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Advanced Higher Chemistry data booklet: relationships, tables, IR, NMR and thermodynamics

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Formula sheet

The card below opens today's Advanced Higher Chemistry paper with the booklet's relationships, its constants and our periodic table in the drawer. The contents follow in our own layout. For any number in a table, use the official booklet, published in January 2026.

Formula sheet

Advanced Higher Chemistry

Open formula sheet

Relationships

E_h=cm\Delta Theat energy to change the temperature of a liquid
\%\ \text{yield}=\frac{\text{actual yield}}{\text{theoretical yield}}\times100percentage yield
n=cVmoles from concentration and volume
n=\frac{m}{\text{GFM}}moles from mass
\frac{c_1V_1}{n_1}=\frac{c_2V_2}{n_2}titration: the volumes and concentrations of two solutions
\text{average rate}=\frac{\Delta\text{quantity}}{\Delta t}average rate of a reaction
\text{reaction rate}=\frac{1}{t}reaction rate from the time taken
\%\ \text{by mass}=\frac{m}{\text{GFM}}\times100percentage by mass
\%\ \text{atom economy}=\frac{\text{mass of desired product(s)}}{\text{total mass of reactants}}\times100percentage atom economy
c=f\lambdawave speed
E=\frac{Lhc}{\lambda}energy of a mole of photons from the wavelength
E=Lhfenergy of a mole of photons from the frequency
K=\frac{[C]^c[D]^d}{[A]^a[B]^b}equilibrium constant for aA + bB ⇌ cC + dD
\text{pH}=-\log_{10}[\text{H}_3\text{O}^+]pH
\text{pOH}=-\log_{10}[\text{OH}^-]pOH
K_w=[\text{H}_3\text{O}^+][\text{OH}^-]ionic product of water
\text{pH}+\text{pOH}=14pH and pOH together
\text{p}K_a=-\log_{10}K_apKa from Ka
\text{pH}=\frac{1}{2}\text{p}K_a-\frac{1}{2}\log_{10}cpH of a weak acid of concentration c
\text{pH}=\text{p}K_a-\log_{10}\frac{[\text{acid}]}{[\text{salt}]}pH of a buffer
K_{In}=\frac{[\text{H}_3\text{O}^+][\text{In}^-]}{[\text{HIn}]}indicator dissociation constant
\text{pH}=\text{p}K_{In}\pm1indicator colour change range
\Delta H^{\circ}=\sum\Delta H_f^{\circ}(\text{products})-\sum\Delta H_f^{\circ}(\text{reactants})enthalpy change from enthalpies of formation
\Delta S^{\circ}=\sum S^{\circ}(\text{products})-\sum S^{\circ}(\text{reactants})entropy change
\Delta G^{\circ}=\sum\Delta G_f^{\circ}(\text{products})-\sum\Delta G_f^{\circ}(\text{reactants})free energy change from free energies of formation
\Delta G^{\circ}=\Delta H^{\circ}-T\Delta S^{\circ}free energy change

Physical constants and properties of water

Data in the booklet

TableWhat it gives
Names, symbols, relative atomic masses and densitiesOne row per element
Melting and boiling points of selected elementsIn degrees Celsius
Covalent radii of selected elementsValues for selected elements
Electron arrangements of elementsThe arrangement for each element
Formulae of selected ions with more than one kind of atomFormula and charge
Solubilities of selected compounds in waterWhich combinations of ions dissolve
Melting and boiling points of selected oxides, chlorides and organic compoundsThree tables, in degrees Celsius
Enthalpies of formation and combustion of selected substancesValues for selected substances
Selected bond and mean bond enthalpiesBond enthalpy values
Enthalpy of sublimation of carbonOne value
Ionisation energies and electronegativities of selected elementsSuccessive ionisation energies and electronegativity values
Electrochemical seriesStandard reduction potentials
Electrolysis of waterData for the electrolysis of water
Dissociation constants of selected speciesDissociation constants
Acid-base indicatorsData for each indicator
Infra-red correlation tableAbsorptions for particular bonds, as wavenumbers
Spectral lines and flame coloursWavelengths and colours
Proton NMR correlation chartChemical shifts for hydrogen in different environments
Ionic radii of selected ionsValues for selected ions
Standard entropy values for selected substancesValues for selected substances
Colour wheelA wheel of colours
SI units, SI prefixes and conversion factorsUnits, multipliers, and litre and kelvin conversions

The Advanced Higher specification says the Planck constant and the Avogadro constant are given in the data booklet, as are the characteristic infra-red absorptions and the chemical shifts for ¹H in different environments.

