IB Chemistry data booklet (2025): formulas and tables

This page covers the IB Diploma Programme Chemistry data booklet for first assessment 2025 (version 1.1), which every student receives in the exam, arranged by the Structure and Reactivity topics of the 2025 syllabus. The booklet does not label HL equations, so the HL tags here follow the additional higher level statements in the subject guide. This is CuratedPrep's own summary, not a copy of the booklet: use it to see what you can look up and what you must recall.

Board	Official document
International Baccalaureate Diploma Programme Chemistry (SL and HL, first assessment 2025)	Chemistry data booklet, first assessment 2025, version 1.1, and Chemistry guide, first assessment 2025

In the booklet means the formula is printed in the official booklet or sheet in the exam; Learn it means students must recall it.

Structure 1: atoms, moles and gases

Equations printed in the booklet; rows marked HL only sit in additional higher level statements of the guide.

Formula	Equation	In the exam
Wave equation for lightHL only (S1.3.6, S3.1.10). c is the speed of light, f frequency in Hz, λ wavelength in m.In the booklet	$c = f λ$	In the booklet
Photon energyHL only (S1.3.6). E is energy in J, h the Planck constant, f frequency in Hz.In the booklet	$E = h f$	In the booklet
Amount from massn in mol, m in g, M in g mol⁻¹ (S1.4).In the booklet	$n = \frac{m}{M}$	In the booklet
Amount from concentrationn in mol, C in mol dm⁻³, V in dm³ (S1.4).In the booklet	$n = C V$	In the booklet
Ideal gas equationUse SI units: P in Pa, V in m³, T in K (S1.5).In the booklet	$P V = n RT$	In the booklet
Combined gas lawFixed amount of gas; T in kelvin, same units for both pressures and both volumes (S1.5).In the booklet	$\frac{P _{1} V _{1}}{T _{1}} = \frac{P _{2} V _{2}}{T _{2}}$	In the booklet

Reactivity 1: energy changes and spontaneity

Formula	Equation	In the exam
Heat energy from a temperature changeQ in J, m in g, c in J g⁻¹ K⁻¹ (water 4.18), change in T in K or °C (R1.1).In the booklet	$Q = m c Δ T$	In the booklet
Enthalpy change from enthalpies of formationProducts minus reactants; multiply each value by its coefficient (R1.2.4).In the booklet	$Δ H^{\circ} = \sum Δ H_{f}^{\circ} (products) - \sum Δ H_{f}^{\circ} (reactants)$	In the booklet
Enthalpy change from enthalpies of combustionReactants minus products, the opposite way round to formation data (R1.2.4).In the booklet	$Δ H^{\circ} = \sum Δ H_{c}^{\circ} (reactants) - \sum Δ H_{c}^{\circ} (products)$	In the booklet
Gibbs energy changeHL only (R1.4.2). Convert so that all terms use kJ or all use J; T in K.In the booklet	$Δ G^{\circ} = Δ H^{\circ} - T Δ S^{\circ}$	In the booklet
Gibbs energy away from standard stateHL only (R1.4.4). Q is the reaction quotient; R = 8.31 J K⁻¹ mol⁻¹.In the booklet	$Δ G = Δ G^{\circ} + RT ln Q$	In the booklet
Gibbs energy and equilibrium constantHL only (R1.4.4, R2.3.7). With R in J, ΔG comes out in J mol⁻¹.In the booklet	$Δ G^{\circ} = - RT ln K$	In the booklet

Reactivity 2: how much, how fast, how far

Formula	Equation	In the exam
Percentage atom economyUse the balanced equation, including coefficients (R2.1.5).In the booklet	$% atom economy = \frac{molar mass of desired product}{molar mass of all reactants} \times 100$	In the booklet
Arrhenius equationHL only (R2.2.12). k rate constant, A Arrhenius factor, Ea in J mol⁻¹, T in K.In the booklet	$k = A e^{- E_{a} / RT}$	In the booklet
Arrhenius equation, linear formHL only (R2.2.12). Plot ln k against 1/T: gradient is -Ea/R, intercept is ln A.In the booklet	$ln k = - \frac{E _{a}}{RT} + ln A$	In the booklet

Reactivity 3: acids, bases and electron transfer

Formula	Equation	In the exam
pHThe booklet also prints the form with [H3O+]; they mean the same thing (R3.1.4).In the booklet	$pH = - lo g_{10} [H^{+}]$	In the booklet
Ionic product of waterThe value of Kw at 298 K is printed in the constants table (R3.1.5).In the booklet	$K_{w} = [H^{+}] [OH^{-}]$	In the booklet
pOHHL only (R3.1.9).In the booklet	$pOH = - lo g_{10} [OH^{-}]$	In the booklet
Gibbs energy and cell potentialHL only (R3.2.14). n electrons transferred, F the Faraday constant in C mol⁻¹, E in V.In the booklet	$Δ G^{\circ} = - n F E^{\circ}$	In the booklet

Uncertainties

Three propagation rules for processed data, added in the February 2024 version of the booklet; they apply at SL and HL.

