Free resource · A-Level H2 (9476)

H2 Chemistry Data Booklet (9476): Free PDF

The H2 Chemistry data booklet is the set of tables SEAB provides in the A-Level written papers for H2 9476, H1 8873 and H3 9813, for use from 2026. It gives important constants, ionisation energies, bond energies, standard electrode potentials, atomic and ionic radii and other data you look up rather than memorise. Older 9729 copies are out of date.

Download the free PDF View it on this page

PDF · 10 pages · A4 portrait · free, no sign-up

First page of the H2 Chemistry Data Booklet PDF

1Important values, constants and standards

Quantity	Value
molar gas constant	R = 8.31 J K⁻¹ mol⁻¹
the Faraday constant	F = 9.65 × 10⁴ C mol⁻¹
the Avogadro constant	L = 6.02 × 10²³ mol⁻¹
the Planck constant	h = 6.63 × 10⁻³⁴ J s
speed of light in a vacuum	c = 3.00 × 10⁸ m s⁻¹
rest mass of proton, ¹₁H	mₚ = 1.67 × 10⁻²⁷ kg
rest mass of neutron, ¹₀n	mₙ = 1.67 × 10⁻²⁷ kg
rest mass of electron, ⁰₋₁e	mₑ = 9.11 × 10⁻³¹ kg
elementary charge	e = 1.60 × 10⁻¹⁹ C
molar volume of gas	Vₘ = 22.7 dm³ mol⁻¹ at s.t.p. Vₘ = 24 dm³ mol⁻¹ at r.t.p. (where s.t.p. is expressed as 10⁵ Pa [1 bar] and 273 K [0 °C], r.t.p. is expressed as 101 325 Pa [1 atm] and 293 K [20 °C])
ionic product of water	Kw = 1.00 × 10⁻¹⁴ mol² dm⁻⁶ (at 298 K [25 °C])
specific heat capacity of water	c = 4.18 kJ kg⁻¹ K⁻¹ (= 4.18 J g⁻¹ K⁻¹)

Back to all sections

2Ionisation energies (1st, 2nd, 3rd and 4th) of selected elements, in kJ mol⁻¹

Element	Proton Number	First	Second	Third	Fourth
H	1	1310	–	–	–
He	2	2370	5250	–	–
Li	3	519	7300	11800	–
Be	4	900	1760	14800	21000
B	5	799	2420	3660	25000
C	6	1090	2350	4610	6220
N	7	1400	2860	4590	7480
O	8	1310	3390	5320	7450
F	9	1680	3370	6040	8410
Ne	10	2080	3950	6150	9290
Na	11	494	4560	6940	9540
Mg	12	736	1450	7740	10500
Al	13	577	1820	2740	11600
Si	14	786	1580	3230	4360
P	15	1060	1900	2920	4960
S	16	1000	2260	3390	4540
Cl	17	1260	2300	3850	5150
Ar	18	1520	2660	3950	5770
K	19	418	3070	4600	5860
Ca	20	590	1150	4940	6480
Sc	21	632	1240	2390	7110
Ti	22	661	1310	2720	4170
V	23	648	1370	2870	4600
Cr	24	653	1590	2990	4770
Mn	25	716	1510	3250	5190
Fe	26	762	1560	2960	5400
Co	27	757	1640	3230	5100
Ni	28	736	1750	3390	5400
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

Back to all sections

3Bond energies

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

Bond	Energy/kJ mol⁻¹
H–H	436
D–D	442
N≡N	944
O=O	496
F–F	158
Cl–Cl	244
Br–Br	193
I–I	151

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

Bond	Energy/kJ mol⁻¹
H–F	562
H–Cl	431
H–Br	366
H–I	299
C≡O	1077

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

Bond	Energy / kJ mol⁻¹
C–C	350
C=C	610
C≡C	840
C⎓C (benzene)	520
N–N	160
N=N	410
O–O	150
Si–Si	222
P–P	200
S–S	264

