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Cambridge Pre-U Chemistry Revised Syllabus: Tables of Chemical Data, Study Guides, Projects, Research of Chemistry

University of Canberra (UC)Chemistry

A revised syllabus for the Cambridge Pre-U Advanced Subsidiary and Advanced Level Chemistry course, focusing on tables of chemical data. It includes important values, constants, and standards, ionisation energies, bond energies, standard electrode potentials, atomic and ionic radii, typical proton and carbon chemical shift values, and characteristic infra-red absorption frequencies for some selected bonds.

Typology: Study Guides, Projects, Research

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Cambridge Pre-U Revised Syllabus
Cambridge International Advanced Subsidiary and Advanced Level
in Chemistry (9701)
For use from 2016 in all papers for the above
syllabus, except practical examinations.
CSTxxx
**
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Partial preview of the text

Download Cambridge Pre-U Chemistry Revised Syllabus: Tables of Chemical Data and more Study Guides, Projects, Research Chemistry in PDF only on Docsity!

Cambridge International Advanced Subsidiary and Advanced Level

in Chemistry (9701)

For use from 2016 in all papers for the above

syllabus, except practical examinations.

CSTxxx

Contents: Tables of Chemical Data

Proton

number First Second Third Fourth H 1 1310 – – –

He 2 2370 5250 – –

Cs 55 376 2420 3300 –

3 Bond Energies

3(a) Bond energies in diatomic molecules (these are exact values)

4 Standard electrode potential and redox potentials, E at 298 K (25 oC)

For ease of reference, two tables are given:

(a) an extended list in alphabetical order; (b) a shorter list in decreasing order of magnitude, i.e. a redox series.

