A Level chemistry data booklet: AQA, Edexcel, 9701

This page covers AQA A Level Chemistry 7405 and follows its four page data booklet, then lists the calculation equations from the specification with a given or not given label. Read it to see what the booklet really contains before you open it in the exam. A comparison section at the end shows what the Pearson Edexcel International A Level (YCH11), Pearson Edexcel A Level (9CH0) and Cambridge 9701 booklets print.

Board	Official document
AQA A Level Chemistry (7405)	A-level Chemistry 7405 Data Booklet (insert provided with the papers) and the AQA specification
Pearson Edexcel International A Level Chemistry (YCH11)	IAL Chemistry data booklet (specification appendix, pages 100 to 105)
Pearson Edexcel A Level Chemistry (9CH0)	GCE Chemistry (9CH0) Data Booklet, Issue 2, Summer 2017
Cambridge International AS & A Level Chemistry (9701)	Syllabus 2025, 2026 and 2027, Data section (pages 80 to 91)

In the booklet means the formula is printed in the official booklet or sheet in the exam; Learn it means students must recall it; In the question means the value is given in the exam question when it is needed; See note means it depends on the board.

What the AQA data booklet provides

The AQA 7405 booklet is only four pages and contains data tables, not equations or constants; all of it is printed for the exam.

Formula	Equation	In the exam
The Periodic Table of the ElementsPage 2. Gives atomic number, symbol, name and relative atomic mass, so use these Ar values in Mr and mole calculations.In the booklet	$A_{r} for every element$	In the booklet
Table A: infrared absorption dataPage 3. Also lists N-H 3300 to 3500, O-H (alcohols) 3230 to 3550, O-H (acids) 2500 to 3000, C-H 2850 to 3300, C≡N 2220 to 2260, C=C 1620 to 1680, C-O 1000 to 1300 and C-C 750 to 1100 cm⁻¹.In the booklet	$C=O: 1680 to 1750 cm^{- 1}$	In the booklet
Table B: 1H NMR chemical shift dataPage 3. Covers ROH, RNH2, CH2, CH, protons next to C=O, O or halogens, alkene H, aldehyde H (9.0 to 10.0) and acid H (10.0 to 12.0).In the booklet	$δ for RCH_{3} = 0.7 to 1.2 ppm$	In the booklet
Table C: 13C NMR chemical shift dataPage 3. Also gives alkane C, C-halogen, C-N, C-O, C=C and arene, nitrile and ester or acid C=O ranges.In the booklet	$δ for C=O (aldehyde or ketone) = 190 to 220 ppm$	In the booklet
Phosphate, glucose and 2-deoxyribosePage 4. Skeletal structures for the DNA backbone and sugars (3.3.13 amino acids, proteins and DNA).In the booklet	structures	In the booklet
The four DNA basesPage 4. Structures only, so you still need to know which bases pair and how.In the booklet	adenine, guanine, cytosine, thymine	In the booklet
Six amino acidsPage 4. Structures only; other amino acids will be drawn in the question if needed.In the booklet	alanine, aspartic acid, cysteine, lysine, phenylalanine, serine	In the booklet
Haem BPage 4. Printed with the biochemistry structures.In the booklet	structure	In the booklet

Constants and data AQA does not print

AQA states that you are not expected to recall these values; the question supplies them when they are needed.

Formula	Equation	In the exam
Avogadro constantNot in the AQA booklet. The spec says you will not be expected to recall it; check the value printed in the question.In the question	$L \approx 6.02 \times 1 0^{23} mol^{- 1}$	In the question
Gas constantNot in the AQA booklet. The spec says R will be given when required. Use it with pressure in Pa, volume in m³ and temperature in K.In the question	$R = 8.31 J K^{- 1} mol^{- 1}$	In the question
Specific heat capacity of waterNot in the AQA booklet. The spec says you will not be expected to recall c; the question gives the value and units to use.Learn it	$c = 4.18 J g^{- 1} K^{- 1}$	Learn it
Ionic product of waterNot in the AQA booklet. Kw changes with temperature, so use the value in the question for any other temperature.Learn it	$K_{w} = 1.00 \times 1 0^{- 14} mol^{2} dm^{- 6} at 298 K$	Learn it
Standard electrode potentials and bond enthalpiesNot in the AQA booklet. Values are supplied in the question when a calculation needs them; the spec only expects you to use them.In the question	$E^{⊖} (V), bond enthalpy (kJ mol^{- 1})$	In the question

Amount of substance and concentration

None of these equations is printed in the AQA booklet. Learn them and the units.