Formula	Equation	In the exam
Adding or subtracting measurementsAdd the absolute uncertainties, even when you subtract the values.In the booklet	$y = a \pm b \Rightarrow Δ y = Δ a + Δ b$	In the booklet
Multiplying or dividing measurementsAdd the percentage (relative) uncertainties.In the booklet	$y = \frac{ab}{c} \Rightarrow \frac{Δ y}{y} = \frac{Δ a}{a} + \frac{Δ b}{b} + \frac{Δ c}{c}$	In the booklet
Raising to a powerMultiply the relative uncertainty by the size of the power.In the booklet	$y = a^{n} \Rightarrow \frac{Δ y}{y} = ∣ n ∣ \frac{Δ a}{a}$	In the booklet

Data tables in the booklet

What each table is for; the values are in the booklet you receive in the exam, so learn how to use them rather than the numbers.

Formula	Equation	In the exam
Physical constantsGives e, electron, proton and neutron masses, c, h, the Avogadro constant, R, molar volume at STP (22.7 dm³ mol⁻¹), specific heat capacity of water, Kw and the Faraday constant. SL and HL.In the booklet	Table: physical constants	In the booklet
Metric (SI) multipliersConverts between prefixes such as kilo, milli, micro, nano and pico. SL and HL.In the booklet	Table: SI prefixes	In the booklet
Unit conversions and standard conditionsGives K = °C + 273.15, dm³ to m³, and defines STP (273.15 K, 100 kPa) and SATP (298.15 K, 100 kPa). SL and HL.In the booklet	Table: unit conversions and STP/SATP	In the booklet
Electromagnetic spectrumOrders the regions by wavelength and energy and shows visible light as 400 to 700 nm; used with c = f λ. SL and HL.In the booklet	Table: electromagnetic spectrum	In the booklet
Names of the elementsLists each element with its symbol and atomic number. SL and HL.In the booklet	Table: names of elements	In the booklet
Periodic tableGives groups, periods and relative atomic masses for calculating molar masses. SL and HL.In the booklet	Table: periodic table	In the booklet
Melting and boiling points of the elementsCompares physical properties and explains periodic trends in bonding and structure. SL and HL.In the booklet	Table: melting and boiling points	In the booklet
First ionisation energy, electron affinity and electronegativityExplains periodic trends, bond polarity and (with the triangle) bond type. SL and HL.In the booklet	Table: ionisation energy, electron affinity, electronegativity	In the booklet
Atomic and ionic radiiExplains trends across periods and down groups, and why cations are smaller and anions larger than their atoms. SL and HL.In the booklet	Table: atomic and ionic radii	In the booklet
Covalent bond lengthsCompares single, double and triple bond lengths and links length to bond strength. SL and HL.In the booklet	Table: bond lengths	In the booklet
Bond enthalpiesEstimates enthalpy changes from bonds broken minus bonds formed (average values, so approximate). SL and HL.In the booklet	Table: bond enthalpies	In the booklet
Thermodynamic data for selected compoundsFormation enthalpies feed Hess's law calculations at SL and HL; standard entropies and Gibbs energies of formation are for the HL entropy and spontaneity topic.In the booklet	Table: enthalpy of formation, Gibbs energy of formation, entropy	In the booklet
Enthalpies of combustionGives molar combustion enthalpies for Hess's law and for comparing fuels. SL and HL.In the booklet	Table: enthalpies of combustion	In the booklet
Colour wheel with wavelengthsHL only (S3.1.10). Finds the colour absorbed or observed for transition element complexes, with wavelength ranges.In the booklet	Table: colour wheel	In the booklet
Lattice enthalpiesCompares ionic bond strength and completes Born-Haber cycle values; the values are for the endothermic separation of gaseous ions. SL and HL.In the booklet	Table: lattice enthalpies	In the booklet
Triangular bonding diagramPlaces a binary compound as ionic, covalent, metallic or in between using average electronegativity and the difference. SL and HL.In the booklet	Table: van Arkel-Ketelaar bonding triangle	In the booklet
Acid-base indicatorsHL only (R3.1.14, R3.1.15). Gives pKa, pH range and colours so you can choose an indicator for a titration.In the booklet	Table: acid-base indicators	In the booklet
Standard reduction potentialsHL only (R3.2.12 to R3.2.15). Gives E-standard for half-cells to predict spontaneity, work out cell potential and predict electrolysis products.In the booklet	Table: standard reduction potentials	In the booklet
Infrared dataHL only (S3.2.9). Matches wavenumber ranges to bonds and functional groups in IR spectra.In the booklet	Table: infrared absorptions	In the booklet
Proton NMR dataHL only (S3.2.10, S3.2.11). Matches chemical shifts to proton environments when deducing structures.In the booklet	Table: 1H NMR chemical shifts	In the booklet
Mass spectral fragments lostHL only (S3.2.8). Links the mass lost from the molecular ion to the fragment that left.In the booklet	Table: mass spectral fragments	In the booklet

