Cambridge AS and A Level Chemistry (9701) Syllabus

Chemistry (9701) syllabus — full chapter and topic list

Expand any chapter to see its topics and sub-topics. This is the whole examinable outline for Chemistry (9701) in Cambridge AS and A Level, not a summary of it.

1. 1

   Atomic Structure

   2 topics

   • Particles in the atom
   • Electronic configuration
2. 2

   Atoms, Molecules and Stoichiometry

   3 topics

   • Relative masses and the mole
   • Empirical and molecular formulae
   • Reacting masses and volumes
3. 3

   Chemical Bonding

   4 topics

   • Ionic, covalent and metallic bonding
   • Shapes of molecules and VSEPR
   • Intermolecular forces
   • Electronegativity and polarity
4. 4

   States of Matter

   2 topics

   • Gases and the ideal gas equation
   • Bonding and structure of solids
5. 5

   Chemical Energetics

   4 topics

   • Enthalpy changes
   • Hess's law and energy cycles
   • Bond energies
   • Lattice energy and Born-Haber cycles
6. 6

   Electrochemistry

   3 topics

   • Redox and oxidation numbers
   • Electrolysis
   • Electrode potentials
7. 7

   Equilibria

   4 topics

   • Chemical equilibrium and Le Chatelier's principle
   • Equilibrium constants Kc and Kp
   • Acids, bases and pH
   • Solubility product Ksp
8. 8

   Reaction Kinetics

   3 topics

   • Rate of reaction and collision theory
   • Catalysis
   • Rate equations and order of reaction
9. 9

   The Periodic Table

   4 topics

   • Periodicity of physical and chemical properties
   • Group 2 elements
   • Group 17 halogens
   • Transition elements
10. 10

    Organic Chemistry

    7 topics

    • Formulae, functional groups and isomerism
    • Hydrocarbons
    • Halogenoalkanes
    • Alcohols, esters and carboxylic acids
    • Carbonyl compounds
    • Nitrogen compounds
    • Polymerisation
11. 11

    Analytical Techniques

    3 topics

    • Test-tube reactions and qualitative analysis
    • Chromatography
    • Spectroscopy

Chemistry (9701) flashcards for Cambridge AS and A Level

25 of 50 cards from the Chemistry (9701) deck — real questions with worked answers.

1. What are the three subatomic particles in an atom, and what is the relative charge of each?

   Proton (+1), neutron (0), and electron (-1).

2. State the relative masses of a proton, neutron and electron.

   Proton = 1, neutron = 1, electron = 1/1836 (approximately 0).

3. Define the atomic (proton) number, Z.

   The number of protons in the nucleus of an atom.

4. Define the mass (nucleon) number, A.

   The total number of protons and neutrons in the nucleus of an atom.

5. 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).

6. How is the number of neutrons in an atom calculated?

   Number of neutrons = mass number (A) - atomic number (Z).

7. 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).

8. 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).

9. 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.

10. Write the full electronic configuration of an iron atom (Z = 26).

    1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁶ 4s².

11. State Hund's rule for filling orbitals.

    Electrons occupy orbitals of the same energy (degenerate orbitals) singly with parallel spins before pairing up.

12. 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.

13. 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.

14. 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.

15. 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.

16. 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).

17. 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.

18. State the formula relating number of moles, mass and molar mass.

    Moles (n) = mass (m) / molar mass (M).

19. How is the Ar of an element calculated from mass spectrometry data?

    Ar = Σ(isotopic mass × relative abundance) / Σ(relative abundances).

20. Chlorine has isotopes 35 (75%) and 37 (25%). Calculate its relative atomic mass.

    (35 × 75 + 37 × 25) / 100 = (2625 + 925) / 100 = 35.5.

21. Define the empirical formula of a compound.

    The formula showing the simplest whole-number ratio of atoms of each element in a compound.

22. Define the molecular formula of a compound.

    The formula showing the actual number of atoms of each element in one molecule of a compound.

23. 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.

24. 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.

25. State the formula linking concentration, moles and volume of a solution.

    Concentration (mol dm⁻³) = moles / volume (dm³).

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