Chemistry data booklet

Lattice enthalpies at 298 K experimental and theoretical values 10 15.. Structural formulas of some food chemistry molecules 22 Notes This booklet cannot be used for paper 1 of the exami

Chemistry data booklet

First examinations 2009

4019a Printed in the United Kingdom by Antony Rowe Ltd, Chippenham, Wiltshire

First published March 2007 Revised edition published September 2008 International Baccalaureate Peterson House, Malthouse Avenue, Cardiff Gate

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1 Some relevant equations 1

2 Physical constants and unit conversions 1

6 Melting points and boiling points of the elements 4

7 First ionization energy, electron affinity and electronegativity of the 5 elements

8 Atomic and ionic radii of the elements 6

10 Bond enthalpies and average bond enthalpies at 298 K 7

11 Organic compounds—thermodynamic data 8

13 Lattice enthalpies at 298 K (experimental and theoretical values) 10

15 Strengths of organic acids and bases 13

20 Structural formulas of some medicines and drugs 19

21 Structural formulas of some biological molecules 21

22 Structural formulas of some food chemistry molecules 22

Notes

This booklet cannot be used for paper 1 of the examination (SLP1 and HLP1), but the periodic table given on page 3 will be available as part of these examination papers Clean copies of this booklet must be made available to candidates for papers 2 and 3 (SLP2, SLP3, HLP2 and HLP3).

1 Some relevant equations

0 10

2 Physical constants and unit conversions

Avogadro’s constant (L) = 6.02 × 1023 mol–1

Gas constant (R) = 8.31 J K–1 mol–1

Molar volume of an ideal gas at 273 K and 1.01 × 105 Pa = 2.24 × 10–2 m3 mol–1 (= 22.4 dm3 mol–1)

Planck’s constant (h) = 6.63 × 10–34 J s

Specific heat capacity of water = 4.18 kJ kg–1 K–1 (= 4.18 J g–1 K–1)

Ionic product constant for water (Kw) = 1.00 × 10–14 at 298 K

V I B G Y O R wavelength / nm700400

4 Names of the elements

number Element Symbol number Atomic

89 13 95 51 18 33 85 56 97 4 83 107 5 35 48 55 20 98 6 58 17 24 27 29 96 105 66 99 68 63 100 9 87 64 31 32 79 72 108 2 67 1 49 53 77 26 36 57 103 82 3 71 12 25 109

mendelevium mercury molybdenum neodymium neon neptunium nickel niobium nitrogen nobelium osmium oxygen palladium phosphorus platinum plutonium polonium potassium praseodymium promethium protactinium radium radon rhenium rhodium rubidium ruthenium rutherfordium samarium scandium seaborgium selenium silicon silver sodium strontium sulfur tantalum technetium tellurium terbium thallium thorium thulium tin titanium tungsten uranium vanadium xenon ytterbium yttrium zinc zirconium

Md Hg Mo Nd Ne Np Ni Nb N No Os O Pd P Pt Pu Po K Pr Pm Pa Ra Rn Re Rh Rb Ru Rf Sm Sc Sg Se Si Ag Na Sr S Ta Tc Te Tb Tl Th Tm Sn Ti W U V Xe Yb Y Zn Zr

101 80 42 60 10 93 28 41 7 102 76 8 46 15 78 94 84 19 59 61 91 88 86 75 45 37 44 104 62 21 106 34 14 47 11 38 16 73 43 52 65 81 90 69 50 22 74 92 23 54 70 39 30 40

9 Covalent bond lengths

C–HSi–HN–HP–HO–HS–HF–HCl–HBr–HI–HC–OC=OC–NC=N

C≡NC–FC–ClC–BrC–ISi–O

0.1080.1480.1010.1440.0960.1340.0920.1270.1410.1610.1430.1200.1470.1300.1160.1380.1770.1940.2140.161

10 Bond enthalpies and average bond enthalpies at 298 K

C–HSi–HN–HP–HO–HS–HF–HCl–HBr–HI–HC–OC=OC–NC=N

C≡NC–FC–ClC–BrC–ISi–O

413318391321464364568432366298358746286615887467346290228466

11 Organic compounds—thermodynamic data

CH3CHO(CH3)2COHCOOH

CH3COOH

C6H5COOH

CH3NH2

ggggllgggggggglllllgllglgllllsgglllsg

–75–85–105–127–173–19952200*

–8–12228187110–1564912–13104–82–124–135–37–16–137–9111–239–277–165–109–191–248–425–485–385–23

–51–33–23–16–9–4687572666320919415227125111120203–57–63–71–2613–5394–166–175–48–113–128–155–361–390–24532

186230270310261296220267306301296201248279204173320255345235178202246163

240161219160129160243

* (–0.4)

