Yes, you get a periodic table in AQA A Level Chemistry (7405) exams. It is in the AQA Data Booklet, an insert given out with every paper, which also contains infrared absorption data, ¹H and ¹³C NMR chemical shift data and a data sheet of biological structures. You do not need to memorise the table, but you do need to know the periodic trends and the chemistry of Period 3, Group 2, Group 7 and the transition metals, which run through both years of the course and are examined mainly in Paper 1. Lift College teaches AQA A Level Chemistry online with a named UK tutor for £49.99 a month when you pay today, or £59.99 a month after a 7-day free trial; see the A Level Chemistry course.
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Need the actual periodic table?
The periodic table you use in the exam is in the AQA A Level Chemistry Data Booklet, which AQA hands out as an insert with each paper. Download it free from AQA's website and revise with the same layout you will see in the exam. If you sit OCR or Pearson Edexcel A Level Chemistry, use that board's own data booklet; the chemistry is the same but the layout and extra data differ. For the GCSE version, see our GCSE periodic table guide, and for the marks each grade needed in June 2026, our A Level grade boundaries guide.
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| What is in the AQA Data Booklet | Use it for |
|---|---|
| Periodic table | Relative atomic masses, atomic numbers and element positions |
| Table A: infrared absorption data | Identifying bonds from an IR spectrum |
| Table B: ¹H NMR chemical shift data | Proton NMR questions |
| Table C: ¹³C NMR chemical shift data | Carbon 13 NMR questions |
| Data sheet | Structures such as phosphate and sugars, bases and amino acids |
What does the AQA A-level Chemistry specification say about the periodic table?
AQA A-level Chemistry (specification code 7405) organises its periodic table content into several distinct topic areas that build progressively from AS level through to the full A-level. Understanding the structure of the specification helps you plan your revision and ensures you cover every examinable area.
Year 1 / AS-level periodic table content
- Periodicity: trends across Period 3 in atomic radius, first ionisation energy, melting point and electrical conductivity
- Group 2 (alkaline earth metals): reactions of the elements and their oxides, hydroxides and carbonates with water and acids; uses of Group 2 compounds in medicine and agriculture (calcium carbonate, magnesium hydroxide)
- Group 7 (halogens): trends in physical properties; reactions of halide ions as reducing agents; disproportionation of chlorine; uses of chlorine in water treatment; halogen displacement reactions
Year 2 / A2-level periodic table content
- Period 3 oxides: reactions of Na2O, MgO, Al2O3, SiO2, P4O10 and SO3 with water; acid-base character across the period
- Transition metals (3d block): electronic configurations, variable oxidation states, formation of coloured ions, catalytic behaviour, complex ion formation, ligand substitution and the chemistry of iron, copper, cobalt and other d-block elements
- Reactions of ions in aqueous solution: precipitation reactions, amphoteric hydroxides, and the use of aqueous ammonia as a ligand
Always cross-reference the AQA Chemistry specification document (7405) directly on the AQA website to confirm the exact sub-topics and required practicals for your examination series. Specifications can be updated between cohorts.
How is the periodic table examined in AQA A-level Chemistry?
AQA A-level Chemistry is assessed entirely by written examination; there is no coursework component. The three papers are sat at an approved examination centre. Paper 1 (Inorganic and Physical Chemistry) is 2 hours and 105 marks, and includes all inorganic (periodic table) topics plus relevant physical chemistry. Paper 2 (Organic and Physical Chemistry) is 2 hours and 105 marks, covering organic chemistry plus further physical chemistry. Paper 3 (Practical and Synoptic Chemistry) is 2 hours and 90 marks, with synoptic questions drawing on the whole specification, including data analysis.
Alongside the three papers, AQA requires students to complete a minimum of 12 required practical activities. These are assessed separately by your teacher and reported as a pass/fail endorsement on your certificate; they do not contribute to your A to E grade. Required practicals relevant to the periodic table include the preparation of inorganic compounds and qualitative analysis of ions.
