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GCE Advanced Level H2 Chemistry Syllabus: Tables of Chemical Data, Lecture notes of Engineering

Technische Universiteit DelftEngineering

The syllabus for the GCE Advanced Level Chemistry H2 course, focusing on tables of chemical data. It includes important values, constants, and standards, ionization energies, bond energies, standard electrode potentials, atomic and ionic radii, typical proton chemical shift values, and characteristic infra-red absorption frequencies for various bonds. Useful for students preparing for the Advanced Level Chemistry H2 exam.

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9729 CHEMISTRY GCE ADVANCED LEVEL H2 SYLLABUS
40
Data Booklet
for
Chemistry
(Advanced Level)
For use from 2017 in all papers, except practical
examinations, for the 9729 H2 Chemistry and H3
Chemistry syllabuses.
For use from 2018 in all papers, for the 8873 H1
Chemistry syllabuses.
Accelerate your learning at https://www.ALevelH2Chemistry.com for more H2 Chemistry notes, questions & videos
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Download GCE Advanced Level H2 Chemistry Syllabus: Tables of Chemical Data and more Lecture notes Engineering in PDF only on Docsity!

Data Booklet

for

Chemistry

(Advanced Level)

examinations, for the 9729 H2 Chemistry and H3^ For use from 2017 in all papers, except practical Chemistry syllabuses. For use from 2018 in all papers, for the 8873 H1Chemistry syllabuses.

Accelerate your learning at https://www.ALevelH2Chemistry.com for more H2 Chemistry notes, questions & videos

Contents: Tables of Chemical data

1 Important values, constants and standards 2 Ionisation energies (1st, 2nd, 3rd and 4th) of selected elements in kJ mol – 3 Bond energies 4 Standard electrode potential and redox potentials, E ⦵ at 298 K (25 °C) 5 Atomic and ionic radii 6 Typical proton ( 1 H) chemical shift values (δ) relative to TMS = 0 7 Characteristic infra-red absorption frequencies for some selected bonds 8 The orientating effect of groups in aromatic substitution reactions 9 Qualitative Analysis Notes 10 The Periodic Table of Elements

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Proton Number First Second Third Fourth

H 1 1310 – – – He 2 2370 5250 – –

Proton Number First Second Third Fourth Cu 29 745 1960 3350 5690 Zn 30 908 1730 3828 5980 Ga 31 577 1980 2960 6190 Ge 32 762 1540 3300 4390 Br 35 1140 2080 3460 4850 Rb 37 403 2632 3900 5080 Sr 38 548 1060 4120 5440 Ag 47 731 2074 3361 – Sn 50 707 1410 2940 3930 I 53 1010 1840 3200 4030 Cs 55 376 2420 3300 – Ba 56 502 966 3390 – Pb 82 716 1450 3080 4080

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3(b) Bond energies in polyatomic molecules (these are average values)

4 Standard electrode potential and redox potentials, E ⦵^ at 298 K (25 ° C)

For ease of reference, two tabulations are given:(a) an extended list in alphabetical order; (b) a shorter list in decreasing order of magnitude, i.e. a redox series. 4(a) E ⦵^ in alphabetical order

All ionic states refer to aqueous ions but other state symbols have been omitted.

4(b) E (a selection only – see also the extended alphabetical list on the previous pages)⦵ in decreasing order of oxidising power