(a) E in alphabetical order

5 Atomic and ionic radii

(g) First row transition elements

  • 1 Important values, constants and standards Page no.
  • 2 Ionisation energies (1st, 2nd, 3rd and 4th) of selected elements in kJ mol–1
  • 3 Bond energies
  • 4 Standard electrode potential and redox potentials, E at 298K (25 °C)
  • 5 Atomic and ionic radii
  • 6 Typical proton (^1 H) chemical shift values (δ) relative to TMS =
  • 7 Typical carbon (^13 C) chemical shift values (δ) relative to TMS =
  • 8 Characteristic infra-red absorption frequencies for some selected bonds
  • 9 The orientating effect of groups in aromatic substitution reactions
  • 10 Names, structures and abbreviations of some amino acids
  • 11 The Periodic Table of Elements
  • 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
  • Al
  • Si
  • P
  • S
  • Cl
  • Ar
  • K
  • Ca
  • Sc
  • Ti
  • V
  • Cr
  • Mn
  • Fe
  • Co
  • Ni
  • Cu
  • Zn
  • Ga
  • Br
  • Rb
  • Sr
  • I Ag 47 731 2074 3361 –
  • Bond Energy / kJ mol–^1 Bond Energy / kJ mol– Homonuclear Heteronuclear
  • HH 436 HF
  • DD 442 HCl
  • N≡N 944 HBr
  • O=O 496 HI
  • P≡P 485 C≡O
  • S=S
  • FF
  • Cl Cl
  • BrBr
  • II
  • Bond Energy / kJ mol–^1 Bond Energy / kJ mol– Homonuclear Heteronuclear
  • CC 350 CH
  • C=C 610 CCl
  • C≡C 840 CBr
  • C….C (benzene) 520 CI
  • NN 160 CN
  • N=N 410 C=N
  • OO 150 C≡N
  • SiSi 222 CO
  • PP 200 C=O
  • SS 264 C=O in CO
  • NH
  • NCl
  • OH
  • SiCl
  • SiH
  • SiO (in SiO 2 (s))
  • Si=O (in SiO 2 (g))
  • PH
  • PCl
  • PO
  • P=O
  • SH
  • SCl
  • SO
  • S=O
  • Ag+ + e– Ag +0. Electrode reaction E / V
  • Al 3+ + 3e– Al –1.
  • Ba2+ + 2e– Ba –2.
  • Br 2 + 2e– 2Br– +1.
  • Ca2+ + 2e– Ca –2.
  • Cl 2 + 2e– 2Cl – +1.
  • 2HOCl + 2H+ + 2e– Cl 2 + 2H 2 O +1.
  • Cl O– + H 2 O + 2e– Cl – + 2OH– +0.
  • Co2+ + 2e– Co –0.
  • Co3+ + e– Co2+ +1.
  • [Co(NH 3 ) 6 ]2+ + 2e– Co + 6NH 3 –0.
  • Cr2+ + 2e– Cr –0.
  • Cr3+ + 3e– Cr –0.
  • Cr3+ + e– Cr2+ –0.
  • Cr 2 O 7 2– + 14H+ + 6e– 2Cr3+ + 7H 2 O +1.
  • Cu+ + e– Cu +0.
  • Cu2+ + 2e– Cu +0.
  • Cu2+ + e– Cu+ +0.
  • [Cu(NH 3 ) 4 ]2+ + 2e– Cu + 4NH 3 –0.
  • F 2 + 2e– 2F– +2.
  • Fe2+ + 2e– Fe –0.
  • Fe3+ + 3e– Fe –0.
  • Fe3+ + e– Fe2+ +0.
  • [Fe(CN) 6 ]3– + e– [Fe(CN) 6 ]4– +0.
  • Fe(OH) 3 + e– Fe(OH) 2 + OH– –0.
  • 2H+ + 2e– H 2 0.
  • 2H 2 O + 2e– H 2 + 2OH– –0.
  • I 2 + 2e–^2 I– +0.
  • K+ + e– K –2.
  • Li+ + e– Li –3.
  • Mg2+ + 2e– Mg –2.
  • Mn2+ + 2e– Mn –1.
  • Mn3+ + e– Mn2+ +1.
  • MnO 2 + 4H+ + 2e– Mn2+ + 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– Mn2+ + 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. Electrode reaction E / V
  • 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.
  • Pb2+ + 2e– Pb –0.
  • Pb4+ + 2e– Pb2+ +1.
  • PbO 2 + 4H+ + 2e– Pb2+ + 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.
  • Sn2+ + 2e– Sn –0.
  • Sn4+ + 2e– Sn2+ +0.
  • V2+ + 2e– V –1.
  • V3+ + e– V2+ –0.
  • VO2+ + 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.
  • Zn2+ + 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– Mn2+ + 4H 2 O +1.
  • PbO 2 + 4H+ + 2e– Pb2+ + 2H 2 O +1.
  • Cl 2 + 2e– 2Cl – +1.
  • Cr 2 O 7 2– + 14H+ + 6e– 2Cr3+ + 7H 2 O +1.
  • O 2 + 4H+ + 4e– 2H 2 O +1.
  • Br 2 + 2e– 2Br– +1.
  • ClO – + H 2 O + 2e– Cl – + 2OH– +0.
  • NO 3 – + 10H+ + 8e– NH 4 + + 3H 2 O +0.
  • NO 3 – + 2H+ + e– NO 2 + H 2 O +0.
  • Ag+ + e– Ag +0.
  • Fe3+ + e– Fe2+ +0.
  • I 2 + 2e–^2 I– +0.
  • O 2 + 2H 2 O + 4e– 4OH– +0.
  • Cu2+ + 2e– Cu +0.
  • SO 4 2– + 4H+ + 2e– SO 2 + 2H 2 O +0.
  • Sn4+ + 2e– Sn2+ +0.
  • S 4 O 6 2–+ 2e– 2S 2 O 3 2– +0.
  • 2H+ + 2e– H 2 0.
  • Pb2+ + 2e– Pb –0.
  • Sn2+ + 2e– Sn –0.
  • Fe2+ + 2e– Fe –0.
  • Zn2+ + 2e– Zn –0.
  • 2H 2 O + 2e– H 2 + 2OH– –0.
  • V2+ + 2e– V –1.
  • Mg2+ + 2e– Mg –2.
  • Ca2+ + 2e– Ca –2.
  • K+ + e– K –2.
  • single covalent H 0.037 H– 0. (a) Period 1 atomic / nm ionic / nm
  • van der Waals He 0.
  • metallic Li 0.152 Li+ 0. (b) Period 2 atomic / nm ionic / nm
  • Be 0.112 Be2+ 0.
  • single covalent B 0.080 B3+ 0.
  • C 0.077 C4+ 0.015 C4– 0.
  • N 0.074 N3– 0.
  • O 0.073 O2– 0.
  • F 0.072 F– 0.
  • van der Waals Ne 0.
  • metallic Na 0.186 Na+ 0. (c) Period 3 atomic / nm ionic / nm
  • Mg 0.160 Mg2+ 0.
  • Al 0.143 Al 3+ 0.
  • single covalent Si 0.117 Si4+ 0.
  • P 0.110 P3– 0.
  • S 0.104 S2– 0.
  • Cl 0.099 Cl – 0.
  • van der Waals Ar 0.
  • metallic Be 0.112 Be2+ 0. (d) Group 2 atomic / nm ionic / nm
  • Mg 0.160 Mg2+ 0.
  • Ca 0.197 Ca2+ 0.
  • Sr 0.215 Sr2+ 0.
  • Ba 0.217 Ba2+ 0.
  • Ra 0.220 Ra2+ 0.
  • single covalent C 0.077 C4+ 0. (e) Group 14 atomic / nm ionic / nm
  • Si 0.117 Si4+ 0.
  • Ge 0.122 Ge2+ 0.
  • metallic Sn 0.162 Sn2+ 0.
  • Pb 0.175 Pb2+ 0.
  • single covalent F 0.072 F– 0. (f) Group 17 atomic / nm ionic / nm
  • Cl 0.099 Cl – 0.
  • Br 0.114 Br– 0.
  • I 0.133 I– 0.
  • At 0.
  • metallic Sc 0.164 Sc3+ 0. atomic / nm ionic / nm
  • Ti 0.146 Ti2+ 0.090 Ti3+ 0.
  • V 0.135 V2+ 0.079 V3+ 0.
  • Cr 0.129 Cr2+ 0.073 Cr3+ 0.
  • Mn 0.132 Mn2+ 0.067 Mn3+ 0.
  • Fe 0.126 Fe2+ 0.061 Fe3+ 0.
  • Co 0.125 Co2+ 0.078 Co2+ 0.
  • Ni 0.124 Ni2+ 0.070 Ni3+ 0.
  • Cu 0.128 Cu2+ 0.
  • Zn 0.135 Zn2+ 0.