What are the key periodic table trends you need to know for AQA A-level?
Examiners regularly test your ability to explain trends, not just recall them. Below are the most frequently examined patterns.
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| Trend | Across a period (→) | Down a group (↓) | One-line reason (what the examiner wants) |
|---|---|---|---|
| Atomic radius | Decreases | Increases | Across: more protons, same shielding, stronger pull. Down: extra shells outweigh nuclear charge. |
| First ionisation energy | Increases (dips at Al and S) | Decreases | Across: greater nuclear charge, smaller radius. Dips: new p-subshell (Al); paired-electron repulsion (S). |
| Electronegativity | Increases | Decreases | Same nuclear-charge/radius logic; F is the most electronegative element. |
| Melting point (Period 3) | Rises Na→Si, falls sharply Si→S₈/P₄, lowest at Ar | - | Metallic bonding strengthens Na→Al; Si is giant covalent (peak); simple molecular after. |
Atomic radius
Atomic radius decreases across a period (left to right) because the number of protons increases while electrons are added to the same shell, increasing the effective nuclear charge pulling electrons inward. Atomic radius increases down a group because each successive period adds a new electron shell, increasing the distance between the nucleus and the outermost electrons.
First ionisation energy
First ionisation energy generally increases across a period due to greater nuclear charge and smaller atomic radius. There are two notable dips in Period 2 and Period 3: between Group 2 and Group 3 (the Group 3 electron is in a higher-energy p sub-shell, which is easier to remove than the Group 2 s electron), and between Group 5 and Group 6 (the Group 6 electron is paired in a p orbital, and electron-electron repulsion makes it easier to remove than the unpaired Group 5 electron).
Electronegativity
Electronegativity increases across a period and decreases down a group, following the same logic as ionisation energy. Fluorine is the most electronegative element on the Pauling scale.
Melting points across Period 3
Na, Mg and Al form giant metallic lattices; melting points increase (more delocalised electrons, stronger metallic bonding). Si forms a giant covalent lattice with a very high melting point (strong covalent bonds throughout). P, S, Cl and Ar exist as simple molecular or monatomic species with low melting points (only weak van der Waals forces between molecules).
What do you need to know about Group 2 for AQA A-level?
Group 2 (the alkaline earth metals) is a heavily examined section of the AQA inorganic chemistry content. Reactivity increases down the group because ionisation energies decrease as atomic radius increases, so electrons are lost more easily. Reactivity with water also increases from magnesium (reacts slowly with steam) to barium (vigorous reaction with cold water), producing a metal hydroxide and hydrogen gas.
Solubility trends are important: the solubility of Group 2 hydroxides increases down the group (Mg(OH)2 is sparingly soluble; Ba(OH)2 is soluble), while the solubility of Group 2 sulphates decreases down the group (MgSO4 is soluble; BaSO4 is insoluble and used in barium meals for medical imaging). Thermal decomposition of carbonates requires higher temperatures further down the group, explained by the polarising power of the smaller cations.
What do you need to know about Group 7 (the halogens) for AQA A-level?
Group 7 content tests both descriptive chemistry and your ability to write and balance equations. Boiling points increase down the group due to stronger London dispersion forces as molecular mass increases. Oxidising power decreases down the group; fluorine is the strongest oxidising agent and iodine is the weakest, which explains halogen displacement reactions.
The reducing power of halide ions increases down the group. Chloride ions are poor reducing agents; iodide ions can reduce concentrated H2SO4 to H2S. When chlorine dissolves in water or reacts with cold dilute NaOH, it undergoes disproportionation (simultaneously oxidised and reduced); this is the basis of water chlorination and the manufacture of bleach. Tests for halide ions use acidified silver nitrate solution, producing white (AgCl), cream (AgBr) or yellow (AgI) precipitates, confirmed by solubility in ammonia solution.