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

Bond	Energy / kJ mol⁻¹
C–H	410
C–F	485
C–Cl	340
C–Br	280
C–I	240
C–N	305
C=N	610
C≡N	890
C–O	360
C=O	740
C=O in CO₂	805
N–H	390
N–Cl	310
O–H	460
Si–Cl	359
Si–H	320
Si–O (in SiO₂(s))	460
Si=O (in SiO₂(g))	640
P–H	320
P–Cl	330
P–O	340
P=O	540
S–H	347
S–Cl	250
S–O	360
S=O	500

Back to all sections

4Standard 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

Electrode reaction	E⦵ / V
Ag⁺ + e⁻ ⇌ Ag	+0.80
Al³⁺ + 3e⁻ ⇌ Al	−1.66
Ba²⁺ + 2e⁻ ⇌ Ba	−2.90
Br₂ + 2e⁻ ⇌ 2Br⁻	+1.07
Ca²⁺ + 2e⁻ ⇌ Ca	−2.87
Cl₂ + 2e⁻ ⇌ 2Cl⁻	+1.36
2HOCl + 2H⁺ + 2e⁻ ⇌ Cl₂ + 2H₂O	+1.64
ClO⁻ + H₂O + 2e⁻ ⇌ Cl⁻ + 2OH⁻	+0.81
Co²⁺ + 2e⁻ ⇌ Co	−0.28
Co³⁺ + e⁻ ⇌ Co²⁺	+1.89
[Co(NH₃)₆]²⁺ + 2e⁻ ⇌ Co + 6NH₃	−0.43
Cr²⁺ + 2e⁻ ⇌ Cr	−0.91
Cr³⁺ + 3e⁻ ⇌ Cr	−0.74
Cr³⁺ + e⁻ ⇌ Cr²⁺	−0.41
Cr₂O₇²⁻ + 14H⁺ + 6e⁻ ⇌ 2Cr³⁺ + 7H₂O	+1.33
Cu⁺ + e⁻ ⇌ Cu	+0.52
Cu²⁺ + 2e⁻ ⇌ Cu	+0.34
Cu²⁺ + e⁻ ⇌ Cu⁺	+0.15
[Cu(NH₃)₄]²⁺ + 2e⁻ ⇌ Cu + 4NH₃	−0.05
F₂ + 2e⁻ ⇌ 2F⁻	+2.87
Fe²⁺ + 2e⁻ ⇌ Fe	−0.44
Fe³⁺ + 3e⁻ ⇌ Fe	−0.04
Fe³⁺ + e⁻ ⇌ Fe²⁺	+0.77
[Fe(CN)₆]³⁻ + e⁻ ⇌ [Fe(CN)₆]⁴⁻	+0.36
Fe(OH)₃ + e⁻ ⇌ Fe(OH)₂ + OH⁻	−0.56
2H⁺ + 2e⁻ ⇌ H₂	0.00
I₂ + 2e⁻ ⇌ 2I⁻	+0.54
K⁺ + e⁻ ⇌ K	−2.92
Li⁺ + e⁻ ⇌ Li	−3.04
Mg²⁺ + 2e⁻ ⇌ Mg	−2.38
Mn²⁺ + 2e⁻ ⇌ Mn	−1.18
Mn³⁺ + e⁻ ⇌ Mn²⁺	+1.54
MnO₂ + 4H⁺ + 2e⁻ ⇌ Mn²⁺ + 2H₂O	+1.23
MnO₄⁻ + e⁻ ⇌ MnO₄²⁻	+0.56
MnO₄⁻ + 4H⁺ + 3e⁻ ⇌ MnO₂ + 2H₂O	+1.67
MnO₄⁻ + 8H⁺ + 5e⁻ ⇌ Mn²⁺ + 4H₂O	+1.52
NO₃⁻ + 2H⁺ + e⁻ ⇌ NO₂ + H₂O	+0.81
NO₃⁻ + 3H⁺ + 2e⁻ ⇌ HNO₂ + H₂O	+0.94
NO₃⁻ + 10H⁺ + 8e⁻ ⇌ NH₄⁺ + 3H₂O	+0.87
Na⁺ + e⁻ ⇌ Na	−2.71
Ni²⁺ + 2e⁻ ⇌ Ni	−0.25
[Ni(NH₃)₆]²⁺ + 2e⁻ ⇌ Ni + 6NH₃	−0.51
H₂O₂ + 2H⁺ + 2e⁻ ⇌ 2H₂O	+1.77
HO₂⁻ + H₂O + 2e⁻ ⇌ 3OH⁻	+0.88
O₂ + 4H⁺ + 4e⁻ ⇌ 2H₂O	+1.23
O₂ + 2H₂O + 4e⁻ ⇌ 4OH⁻	+0.40
O₂ + 2H⁺ + 2e⁻ ⇌ H₂O₂	+0.68
O₂ + H₂O + 2e⁻ ⇌ HO₂⁻ + OH⁻	−0.08
2H₂O + 2e⁻ ⇌ H₂ + 2OH⁻	−0.83
Pb²⁺ + 2e⁻ ⇌ Pb	−0.13
Pb⁴⁺ + 2e⁻ ⇌ Pb²⁺	+1.69
PbO₂ + 4H⁺ + 2e⁻ ⇌ Pb²⁺ + 2H₂O	+1.47
SO₄²⁻ + 4H⁺ + 2e⁻ ⇌ SO₂ + 2H₂O	+0.17
S₂O₈²⁻ + 2e⁻ ⇌ 2SO₄²⁻	+2.01
S₄O₆²⁻ + 2e⁻ ⇌ 2S₂O₃²⁻	+0.09
Sn²⁺ + 2e⁻ ⇌ Sn	−0.14
Sn⁴⁺ + 2e⁻ ⇌ Sn²⁺	+0.15
V²⁺ + 2e⁻ ⇌ V	−1.20
V³⁺ + e⁻ ⇌ V²⁺	−0.26
VO²⁺ + 2H⁺ + e⁻ ⇌ V³⁺ + H₂O	+0.34
VO₂⁺ + 2H⁺ + e⁻ ⇌ VO²⁺ + H₂O	+1.00
VO₃⁻ + 4H⁺ + e⁻ ⇌ VO²⁺ + 2H₂O	+1.00
Zn²⁺ + 2e⁻ ⇌ Zn	−0.76

