6.022 x mol C mol J g 1 K 1. One litre (1.00 L) 1000 ml or 1000 cm L

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hemistry Subject ode: M315114 2014 External Examination Information Sheet hemical Data and onstants QUANTITY Standard atmospheric pressure Absolute zero temperature (zero kelvin) Standard temperature

1 hemistry Subject ode: M External Examination Information Sheet hemical Data and onstants QUANTITY Standard atmospheric pressure Absolute zero temperature (zero kelvin) Standard temperature & pressure (S.T.P.) Standard laboratory conditions (S.L..) Avogadro's constant (N A ) Ideal gas constant (R) Molar volume of an ideal gas (S.T.P.) Molar volume of an ideal gas (S.L..) harge on the electron Faraday s constant (F) Specific heat of water (c w ) Density of liquid water APPRXIMATE VALUE atm kpa mm g (273 K) and kpa 25 (298 K) and kpa x mol L atm K 1 mol J K 1 mol L kpa K 1 mol L mm g K 1 mol L mol L mol x mol J g 1 K g ml 1 ne litre (1.00 L) 1000 ml or 1000 cm 3 ne cubic metre (1.00 m 3 ) 1000 L Unit prefixes: nano (n) micro (µ) milli (m) kilo (k) mega (M) giga (G) tera (T) Page 1 of 10

2 hemical Information n = m M N = n N A n = amount of substance (mol) m = mass (g) M = molar mass (g mol 1 ) N = number of particles N A = Avogadro's constant (see p.1) n = cv c = concentration (mol L 1 ) V = volume of solution (L) P 1 V 1 T 1 = P 2V 2 T 2 ombined Gas Equation (n constant) PV = nrt n(e ) = q F = It F E = VIt V = gas volume P = gas pressure T = temperature (K) R = Ideal Gas onstant (see p.1) n(e ) = amount of electrons (mol) q = electrical charge () F = Faraday onstant (see p.1) E = energy change (J) V = potential difference (V) I = electrical current (A) t = time (s) E = mcδt c = specific heat capacity (J g 1 K 1 ) c f = E ΔT = VIt ΔT ΔT = temperature change (K) c f = calibration factor (J K 1 ) ρ = m V ρ = density (g ml 1 or g L 1 ) Page 2 of 10

3 MMN PSITIVE INS (ATINS) ammonium N 4 barium Ba 2+ aluminium Al 3+ tin (IV) Sn 4+ hydrogen + calcium a 2+ chromium (III) r 3+ lead (IV) Pb 4+ lithium Li + copper (II) u 2+ iron (III) Fe 3+ potassium K + iron (II) Fe 2+ silver Ag + lead (II) Pb 2+ sodium Na + mercury (II) g 2+ magnesium Mg 2+ nickel (II) Ni 2+ tin (II) Sn 2+ zinc Zn 2+ MMN NEGATIVE INS (ANINS) ethanoate (acetate) 3 2 carbonate 3 nitride N 3 bromide Br chromate r 4 2 dichromate r chloride l hydrogen phosphate P 4 2 dihydrogen phosphate 2 P 4 oxide 2 fluoride F 2 sulfate S 4 hydrogen carbonate 3 hydrogen sulfate S 4 sulfide S 2 sulfite S 3 2 hydrogen sulfide S thiosulfate S hydrogen sulfite S 3 hydroxide iodide I nitrate N 3 nitrite N 2 permanganate Mn 4 hydride Negative Ions (anions) ethanoates (acetates) ( 3 ) nitrates (N 3 ) oxalate phosphate P 4 3 phosphide P 3 SLUBILITY TABLE FR MMN INI MPUNDS All soluble All soluble chlorides (l ) All soluble except Agl, Pbl 2, gl 2 bromides (Br ) All soluble except AgBr, PbBr 2, gbr 2 iodides (I ) All soluble except AgI, PbI 2, gi 2 Solubility of ompounds sulfates (S 4 2 ) All soluble except BaS 4, as 4, SrS 4, PbS 4, Ag 2 S 4, SnS 4 hydroxides ( ) All insoluble except Li, Na, K, Rb, N 4,Sr() 2, Ba() 2 sulfides (S 2 ) All insoluble except Li 2 S, Na 2 S, K 2 S, Rb 2 S, (N 4 ) 2 S, MgS, as, SrS, BaS carbonates ( 2 3 ) All insoluble except Li 2 3, Na 2 3, K 2 3, Rb 2 3, (N 4 ) 2 3 phosphates (P 3 4 ) All insoluble except Li 3 P 4, Na 3 P 4, K 3 P 4, Rb 3 P 4, (N 4 ) 3 P 4 sulfites (S 2 3 ) All insoluble except Li 2 S 3, Na 2 S 3, K 2 S 3, Rb 2 S 3 (N 4 ) 2 S 3 Page 3 of 10