What do you need to know about transition metals for AQA A-level?
Transition metal chemistry forms a substantial part of the Year 2 content and is examined in Paper 1.
Why are transition metals different from other d-block elements?
AQA defines a transition metal as a d-block element that forms at least one stable ion with an incomplete d sub-shell. This is why scandium (Sc) and zinc (Zn) are d-block elements but are not classified as transition metals under the AQA definition; Sc3+ has an empty d sub-shell and Zn2+ has a full d sub-shell.
Key properties to revise
- Variable oxidation states: d electrons are close in energy to 4s electrons; multiple oxidation states are accessible
- Coloured ions: d-d electron transitions absorb visible light; the colour observed is the complementary colour
- Catalytic activity: variable oxidation states allow transition metals to accept and donate electrons in reaction mechanisms (Fe in the Haber process, MnO4- as an oxidising agent)
- Complex ion formation: transition metal ions act as Lewis acids, accepting lone pairs from ligands (H2O, NH3, Cl-, CN-)
Ligand substitution and colour changes
A classic AQA exam question asks you to describe what happens when aqueous ammonia or concentrated hydrochloric acid is added to a transition metal complex. Adding excess NH3 to [Cu(H2O)6]2+ (pale blue) produces [Cu(NH3)4(H2O)2]2+ (deep blue), a ligand substitution reaction. Adding concentrated HCl to [Cu(H2O)6]2+ produces [CuCl4]2- (yellow-green), both a ligand substitution and a change in coordination number (6 to 4).
How should you revise the periodic table for AQA A-level Chemistry?
Effective revision of this topic combines understanding with practice. Use the specification as a checklist: download the AQA Chemistry specification (7405) and tick off each bullet point as you can confidently explain it. Draw and annotate periodic table diagrams: sketching trends (ionisation energy graphs, solubility trend tables) by hand reinforces memory.
Write equations for every reaction; AQA mark schemes award marks for balanced equations. Practise past papers under timed conditions; AQA publishes mark schemes and examiner reports that highlight the most common errors. Focus on explain questions; the periodic table section is rich in 6-mark extended-response questions asking you to explain trends using atomic structure and bonding.
AQA A-level Chemistry at a glance: citable facts
Subject: Chemistry. Exam board: AQA. Specification code: 7405 (A-level); 7404 (AS-level). Typical study duration: 2 years full-time; flexible timeline with online study. Assessment: 3 written papers (no coursework) plus practical endorsement (pass/fail). Grading scale: A* to E (A-level); A to E (AS-level).
UCAS points (A-level): A* = 56, A = 48, B = 40, C = 32, D = 24, E = 16. Exams sat at: an approved external examination centre. Entry requirements at Lift College: no formal academic entry requirements; you will need a reasonable level of prior science study (typically GCSE grade 6 or above in the relevant sciences) to access the course materials. Facilitating subject: yes, Chemistry is a Russell Group facilitating subject.
For current course fees, see our A-level courses page.
Frequently asked questions
Is the periodic table a big part of AQA A-level Chemistry?
Yes. Periodic table content, including periodicity, Group 2, Group 7 and transition metals, runs throughout both years of the AQA Chemistry specification and is examined primarily in Paper 1 (Inorganic and Physical Chemistry). It is one of the most consistently examined topic areas and typically accounts for a significant proportion of Paper 1 marks.
Do I need to memorise the periodic table for AQA A-level?
You are not required to memorise the entire periodic table. AQA provides a Data Booklet in the examination that includes the periodic table, infrared and NMR data and a data sheet. However, you are expected to know the positions and properties of the elements discussed in the specification (particularly Groups 1, 2, 7 and the Period 3 and transition metal elements) well enough to answer questions without needing to look up basic facts.
What are the hardest periodic table topics in AQA A-level Chemistry?
