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Cambridge AS and A Level Chemistry (9701) Syllabus
The Chemistry (9701) syllabus for Cambridge AS and A Level in full: 11 chapters and 39 topics, every one listed below, plus 50 Chemistry (9701) flashcards with answers.
Chemistry (9701) syllabus: all 11 chapters
Expand any chapter to see its topics and sub-topics.
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Atomic Structure
2 topics- Particles in the atom
- Electronic configuration
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Atoms, Molecules and Stoichiometry
3 topics- Relative masses and the mole
- Empirical and molecular formulae
- Reacting masses and volumes
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Chemical Bonding
4 topics- Ionic, covalent and metallic bonding
- Shapes of molecules and VSEPR
- Intermolecular forces
- Electronegativity and polarity
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States of Matter
2 topics- Gases and the ideal gas equation
- Bonding and structure of solids
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Chemical Energetics
4 topics- Enthalpy changes
- Hess's law and energy cycles
- Bond energies
- Lattice energy and Born-Haber cycles
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Electrochemistry
3 topics- Redox and oxidation numbers
- Electrolysis
- Electrode potentials
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Equilibria
4 topics- Chemical equilibrium and Le Chatelier's principle
- Equilibrium constants Kc and Kp
- Acids, bases and pH
- Solubility product Ksp
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Reaction Kinetics
3 topics- Rate of reaction and collision theory
- Catalysis
- Rate equations and order of reaction
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The Periodic Table
4 topics- Periodicity of physical and chemical properties
- Group 2 elements
- Group 17 halogens
- Transition elements
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Organic Chemistry
7 topics- Formulae, functional groups and isomerism
- Hydrocarbons
- Halogenoalkanes
- Alcohols, esters and carboxylic acids
- Carbonyl compounds
- Nitrogen compounds
- Polymerisation
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Analytical Techniques
3 topics- Test-tube reactions and qualitative analysis
- Chromatography
- Spectroscopy
Cambridge AS and A Level Chemistry (9701) flashcards — 50 questions with answers
What are the three subatomic particles in an atom, and what is the relative charge of each?
Proton (+1), neutron (0), and electron (-1).
State the relative masses of a proton, neutron and electron.
Proton = 1, neutron = 1, electron = 1/1836 (approximately 0).
Define the atomic (proton) number, Z.
The number of protons in the nucleus of an atom.
Define the mass (nucleon) number, A.
The total number of protons and neutrons in the nucleus of an atom.
What are isotopes?
Atoms of the same element with the same number of protons but different numbers of neutrons (same atomic number, different mass number).
How is the number of neutrons in an atom calculated?
Number of neutrons = mass number (A) - atomic number (Z).
How do isotopes of an element differ in their physical and chemical properties?
They have identical chemical properties (same electronic configuration) but slightly different physical properties (e.g. density, due to different masses).
State the order in which the first four sub-shells (s, p, d) fill, including the 4s/3d anomaly.
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p (4s fills before 3d).
What is the maximum number of electrons that an s, p, d and f sub-shell can each hold?
s = 2, p = 6, d = 10, f = 14.
Write the full electronic configuration of an iron atom (Z = 26).
1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁶ 4s².
State Hund's rule for filling orbitals.
Electrons occupy orbitals of the same energy (degenerate orbitals) singly with parallel spins before pairing up.
What shape is an s orbital and what shape is a p orbital?
An s orbital is spherical; a p orbital is dumb-bell shaped.
When forming ions, from which sub-shell are electrons removed first in transition elements like iron?
The 4s electrons are removed before the 3d electrons.
Define relative atomic mass (Ar).
The weighted average mass of an atom of an element relative to 1/12 the mass of an atom of carbon-12.
Define relative isotopic mass.
The mass of an atom of a particular isotope relative to 1/12 the mass of an atom of carbon-12.
Define relative molecular mass (Mr).
The weighted average mass of a molecule relative to 1/12 the mass of an atom of carbon-12 (the sum of the relative atomic masses of all atoms in the molecule).
What is the value of the Avogadro constant and what does it represent?
6.02 × 10²³ mol⁻¹; the number of particles in one mole of a substance.
State the formula relating number of moles, mass and molar mass.
Moles (n) = mass (m) / molar mass (M).
How is the Ar of an element calculated from mass spectrometry data?
Ar = Σ(isotopic mass × relative abundance) / Σ(relative abundances).
Chlorine has isotopes 35 (75%) and 37 (25%). Calculate its relative atomic mass.
(35 × 75 + 37 × 25) / 100 = (2625 + 925) / 100 = 35.5.
Show the other 30 Chemistry (9701) flashcards
Define the empirical formula of a compound.
The formula showing the simplest whole-number ratio of atoms of each element in a compound.
Define the molecular formula of a compound.
The formula showing the actual number of atoms of each element in one molecule of a compound.
How do you determine an empirical formula from percentage composition by mass?
Divide each element's percentage (or mass) by its Ar to get moles, then divide all by the smallest value to get the simplest whole-number ratio.
A compound has empirical formula CH₂ and Mr = 42. What is its molecular formula?