4 hemical Equilibrium Formulae For the equilibrium system: xp + yq zr + ws (where none of components P, Q, R or S is a solid) K c = R P [ ] z [ S] w [ ] x [ Q] y K w =! " + (aq) p = log! " + # (aq) $! " + # (aq) $ =10 p # $! " # (aq) $ = mol 2 L 2 at 25 ommon oloured Aqueous Ions LURED ATINS NTE:! " + # (aq) $ =! " 3 + # (aq) $ LURED ANINS chromium (III) r 3+ green chromate 2 r 4 yellow cobalt (II) o 2+ pink dichromate 2 r 2 7 orange copper (II) u 2+ blue permanganate Mn 4 purple iron (II) Fe 2+ pale green iron (III) Fe 3+ orange/brown (*most other non listed aqueous ions manganese (II) Mn 2+ pale pink are colourless in solution) nickel (II) Ni 2+ green rganic hemistry Alkanes: n 2n+2 Benzene 6 6 Alkenes: n 2n Alkynes: n 2n 2 yclic Alkanes: n 2n yclic Alkenes: n 2n 2 Stem Names arbon Atoms in hain Stem Name meth- eth- prop- but- pent- hex- hept- oct- non- dec- Side chains and substitutes methyl 3 bromo Br ethyl 2 5 chloro l propyl 3 7 fluoro F iodo I Prefixes Atoms in molecule Prefix mono- di- tri- tetra- penta- hexa- hepta- octa- nona- deca- Page 4 of 10

5 Functional Groups class of compound functional group general formula example of compound alcohols R n 2n+2 propan-1-ol aldehydes R n 2n ethanal carboxylic acids n 2n 2 R butanoic acid ketones R R ' n 2n pentan-3-one esters n 2n 2 R R ' alkyl halides R F n 2n+1 X R l R Br R l methyl propanoate l 1-chlorobutane Page 5 of 10

6 Some rganic Reactions of Aliphatic ompounds Alkyl halide RX (X is F, l, Br or I). Alkane X(g) Dilute. Na (aq) Alkoxide eg (R 2..Na + ) + ½ 2 2 Alkene Addition polymerisation (atalyst) Loss of 2 (use 2 S 4 (l)) + 2 (g) Primary R 2 Alcohol Active metal(eg Na) Secondary RR' [] Ketone RR' Polymer [] using mild oxidiser eg acidified dichromate [] with excess stronger oxidiser eg acidified permanganate onc 2 S 4 Ester RR' Aldehyde R ydrolysis (in presence of catalyst) [] Salt (eg R..Na + ) + 2 Salt (eg R..Na + + ½ 2 Salt (eg R..Na + ) base eg Na or active metal or carbonate arboxylic acid R arboxylic acid + alcohol R + R' Page 6 of 10

