Chemistry Senior External Examination. Paper Two Resource book. Wednesday 28 October :00 pm to 3:10 pm. Directions.

Transcription

1 Directions You may write in this book during perusal time. Contents Table of constants Simple rules for solubility of salts in water Standard reduction potentials for half-reactions Periodic classification of the elements List of elements by name After the examination Take this book when you leave the examination room Senior External Examination Chemistry Paper Two Resource book Wednesday 28 October :00 pm to 3:10 pm The State of Queensland (Queensland Studies Authority) 2009

2 Planning space

3 Table of constants Negative charge on the electron 1.6 x coulomb Negative charge on a mole of electrons coulomb = 1 Faraday Avogadro s Number (N A ) 6.02 x Gas constant (R) L atm K 1 mole J K 1 mole 1 Normal atmospheric pressure 1 atm = kpa = 760 mm Hg Specific heat of water 4.2 Jg 1 K 1 = 75 J mole 1 K 1 Dissociation constant for water at 25 C (K W ) 1.00 x Molar volume of gas at S.T.P L = 22.4 dm 3 Molar volume of gas at 25 C and 1 atm 24.5 L = 24.5 dm 3 1 atomic mass unit (1 amu) 1.66 x g = 1.66 x kg Simple rules for solubility of salts in water 1 All nitrate (NO 3 ) salts are soluble. 2 Most salts of Na +, K + and NH + 4 are soluble. 3 Most chloride salts are soluble. Notable exceptions are AgCl, PbCl 2 and Hg 2 Cl 2. 4 Most sulfate salts are soluble. Notable exceptions are BaSO 4, PbSO 4, and CaSO Most hydroxides are only slightly soluble. The important soluble hydroxides are NaOH, KOH, and Ca(OH) 2. Most sulfide (S 2 ), carbonate (CO 3 2 ), and phosphate (PO 4 3 ) salts are only slightly soluble Chemistry Paper Two Resource book 1

4 Standard reduction potentials for half-reactions Ionic concentrations = 1 molar in water Temperature = 25 C All ions are in water Strength as E Strength as Half-reaction oxidising agent (Volts) reducing agent Very strong F 2 (g) + 2e 2F Very weak oxidising agents H 2 O 2 + 2H + + 2e 2H 2 O reducing agents MnO 4 + 8H + + 5e Mn H 2 O Au e Au(s) Cl 2 (g) + 2e 2Cl Cr 2 O H + + 6e 2Cr H 2 O MnO 2 (s) + 4H + + 2e Mn H 2 O ½O 2 (g) + 2H + + 2e H 2 O Br 2 (l) + 2e 2Br AuCl 4 + 3e Au(s) + 4Cl NO 3 + 4H + + 3e NO(g) + 2H 2 O ½O 2 (g) + 2H + (10-7 M) + 2e H 2 O Weak reducing Ag + + e Ag(s) agents ½Hg e Hg(l) Hg e Hg(l) NO 3 + 2H + + e NO 2 (g) + H 2 O Fe 3+ + e Fe O 2 (g) + 2H + + e H 2 O Increasing l 2 (s) + 2e 2l strength as Cu + + e Cu(s) reducing agent Cu e Cu(s) SO H + + 2e SO 2 (g) + 2H 2 O Increasing Cu 2+ + e Cu strength as Sn e Sn oxidising agent S + 2H + + 2e H 2 S(g) H + + 2e H 2 (g) 0.00 Pb e Pb(s) Sn e Sn(s) Ni e Ni(s) Co e Co(s) Se + 2H + + 2e H 2 Se(g) Cr 3+ + e Cr H + (10-7 M) + 2e H 2 (g) Fe e Fe(s) Weak Ag 2 S + 2e 2Ag(s) + S oxidising Te + 2H + + 2e H 2 Te(g) agents Cr e Cr(s) Zn e Zn(s) H 2 O + 2e 2OH + H 2 (g) Mn e Mn(s) Al e Al(s) Mg e Mg(s) Na + + e Na(s) Ca e Ca(s) Sr e Sr(s) Ba e Ba(s) Cs + + e Cs(s) Very weak K + + e K(s) Very strong oxidising Rb + + e Rb(s) reducing agents Li + + e Li(s) agents Chemistry Paper Two Resource book