5 Atomic and ionic radii

  • 2 Ionisation energies (1st, 2nd, 3rd and 4th) of selected elements, in kJ mol –
    • Be Li 3 519 7300 11800 –
    • B
    • C
    • N
    • O
    • F
    • Ne
    • Na
    • Mg
    • A l
    • Si
    • P
    • S
    • C l
    • Ar
    • K
    • Ca
    • Sc
    • Ti
    • V
    • Cr
    • Mn
    • Fe
    • Co
    • Ni
  • Bond Energy/kJ mol–1 Bond Energy/kJ mol– Homonuclear Heteronuclear
  • C―C 350 C―H
  • C=C 610 C―F
  • C≡C 840 C―C l
  • C C (benzene) 520 C―Br
  • N―N 160 C―I
  • N=N 410 C―N
  • O―O 150 C=N
  • Si―Si 222 C≡N
  • P―P 200 C―O
  • S―S 264 C=O
    • C=O in CO
    • N―H
    • N―C l
    • O―H
    • Si―C l
    • Si―H
    • Si―O (in SiO 2 (s))
    • Si=O (in SiO 2 (g))
    • P―H
    • P―C l
    • P―O
    • P=O
    • S―H
    • S―C l
    • S―O
    • S=O - Ag + + e – ⇌ Ag +0. Electrode reaction E ⦵ / V - A l 3+ + 3e – ⇌ A l –1. - Ba 2+ + 2e – ⇌ Ba –2. - Br 2 + 2e – ⇌ 2Br – +1. - Ca 2+ + 2e – ⇌ Ca –2. - C l 2 + 2e – ⇌ 2C l – +1.
    • 2HOC l + 2H + + 2e – ⇌ C l 2 + 2H 2 O +1. - C l O – + H 2 O + 2e – ⇌ C l – + 2OH – +0. - Co 2+ + 2e – ⇌ Co –0. - Co 3+ + e – ⇌ Co 2+ +1.
      • [Co(NH 3 ) 6 ]2+ + 2e – ⇌ Co + 6NH 3 –0. - Cr 2+ + 2e – ⇌ Cr –0. - Cr 3+ + 3e – ⇌ Cr –0. - Cr 3+ + e – ⇌ Cr 2+ –0.
  • Cr 2 O 7 2– + 14H + + 6e – ⇌ 2Cr 3+ + 7H 2 O +1. - Cu + + e – ⇌ Cu +0. - Cu 2+ + 2e – ⇌ Cu +0. - Cu 2+ + e – ⇌ Cu + +0. - [Cu(NH 3 ) 4 ]2+ + 2e – ⇌ Cu + 4NH 3 –0. - F 2 + 2e – ⇌ 2F– +2. - Fe 2+ + 2e – ⇌ Fe –0. - Fe 3+ + 3e – ⇌ Fe –0. - Fe 3+ + e – ⇌ Fe2+ +0. Electrode reaction E ⦵ / V - [Fe(CN) 6 ]3– + e – ⇌ [Fe(CN) 6 ]4– +0. - Fe(OH) 3 + e – ⇌ Fe(OH) 2 + OH – –0. - 2H + + 2e – ⇌ H 2 0. - I 2 + 2e – ⇌^2 I– +0. - K+ + e – ⇌ K –2. - Li+ + e – ⇌ Li –3. - Mg 2+ + 2e – ⇌ Mg –2. - Mn 2+ + 2e – ⇌ Mn –1. - Mn 3+ + e – ⇌ Mn 2+ +1. - MnO 2 + 4H + + 2e – ⇌ Mn 2+ + 2H 2 O +1. - MnO 4 – + e – ⇌ MnO 4 2– +0.
  • MnO 4 – + 4H + + 3e – ⇌ MnO 2 + 2H 2 O +1.
  • MnO 4 – + 8H + + 5e – ⇌ Mn 2+ + 4H 2 O +1. - NO 3 – + 2H + + e – ⇌ NO 2 + H 2 O +0. - NO 3 – + 3H + + 2e – ⇌ HNO 2 + H 2 O +0.
    • NO 3 – + 10H + + 8e – ⇌ NH 4 + + 3H 2 O +0. - Na + + e – ⇌ Na –2. - Ni2+ + 2e – ⇌ Ni –0. - [Ni(NH 3 ) 6 ]2+ + 2e – ⇌ Ni + 6NH 3 –0. - H 2 O 2 + 2H + + 2e – ⇌ 2H 2 O +1. - HO 2 – + H 2 O + 2e – ⇌ 3OH – +0. - O 2 + 4H + + 4e – ⇌ 2H 2 O +1. - O 2 + 2H 2 O + 4e – ⇌ 4OH – +0. - O 2 + 2H + + 2e – ⇌ H 2 O 2 +0. - O 2 + H 2 O + 2e – ⇌ HO 2 – + OH – –0. Electrode reaction E ⦵ / V - 2H 2 O + 2e – ⇌ H 2 + 2OH – –0. - Pb 2+ + 2e – ⇌ Pb –0. - Pb 4+ + 2e – ⇌ Pb 2+ +1.
    • PbO 2 + 4H + + 2e – ⇌ Pb 2+ + 2H 2 O +1.