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

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

Electrode reaction	E⦵ / V
F₂ + 2e⁻ ⇌ 2F⁻	+2.87
S₂O₈²⁻ + 2e⁻ ⇌ 2SO₄²⁻	+2.01
H₂O₂ + 2H⁺ + 2e⁻ ⇌ 2H₂O	+1.77
MnO₄⁻ + 8H⁺ + 5e⁻ ⇌ Mn²⁺ + 4H₂O	+1.52
PbO₂ + 4H⁺ + 2e⁻ ⇌ Pb²⁺ + 2H₂O	+1.47
Cl₂ + 2e⁻ ⇌ 2Cl⁻	+1.36
Cr₂O₇²⁻ + 14H⁺ + 6e⁻ ⇌ 2Cr³⁺ + 7H₂O	+1.33
O₂ + 4H⁺ + 4e⁻ ⇌ 2H₂O	+1.23
Br₂ + 2e⁻ ⇌ 2Br⁻	+1.07
NO₃⁻ + 10H⁺ + 8e⁻ ⇌ NH₄⁺ + 3H₂O	+0.87
ClO⁻ + H₂O + 2e⁻ ⇌ Cl⁻ + 2OH⁻	+0.81
NO₃⁻ + 2H⁺ + e⁻ ⇌ NO₂ + H₂O	+0.81
Ag⁺ + e⁻ ⇌ Ag	+0.80
Fe³⁺ + e⁻ ⇌ Fe²⁺	+0.77
I₂ + 2e⁻ ⇌ 2I⁻	+0.54
O₂ + 2H₂O + 4e⁻ ⇌ 4OH⁻	+0.40
Cu²⁺ + 2e⁻ ⇌ Cu	+0.34
SO₄²⁻ + 4H⁺ + 2e⁻ ⇌ SO₂ + 2H₂O	+0.17
Sn⁴⁺ + 2e⁻ ⇌ Sn²⁺	+0.15
S₄O₆²⁻ + 2e⁻ ⇌ 2S₂O₃²⁻	+0.09
2H⁺ + 2e⁻ ⇌ H₂	0.00
Pb²⁺ + 2e⁻ ⇌ Pb	−0.13
Sn²⁺ + 2e⁻ ⇌ Sn	−0.14
Fe²⁺ + 2e⁻ ⇌ Fe	−0.44
Zn²⁺ + 2e⁻ ⇌ Zn	−0.76
2H₂O + 2e⁻ ⇌ H₂ + 2OH⁻	−0.83
V²⁺ + 2e⁻ ⇌ V	−1.20
Mg²⁺ + 2e⁻ ⇌ Mg	−2.38
Ca²⁺ + 2e⁻ ⇌ Ca	−2.87
K⁺ + e⁻ ⇌ K	−2.92