Based on AQA examiner reports, students most commonly lose marks on: explaining the two dips in the first ionisation energy graph across Period 2/3; writing correct equations for the reactions of Period 3 oxides with water; explaining colour changes in transition metal complex ion reactions; and distinguishing between ligand substitution and redox reactions in transition metal chemistry. For how Chemistry compares with other subjects, see the hardest A-levels ranked.
Can I study AQA A-level Chemistry online?
Yes. Lift College offers an A-level Chemistry online course through AQA, delivered entirely online with tutor support. You study at your own pace and sit your examinations at an approved external examination centre. This makes it suitable for adult learners, career changers, home-educators and students resitting to improve their grades.
How long does it take to complete AQA A-level Chemistry online?
A typical full-time student completes A-level Chemistry over two academic years. Most learners complete the course in 12 to 18 months studying at their own pace with Lift College, subject to exam series availability.
What grade do I need in A-level Chemistry for medicine or pharmacy?
Entry requirements vary by university and course. Most medical schools in the UK require an A or A* in A-level Chemistry, often alongside Biology and/or Mathematics. Pharmacy degrees typically require at least a B or A in Chemistry. Always check the specific entry requirements on each university's admissions page and on UCAS, as requirements change annually. Lift College's course can help you work towards the grade you need, but Lift College does not guarantee any specific grade.
Does the AQA A-level Chemistry practical endorsement affect my grade?
No, the practical endorsement is reported separately on your certificate as either a pass or a not-classified result. It does not contribute numerically to your A* to E grade. However, some universities do ask for a pass in the practical endorsement as part of their conditional offer, so it is important to complete the required practicals. On Lift College's +Exams & CPAC plan the practical endorsement is booked for you at a Tutors & Exams laboratory venue.
What is the difference between AQA A-level Chemistry and AS-level Chemistry?
AQA AS-level Chemistry (specification 7404) covers the Year 1 content only and is assessed by two papers. It is a standalone qualification carrying UCAS tariff points on the AS scale (up to 20 at grade A). The full A-level (specification 7405) covers both Year 1 and Year 2 content and is assessed by three papers. AS results no longer count towards the full A-level grade under the current linear qualification structure.
Does Lift College offer AQA A-level Chemistry?
Yes. Lift College delivers A-level Chemistry through AQA. For full course details, including the syllabus overview and current fees, see the A-level courses page.
What is first ionisation energy?
First ionisation energy is the energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous 1+ ions. It is always endothermic, and the AQA definition must include the gaseous state to earn the mark.
Why does ionisation energy increase across a period?
Nuclear charge increases while electrons enter the same shell, so shielding stays roughly constant and atomic radius shrinks. The outer electron is held more strongly and needs more energy to remove - with dips at aluminium (new 3p subshell) and sulfur (paired-electron repulsion).
Why does ionisation energy decrease down a group?
Each element down a group adds a full electron shell, so the outer electron is further from the nucleus and better shielded. These effects outweigh the increased nuclear charge, so the outer electron is easier to remove.
Why is the second ionisation energy higher than the first?
The second electron is removed from a 1+ ion, where the remaining electrons feel a greater effective nuclear pull and the ion is smaller. A very large jump between successive ionisation energies signals a change of shell - a classic AQA question for identifying an element's group.
Is the A Level Chemistry data booklet the same for every exam board?
No. Each exam board provides its own data booklet with its own layout and extra data, so revise with your own board's version.
What is in the AQA A Level Chemistry data booklet?
The periodic table, infrared absorption data, ¹H NMR and ¹³C NMR chemical shift data, and a data sheet of structures including phosphate, sugars, bases and amino acids.
Where can I download the AQA A Level Chemistry periodic table?
From the AQA website, where the AQA A Level Chemistry (7405) Data Booklet is a free PDF. It is the same booklet you are given in the exam.
Ready to take the next step? Explore AQA A-level Chemistry at Lift College or contact our advisors to discuss the right route for your goals.
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