CHEMISTRY ATAR COURSE DATA BOOKLET 2019 Chemistry ATAR Course Data Booklet 2019 Ref: 19-012 Table of contents Periodic table of the elements........................................................................................................ 3 Formulae........................................................................................................................................ 4 Units............................................................................................................................................... 4 Constants....................................................................................................................................... 4 Solubility rules for ionic solids in water........................................................................................... 4 Colours of selected substances .................................................................................................... 5 α-amino acids............................................................................................................................. 6–7 Standard reduction potentials at 25 0C........................................................................................... 8 Copyright © School Curriculum and Standards Authority, 2018 2016 This document – apart from any third party copyright material contained in it – may be freely copied, or communicated on an intranet, for non-commercial purposes in educational institutions, provided that it is not changed and that the School Curriculum and This document – apart from any thirdas party contained it – may be freelyrights copied, on an Standards Authority is acknowledged the copyright copyright material owner, and that theinAuthority’s moral are or notcommunicated infringed. intranet, for non-commercial purposes in educational institutions, provided that it is not changed and that the School Curriculum and Standards Authority is acknowledged aspurpose the copyright owner, thethe Authority’s rights are not infringed. 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Published by the School Curriculum and Standards Authority of Western Australia 303 Sevenoaks Street CANNINGTON WA 6107 2 Periodic table of the elements [Data source: The International Union of Pure and Applied Chemistry Periodic Table of the Elements (2016)] 3 Formulae m = M cV V mass molar mass Number of moles n = Number of moles of solute n = Number of moles of a gas at STP n Ideal gas law PV = 22.71 = nRT Parts per million ppm = mass of solution (kg) pH of a solution pH + = - log10 [H ] mass of solute (mg) Units Volumes are given in the units of litres (L), or millilitres (mL) Temperatures are given in the units of degrees Celsius (°C) or kelvin (K) It may be assumed that 0.0 °C = 273.15 K Energy changes are given in kilojoules (kJ) Pressures are given in kilopascals (kPa) Solution concentrations are given in the units moles per litre (mol L-1), grams per litre (g L-1) or parts per million (ppm) Constants Universal gas constant, R = 8.314 J K-1 mol-1 Avogadro constant, N = 6.022×1023 mol-1 Volume of 1.00 mol of an ideal gas at 0.0 °C and 100.0 kPa is 22.71 L STP is 0.0 °C and 100.0 kPa Equilibrium constant for water at 25 °C, Kw = 1.00×10-14 Solubility rules for ionic solids in water Soluble in water Exceptions Soluble Most chlorides Most bromides Most iodides Slightly soluble PbCℓ2 PbBr2 Insoluble AgCℓ AgBr AgI, PbI2 All nitrates No exceptions All ethanoates Most sulfates CaSO4, Ag2SO4 SrSO4, BaSO4, PbSO4 Insoluble in water Insoluble Exceptions Soluble Slightly soluble Most hydroxides NaOH, KOH, Ba(OH)2 NH4OH*, AgOH** Ca(OH)2, Sr(OH)2 Most carbonates Na2CO3, K2CO3, (NH4)2CO3 Most phosphates Na3PO4, K3PO4, (NH4)3PO4 Most sulfides Na2S, K2S, (NH4)2S * ** NH3 dissolves in water to form both NH3 (aq) and NH4+(aq)/OH–(aq) Ag+(aq) reacts with OH–(aq) to form insoluble Ag2O