Back to all sections

5Atomic and ionic radii

(a) Period 1

	Element	atomic/nm	Ion	ionic/nm	Ion	ionic/nm
single covalent	H	0.037			H⁻	0.208
van der Waals	He	0.140

(b) Period 2

	Element	atomic/nm	Ion	ionic/nm	Ion	ionic/nm
metallic	Li	0.152	Li⁺	0.060
	Be	0.112	Be²⁺	0.031
single covalent	B	0.080	B³⁺	0.020
	C	0.077	C⁴⁺	0.015	C⁴⁻	0.260
	N	0.074			N³⁻	0.171
	O	0.073			O²⁻	0.140
	F	0.072			F⁻	0.136
van der Waals	Ne	0.160

	Element	atomic/nm	Ion	ionic/nm	Ion	ionic/nm
metallic	Na	0.186	Na⁺	0.095
	Mg	0.160	Mg²⁺	0.065
	Al	0.143	Al³⁺	0.050
single covalent	Si	0.117	Si⁴⁺	0.041
	P	0.110			P³⁻	0.212
	S	0.104			S²⁻	0.184
	Cl	0.099			Cl⁻	0.181
van der Waals	Ar	0.190

(d) Group 2

	Element	atomic/nm	Ion	ionic/nm
metallic	Be	0.112	Be²⁺	0.031
	Mg	0.160	Mg²⁺	0.065
	Ca	0.197	Ca²⁺	0.099
	Sr	0.215	Sr²⁺	0.113
	Ba	0.217	Ba²⁺	0.135
	Ra	0.220	Ra²⁺	0.140

(e) Group 14

	Element	atomic/nm	Ion	ionic/nm
single covalent	C	0.077
	Si	0.117	Si⁴⁺	0.041
	Ge	0.122	Ge²⁺	0.093
metallic	Sn	0.162	Sn²⁺	0.112
	Pb	0.175	Pb²⁺	0.120

(f) Group 17

	Element	atomic/nm	Ion	ionic/nm
single covalent	F	0.072	F⁻	0.136
	Cl	0.099	Cl⁻	0.181
	Br	0.114	Br⁻	0.195
	I	0.133	I⁻	0.216
	At	0.140

(g) First row d block elements

	Element	atomic/nm	Ion	ionic/nm	Ion	ionic/nm
metallic	Sc	0.164			Sc³⁺	0.075
	Ti	0.146	Ti²⁺	0.086	Ti³⁺	0.067
	V	0.135	V²⁺	0.079	V³⁺	0.064
	Cr	0.129	Cr²⁺	0.073	Cr³⁺	0.062
	Mn	0.132	Mn²⁺	0.083	Mn³⁺	0.058
	Fe	0.126	Fe²⁺	0.061	Fe³⁺	0.055
	Co	0.125	Co²⁺	0.065	Co³⁺	0.055
	Ni	0.124	Ni²⁺	0.069	Ni³⁺	0.056
	Cu	0.128	Cu²⁺	0.073
	Zn	0.135	Zn²⁺	0.074