13 Lattice enthalpies at 298 K (experimental and theoretical values)

The lattice enthalpy values ( ∆ HlatticeÖ )

given relate to the endothermic process for a solid crystal breaking into gaseous ions

For example, for an alkali metal halide:

864790720695670

820754691668647

764705650632613

CuCl2AgFAgClAgBrAgI

2824974918905892

Theoretical values

These two tables contain lattice enthalpies calculated from electrostatic principles on the basis of

a purely ionic model for the crystal

834769701680657

788732671651632

730682632617600

Other

substances ∆HlatticeÖ / kJ mol –1

Other substances ∆Hlattice Ö

AgFAgClAgBrAgI

953910897881

14 Standard electrode potentials

Oxidized species Reduced species EÖ / V

Cr2O72–(aq) + 14H+(aq) + 6e– 2Cr3+(aq) + 7H2O(l) +1.33

MnO4–(aq) + 8H+(aq) + 5e– Mn2+(aq) + 4H2O(l) +1.51

15 Strengths of organic acids and bases

The acid strengths in the following tables are given in terms of pKa values, where

pKa = –log10 Ka

The dissociation constant Ka values are for aqueous solutions at 298 K

Base strengths are given in terms of pKb values

CH3(CH2)3COOH(CH3)3CCOOH

C6H5COOH

C6H5CH2COOH

3.754.764.874.834.844.835.034.204.31

Halogenated carboxylic acids

CH2FCOOH

CH2BrCOOH

CH2ICOOH

2.871.350.662.592.903.18

9.997.238.367.154.070.42

4.753.343.353.274.203.163.259.13

3.2–4.43.0–4.63.8–5.44.8–6.06.0–7.66.6–8.08.2–10.0

redyellowyellowredyellowyellowcolourless

yellowblueblueyellowblueredpink

aldehydes, ketones, carboxylic acids and esters

alkyneshydrogen bonding in carboxylic acidsalkanes, alkenes, arenes

hydrogen bonding in alcohols and phenols

primary amines

490–620500–600600–8001000–14001050–14101610–1680

1700–17502100–22602500–33002850–31003200–36003300–3500

18 1 H NMR data

Typical proton chemical shift values (δ) relative to tetramethylsilane (TMS) = 0

R represents an alkyl group, and Hal represents F, Cl, Br, or I

These values may vary in different solvents and conditions

7.6

H2N CH CH

CH2 CH2 CH2 NH2 9.7

Common name Symbol Structural formula pH of isoelectric point

H2N CH

CH2 CH2 S CH3COOH

20 Structural formulas of some medicines

and drugs

C OH O

O C

CH3

aspirin paracetamol (acetaminophen) ibuprofen

O OH

CH3O

HO O

H N C R O

H N

N O

H2N

CH2O

CH2

H2C OH

N H

CH3

C N O

O

NH O O

NH3

NH3

cisplatin

psilocybin

21 Structural formulas of some biological molecules

H

OHHOH

H OH

H H

O O

CH2OH H

H

OH H HO

OH H HO

CH2HO HO

ascorbic acid (vitamin C)

HO

CH3

CH3

H C

N CH N

NH2

H

N C

N C

C C N CH N O

H

H2N

H

N C

N CH

CH C

NH2

O H

N

C

N CH

CH C O

O

H

H

N C

N CH

C C O

O H

OH

O glucose

O

R OH R HO

N N

N N

H2C H

CH2C O O

C20H39

CH2

CH3

H C

O O

CH3O

R=CH3(Chlorophyll a) R=CHO (Chlorophyll b)

CH3

CH3 CH3

OH C

3,5-di-tert-butyl-4-Fatty acids

Linoleic acid CH3(CH2)4(CH═CHCH2)2(CH2)6COOHLinolenic acid CH3CH2(CH═CHCH2)3(CH2)6COOH

23 References

The data in tables 4–16 can be found in the following three sources

Lide, DR 2008 CRC Handbook of Chemistry and Physics Boca Raton, USA CRC Press Copyright 2008 by CRC Handbook of Chemistry and Physics David R Lide Reproduced by

permission from Taylor and Francis Group, LLC, a division of Informa plc

NVON 2007 Binas English Edition Groningen, The Netherlands Wolters–Noordhoff.

Royal Society of Chemistry 2002 Royal Society of Chemistry Electronic Data Book CD-Rom

London, UK Reproduced by permission of The Royal Society of Chemistry

For tables 17 and 18, in addition to the sources above, the data were informed by the following

Aylward, G and Findlay, T 2002 SI Chemical Data 5th Edition Queensland, Australia John

Wiley & Sons

Clugston, M and Flemming, R 2000 Advanced Chemistry Oxford, UK Oxford University

Press

Morrison, RT and Boyd, RN 1987 Organic Chemistry 5th Edition Boston, Massachusetts,

USA Allyn and Bacon, Inc