Empirical mass = 14; 42/14 = 3, so molecular formula is C₃H₆.
State the formula linking concentration, moles and volume of a solution.
Concentration (mol dm⁻³) = moles / volume (dm³).
What is the molar gas volume at room temperature and pressure (r.t.p.)?
24 dm³ (24000 cm³) per mole of any gas at r.t.p.
How is the number of moles of a gas calculated from its volume at r.t.p.?
Moles = volume (dm³) / 24 (or volume in cm³ / 24000).
Define percentage yield.
Percentage yield = (actual amount of product / theoretical amount of product) × 100.
What is the limiting reagent in a reaction?
The reactant that is completely used up first, which therefore determines the maximum amount of product formed.
Define an ionic bond.
The electrostatic attraction between oppositely charged ions, formed by the transfer of electrons from a metal to a non-metal.
Define a covalent bond.
A shared pair of electrons between two atoms, where the shared electrons are attracted to both nuclei.
Define a dative (coordinate) covalent bond.
A covalent bond in which both shared electrons are provided by one atom.
Define metallic bonding.
The electrostatic attraction between positive metal ions and a sea of delocalised electrons.
Why do metals conduct electricity and are malleable?
Delocalised electrons are free to move and carry charge; layers of ions can slide over one another without breaking the metallic bonding.
State the main idea of VSEPR theory.
Electron pairs around a central atom repel each other and arrange themselves as far apart as possible to minimise repulsion, determining molecular shape.
What is the shape and bond angle of a molecule with 4 bonding pairs and no lone pairs (e.g. CH₄)?
Tetrahedral, with a bond angle of 109.5°.
What is the shape and bond angle of ammonia (NH₃, 3 bonding pairs and 1 lone pair)?
Pyramidal (trigonal pyramidal), with a bond angle of about 107°.
What is the shape and bond angle of water (H₂O, 2 bonding pairs and 2 lone pairs)?
Bent (non-linear), with a bond angle of about 104.5°.
What are the shapes and bond angles for 2, 3, 5 and 6 bonding pairs (no lone pairs)?
2 = linear (180°), 3 = trigonal planar (120°), 5 = trigonal bipyramidal (90° and 120°), 6 = octahedral (90°).
Rank the repulsion strengths of lone pair (lp) and bonding pair (bp) interactions.
lp–lp > lp–bp > bp–bp (lone pairs repel more strongly, reducing bond angles).
List the three types of intermolecular forces in order of increasing strength.
Van der Waals (London dispersion) forces < permanent dipole-dipole forces < hydrogen bonding.
What causes van der Waals (London dispersion) forces?
Temporary instantaneous dipoles caused by the random movement of electrons, which induce dipoles in neighbouring molecules.
What three conditions are required for hydrogen bonding?
Hydrogen bonded to a highly electronegative atom (N, O or F), and a lone pair on the N, O or F of a neighbouring molecule.
Why does ice have a lower density than liquid water?
Hydrogen bonds hold water molecules in an open, ordered lattice in ice, so the molecules are spaced further apart than in liquid water.
Define electronegativity.
The ability of an atom to attract the bonding (shared) pair of electrons in a covalent bond towards itself.
How does electronegativity vary across a period and down a group?
It increases across a period (left to right) and decreases down a group.
Why is CO₂ a non-polar molecule even though it has polar bonds?
It is linear and symmetrical, so the two bond dipoles act in opposite directions and cancel out, giving no overall dipole.
State the ideal gas equation and define each term with its SI unit.
pV = nRT, where p = pressure (Pa), V = volume (m³), n = moles, R = gas constant (8.31 J K⁻¹ mol⁻¹), T = temperature (K).
Why does graphite conduct electricity but diamond does not?
In graphite each carbon forms 3 bonds, leaving one delocalised electron per atom free to move; in diamond all 4 outer electrons are used in covalent bonds, leaving none free.
Define standard enthalpy change of formation (ΔHf°) and standard enthalpy change of combustion (ΔHc°).
ΔHf°: enthalpy change when one mole of a compound is formed from its elements in their standard states under standard conditions. ΔHc°: enthalpy change when one mole of a substance is completely burned in oxygen under standard conditions.
Cambridge AS and A Level Chemistry (9701) FAQ
What is in the Cambridge AS and A Level Chemistry (9701) syllabus?
Cambridge AS and A Level Chemistry (9701) is split into 11 chapters: Atomic Structure, Atoms, Molecules and Stoichiometry, Chemical Bonding, States of Matter, Chemical Energetics, Electrochemistry, Equilibria, Reaction Kinetics, The Periodic Table, Organic Chemistry and Analytical Techniques. Together they contain 39 topics.
How many chapters are in Cambridge AS and A Level Chemistry (9701)?
11 chapters, containing 39 topics. The largest chapter is Organic Chemistry, with 7 topics.
Are there flashcards for Cambridge AS and A Level Chemistry (9701)?
Yes — a 50-card Chemistry (9701) deck, printed in full in the flashcards section of this page and available in the Examius app with spaced repetition. The free plan covers one exam of your choice, including its flashcards; Examius Pro, a one-time purchase, unlocks every other exam and deck.