Formula	Equation	In the exam
Moles from massn in mol, m in g, Mr in g mol⁻¹. Use Ar from the periodic table.Learn it	$n = \frac{m}{M _{r}}$	Learn it
Moles in solutionc in mol dm⁻³, V in dm³. Convert cm³ to dm³ by dividing by 1000.Learn it	$n = c \times V$	Learn it
ConcentrationMass concentration in g dm⁻³ = c × M_r.Learn it	$c = \frac{n}{V}$	Learn it
Number of particlesL is the Avogadro constant. Use it for atoms, molecules, ions or electrons.Learn it	$N = n \times L$	Learn it
DilutionA rearrangement of n = cV with n unchanged. Keep both volumes in the same unit.Learn it	$c_{1} V_{1} = c_{2} V_{2}$	Learn it
Empirical formulaDivide by the smallest number of moles, then scale up if you get halves or thirds.Learn it	$moles of each element = \frac{mass}{A _{r}} \Rightarrow simplest whole-number ratio$	Learn it

Ideal gas equation

Formula	Equation	In the exam
Ideal gas equationp in Pa, V in m³, n in mol, T in K. 1 dm³ = 1 × 10⁻³ m³; 1 kPa = 1000 Pa. R is given in the question.Learn it	$p V = n RT$	Learn it
Relative molecular mass of a volatile liquidRearranged from pV = nRT with n = m/Mr. Mass in g gives Mr in g mol⁻¹.Learn it	$M_{r} = \frac{m RT}{p V}$	Learn it

Percentage yield and atom economy

Formula	Equation	In the exam
Percentage yieldCompare moles with moles or mass with mass, not one of each.Learn it	$% yield = \frac{actual amount of product}{theoretical amount of product} \times 100$	Learn it
Percentage atom economyUse the balanced equation and include the coefficients. This is the AQA definition.Learn it	$% atom economy = \frac{M _{r} of desired product}{sum of M _{r} of all reactants} \times 100$	Learn it

Energetics: calorimetry, Hess and bond enthalpies

Formula	Equation	In the exam
Heat change in calorimetrym in g (mass of the substance heated, usually the water or solution), c in J g⁻¹ K⁻¹, q in J. c is given in the question.Learn it	$q = m c Δ T$	Learn it
Molar enthalpy changeConvert q to kJ first (divide by 1000) so that the answer is in kJ mol⁻¹. Negative for a temperature rise (exothermic).Learn it	$Δ H = - \frac{q}{n}$	Learn it
Hess's law with formation dataMultiply each value by its coefficient. Elements in their standard states have Δ_fH = 0.Learn it	$Δ_{r} H = \sum Δ_{f} H^{⊖} (products) - \sum Δ_{f} H^{⊖} (reactants)$	Learn it
Hess's law with combustion dataNote the reversed order compared with formation data.Learn it	$Δ_{r} H = \sum Δ_{c} H^{⊖} (reactants) - \sum Δ_{c} H^{⊖} (products)$	Learn it
Mean bond enthalpiesGives an approximate value because the bond enthalpies are averages and the species are gases.Learn it	$Δ H = \sum (bonds broken) - \sum (bonds formed)$	Learn it
Enthalpy of solution from a cycleA Level only. Lattice dissociation enthalpy is the negative of lattice formation enthalpy.Learn it	$Δ_{sol} H = Δ H_{lattice dissociation} + \sum Δ_{hyd} H$	Learn it
Born-Haber cycleA Level only. Draw the cycle and apply Hess's law to find any one missing step, usually the lattice enthalpy.Learn it	$Δ_{f} H = atomisation + ionisation energies + bond enthalpy terms + electron affinities + lattice formation$	Learn it

Equilibrium: Kc and Kp

For the reaction aA + bB ⇌ cC + dD at a fixed temperature.

