Cambrıdge Internatıonal (9701) & Edexcel

AS-Level Chemistry Topics
2025–2026 | Complete Syllabus

AS-Level Chemistry provides a solid foundation for A2-Level Chemistry and science-related university degrees. Full topic breakdown based on Cambridge (9701) and Edexcel specifications.

🧪 22+ Topics 📘 Cambridge 9701 📘 Edexcel 🎯 A2 Preparation
View All Topics ↓ Free AS Chemistry Consult →

In this guide

✓
Complete AS-Level topicsPhysical, inorganic, organic chemistry
✓
Detailed learning outcomesCambridge 9701 syllabus breakdown
✓
Exam structure & papersPaper 1 & 2 format, core practicals
✓
Path to A2-LevelTransition support
26 yearsChemistry teaching
METUGraduate
Cambridge & EdexcelSpecialist
FreeTrial lesson

📚 Physical Chemistry

Atomic structure, energetics, kinetics, equilibrium

🧪 Inorganic Chemistry

Periodicity, Group 2, Group 17, Nitrogen & Sulfur

🔬 Organic Chemistry

Hydrocarbons, halogen compounds, alcohols, carbonyls

📝 Exam Papers

Paper 1 + Paper 2 (1h30m each)
Cambrıdge AS-Level Chemıstry (9701)

Complete Topic List

Based on the Cambridge International AS-Level Chemistry syllabus (9701). These topics form the foundation for A2-Level Chemistry and university science courses.

1. Atoms, Molecules and Stoichiometry
2. Atomic Structure
3. Chemical Bonding
4. States of Matter
5. Chemical Energetics
6. Electrochemistry
7. Equilibria
8. Reaction Kinetics
9. The Periodic Table: Chemical Periodicity
10. Group 2
11. Group 17
12. Nitrogen and Sulfur
13. Organic Chemistry (Introduction)
14. Hydrocarbons
15. Halogen Compounds
16. Hydroxy Compounds
17. Carbonyl Compounds
18. Carboxylic Acids and Derivatives
19. Nitrogen Compounds
20. Polymerisation
21. Organic Synthesis
22. Analytical Techniques
Detaıled Learnıng Outcomes

Cambridge 9701 Syllabus Breakdown

Below are the complete learning outcomes for AS-Level Chemistry. Each topic includes specific objectives that students must master for examination success.

1. Atoms, Molecules and Stoichiometry

1.1 Particles in the atom and atomic radius

1 understand that atoms are mostly empty space surrounding a very small, dense nucleus that contains protons and neutrons; electrons are found in shells in the empty space around the nucleus
2 identify and describe protons, neutrons and electrons in terms of their relative charges and relative masses
3 understand the terms atomic and proton number; mass and nucleon number
4 describe the distribution of mass and charge within an atom
5 describe the behaviour of beams of protons, neutrons and electrons moving at the same velocity in an electric field
6 determine the numbers of protons, neutrons and electrons present in both atoms and ions given atomic or proton number, mass or nucleon number and charge
7 state and explain qualitatively the variations in atomic radius and ionic radius across a period and down a group

1.2 Isotopes

1 define the term isotope in terms of numbers of protons and neutrons
2 understand the notation for isotopes, where x is the mass or nucleon number and y is the atomic or proton number
3 state that and explain why isotopes of the same element have the same chemical properties
4 state that and explain why isotopes of the same element have different physical properties, limited to mass and density

1.3 Electrons, energy levels and atomic orbitals

1 understand the terms: shells, sub-shells and orbitals; principal quantum number (n); ground state
2 describe the number of orbitals making up s, p and d sub-shells, and the number of electrons that can fill s, p and d sub-shells
3 describe the order of increasing energy of the sub-shells within the first three shells and the 4s and 4p sub-shells
4 describe the electronic configurations to include the number of electrons in each shell, sub-shell and orbital
5 explain the electronic configurations in terms of energy of the electrons and inter-electron repulsion
6 determine the electronic configuration of atoms and ions given the atomic or proton number and charge
7 understand and use the electrons in boxes notation
8 describe and sketch the shapes of s and p orbitals
9 describe a free radical as a species with one or more unpaired electrons

1.4 Ionisation energy

1 define and use the term first ionisation energy, IE
2 construct equations to represent first, second and subsequent ionisation energies
3 identify and explain the trends in ionisation energies across a period and down a group of the Periodic Table
4 identify and explain the variation in successive ionisation energies of an element
5 understand that ionisation energies are due to the attraction between the nucleus and the outer electron
6 explain the factors influencing the ionisation energies of elements in terms of nuclear charge, atomic/ionic radius, shielding by inner shells and sub-shells and spin-pair repulsion
7 deduce the electronic configurations of elements using successive ionisation energy data
8 deduce the position of an element in the Periodic Table using successive ionisation energy data

2. Atomic Structure

2.1 Relative masses of atoms and molecules

1 define the unified atomic mass unit as one twelfth of the mass of a carbon-12 atom
2 define relative atomic mass, Ar, relative isotopic mass, relative molecular mass, Mr, and relative formula mass in terms of the unified atomic mass unit

2.2 The mole and the Avogadro constant

1 define and use the term mole in terms of the Avogadro constant

2.3 Formulas

1 write formulas of ionic compounds from ionic charges and oxidation numbers
2 write and construct balanced equations, including ionic equations, with state symbols
3 define and use the terms empirical and molecular formula
4 understand and use the terms anhydrous, hydrated and water of crystallisation
5 calculate empirical and molecular formulas, using given data