  • SO 4 2– + 4H + + 2e – ⇌ SO 2 + 2H 2 O +0. - S 2 O 8 2– + 2e – ⇌ 2SO 4 2– +2. - S 4 O 6 2– + 2e – ⇌ 2S 2 O 3 2– +0. - Sn 2+ + 2e – ⇌ Sn –0. - Sn 4+ + 2e – ⇌ Sn 2+ +0. - V2+ + 2e – ⇌ V –1. - V3+ + e – ⇌ V2+ –0. - VO 2+ + 2H + + e – ⇌ V3+ + H 2 O +0. - VO 2 + + 2H + + e – ⇌ VO2+ + H 2 O +1. - VO 3 – + 4H + + e – ⇌ VO2+ + 2H 2 O +1. - Zn 2+ + 2e – ⇌ Zn –0. - F 2 + 2e – ⇌ 2F – +2. Electrode reaction E ⦵ / V - S 2 O 8 2– + 2e – ⇌ 2SO 4 2– +2. - H 2 O 2 + 2H + + 2e – ⇌ 2H 2 O +1.
    • MnO 4 – + 8H + + 5e – ⇌ Mn 2+ + 4H 2 O +1. - PbO 2 + 4H + + 2e – ⇌ Pb 2+ + 2H 2 O +1. - C l 2 + 2e – ⇌ 2C l – +1.
  • Cr 2 O 7 2– + 14H + + 6e – ⇌ 2Cr 3+ + 7H 2 O +1. - O 2 + 4H + + 4e – ⇌ 2H 2 O +1. - Br 2 + 2e – ⇌ 2Br – +1. - NO 3 – + 10H + + 8e – ⇌ NH 4 + + 3H 2 O +0. - C l O – + H 2 O + 2e – ⇌ C l – + 2OH – +0. - NO 3 – + 2H + + e – ⇌ NO 2 + H 2 O +0. - Ag + + e – ⇌ Ag +0. - Fe 3+ + e – ⇌ Fe 2+ +0. - I 2 + 2e – ⇌^2 I– +0. - O 2 + 2H 2 O + 4e – ⇌ 4OH – +0. - Cu 2+ + 2e – ⇌ Cu +0. - SO 4 2– + 4H + + 2e – ⇌ SO 2 + 2H 2 O +0. - Sn 4+ + 2e – ⇌ Sn 2+ +0. - S 4 O 6 2– + 2e – ⇌ 2S 2 O 3 2– +0. - 2H + + 2e – ⇌ H 2 0. - Pb 2+ + 2e – ⇌ Pb –0. - Sn 2+ + 2e – ⇌ Sn –0. - Fe 2+ + 2e – ⇌ Fe –0.
    • single covalent H 0.037 H – 0. (a) Period 1 atomic/nm ionic/nm
    • van der Waals He 0.
  • (b) Period
    • metallic Li 0.152 Li+ 0.
      • Be 0.112 Be 2+ 0.
    • single covalent B 0.080 B 3+ 0.
      • C 0.077 C 4+ 0.015 C 4– 0.
      • N 0.074 N 3– 0.
      • O 0.073 O2– 0.
      • F 0.072 F– 0.
    • van der Waals Ne 0.
  • (c) Period
    • metallic Na 0.186 Na+ 0.
      • Mg 0.160 Mg 2+ 0.
      • A l 0.143 A l 3+ 0.
    • single covalent Si 0.117 Si 4+ 0.
      • P 0.110 P3– 0.
      • S 0.104 S2– 0.
      • C l 0.099 C l – 0.
    • van der Waals Ar 0.
  • (d) Group
    • metallic Be 0.112 Be 2+ 0.
      • Mg 0.160 Mg 2+ 0.
      • Ca 0.197 Ca2+ 0.
      • Sr 0.215 Sr 2+ 0.
      • Ba 0.217 Ba 2+ 0.
      • Ra 0.220 Ra2+ 0.
    • single covalent C 0. (e) Group 14 atomic/nm ionic/nm
      • Si 0.117 Si4+ 0.
      • Ge 0.122 Ge2+ 0.
    • metallic Sn 0.162 Sn 2+ 0.
      • Pb 0.175 Pb 2+ 0.
  • (f) Group
    • single covalent F 0.072 F – 0.
      • C l 0.099 C l – 0.
      • Br 0.114 Br – 0.
      • I 0.133 I– 0.
      • At 0.
    • metallic Sc 0.164 Sc 3+ 0. (g) First row d block elements
      • Ti 0.146 Ti2+ 0.086 Ti3+ 0.
      • V 0.135 V2+ 0.079 V3+ 0.
      • Cr 0.129 Cr 2+ 0.073 Cr 3+ 0.
      • Mn 0.132 Mn 2+ 0.083 Mn 3+ 0.
      • Fe 0.126 Fe 2+ 0.061 Fe 3+ 0.
      • Co 0.125 Co2+ 0.065 Co3+ 0.
      • Ni 0.124 Ni2+ 0.069 Ni3+ 0.
      • Cu 0.128 Cu2+ 0.
      • Zn 0.135 Zn 2+ 0.
7 Characteristic infra-red absorption frequencies for some selected bonds
Bond Functional groups containingthe bond wavenumbers) / cmAbsorption range (in –1 Appearance of peak(s = strong,
w = weak)