Back to all sections

6Typical proton (¹H) chemical shift values (δ) relative to TMS = 0

Type of proton	Environment of proton	Example structures	Chemical Shift range (δ)
C–H	alkane	–CH₃, –CH₂–, >CH–	0.9–1.7
	alkyl next to C=O	CH₃–C=O, –CH₂–C=O, >CH–C=O	2.2–3.0
	alkyl next to aromatic ring	CH₃–Ar, –CH₂–Ar, >CH–Ar	2.3–3.0
	alkyl next to electronegative atom	CH₃–O, –CH₂–O, –CH₂–Cl, >CH–Br	3.2–4.0
	attached to alkyne	≡C–H	1.8–3.1
	attached to alkene	=CH₂, =CH–	4.5–6.0
	attached to aromatic ring	C₆H₅–H	6.0–9.0
	aldehyde	R–C(=O)–H	9.3–10.5
O–H (see note below)	alcohol	RO–H	0.5–6.0
	phenol	C₆H₅–OH	4.5–7.0
	carboxylic acid	R–C(=O)–O–H	9.0–13.0
N–H (see note below)	alkyl amine	R–NH–	1.0–5.0
	aryl amine	C₆H₅–NH₂	3.0–6.0
	amide	R–C(=O)–NH–	5.0–12.0

Note: δ values for –O–H and –N–H protons can vary depending on solvent and concentration.
Example structures drawn as skeletal diagrams in the booklet (>CH–, the benzene ring, and the R–C(=O)– groups) are given here as condensed formulae.

Back to all sections

7Characteristic infra-red absorption frequencies for some selected bonds

Bond	Functional groups containing the bond	Absorption range (in wavenumbers) / cm⁻¹	Appearance of peak (s = strong, w = weak)
C–Cl	chloroalkanes	700–800	s
C–O	alcohol	970–1260	s
	ether	1000–1310	s
	ester	1050–1330	s
	carboxylic acids	1210–1440	s
C=C	aromatic	1475–1625	s
	alkenes	1635–1690	w
C=O	amides	1640–1690	s
	ketones and aldehydes	1670–1740	s
	carboxylic acids	1680–1730	s
	esters	1710–1750	s
C≡C	alkynes	2150–2250	w unless conjugated
C≡N	nitriles	2200–2250	w
C–H	alkanes, CH₂–H	2850–2950	s
	alkenes/arenes, =C–H	3000–3100	w
N–H	amines, amides	3300–3500	w
O–H	carboxylic acid, RCO₂–H	2500–3000	s and very broad
	H-bonded alcohol/phenol, RO–H	3200–3600	s
	free alcohol, RO–H	3580–3650	s and sharp

Back to all sections

8The orientating effect of groups in aromatic substitution reactions

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

G	Reactivity of ring (compared to benzene)	Position of E (relative to position of G)
–alkyl –OH or –OR –NH₂, –NHR or –NR₂ –NHCOR	Activated	2- and/or 4-
–Cl, –Br, –I	Deactivated	2- and/or 4-
–CHO, –COR –CO₂H, –CO₂R –NH₃⁺ –NO₂, –CN	Deactivated	3-

The booklet prints this table with G, reactivity and position as rows. Here they are columns.
Scheme printed above the table: a benzene ring bearing G (ring positions 2, 3 and 4 numbered from G) + E⁺ → the ring bearing G and E + H⁺.