7 STANDARD REDUTIN PTENTIALS AQUEUS INS (1 mol/l and 25 ) VERY STRNG XIDISERS INREASING STRENGT AS XIDISERS VERY WEAK XIDISERS REDUTIN ALF EQUATINS VERY WEAK E (volts) REDUERS F 2 (g) + 2e 2F (aq) (aq) (aq) + 2e 2 2 (l) Au 3+ (aq) + 3e Au(s) Mn 4 (aq) (aq) + 5e Mn 2+ (aq) (l) l 2 (g) + 2e 2l (aq) r (aq) (aq) + 6e 2r 3+ (aq) (l) Mn 2 (s) (aq) + 2e Mn 2+ (aq) (l) (g) (aq) + 4e 2 2 (l) Br 2 (l) + 2e 2Br (aq) N 3 (aq) (aq) + 3e N(g) (l) Ag + (aq) + e Ag(s) g 2+ (aq) + 2e g(l) N 3 (aq) (aq) + e N 2 (g) + 2 (l) Fe 3+ (aq) + e Fe 2+ (aq) (g) (aq) + 2e 2 2 (aq) I 2 (s) + 2e 2I INREASING (aq) STRENGT 2 (g) (l) + 4e 4 (aq) AS REDUERS u 2+ (aq) + 2e u(s) S 2-4 (aq) (aq) + 2e S 2 (g) (l) Sn 4+ (aq) + 2e Sn 2+ (aq) S(s) (aq) + 2e 2 S(g) (aq) + 2e 2 (g) 0.00 Pb 2+ (aq) + 2e Pb(s) 0.13 Sn 2+ (aq) + 2e Sn(s) 0.14 Ni 2+ (aq) + 2e Ni(s) 0.25 o 2+ (aq) + 2e o(s) 0.28 d 2+ (aq) + 2e d(s) 0.40 Fe 2+ (aq) + 2e Fe(s) 0.41 r 3+ (aq) + 3e r(s) 0.74 Zn 2+ (aq) + 2e Zn(s) (l) + 2e 2 (aq) + 2 (g) 0.83 Mn 2+ (aq) + 2e Mn(s) 1.18 Al 3+ (aq) + 3e Al(s) 1.71 Mg 2+ (aq) + 2e Mg(s) 2.38 Na + (aq) + e Na(s) 2.71 a 2+ (aq) + 2e a(s) 2.87 Sr 2+ (aq) + 2e Sr(s) 2.89 VERY K + (aq) + e K(s) STRNG 2.92 Li + (aq) + e Li(s) REDUERS 3.05 XIDATIN ALF EQUATINS Page 7 of 10

8 Name TABLE F RELATIVE ATMI MASSES (BASED N 12 =12.00 ) Symbol Atomic Number Relative Atomic Mass Name Symbol Atomic Number Relative Atomic Mass actinium Ac mercury g aluminium Al molybdenum Mo americium Am 95 - neodymium Nd antimony Sb neon Ne argon Ar neptunium Np 93 - arsenic As nickel Ni astatine At 85 - niobium Nb barium Ba nitrogen N berkelium Bk 97 - nobelium No beryllium Be osmium s bismuth Bi oxygen boron B palladium Pd bromine Br phosphorus P cadmium d platinum Pt caesium s plutonium Pu 94 - calcium a polonium Po 84 - californium f 98 - potassium K carbon praseodymium Pr cerium e promethium Pm 61 - chlorine l protactinium Pa 91 - chromium r radium Ra cobalt o radon Rn 86 - copper u rhenium Re curium m 96 - rhodium Rh dysprosium Dy rubidium Rb einsteinium Es 99 - ruthenium Ru erbium Er samarium Sm europium Eu scandium Sc fermium Fm selenium Se fluorine F silicon Si francium Fr 87 - silver Ag gadolinium Gd sodium Na gallium Ga strontium Sr germanium Ge sulfur S gold Au tantalum Ta hafnium f technetium Tc 43 - helium e tellurium Te holmium o terbium Tb hydrogen thallium Tl indium In thorium Th iodine I thulium Tm iridium Ir tin Sn iron Fe titanium Ti krypton Kr tungsten W lanthanum La uranium U lawrencium Lr vanadium V lead Pb xenon Xe lithium Li ytterbium Yb lutetium Lu yttrium Y magnesium Mg zinc Zn manganese Mn zirconium Zr mendelevium Md Page 8 of 10