7 Typical carbon (^13 C) chemical shift values (δ) relative to TMS = 0

hybridisation of the carbon atom

environment of carbon atom

example structures chemical shift range (δ)

sp^3 alkyl CH 3 –, –CH 2 –, –CH< 0–

sp^3 next to alkene/arene

  • CH 2 –C=C,

sp^3 next to carbonyl/carboxyl – CH 2 –COR, –CH 2 –CO 2 R 25–

sp^3 next to nitrogen – CH 2 –NH 2 , –CH 2 –NR 2 ,

  • CH 2 –NHCO

sp^3

next to chlorine (-CH 2 -Br and -CH 2 - I are in the same range as alkyl)

  • CH 2 –Cl 30–

sp^3 next to oxygen – CH 2 –OH, –CH 2 –O–CO– 50–

sp^2 alkene or arene

C=C<,

sp^2 carboxyl R–CO 2 H, R–CO 2 R 160–

sp^2 carbonyl R–CHO, R–CO–R 190–

sp alkyne (^) R–C≡C– 65–

sp nitrile (^) R–C≡N 100–

C H 2
C C
C
C C
C

8 Characteristic infra-red absorption frequencies for some selected bonds

bond functional groups containing the bond

absorption range (in wavenumbers) /cm–

appearance of peak (s = strong, w = weak)

C–O alcohols, ethers, esters 1040–1300 s

C=C aromatic compounds,alkenes 1500–1680 w unless conjugated

C=O

amides, ketones and aldehydes esters,

s s s

C≡C alkynes 2150–2250 w unless conjugated

C≡N nitriles 2200–2250 w

C–H alkanes, CH^2 –H alkenes/arenes, =C–H

s w

N–H amines, amides 3300–3500 w

O–H

carboxylic acids, RCO 2 –H H–bonded alcohol, RO–H free alcohol, RO–H

s and very broad s s and sharp

10 Names, structures and abbreviations of some amino acids

name 3-letter abbreviation 1-letter symbol

structure of side chain R- in

R CH

NH 2

CO 2 H

alanine Ala A CH 3 –

aspartic acid Asp D HO 2 CCH 2 –

cysteine Cys C HSCH 2 –

glutamic acid Glu E HO 2 CCH 2 CH 2 –

glycine Gly G H–

lysine Lys K H 2 NCH 2 CH 2 CH 2 CH 2 –

phenylalanine Phe F CH 2

serine Ser S HOCH 2 –

tyrosine Tyr Y HO CH 2

valine Val V

CH 3

CH

CH 3

The Periodic Table of Elements

Group

Key

1 H

hydrogen

2 He

helium^ 4.