Back to all sections

9Qualitative Analysis Notes

[ppt. = precipitate]

9(a) Reactions of aqueous cations

cation	reaction with NaOH(aq)	reaction with NH₃(aq)
aluminium, Al³⁺(aq)	white ppt. soluble in excess	white ppt. insoluble in excess
ammonium, NH₄⁺(aq)	ammonia produced on heating	–
barium, Ba²⁺(aq)	no ppt. (if reagents are pure)	no ppt.
calcium, Ca²⁺(aq)	white ppt. with high [Ca²⁺(aq)]	no ppt.
chromium(III), Cr³⁺(aq)	grey-green ppt. soluble in excess giving dark green solution	grey-green ppt. insoluble in excess
copper(II), Cu²⁺(aq),	pale blue ppt. insoluble in excess	blue ppt. soluble in excess giving dark blue solution
iron(II), Fe²⁺(aq)	green ppt., turning brown on contact with air insoluble in excess	green ppt., turning brown on contact with air insoluble in excess
iron(III), Fe³⁺(aq)	red-brown ppt. insoluble in excess	red-brown ppt. insoluble in excess
magnesium, Mg²⁺(aq)	white ppt. insoluble in excess	white ppt. insoluble in excess
manganese(II), Mn²⁺(aq)	off-white ppt., rapidly turning brown on contact with air insoluble in excess	off-white ppt., rapidly turning brown on contact with air insoluble in excess
zinc, Zn²⁺(aq)	white ppt. soluble in excess	white ppt. soluble in excess

9(b) Reactions of anions

anion	reaction
carbonate, CO₃²⁻	CO₂ liberated by dilute acids
chloride, Cl⁻(aq)	gives white ppt. with Ag⁺(aq) (soluble in NH₃(aq))
bromide, Br⁻(aq)	gives pale cream ppt. with Ag⁺(aq) (partially soluble in NH₃(aq))
iodide, I⁻(aq)	gives yellow ppt. with Ag⁺(aq) (insoluble in NH₃(aq))
nitrate, NO₃⁻(aq)	NH₃ liberated on heating with OH⁻(aq) and Al foil
nitrite, NO₂⁻(aq)	NH₃ liberated on heating with OH⁻(aq) and Al foil; NO liberated by dilute acids (colourless NO → (pale) brown NO₂ in air)
sulfate, SO₄²⁻(aq)	gives white ppt. with Ba²⁺(aq) (insoluble in excess dilute strong acids)
sulfite, SO₃²⁻(aq)	SO₂ liberated with dilute acids; gives white ppt. with Ba²⁺(aq) (soluble in dilute strong acids)

9(c) Tests for gases

gas	test and test result
ammonia, NH₃	turns damp red litmus paper blue
carbon dioxide, CO₂	gives a white ppt. with limewater (ppt. dissolves with excess CO₂)
chlorine, Cl₂	bleaches damp litmus paper
hydrogen, H₂	“pops” with a lighted splint
oxygen, O₂	relights a glowing splint
sulfur dioxide, SO₂	turns aqueous acidified potassium manganate(VII) from purple to colourless

9(d) Colour of halogens

halogen	colour of element	colour in aqueous solution	colour in hexane
chlorine, Cl₂	greenish yellow gas	pale yellow	pale yellow
bromine, Br₂	reddish brown gas / liquid	orange	orange-red
iodine, I₂	black solid / purple gas	brown	purple

Back to all sections

10The Periodic Table of Elements

Key: atomic number, atomic symbol, name, relative atomic mass

The Periodic Table of Elements, with the values printed in the data booklet

Group 1 (alkali metals)
Group 2
Transition elements
Group 17 (halogens)
Group 18 (noble gases)
Lanthanoids and actinoids
Other elements

Swipe sideways to see all 18 groups.