Formula	Equation	In the exam
Equilibrium constant KcConcentrations in mol dm⁻³ at equilibrium. Work out the units from the expression. Only temperature changes Kc.Learn it	$K_{c} = \frac{[ C ] ^{c} [ D ] ^{d}}{[ A ] ^{a} [ B ] ^{b}}$	Learn it
Equilibrium constant KpA Level only. Gases only, partial pressures at equilibrium. Units follow from the pressure unit used.Learn it	$K_{p} = \frac{p _{C}^{c} p _{D}^{d}}{p _{A}^{a} p _{B}^{b}}$	Learn it
Mole fractionMoles of the gas at equilibrium divided by the total moles of gas.Learn it	$x_{A} = \frac{n _{A}}{n _{total}}$	Learn it
Partial pressureThe partial pressures add up to the total pressure, which is a quick check.Learn it	$p_{A} = x_{A} \times P_{total}$	Learn it

Rate equations and the Arrhenius equation

A Level only. The AQA spec says the Arrhenius equations and R will be given when required, but they are not in the booklet, so the question supplies them.

Formula	Equation	In the exam
Rate equationm and n are orders (0, 1 or 2) found from experiment, not from the balanced equation. k is the rate constant.Learn it	$rate = k [A]^{m} [B]^{n}$	Learn it
Overall orderUse it to work out the units of k, for example mol⁻¹ dm³ s⁻¹ for second order.Learn it	$overall order = m + n$	Learn it
Arrhenius equationSupplied in the question when required. Ea in J mol⁻¹, T in K, A is the Arrhenius constant. Raising T increases k.In the question	$k = A e^{- E_{a} / RT}$	In the question
Arrhenius, logarithmic formSupplied when required. Plot ln k (y) against 1/T (x): gradient = -Ea/R and intercept = ln A. Convert Ea to kJ mol⁻¹ at the end.In the question	$ln k = - \frac{E _{a}}{RT} + ln A$	In the question

Acids, bases, pH and buffers

A Level only. Use the units and approximations the AQA spec describes.

Formula	Equation	In the exam
pHConvert back with [H⁺] = 10^−pH. For a strong monoprotic acid, [H+] equals the acid concentration.Learn it	$pH = - lo g_{10} [H^{+}]$	Learn it
Ionic product of waterUse it to find the pH of a strong base: [H+] = Kw / [OH-], then take -log.Learn it	$K_{w} = [H^{+}] [OH^{-}]$	Learn it
Acid dissociation constantUnits mol dm⁻³. Written for HA ⇌ H+ + A-.Learn it	$K_{a} = \frac{[ H ^{+} ] [ A ^{-} ]}{[ HA ]}$	Learn it
pKaConvert back with K_a = 10^−pKa. pKa has no units.Learn it	$p K_{a} = - lo g_{10} K_{a}$	Learn it
pH of a weak acid (approximation)Assumes [H+] = [A-] and that [HA] at equilibrium equals the starting concentration. State both assumptions.Learn it	$[H^{+}] = K_{a} [HA]$	Learn it
Acidic bufferRearranged from Ka with [HA] and [A-] taken as the amounts of weak acid and its salt. Take -log to get pH.Learn it	$[H^{+}] = K_{a} \times \frac{[ HA ]}{[ A ^{-} ]}$	Learn it
Acidic buffer, Henderson formEquivalent to the line above. Check what your teacher accepts, but the previous form follows the AQA wording.Learn it	$pH = p K_{a} + lo g_{10} \frac{[ A ^{-} ]}{[ HA ]}$	Learn it
Titration calculationFind moles from c × V of the known solution, then use the equation ratio.Learn it	$n (acid) = \frac{coefficient of acid}{coefficient of base} \times n (base)$	Learn it

Entropy and Gibbs free-energy change

A Level only.

Formula	Equation	In the exam
Entropy change of a reactionAbsolute entropies are supplied in the question. Units J K⁻¹ mol⁻¹.Learn it	$Δ S^{⊖} = \sum S^{⊖} (products) - \sum S^{⊖} (reactants)$	Learn it
Gibbs free-energy changeThe spec gives this as the relationship to learn. Convert ΔS to kJ K⁻¹ mol⁻¹ (divide by 1000) so all terms are in kJ mol⁻¹.Learn it	$Δ G = Δ H - T Δ S$	Learn it
Feasibility conditionA reaction is feasible when the free-energy change is zero or negative.Learn it	$Δ G \leq 0$	Learn it
Temperature at which a reaction becomes feasibleSet ΔG = 0 and rearrange. Check the units of ΔS first.Learn it	$T = \frac{Δ H}{Δ S}$	Learn it
ΔG against T graphPlot ΔG (y) against T (x) in kelvin.Learn it	$gradient = - Δ S, intercept = Δ H$	Learn it

Electrode potentials and cells

A Level only. AQA does not require the Nernst equation.

