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Data Booklet for Singapore A Level Chemistry (H1, H2, H3)

Disclaimer: This is the web version of the Data Booklet for Singapore–Cambridge GCE Advanced Level Chemistry (H1, H2 and H3), painstakingly reproduced by Chemistry Guru, Singapore's most reputable JC chemistry tuition centre. Minor adjustments are made for alignment and easier web navigation.

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.

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^–1

3. Bond energies

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

5. Atomic and ionic radii

6. Typical proton (¹H) 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

1. Important values, constants and standards

molar gas constant	R	= 8.31 J K^–1 mol^–1
the Faraday constant	F	= 9.65 x10⁴ C mol^–1
the Avogadro constant	L	= 6.02 x10²³ mol^–1
the Planck constant	h	= 6.63 x10^–34 J s
speed of light in a vacuum	c	= 3.00 x10⁸ m s^–1
rest mass of proton, ¹₁H	m_p= 1.67 x10^–27 kg
rest mass of neutron, ¹₀n	m_n= 1.67 x10^–27 kg
rest mass of electron, ⁰_–1e	m_e= 9.11 x 10^–31 kg
electronic charge	e	= –1.60 x10^–19 C
molar volume of gas	V_m= 22.7 dm³ mol^–1 at s.t.p. V_m= 24 dm³ mol^–1 at r.t.p. (where s.t.p. is expressed as 10⁵ Pa [1 bar] and 273 K [0 ^oC], r.t.p. is expressed as 101325 Pa [1 atm] and 293 K [20 ^oC])
ionic product of water	K_w= 1.00 x10^–14 mol² dm^–6(at 298 K [25 ^oC])
specific heat capacity of water	= 4.18 kJ kg^–1 K^–1 (= 4.18 J g^–1 K^–1)

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

	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

	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

3. Bond 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

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

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

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

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^θ in alphabetical order

Electrode reaction			E^θ/ 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
Cr₂O₇^2– + 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

Electrode reaction			E^θ/ V
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^–	⇌	MnO₄^2–	+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

Electrode reaction			E^θ/ V
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
SO₄^2– + 4H⁺ + 2e^–	⇌	SO₂+ 2H₂O	+0.17
S₂O₈^2– + 2e^–	⇌	2SO₄^2–	+2.01
S₄O₆^2– + 2e^–	⇌	2S₂O₃^2–	+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^θ in decreasing order of oxidising power**

(a selection only – see also the extended alphabetical list on the previous pages)

Electrode reaction			E^θ/ V
F₂+ 2e^–	⇌	2F^–	+2.87
S₂O₈^2– + 2e^–	⇌	2SO₄^2–	+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
Cr₂O₇^2– + 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
SO₄^2– + 4H⁺ + 2e^–	⇌	SO₂+ 2H₂O	+0.17
Sn⁴⁺ + 2e^–	⇌	Sn²⁺	+0.15
S₄O₆^2– + 2e^–	⇌	2S₂O₃^2–	+0.09
2H⁺ + 2e^–	⇌	H₂	0.00
Pb²⁺ + 2e^–	⇌	Pb	–0.13
Sn²⁺ + 2e^–	⇌	Sn	–0.14
Fe²⁺ + 2e^–	⇌	Fe	–0.44

Electrode reaction			E^θ/ V
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

5. Atomic and ionic radii

(a) Period 1	atomic/nm		ionic/nm
single covalent	H	0.037			H^–	0.208
van der Waals	He	0.140
(b) Period 2
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	C^4–	0.260
	N	0.074			N^3–	0.171
	O	0.073			O^2–	0.140
	F	0.072			F^–	0.136

van der Waals	Ne	0.160
(c) Period 3
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			P^3–	0.212
	S	0.104			S^2–	0.184
	Cl	0.099			Cl^–	0.181

van der Waals	Ar	0.190
(d) Group 2
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	atomic/nm		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
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
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

6. Typical 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		0.9–1.7
	alkyl next to C=O		2.2–3.0
	alkyl next to aromatic ring		2.3–3.0
	alkyl next to electronegative atom		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		6.0–9.0
	aldehyde		9.3–10.5
O―H (see note below)	alcohol	RO―H	0.5–6.0
	phenol		4.5–7.0
	carboxylic acid		9.0–13.0
N―H (see note below)	alkyl amine	R―NH―	1.0–5.0
	aryl amine		3.0–6.0
	amide		5.0–12.0

Note: δvalues for ―O―H and ―N―H protons can vary depending on solvent and concentration.

7. Characteristic infra-red absorption frequencies for some selected bonds

Bond	Functional groups containing the bond	Absorption range (in wave numbers) / 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

8. The 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.

databooklet 8

―alkyl

―OH or ―OR

―NH₂, ―NHR or ―NR₂

―NHCOR

―Cl, ―Br, ―I

―CHO, ―COR

―CO₂H, ―CO₂R

―NH₃⁺

―NO₂, ―CN

Reactivity of ring (compared to benzene)

Activated

Deactivated

Position of E (relative to position of G)

2- and/or 4-

9. Qualitative Analysis Notes

[ppt. = precipitate]

9(a) Reactions of aqueous cations

cation	reaction with
cation	NaOH(aq)	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, CO₃^2–	CO₂liberated 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)	NH₃liberated on heating with OH^–(aq) and Al foil
nitrite, NO₂^–(aq)	NH₃liberated on heating with OH^–(aq) and Al foil; NO liberated by dilute acids (colourless NO →(pale) brown NO₂in air)
sulfate, SO₄^2–(aq)	gives white ppt. with Ba²⁺(aq) (insoluble in excess dilute strong acids)
sulfite, SO₃^2–(aq)	SO₂liberated 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

10. The Periodic Table of Elements

databooklet periodictable

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Data Booklet for Singapore A Level Chemistry (H1, H2, H3)

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^–1

3. Bond energies

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

**4(b) E^θ in decreasing order of oxidising power**

5. Atomic and ionic radii

6. Typical proton (¹H) 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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Data Booklet for Singapore A Level Chemistry (H1, H2, H3)

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–1

3. Bond energies

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

4(b) Eθ in decreasing order of oxidising power

5. Atomic and ionic radii

6. Typical proton (1H) 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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2. Ionisation energies (1st, 2nd, 3rd and 4th) of selected elements, in kJ mol^–1

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

**4(b) E^θ in decreasing order of oxidising power**

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