5 Blank page 2009 Chemistry Paper Two Resource book 3

6 Periodic classification of the elements Groups (IUPAC)* Atomic 18 1 Number H Li Na 23.0 K Rb Cs Fr (223) Be Mg Symbol Isotopic mass** (average to one decimal place) Ca Sr Ba Ra Sc 45.0 Y Lu Lr (260) 22 Ti Zr Hf Rf (261) V Nb Ta Db (262) 24 Cr Mo W Sg (263) 25 Mn Tc (98) 75 Re Bh (264) Fe 55.8 Ru Os Hs (269) 27 Co Rh Ir Mt (268) 28 Ni Pd Pt Ds (271) 29 Cu Ag Au Rg (272) 30 Zn Cd Hg B Al Ga In Tl C Si Ge Sn Pb N 14.0 P As Sb Bi O 16.0 S Se Te Po (209) F Cl Br I At (210) He Ne Ar Kr Xe Rn (222) 57 La Ce Pr Nd Ac Th Pa U (227) (231) * Groups are in accordance with IUPAC nomenclature. 61 Pm (145) ** Values in brackets are for the isotope with the longest half-life. Np (237) Sm Pu (244) 63 Eu Am (243) 64 Gd Cm (247) 65 Tb Bk (247) 66 Dy Cf (251) 67 Ho Es (252) 68 Er Fm (257) 69 Tm Md (258) 70 Yb No (259)

7 List of elements by name Name No. Symbol Name No. Symbol Name No. Symbol Name No. Symbol Hydrogen 1 H Selenium 34 Se Holmium 67 Ho Fermium 100 Fm Helium 2 He Bromine 35 Br Erbium 68 Er Mendelevium 101 Md Lithium 3 Li Krypton 36 Kr Thulium 69 Tm Nobelium 102 No Beryllium 4 Be Rubidium 37 Rb Ytterbium 70 Yb Lawrencium 103 Lr Boron 5 B Strontium 38 Sr Lutetium 71 Lu Rutherfordium 104 Rf Carbon 6 C Yttrium 39 Y Hafnium 72 Hf Dubnium 105 Db Nitrogen 7 N Zirconium 40 Zr Tantalum 73 Ta Seaborgium 106 Sg Oxygen 8 O Niobium 41 Nb Tungsten 74 W Bohrium 107 Bh Fluorine 9 F Molybdenum 42 Mo Rhenium 75 Re Hassium 108 Hs Neon 10 Ne Technetium 43 Tc Osmium 76 Os Meitnerium 109 Mt Sodium 11 Na Ruthenium 44 Ru Iridium 77 Ir Darmstadtium 110 Ds Magnesium 12 Mg Rhodium 45 Rh Platinum 78 Pt Roentgenium 111 Rg Aluminum 13 Al Palladium 46 Pd Gold 79 Au Silicon 14 Si Silver 47 Ag Mercury 80 Hg Phosphorus 15 P Cadmium 48 Cd Thallium 81 Tl Sulfur 16 S Indium 49 In Lead 82 Pb Chlorine 17 Cl Tin 50 Sn Bismuth 83 Bi Argon 18 Ar Antimony 51 Sb Polonium 84 Po Potassium 19 K Tellurium 52 Te Astatine 85 At Calcium 20 Ca Iodine 53 I Radon 86 Rn Scandium 21 Sc Xenon 54 Xe Francium 87 Fr Titanium 22 Ti Cesium 55 Cs Radium 88 Ra Vanadium 23 V Barium 56 Ba Actinium 89 Ac Chromium 24 Cr Lanthanum 57 La Thorium 90 Th Manganese 25 Mn Cerium 58 Ce Protactinium 91 Pa Iron 26 Fe Praseodymium 59 Pr Uranium 92 U Cobalt 27 Co Neodymium 60 Nd Neptunium 93 Np Nickel 28 Ni Promethium 61 Pm Plutonium 94 Pu Copper 29 Cu Samarium 62 Sm Americium 95 Am Zinc 30 Zn Europium 63 Eu Curium 96 Cm Gallium 31 Ga Gadolinium 64 Gd Berkelium 97 Bk Germanium 32 Ge Terbium 65 Tb Californium 98 Cf Arsenic 33 As Dysprosium 66 Dy Einsteinium 99 Es 2009 Chemistry Paper Two Resource book 5