C―C l chloroalkanes 700–800 s C―O alcoholether estercarboxylic acids 1000–1310970– 1050–13301210–

ss ss C=C aromaticalkenes 1475–16251635–1690 w^ s C=O amidesketones and aldehydes carboxylic acidsesters

1640–16901670– 1680–17301710–

ss ss C≡C alkynes 2150–2250 w unless conjugated C≡N nitriles 2200–2250 w C―H alkanes, CHalkenes/arenes, 2 ―H =C―H 2850–29503000–3100 w s N―H amines, amides 3300–3500 w O―H carboxylic acid, RCOH-bonded alcohol/phenol, RO 2 ―H ―H free alcohol, RO―H

2500–30003200– 3580–

s and very broad s s and sharp

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8 The orientating effect of groups in aromatic substitution reactions

The position of the incoming group,and not by the nature of the incoming group E , is determined by the nature of the group, E. G , already bonded to the ring,

G

― ―alkylOH or ―OR ― ―NHNHCOR 2 , ―NHR or ―NR 2 ―C l ,^ ―Br,^ ―I

― ―CHO,CO 2 H, ― ―CORCO 2 R ― ―NHNO 32 +, ―CN Reactivity of ring(compared to benzene)^ Activated^ Deactivated^ Deactivated (relative to position^ Position of E of G)^ 2- and/or 4-^ 2- and/or 4-^ 3-

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9(b) Reactions of anions

anion reaction carbonate,CO 3 2– CO 2 liberated by dilute acids chloride,C l – (aq) gives white ppt. with Ag +(aq) (soluble in NH 3 (aq)) bromide,Br – (aq) gives pale cream ppt. with Ag +(aq) (partially soluble in NH 3 (aq)) iodide, I–(aq) gives yellow ppt. with Ag +(aq) (insoluble in NH 3 (aq)) nitrate,NO 3 – (^) (aq) NH 3 liberated on heating with OH – (aq) and A l foil

nitrite,NO 2 – (^) (aq) NHNO liberated by dilute acids^3 liberated on heating with OH^ – (aq) and A l^ foil; (colourless NO → (pale) brown NO 2 in air) sulfate,SO 4 2– (^) (aq) gives white ppt. with Ba 2+(aq) (insoluble in excess dilute strong acids) sulfite,SO 3 2– (^) (aq) SOgives white ppt. with Ba 2 liberated with dilute acids; 2+(aq) (soluble in dilute strong acids)

9(c) Tests for gases

gas test and test result ammonia, NH 3 turns damp red litmus paper blue carbon dioxide, CO 2 gives a white ppt. with limewater(ppt. dissolves with excess CO 2 ) chlorine, C l 2 bleaches damp litmus paper hydrogen, H 2 “pops” with a lighted splint oxygen, O 2 relights a glowing splint sulfur dioxide, SO 2 turns aqueous acidified potassium manganate(colourless VII) from purple to

9(d) Colour of halogens

halogen colour of element colour in aqueous solution colour in hexane chlorine, C l 2 greenish yellow gas pale yellow pale yellow bromine, Br 2 reddish brown gas / liquid orange orange-red iodine, I 2 black solid / purple gas^ brown^ purple

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9729 CHEMISTRY GCE ADVANCED LEVEL H2 SYLLABUS

59

The Periodic Table of Elements

Group

1

2

13

14

15

16

17

18

Key

(^1) Hhydrogen1.