3 Li

lithium^ 6.

4 Be

beryllium

atomic number

atomic symbol

name

relative atomic mass

5 B boron 10.

6 C

carbon^ 12.

7 N

nitrogen^ 14.

8 O

oxygen^ 16.

9 F

fluorine^ 19.

10 Ne neon 20.

11 Na sodium 23.

12 Mg

magnesium

13 A

l

aluminium

14 Si silicon 28.

15 P

phosphorus

16 S sulfur 32.

17 C

l

chlorine^ 35.

18 Ar argon 39.

19 K

potassium

20 Ca

calcium^ 40.

21 Sc

scandium^ 45.

22 Ti

titanium^ 47.

23 V

vanadium^ 50.

24 Cr

chromium^ 52.

25 Mn

manganese

26 Fe iron 55.

27 Co cobalt 58.

28 Ni nickel 58.

29 Cu copper 63.

30 Zn zinc 65.

31 Ga gallium 69.

32 Ge

germanium

33 As arsenic 74.

34 Se

selenium^ 79.

35 Br

bromine^ 79.

36 Kr

krypton^ 83.

37 Rb

rubidium^ 85.

38 Sr

strontium^ 87.

39 Y yttrium 88.

40 Zr

zirconium^ 91.

41 Nb

niobium^ 92.

42 Mo

molybdenum

43 Tc

technetium

44 Ru

ruthenium^ 101.

45 Rh

rhodium^ 102.

46 Pd

palladium^ 106.

47 Ag silver

48 Cd

cadmium^ 112.

49 In indium 114.

50 Sn^ tin

51 Sb

antimony^ 121.

52 Te

tellurium^ 127.

53 I iodine 126.

54 Xe xenon

55 Cs

caesium^ 132.

56 Ba barium 137.

57–71 lanthanoids

72 Hf

hafnium^ 178.

73 Ta

tantalum^ 180.

74 W

tungsten^ 183.

75 Re

rhenium^ 186.

76 Os

osmium^ 190.

77 Ir iridium 192.

78 Pt

platinum^ 195.

79 Au gold

80 Hg

mercury^ 200.

81 T

l

thallium^ 204.

82 Pb lead

83 Bi

bismuth^ 209.

84 Po

polonium

85 At

astatine

86 Rn radon^ –

87 Fr

francium

88 Ra radium^ –

89–103^ actinoids

104 Rf

rutherfordium

105 Db dubnium^ –

106 Sg

seaborgium

107 Bh bohrium^ –

108 Hs hassium^ –

109 Mt

meitnerium

110 Ds

darmstadtium

111 Rg

roentgenium

112 Cr

copernicium

114 F

l

flerovium

116 Lv

livermorium

lanthanoids

57 La

lanthanum^ 138.

58 Ce cerium 140.

59 Pr

praseodymium

60 Nd

neodymium

61 Pm

promethium

62 Sm

samarium^ 150.

63 Eu

europium^ 152.

64 Gd

gadolinium^ 157.

65 Tb

terbium^ 158.

66 Dy

dysprosium

67 Ho

holmium^ 164.

68 Er erbium 167.

69 Tm

thulium 168.

70 Yb

ytterbium^ 173.

71 Lu

lutetium^ 175.

actinoids

89 Ac

actinium

90 Th thorium 232.

91 Pa

protactinium

92 U

uranium^ 238.

93 Np

neptunium

94 Pu

plutonium

95 Am

americium

96 Cm curium^ –

97 Bk

berkelium

98 Cf

californium

99 Es

einsteinium

100 Fm fermium^ –

101 Md

mendelevium

102 No

nobelium

103 Lr

lawrencium

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