1Hhydrogen1.0

2Hehelium4.0

3Lilithium6.9

4Beberyllium9.0

5Bboron10.8

6Ccarbon12.0

7Nnitrogen14.0

8Ooxygen16.0

9Ffluorine19.0

10Neneon20.2

11Nasodium23.0

12Mgmagnesium24.3

13Alaluminium27.0

14Sisilicon28.1

15Pphosphorus31.0

16Ssulfur32.1

17Clchlorine35.5

18Arargon39.9

19Kpotassium39.1

20Cacalcium40.1

21Scscandium45.0

22Tititanium47.9

23Vvanadium50.9

24Crchromium52.0

25Mnmanganese54.9

26Feiron55.8

27Cocobalt58.9

28Ninickel58.7

29Cucopper63.5

30Znzinc65.4

31Gagallium69.7

32Gegermanium72.6

33Asarsenic74.9

34Seselenium79.0

35Brbromine79.9

36Krkrypton83.8

37Rbrubidium85.5

38Srstrontium87.6

39Yyttrium88.9

40Zrzirconium91.2

41Nbniobium92.9

42Momolybdenum95.9

43Tctechnetium–

44Ruruthenium101.1

45Rhrhodium102.9

46Pdpalladium106.4

47Agsilver107.9

48Cdcadmium112.4

49Inindium114.8

50Sntin118.7

51Sbantimony121.8

52Tetellurium127.6

53Iiodine126.9

54Xexenon131.3

55Cscaesium132.9

56Babarium137.3

72Hfhafnium178.5

73Tatantalum180.9

74Wtungsten183.8

75Rerhenium186.2

76Ososmium190.2

77Iriridium192.2

78Ptplatinum195.1

79Augold197.0

80Hgmercury200.6

81Tlthallium204.4

82Pblead207.2

83Bibismuth209.0

84Popolonium–

85Atastatine–

86Rnradon–

87Frfrancium–

88Raradium–

104Rfrutherfordium–

105Dbdubnium–

106Sgseaborgium–

107Bhbohrium–

108Hshassium–

109Mtmeitnerium–

110Dsdarmstadtium–

111Rgroentgenium–

112Cncopernicium–

113Nhnihonium–

114Flflerovium–

115Mcmoscovium–

116Lvlivermorium–

117Tstennessine–

118Ogoganesson–

57-71lanthanoids

89-103actinoids

lanthanoids

57Lalanthanum138.9

58Cecerium140.1

59Prpraseodymium140.9

60Ndneodymium144.2

61Pmpromethium–

62Smsamarium150.4

63Eueuropium152.0

64Gdgadolinium157.3

65Tbterbium158.9

66Dydysprosium162.5

67Hoholmium164.9

68Ererbium167.3

69Tmthulium168.9

70Ybytterbium173.1

71Lulutetium175.0

actinoids

89Acactinium–

90Ththorium232.0

91Paprotactinium231.0

92Uuranium238.0

93Npneptunium–

94Puplutonium–

95Amamericium–

96Cmcurium–

97Bkberkelium–

98Cfcalifornium–

99Eseinsteinium–

100Fmfermium–

101Mdmendelevium–

102Nonobelium–

103Lrlawrencium–

All elements A to Z, with relative atomic mass

Element	Symbol	Proton number	Relative atomic mass
actinium	Ac	89	–
aluminium	Al	13	27.0
americium	Am	95	–
antimony	Sb	51	121.8
argon	Ar	18	39.9
arsenic	As	33	74.9
astatine	At	85	–
barium	Ba	56	137.3
berkelium	Bk	97	–
beryllium	Be	4	9.0
bismuth	Bi	83	209.0
bohrium	Bh	107	–
boron	B	5	10.8
bromine	Br	35	79.9
cadmium	Cd	48	112.4
caesium	Cs	55	132.9
calcium	Ca	20	40.1
californium	Cf	98	–
carbon	C	6	12.0
cerium	Ce	58	140.1
chlorine	Cl	17	35.5
chromium	Cr	24	52.0
cobalt	Co	27	58.9
copernicium	Cn	112	–
copper	Cu	29	63.5
curium	Cm	96	–
darmstadtium	Ds	110	–
dubnium	Db	105	–
dysprosium	Dy	66	162.5
einsteinium	Es	99	–
erbium	Er	68	167.3
europium	Eu	63	152.0
fermium	Fm	100	–
flerovium	Fl	114	–