Formula	Equation	In the exam
EMF of a cellThe more positive half-cell is the positive electrode. The E° values are supplied in the question.Learn it	$E_{cell}^{⊖} = E_{positive}^{⊖} - E_{negative}^{⊖}$	Learn it
Conventional cell representationNegative electrode on the left, positive on the right. A double line is the salt bridge.Learn it	$Pt ∣ Fe^{2 +}, Fe^{3 +} ∣∣ Ag^{+} ∣ Ag$	Learn it
Feasibility from E°The direction is predicted only; the rate may still be too slow, and non-standard conditions change E.Learn it	$E_{cell}^{⊖} > 0 \Rightarrow reaction predicted to go$	Learn it

Comparison with other boards

The given column refers to AQA 7405. The notes say what Pearson Edexcel International A Level (YCH11), Pearson Edexcel A Level (9CH0) and Cambridge 9701 (2025 to 2027) print.

Formula	Equation	In the exam
Gas constant RPrinted in Edexcel IAL, Edexcel 9CH0 and Cambridge booklets. AQA supplies it in the question.See note	$R = 8.31 J K^{- 1} mol^{- 1}$	See note
Avogadro constantEdexcel IAL and 9CH0 print 6.02 × 10²³. Cambridge prints 6.022 × 10²³. AQA supplies it in the question.See note	$L = 6.02 \times 1 0^{23} mol^{- 1}$	See note
Molar volume of a gasEdexcel IAL and 9CH0 print 24 dm³ mol⁻¹ at room temperature and pressure (r.t.p.). Cambridge prints 22.4 dm³ mol⁻¹ at standard temperature and pressure (s.t.p.: 101 kPa, 273 K) and 24.0 dm³ mol⁻¹ at room conditions. AQA does not print a molar volume.See note	$V_{m} = 24 dm^{3} mol^{- 1} at r.t.p.$	See note
Ionic product of waterEdexcel IAL, Edexcel 9CH0 and Cambridge (at 298 K) print it. AQA does not.See note	$K_{w} = 1.00 \times 1 0^{- 14} mol^{2} dm^{- 6}$	See note
Elementary chargePrinted by Edexcel IAL, Edexcel 9CH0 and Cambridge (shown as -1.60 × 10⁻¹⁹ C). Not in the AQA booklet.See note	$e = 1.60 \times 1 0^{- 19} C$	See note
Faraday constantPrinted in the Cambridge booklet only. Not in the Edexcel or AQA booklets.See note	$F = 9.65 \times 1 0^{4} C mol^{- 1}$	See note
Specific heat capacity of waterPrinted in the Cambridge booklet only. AQA and Edexcel supply it in the question.See note	$c = 4.18 J g^{- 1} K^{- 1}$	See note
Standard electrode potentialsPrinted by Edexcel IAL and 9CH0 (31 half-equations, 298 K) and by Cambridge (alphabetical list, with other tables). Not in the AQA booklet.See note	$E^{⊖} (V) table$	See note
Bond energiesPrinted in the Cambridge booklet only (diatomic and polyatomic tables). Not in the AQA or Edexcel booklets.See note	$bond energy (kJ mol^{- 1})$	See note
Ionisation energiesPrinted in the Cambridge booklet for selected elements. Not in the AQA or Edexcel booklets.See note	$1st to 4th (kJ mol^{- 1})$	See note
Pauling electronegativitiesPrinted by Edexcel IAL, Edexcel 9CH0 and Cambridge. Not in the AQA booklet.See note	$χ for each element$	See note
IR, 1H NMR and 13C NMR tablesAll four booklets print IR and NMR data. AQA and Cambridge use tables; Edexcel uses a chart for NMR. The values differ between boards, so use the booklet for your own board.In the booklet	spectroscopy data	In the booklet
Periodic TablePrinted in all four booklets.In the booklet	$A_{r}$	In the booklet
Biochemistry structuresPrinted in the AQA booklet only (phosphate, glucose, 2-deoxyribose, four bases, six amino acids, haem B).In the booklet	bases, sugars, amino acids	In the booklet
Calculation equationsNone of the four booklets prints calculation equations. You must learn them for every board; only the values supplied differ.Learn it	$n = \frac{m}{M _{r}}, p V = n RT, Δ G = Δ H - T Δ S$	Learn it

