelevium 102 (259), No nobelium 103 (262) Lr lawrencium

4 Chemistry Notation Symbol Term Unit(s) c specific heat capacity J/(g. C) or J/(g. K) E standard electrical potential V or J/C E k kinetic energy kj E p potential energy kj H enthalpy (heat) kj f H 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) C t time s V volume L c amount concentration mol/l Symbol Term delta (change in) standard [ ] amount concentration 2

5 Miscellaneous C is equivalent to K Specific Heat Capacities at K and kpa c air = 1.01 J/(g. C) c polystyrene foam cup = 1.01 J/(g. C) c copper = J/(g. C) c aluminium = J/(g. C) c iron = J/(g. C) c tin = J/(g. C) c water = 4.19 J/(g. C) Water Autoionization Constant (Dissociation Constant) K w = at K (for ion concentrations in mol/l) Faraday Constant F = C/mol e Quadratic Formula x b! b 4ac = - - 2a 2 Prefix Selected SI Prefixes 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

6 Standard Molar Enthalpies of Formation at K Name Formula 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 cont d Name Formula 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)

8 Solubility of Some Common Ionic Compounds in Water at K Group 1 ions Ion NH 4 + NO 3 ClO 3 ClO 4 CH 3 COO F Cl Br I SO 4 2 CO 3 2 PO 4 3 SO 3 2 IO 3 OOCCOO 2 OH Solubility greater than or equal to 0.1 mol/l (very soluble) most most most most Group 1 ions Group 1 ions Group 1 ions NH 4 + NH 4 + Co(IO 3 ) 2 Fe 2 (OOCCOO) 3 NH 4 + Solubility less than 0.1 mol/l (slightly soluble) RbClO 4 CsClO 4 AgCH 3 COO Hg 2 (CH 3 COO) 2 Li + Mg Ca Sr Ba Fe Hg 2 Pb Cu + Ag + Hg 2 Pb Tl + Ca Sr Ba Ag + Hg 2 Pb Ra most most most 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. Hg 2 is a polyatomic ion of mercury. 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 *For 1.0 mol/l solutions at K (25.00 C) and a pressure of kpa 7 Electrical Potential E (V) F 2 (g) + 2 e 2F (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 (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 2H 2 O(l) MnO 2 (s) + 4 H + (aq) + 2 e Mn (aq) + 2 H 2 O(l) Br 2 (l) + 2 e 2 Br (aq) Hg (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 (aq) O 2 (g) + 2 H + (aq) + 2 e H 2 O 2 (l) I 2 (s) + 2 e 2I (aq) O 2 (g) + 2 H 2 O(l) + 4 e 4 OH (aq) Cu (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 (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 (aq) + 2 e Pb(s) Sn (aq) + 2 e Sn(s) AgI(s) + e Ag(s) + I (aq) Ni (aq) + 2 e Ni(s) Co (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 (aq) + 2 e Cd(s) Cr (aq) + e Cr (aq) Fe (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 (aq) + 2 e Zn(s) H 2 O(l) + 2 e H 2 (g) + 2OH (aq) Cr (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 (aq) + 2 e Mg(s) Na + (aq) + e Na(s) Ca (aq) + 2 e Ca(s) Ba (aq) + 2 e Ba(s) K + (aq) + e K(s) Li + (aq) + e Li(s)

10 Relative Strengths of Acids and Bases at K Common Name IUPAC / Systematic Name Acid Formula Conjugate Base Formula K a 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 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) sulfurous acid aqueous hydrogen sulfite H 2 SO 3 (aq) HSO 3 (aq) hydrogen sulfate ion HSO 4 (aq) SO4 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 C 2 H 5 OCOOH(aq) C 2 H 5 OCOO (aq) ascorbic acid HC H O (aq) (1,2-dihydroxyethyl)-4,5-dihydroxy-furan-3-one H 2 C 6 H 6 O 6 (aq) HC 6 H 6 O 6 8

11 benzoic acid benzenecarboxylic acid acetic acid ethanoic acid C 6 H 5 COOH(aq) C 6 H 5 COO (aq) CH 3 COOH(aq) CH 3 COO (aq) 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) C3 H 5 O(COO) 3 3 (aq) hydrosulfuric acid aqueous hydrogen sulfide H 2 S(aq) HS (aq) hydrogen sulfite ion HSO 3 (aq) SO3 2 (aq) dihydrogen phosphate ion H 2 PO 4 (aq) HPO4 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) NH3 (aq) hydrogen carbonate ion HCO 3 (aq) CO3 2 (aq) hydrogen ascorbate ion HC 6 H 6 O 6 (aq) C6 H 6 O 6 2 (aq) hydrogen phosphate ion HPO 4 2 (aq) PO4 3 (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 ). An approximation can also be used for weak bases. The formulas 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 AcidBase Indicators at K Indicator Suggested Abbreviations ph Range Colour Change as ph Increases K a methyl violet HMv(aq) / Mv (aq) yellow to blue ~ 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 ~ ,3,5trinitrobenzene 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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