(^2) Hehelium4.

(^3) Lilithium6.

(^4) Beberyllium9.

atomic numberatomic symbol

name relative atomic mass

(^5) Bboron10.

(^6) Ccarbon12.

(^7) Nnitrogen14.

(^8) Ooxygen16.

(^9) Ffluorine19.

(^10) Neneon20.

(^11) Nasodium23.

(^12) Mgmagnesium24.^

3

4

5

6

7

8

9

10

11

12

13 A l aluminium27.

14 Sisilicon28.

15 Pphosphorus31.

16 Ssulfur32.

17 C l chlorine35.

18 Arargon39.

19 Kpotassium39.

(^20) Cacalcium40.

21 Scscandium45.

22 Tititanium47.

23 Vvanadium50.

(^24) Crchromium52.

(^25) Mnmanganese54.

(^26) Feiron55.

(^27) Cocobalt58.

28 Ninickel58.

(^29) Cucopper63.

(^30) Znzinc65.

(^31) Gagallium69.

(^32) Gegermanium72.

(^33) Asarsenic74.

(^34) Seselenium79.

35 Brbromine79.

36 Krkrypton83.

(^37) Rbrubidium85.

38 Srstrontium87.

39 Yyttrium88.

40 Zrzirconium91.

(^41) Nbniobium92.

(^42) Mo molybdenum95.

43 Tctechnetium–

(^44) Ruruthenium101.

(^45) Rhrhodium102.

(^46) Pdpalladium106.

(^47) Agsilver107.

(^48) Cdcadmium112.

49 Inindium114.

(^50) Sntin118.

(^51) Sbantimony121.

(^52) Tetellurium127.

53 I iodine126.

(^54) Xexenon131.

(^55) Cscaesium132.

(^56) Babarium137.

57–71lanthanoids

72 Hfhafnium178.

(^73) Tatantalum180.

74 Wtungsten183.

(^75) Rerhenium186.

(^76) Ososmium190.

77 Ir iridium192.

78 Ptplatinum195.

(^79) Augold197.

(^80) Hgmercury200.

81 T l thallium204.

(^82) Pblead207.

83 Bibismuth209.

(^84) Popolonium–

85 Atastatine–

(^86) Rnradon–

87 Frfrancium–

(^88) Raradium–

89–103actinoids

104 Rf rutherfordium

105 Dbdubnium–

106 Sgseaborgium–

107 Bhbohrium–

108 Hshassium–

109 Mtmeitnerium–

110 Ds darmstadtium

111 Rgroentgenium–

112 Cncopernicium–

114 F l flerovium–

116 Lvlivermorium–

lanthanoids

57 Lalanthanum138.

(^58) Cecerium140.

59 Pr praseodymium140.

(^60) Nd neodymium144.

(^61) Pmpromethium–

(^62) Smsamarium150.

(^63) Eueuropium152.

(^64) Gdgadolinium157.

(^65) Tbterbium158.

(^66) Dydysprosium162.

(^67) Hoholmium164.

68 Ererbium167.

(^69) Tmthulium168.

(^70) Ybytterbium173.

71 Lulutetium175.

actinoids

89 Acactinium–

(^90) Ththorium232.

(^91) Pa protactinium231.

92 Uuranium238.

(^93) Npneptunium–

(^94) Puplutonium–

(^95) Amamericium–

(^96) Cmcurium–

(^97) Bkberkelium–

98 Cfcalifornium–

(^99) Eseinsteinium–

100 Fmfermium–

101 Mdmendelevium–

102 Nonobelium–

103 Lrlawrencium–

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