Learn these: not in the booklet

Number of particles $N = n N_{A}$
Relative atomic mass from isotopes $A_{r} = \frac{\sum ( abundance \times isotope mass )}{\sum abundance}$
Gas volume at STP $n = \frac{V}{V _{m}}, V_{m} = 22.7 dm^{3} mol^{- 1}$ The value is printed; the relationship is not.
Mass concentration $concentration in g dm^{- 3} = C \times M$
Dilution $C_{1} V_{1} = C_{2} V_{2}$
Percentage yield $\frac{experimental yield}{theoretical yield} \times 100$
Enthalpy change per mole from calorimetry $Δ H = - \frac{Q}{n}$
Bond enthalpy sum $Δ H = \sum (bonds broken) - \sum (bonds formed)$
Rate of reaction $rate = \frac{Δ [ reactant or product ]}{Δ t}$
Equilibrium constant expression $K_{c} = \frac{[ C ] ^{c} [ D ] ^{d}}{[ A ] ^{a} [ B ] ^{b}}$
Hydrogen ion concentration $[H^{+}] = 1 0^{- pH}$
Percentage uncertainty $\frac{Δ a}{a} \times 100$
Standard entropy change (HL) $Δ S^{\circ} = \sum S^{\circ} (products) - \sum S^{\circ} (reactants)$
Reaction quotient (HL) $Q = \frac{[ C ] ^{c} [ D ] ^{d}}{[ A ] ^{a} [ B ] ^{b}}$ Uses concentrations that are not at equilibrium.
Rate equation (HL) $rate = k [A]^{m} [B]^{n}$
Ionic product link (HL) $pH + pOH = 14 at 298 K, an d [OH^{-}] = 1 0^{- pOH}$
Acid and base constants (HL) $K_{a} = \frac{[ H ^{+} ] [ A ^{-} ]}{[ HA ]}, K_{b} = \frac{[ BH ^{+} ] [ OH ^{-} ]}{[ B ]}$
Conjugate pair relationship (HL) $K_{a} \times K_{b} = K_{w}$
pK values (HL) $p K_{a} = - lo g_{10} K_{a}, p K_{b} = - lo g_{10} K_{b}$
Buffer pH (HL, derived from the K_a expression) $pH = p K_{a} + lo g_{10} \frac{[ A ^{-} ]}{[ HA ]}$
Standard cell potential (HL) $E_{cell}^{\circ} = E_{cathode}^{\circ} - E_{anode}^{\circ}$ Use standard reduction potentials for both electrodes.
Formal charge (HL) $FC = V - N - \frac{1}{2} B$ V valence electrons, N non-bonding electrons, B bonding electrons.

Study booklets

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. Open the dropdown, then click a booklet to open it or use Download to save the PDF.

IB Diploma1 booklet

Chemistry data booklet First assessment 2025PDF, 19 pages, 1.8 MB
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How to use the formula sheet in the exam

Work with the booklet open throughout the course so you know where each table sits before the exam.
Match units before substituting: ΔH is in kJ mol⁻¹ but ΔS and R use J, so convert before using ΔG equations.
The bond enthalpy table gives values only; write the broken minus formed sum yourself and show each bond and its count.
With the reduction potentials table, do not change the sign of E when you multiply a half-equation to balance electrons.
For Arrhenius data (HL), plot ln k against 1/T: the gradient is −E_a/R, so convert E_a to kJ mol⁻¹ only at the end.

Common questions

Can I use the data booklet in IB Chemistry exams?

Yes. The IB requires every student to have a clean copy of the Chemistry data booklet in the examination, and schools supply it. Practise with it all course so you can find values quickly.

Which equations in the data booklet are HL only?

Nine: c = fλ, E = hf, the three Gibbs energy equations with T, Q and K, ΔG = −nFE, both Arrhenius forms, and pOH. The booklet does not mark them; the guide places them in additional higher level content.

Which Chemistry formulas are not in the data booklet?

Percentage yield, the equilibrium constant expression, rate equations, Ka and Kb, Ka times Kb = Kw, the bond enthalpy sum and the entropy change sum are not printed. The learn list above gives them with labels.

Where do I get the official IB Chemistry data booklet?

The IB does not publish it openly. Schools obtain the official copy through the IB and print it for students, so ask your teacher or coordinator for a clean copy.

What changed in version 1.1 of the 2025 booklet?

The February 2024 update corrected the F to I bond length, updated pH ranges for bromocresol green, phenol red and phenolphthalein, and added the uncertainties section.

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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.

IB Chemistry data booklet guide for first assessment 2025

In short