What is not in the Advanced Higher Chemistry data booklet

  • The theory. The booklet does not explain why infra-red absorbs at a wavenumber or why a proton has a chemical shift. You must interpret a spectrum.
  • Which relationship to use. A question on free energy, equilibrium or a buffer does not say which equation applies.
  • Rate equations and orders. The relationships page has no rate equation, so learn how to find the order from data.
  • Units and conversions between them. You must convert kJ and J, and litres and cm³.
  • Mechanisms and reagents. Organic synthesis, mechanisms and the reagents for each step are from your knowledge.
  • Structure determination method. The booklet has tables, and you work out the structure from them.

The course specification says a data booklet containing relevant data and formulae is provided.

How the paper uses the booklet

The specification gives the question paper 100 marks and 2 hours 30 minutes, with 25 marks of multiple choice and 75 of written answers, and the project 25 marks. In the 2027 timetable the exam is on Friday 21 May from 09:00 to 11:30 (Exam Timetable 2027, version 02). Our Advanced Higher Chemistry guide covers the course and the grades. For the Higher level view of the same booklet, see the Higher Chemistry data booklet guide.

Using the booklet under exam pressure

Free energy and spontaneity

A reaction has ΔH° = −92 kJ/mol and ΔS° = −199 J/K/mol at 298 K. Is it feasible? Convert the entropy to kJ first: −0.199 kJ/K/mol.

\Delta G^{\circ}=\Delta H^{\circ}-T\Delta S^{\circ}=-92-298\times(-0.199)=-92+59.3=-32.7\ \text{kJ mol}^{-1}

ΔG° is negative, so the reaction is feasible at this temperature. If you left ΔS in joules you would get −92 + 59,302, which is far too big.

pH of a weak acid

A weak acid has pKa = 4.8 and a concentration of 0.10 mol/l. The weak acid relationship gives

\text{pH}=\frac{1}{2}\text{p}K_a-\frac{1}{2}\log_{10}c=\frac{1}{2}(4.8)-\frac{1}{2}\log_{10}0.10=2.4+0.5=2.9

Energy of a mole of photons

A mole of photons of light with wavelength 450 nm has energy E = Lhc ÷ λ. With L, h and c from the booklet and λ = 4.50 × 10⁻⁷ m:

E=\frac{6.02\times10^{23}\times6.63\times10^{-34}\times3.00\times10^{8}}{4.50\times10^{-7}}=2.66\times10^{5}\ \text{J mol}^{-1}

That is 266 kJ/mol. Practise using a rate equation in the Reaction Kinetics course, then press Mark.

Use rate = k[A] or k[A] squared to work out a rate or the rate constant.

Press Mark to have your answer marked in the Reaction Kinetics course.

Exam answers

The answers and a worked mark scheme come with today's paper once it is marked. Sit the paper with the sheet open beside you, mark it, and the worked answers show which line each question wanted. We do not publish official or past paper answers.

Use the sheet with today's paper

Uni-Sine publishes a free daily paper for Advanced Higher Chemistry. It is a short timed paper of 8 questions worth 25 to 35 marks, not a full SQA paper and not set by SQA. Many schools set a longer prelim in winter: see our prelims guide. Open the sheet, set a timer, and write the line you use at the start of each answer.

Common mistakes

  • Mixing kJ and J in ΔG. Convert the entropy to kJ per kelvin per mole before you use T∆S.
  • Using Celsius for T. Convert to kelvin: add 273.
  • Wrong sign in the buffer equation. Check that more acid than salt gives a pH below the pKa.
  • Misreading the IR table. Match the wavenumber of the peak to the bond in the table.
  • Forgetting the Avogadro constant. Energy per mole needs L, and energy per photon does not.

Common questions

Do you get a data booklet in Advanced Higher Chemistry?
Yes. The specification says a data booklet containing relevant data and formulae is provided with the question paper.
Is the Advanced Higher Chemistry data booklet the same as the Higher one?
Yes. Qualifications Scotland publishes one booklet, titled Higher and Advanced Higher.
Are the IR and NMR tables in the data booklet?
Yes. The booklet has an infra-red correlation table and a proton NMR correlation chart.
Are the free energy equations given?
Yes. The relationships page has the enthalpy, entropy and free energy changes, and ΔG = ΔH − TΔS.
When is the Advanced Higher Chemistry exam in 2027?
Friday 21 May 2027, from 09:00 to 11:30.

Revision cards

Say the answer first, then flip the card to check it.

Where to go next

  • Solve it

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    Use Hess's law and bond enthalpies to find energy changes

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  • Learn it

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    Rates, catalysts and collision theory: what makes reactions fast or slow

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Scotland · Advanced HigherAdvanced Higher Chemistry: 2027 Exam Guide and PracticeAdvanced Higher Chemistry explained: the shorter 2027 exam, the project, the data booklet, 2026 grade boundaries, the topics and worked practice questions.