Soluble = more than 0.1 mole dissolves per litre Slightly soluble = between 0.01 and 0.1 mole dissolves per litre Insoluble = less than 0.01 mole dissolves per litre 4 Colours of selected substances In general, ionic solids have the same colour as that of any coloured ion they contain. Two colourless ions in general produce a white solid. Selected exceptions to these two basic rules are noted below. Ionic Solid copper(II) carbonate copper(II) chloride copper(II) oxide copper(II) sulfide lead(II) iodide lead(II) sulfide manganese(IV) oxide silver carbonate silver iodide silver oxide silver sulfide Colour green green black black yellow grey black yellow pale yellow brown black Other coloured substances Most gases and liquids are colourless, and most metals are silvery or grey. Selected exceptions to these basic rules are noted below. Substance copper(s) gold(s) nitrogen dioxide(g) sulfur(s) Colour salmon pink yellow brown yellow Coloured halogens Halogen F2(g) Cℓ2(g) Br2(ℓ) I2(g) Colour of free element yellow greenish-yellow red purple Halogen Cℓ2(aq) Br2(aq) I2(aq) Colour of halogen in aqueous solution pale yellow orange brown Halogen Br2 Colour of halogen in organic solvent red I2 purple Coloured ions in aqueous solution Cation Cr3+ Co2+ Cu2+ Fe2+ Fe3+ Mn2+ Ni2+ Colour deep green pink blue pale green pale brown pale pink green Anion CrO42– Colour yellow Cr2O72– MnO4– orange purple 5 α–amino acids Name Symbol alanine Ala Structure CH3 H 2N arginine COOH Arg NH H 2N asparagine CH CH2 CH2 CH COOH CH2 NH Asn O CH2 H 2N aspartic acid Asp Cys COOH CH COOH CH2 SH CH COOH Gln O CH2 H2 N glutamic acid H 2N Gly histidine His CH2 CH Glu glycine NH2 COOH CH2 H 2N glutamine C CH H2N cysteine C CH2 CH2 CH COOH H 2N NH2 COOH CH2 COOH COOH N CH2 H 2N isoleucine C Ile CH N H COOH CH3 CH CH2 H2N CH COOH 6 CH3 NH2 α–amino acids Name Symbol leucine Leu Structure CH3 CH CH3 CH2 H 2N lysine Lys H2N methionine CH2 CH2 CH COOH Met H2N phenylalanine CH CH2 CH COOH serine Ser threonine tryptophan CH2 S CH3 CH2 H2N Pro CH2 CH2 Phe proline COOH CH H N CH2 Thr COOH COOH OH H2N CH COOH CH3 CH OH H 2N CH COOH H N Trp CH2 H 2N tyrosine Tyr COOH CH2 H2 N valine CH Val 7 CH OH COOH CH3 CH CH3 H 2N CH COOH NH2 Standard Reduction Potentials at 25 °C Half-reaction F2(g) + 2 e H2O2(aq) + 2 H (aq) + 2 e + PbO2(s) + SO4 (aq) + 4 H (aq) + 2 e 2– + 2 F (aq) + 2.89 – 2 H2O(ℓ) + 1.76 – 2 HCℓO(aq) + 2 H+(aq) + 2 e– MnO4–(aq) + 8 H+(aq) + 5 e– Au3+(aq) + 3 e– HCℓO(aq) + H (aq) + 2 e – PbO2(s) + 4 H (aq) + 2 e – + + Cℓ2(g) + 2 e Cr2O7 (aq) + 14 H (aq) + 6 e 2– + O2(g) + 4 H (aq) + 4 e + E°(volts) – – PbSO4(s) + 2 H2O(ℓ) + 1.69 Cℓ2(g) + 2 H2O(ℓ) + 1.63 Mn2+(aq) + 4 H2O(ℓ) + 1.51 Au(s) + 1.50 Cℓ (aq) + H2O(ℓ) + 1.49 – Pb (aq) + 2 H2O(ℓ) 2+ + 1.46 – 2 Cℓ (aq) – 2 Cr (aq) + 7 H2O(ℓ) + 1.36 – + 1.36 – 3+ 2 H2O(ℓ) + 1.23 – – 2 Br (aq) + 1.08 Ag (aq) + e – Ag(s) + 0.80 Fe (aq) + e – Fe (aq) + 0.77 O2(g) + 2 H (aq) + 2 e – H2O2(aq) + 0.70 Br2(ℓ) + 2 e + 3+ + I2(s) + 2 e 2+ 2 I (aq) + 0.54 – 4 OH (aq) + 0.40 Cu (aq) + 2 e – Cu(s) + 0.34 S(s)+ 2 H (aq) + 2 e – + 0.17 2 H (aq) + 2 e H2S(aq) – Pb (aq) + 2 e – Pb(s) – 0.13 Sn (aq) + 2 e – Sn(s) – 0.14 Ni (aq) + 2 e – Ni(s) – 0.24 Co (aq) + 2 e – Co(s) – O2(g) + 2 H2O(ℓ) + 4 e 2+ + + 2+ 2+ 2+ 2+ PbSO4(s) + 2 e – – – H2(g) 0 exactly – 0.28 Pb(s) + SO4 (aq) 2– – 0.36 Cd (aq) + 2 e – Cd(s) – 0.40 2 CO2(g) + 2 H (aq) + 2 e – – 0.43 Fe2+(aq) + 2 e– H2C2O4(aq) Fe(s) – 0.44 Cr (aq) + 3 e – Cr(s) – 0.74 Zn (aq) + 2 e – Zn(s) 2+ + 3+ 2+ 2 H2O(ℓ) + 2 e – Mn 2+(aq) + 2 e– – 0.76 H2(g) + 2 OH (aq) – – 0.83 Mn(s) – 1.18 Aℓ (aq) + 3 e – Aℓ(s) – 1.68 Mg (aq) + 2 e – Mg(s) – 2.36 Na (aq) + e – Na(s) – 2.71 Ca2+(aq) + 2 e– Ca(s) – 2.87 Sr (aq) + 2 e – Sr(s) – 2.90 Ba (aq) + 2 e – Ba(s) – 2.91 K (aq) + e – K(s) – 2.94 3+ 2+ + 2+ 2+ + [Data source: Aylward, G.H., & Findlay, T. (2008). SI Chemical Data (6th ed.). Queensland: John Wiley & Sons Australia, Ltd.] 8