fluorine	F	9	19.0
francium	Fr	87	–
gadolinium	Gd	64	157.3
gallium	Ga	31	69.7
germanium	Ge	32	72.6
gold	Au	79	197.0
hafnium	Hf	72	178.5
hassium	Hs	108	–
helium	He	2	4.0
holmium	Ho	67	164.9
hydrogen	H	1	1.0
indium	In	49	114.8
iodine	I	53	126.9
iridium	Ir	77	192.2
iron	Fe	26	55.8
krypton	Kr	36	83.8
lanthanum	La	57	138.9
lawrencium	Lr	103	–
lead	Pb	82	207.2
lithium	Li	3	6.9
livermorium	Lv	116	–
lutetium	Lu	71	175.0
magnesium	Mg	12	24.3
manganese	Mn	25	54.9
meitnerium	Mt	109	–
mendelevium	Md	101	–
mercury	Hg	80	200.6
molybdenum	Mo	42	95.9
moscovium	Mc	115	–
neodymium	Nd	60	144.2
neon	Ne	10	20.2
neptunium	Np	93	–
nickel	Ni	28	58.7
nihonium	Nh	113	–
niobium	Nb	41	92.9
nitrogen	N	7	14.0
nobelium	No	102	–
oganesson	Og	118	–
osmium	Os	76	190.2
oxygen	O	8	16.0
palladium	Pd	46	106.4
phosphorus	P	15	31.0
platinum	Pt	78	195.1
plutonium	Pu	94	–
polonium	Po	84	–
potassium	K	19	39.1
praseodymium	Pr	59	140.9
promethium	Pm	61	–
protactinium	Pa	91	231.0
radium	Ra	88	–
radon	Rn	86	–
rhenium	Re	75	186.2
rhodium	Rh	45	102.9
roentgenium	Rg	111	–
rubidium	Rb	37	85.5
ruthenium	Ru	44	101.1
rutherfordium	Rf	104	–
samarium	Sm	62	150.4
scandium	Sc	21	45.0
seaborgium	Sg	106	–
selenium	Se	34	79.0
silicon	Si	14	28.1
silver	Ag	47	107.9
sodium	Na	11	23.0
strontium	Sr	38	87.6
sulfur	S	16	32.1
tantalum	Ta	73	180.9
technetium	Tc	43	–
tellurium	Te	52	127.6
tennessine	Ts	117	–
terbium	Tb	65	158.9
thallium	Tl	81	204.4
thorium	Th	90	232.0
thulium	Tm	69	168.9
tin	Sn	50	118.7
titanium	Ti	22	47.9
tungsten	W	74	183.8
uranium	U	92	238.0
vanadium	V	23	50.9
xenon	Xe	54	131.3
ytterbium	Yb	70	173.1
yttrium	Y	39	88.9
zinc	Zn	30	65.4
zirconium	Zr	40	91.2

Back to all sections

Inside the PDF

10 A4 pages, ready to print. Tap a page to open the PDF there.

Questions students ask

Which data booklet is used for H2 Chemistry 9476?

The SEAB Data Booklet for Chemistry (Advanced Level), for use from 2026 with the H1 8873, H2 9476 and H3 9813 syllabuses. Many copies online are the older 9729 edition, so check that yours says for use from 2026.

Is the data booklet used in the H2 Chemistry practical exam?

No. The booklet states that it is for use in all papers except practical examinations, so the practical paper gives you any data you need within the question itself.

Do I need to memorise standard electrode potentials for H2 Chemistry?

No. The E° values are listed in the data booklet. What you must be able to do is choose the right half-equations, calculate E°cell and decide whether a reaction is feasible.

Keep revising

Source

The exam paper itself is what counts on the day. If anything here differs from the SEAB document, the SEAB document is right. Tell us and we will fix it.

Want a H2 Chemistry tutor?

Tell us the level and we send a shortlist of tutors on WhatsApp within 16 hours. You choose the tutor. About H2 Chemistry tuition

Ask on WhatsApp