Learn these: not in the booklet

Moles from mass $n = \frac{m}{M _{r}}$
Moles in solution $n = c V$
Ideal gas equation $p V = n RT$
Percentage yield $\frac{actual}{theoretical} \times 100$
Percentage atom economy $\frac{M _{r} desired product}{\sum M _{r} reactants} \times 100$
Heat change $q = m c Δ T$
Hess's law $Δ_{r} H = \sum Δ_{f} H (products) - \sum Δ_{f} H (reactants)$
Kc and Kp expressions $p = x P$ Write Kc and Kp from the balanced equation; partial pressure is mole fraction times total pressure.
Rate equation $rate = k [A]^{m} [B]^{n}$
pH $pH = - lo g_{10} [H^{+}] an d K_{w} = [H^{+}] [OH^{-}]$
Ka and pKa $K_{a} = \frac{[ H ^{+} ] [ A ^{-} ]}{[ HA ]}, p K_{a} = - lo g_{10} K_{a}$
Gibbs free energy $Δ G = Δ H - T Δ S$
Cell EMF $E_{cell}^{⊖} = E_{positive}^{⊖} - E_{negative}^{⊖}$

Study booklets for your board

Our printable version of each board's official booklet: everything it prints (formulas, constants, data and statistical tables) in the board's own order, plus what you must learn and exam tips. Choose your board, then click a booklet to open it or use Download to save the PDF.

AQA1 booklet

A Level Chemistry 7405PDF, 8 pages, 0.9 MB
Download

Edexcel2 booklets

A Level Chemistry 9CH0PDF, 9 pages, 1.1 MB
Download
AS Chemistry 8CH0PDF, 5 pages, 0.9 MB
Download

Edexcel International (IAL)1 booklet

International AS and A Level ChemistryPDF, 9 pages, 1.1 MB
Download

Cambridge1 booklet

AS and A Level Chemistry 9701PDF, 10 pages, 1.2 MB
Download

OxfordAQA1 booklet

International AS and A Level Chemistry 9620PDF, 7 pages, 0.9 MB
Download

How to use the formula sheet in the exam

Open the AQA booklet before the exam and find the periodic table on page 2 and the spectroscopy tables on page 3, so you do not search for them under time pressure.
Do not look for equations in the booklet: none is printed. Learn every equation and the units, then check each answer has the right units.
Convert before you substitute: cm³ to dm³ for concentrations, dm³ to m³ and kPa to Pa for pV = nRT, and J to kJ when combining ΔH and TΔS.
For spectra, match the question's compound to the ranges in the table; remember O-H in acids (2500 to 3000) is broader and lower than in alcohols.
When a question gives R, Ka or Kw, use exactly the value in the question, and keep to the number of significant figures in the data.

Common questions

Does the AQA A Level Chemistry data booklet include equations?

No. The AQA 7405 booklet has the periodic table, infrared, 1H NMR and 13C NMR tables and biochemistry structures. You must learn the calculation equations yourself.

Are constants such as R and the Avogadro constant given in the AQA exam?

They are not printed in the booklet. The AQA specification says you are not expected to recall them, so the question supplies the value when it is needed.

Will the Arrhenius equation be given in AQA A Level Chemistry?

The specification says the Arrhenius equations and R will be given when required, so they appear in the question. You still need to know how to use them, including the ln k against 1/T graph.

Which board gives the most data in the booklet?

Cambridge 9701 prints the most, including bond energies, ionisation energies, many electrode potentials and constants such as the Faraday constant. Edexcel prints constants and electrode potentials; AQA prints the least.

Is the Edexcel IAL data booklet the same as Edexcel A Level 9CH0?

The copies we checked list the same sections: physical constants, IR, NMR, Pauling electronegativities, electrode potentials and the periodic table. Check which issue your exam centre uses.

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Formulas checked against the official documents linked above. Boards update their booklets from time to time: always practise with the version your exam uses.

A Level chemistry data booklet: AQA, Edexcel and Cambridge 9701

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