2.4 Reacting masses and volumes

1 perform calculations including use of the mole concept, involving reacting masses, volumes of gases, volumes and concentrations of solutions, limiting reagent and excess reagent
2 deduce stoichiometric relationships from calculations

3. Chemical Bonding

3.1 Electronegativity and bonding

1 define electronegativity as the power of an atom to attract electrons to itself
2 explain the factors influencing electronegativities
3 state and explain trends in electronegativity across a period and down a group
4 use differences in Pauling electronegativity values to predict the formation of ionic and covalent bonds

3.2 Ionic bonding

1 define ionic bonding as the electrostatic attraction between oppositely charged ions
2 describe ionic bonding including examples of sodium chloride, magnesium oxide and calcium fluoride

3.3 Metallic bonding

1 define metallic bonding as the electrostatic attraction between positive metal ions and delocalised electrons

3.4 Covalent bonding and coordinate bonding

1 define covalent bonding as electrostatic attraction between the nuclei of two atoms and a shared pair of electrons
2 describe covalent bonding in molecules including H₂, O₂, N₂, Cl₂, HCl, CO₂, NH₃, CH₄, C₂H₆, C₂H₄
3 describe coordinate (dative covalent) bonding, including in NH₄⁺ and Al₂Cl₆
4 describe covalent bonds in terms of orbital overlap giving σ and π bonds
5 use the concept of hybridisation to describe sp, sp² and sp³ orbitals
6 define bond energy and bond length

3.5 Shapes of molecules

1 state and explain the shapes of, and bond angles in, molecules using VSEPR theory (BF₃, CO₂, CH₄, NH₃, H₂O, SF₆, PF₅)

3.6 Intermolecular forces

1 describe hydrogen bonding, limited to N–H and O–H groups
2 use hydrogen bonding to explain anomalous properties of H₂O
3 describe van der Waals’ forces: instantaneous dipole–induced dipole and permanent dipole–permanent dipole forces

Note: Full detailed learning outcomes for Topics 4–22 (States of Matter, Chemical Energetics, Electrochemistry, Equilibria, Kinetics, Periodicity, Group 2, Group 17, Nitrogen & Sulfur, Organic Chemistry, Hydrocarbons, Halogen Compounds, Hydroxy Compounds, Carbonyl Compounds, Carboxylic Acids, Nitrogen Compounds, Polymerisation, Organic Synthesis, Analytical Techniques) follow the same Cambridge 9701 specification format. For the complete set, refer to the official syllabus or contact us for a detailed breakdown.

Assessment Structure

AS-Level Chemistry Exam Format

📘 Paper 1: Core Inorganic and Physical Chemistry (8CH0/01)

Topics: 1, 2, 3, 4, 5
Duration: 1h 30m
Marks: 80
At least 20% of the assessment tests mathematical skills. Some questions assess understanding of experimental methods.

📘 Paper 2: Core Organic and Physical Chemistry (8CH0/02)

Topics: 2, 5, 6, 7, 8, 9, 10
Duration: 1h 30m
Marks: 80
Same assessment details as Paper 1. Students must complete 8 core practicals, assessed indirectly in written papers.

🎯 Why These Topics Matter

Studying AS-Level Chemistry equips students with:

✓ A deep understanding of chemical concepts
✓ Ability to connect theory with real-world applications
✓ Preparation for A2-Level Chemistry, medicine, engineering, and natural sciences

📞 Strugglıng wıth the transıtıon from AS to A2?

Explore our support programme tailored to this syllabus. One-on-one guidance for both AS and A2-Level Chemistry.

Free Consultation →

📚 Related Resources

IGCSE Chemistry Hub → AS-Level Chemistry Topics → AP Chemistry Topics → IGCSE Chemistry Tutoring →
FAQ

Frequently Asked Questions

What is the difference between AS-Level and A2-Level Chemistry?

AS-Level covers the first half of the A-Level syllabus (typically Year 12). A2 builds on these topics with more advanced content, especially in organic and physical chemistry, and together they form the full A-Level qualification.

Which exam boards use these topics?

The content here is based on Cambridge International (9701) and Edexcel specifications, but overlaps significantly with OCR and AQA syllabuses as well.

Do I need AS-Level Chemistry for medical school?

Yes, most universities require Chemistry at A-Level (AS + A2) for medicine, dentistry, veterinary medicine, and related courses. A strong AS performance is essential for competitive applications.

How are core practicals assessed?

At AS Level, students complete 8 core practicals. These are not directly examined but are assessed indirectly through questions in Papers 1 and 2 that test understanding of experimental methods, data analysis, and practical techniques.

What is the best way to prepare for AS-Level Chemistry?

Master the syllabus systematically, practice past paper questions under timed conditions, understand examiner expectations, and address weak areas early. Personalised tutoring can help accelerate progress and target specific topics where students struggle.

🚀 Master AS-Level Chemistry with Expert Guidance

One-on-one online lessons with an ODTÜ graduate and 26 years of teaching experience. Cambridge & Edexcel specialist.

📞 Contact via WhatsApp 📅 Book a Free 40-Minute Trial Lesson

✔ 26 years experience | ✔ METU Graduate | ✔ Cambridge & Edexcel specialist | ✔ AS to A2 transition support

Scroll to Top