9 PERIDI TABLE F ELEMENTS Atomic number Name Relative atomic mass 5 B Boron Symbol I II III IV V VI VII VIII ydrogen 2 e elium Li Lithium 4 Be Beryllium 5 B Boron 6 arbon 7 N Nitrogen 8 xygen 9 F Fluorine 10 Ne Neon Na Sodium 12 Mg Magnesium 13 Al Aluminium 14 Si Silicon 15 P Phosphorus 16 S Sulfur 17 l hlorine 18 Ar Argon K Potassium 20 a alcium 21 Sc Scandium 22 Ti Titanium 23 V Vanadium 24 r hromium 25 Mn Manganese 26 Fe Iron 27 o obalt 28 Ni Nickel 29 u opper 30 Zn Zinc 31 Ga Gallium 32 Ge Germanium 33 As Arsenic 34 Se Selenium 35 Br Bromine 36 Kr Krypton Rb Rubidium 38 Sr Strontium 39 Y Yttrium 40 Zr Zirconium 41 Nb Niobium 42 Mo Molybdenum 43 Tc Technetium 44 Ru Ruthenium 45 Rh Rhodium 46 Pd Palladium 47 Ag Silver 48 d admium 49 In Indium 50 Sn Tin 51 Sb Antimony 52 Te Tellurium 53 I Iodine 54 Xe Xenon s aesium 56 Ba Barium 57 La Lanthanum 72 f afnium 73 Ta Tantalum 74 W Tungsten 75 Re Rhenium 76 s smium 77 Ir Iridium 78 Pt Platinum 79 Au Gold 80 g Mercury 81 Tl Thallium 82 Pb Lead 83 Bi Bismuth 84 Po Polonium 85 At Astatine 86 Rn Radon Fr Francium 88 Ra Radium 89 Ac Actinium 104 Rf 105 Db 106 Sg 107 Bh 108 s 109 Mt 110 Uun 111 Uun 112 Uub Lanthanide Series 58 e erium Pr Praseodymium Nd Neodymium Pm Promethium 62 Sm Samarium Eu Europium Gd Gadolinium Tb Terbium Dy Dysprosium o olmium Er Erbium Tm Thulium Yb Ytterbium Lu Lutetium Actinide Series 90 Th Thorium Pa Protactinium 92 U Uranium Np Neptunium 94 Pu Plutonium 95 Am Americium 96 m urium 97 Bk Berkelium 98 f alifornium 99 Es Einsteinium 100 Fm Fermium 101 Md Mendelevium 102 No Nobelium 103 Lr Lawrencium

10 General Periodic Trends Atomic radii decreases Nuclear charge increases ation size decreases Anion size decreases Atomic radii increases Nuclear charge increases Ionic size increases 1 3 Li 11 Na 19 K 37 Rb 55 s 4 Be 12 Mg 20 a 38 Sr 56 Ba 21 Sc 39 Y 57 La 22 Ti 40 Zr 72 f 23 V 41 Nb 73 Ta 24 r 42 Mo 74 W 25 Mn 43 Tc 75 Re 26 Fe 44 Ru 76 s 27 o 45 Rh 77 Ir 28 Ni 46 Pd 78 Pt 29 u 47 Ag 79 Au 30 Zn 48 d 80 g 5 B 13 Al 31 Ga 49 In 81 Tl 6 14 Si 32 Ge 50 Sn 82 Pb 7 N 15 P 33 As 51 Sb 83 Bi 8 16 S 34 Se 52 Te 84 Po 9 F 17 l 35 Br 53 I 85 At 2 e 10 Ne 18 Ar 36 Kr 54 Xe 86 Rn Shielding increases Ionisation energy decreases Electronegativity decreases 87 Fr 88 Ra Shielding is constant Ionisation energy increases Electronegativity increases

This resource contains three different versions of the periodic table, including a blank one for colouring!

Teaching notes This resource contains three different versions of the periodic table, including a blank one for colouring! It also contains tables of the Group 0, 1 and 7 elements with a few columns for