Cambridge IGCSE Chemistry (0620) Syllabus

Chemistry (0620) syllabus — full chapter and topic list

Expand any chapter to see its topics and sub-topics. This is the whole examinable outline for Chemistry (0620) in Cambridge IGCSE, not a summary of it.

1. 1

   States of Matter and Atomic Structure

   3 topics

   • Particulate nature of matter
     • Solids, liquids and gases
     • Diffusion and changes of state
   • Atomic structure
     • Protons, neutrons and electrons
     • Electronic configuration
     • Isotopes and relative atomic mass
   • The Periodic Table
     • Groups, periods and trends
     • Group I alkali metals and Group VII halogens
     • Transition elements and noble gases
2. 2

   Bonding and Stoichiometry

   3 topics

   • Chemical bonding
     • Ionic bonding and lattices
     • Covalent bonding and molecules
     • Metallic bonding
   • Formulae and equations
     • Writing formulae and balancing equations
     • Ionic equations and state symbols
   • The mole concept
     • Relative molecular mass and the mole
     • Calculations from equations
     • Percentage yield and purity
3. 3

   Chemical Reactions and Energetics

   5 topics

   • Rates of reaction
     • Effect of concentration, temperature and surface area
     • Catalysts and collision theory
   • Reversible reactions and equilibrium
     • Reversible reactions
     • Le Chatelier's principle
   • Energy changes
     • Exothermic and endothermic reactions
     • Energy level diagrams and bond energies
   • Redox reactions
     • Oxidation and reduction in terms of electrons
     • Oxidation states and oxidising agents
   • Electrochemistry
     • Electrolysis of molten and aqueous compounds
     • Hydrogen-oxygen fuel cells
4. 4

   Acids, Bases and the Chemistry of Elements

   3 topics

   • Acids, bases and salts
     • Properties of acids and bases
     • pH scale and indicators
     • Preparation of soluble and insoluble salts
   • Metals
     • Reactivity series
     • Extraction of metals
     • Corrosion and alloys
   • Chemical analysis
     • Tests for ions and gases
     • Chromatography
5. 5

   Organic and Environmental Chemistry

   4 topics

   • Fuels and the air
     • Fossil fuels and combustion
     • Air pollution and the greenhouse effect
   • Introduction to organic chemistry
     • Homologous series and functional groups
     • Isomerism and naming
   • Hydrocarbons and reactions
     • Alkanes and alkenes
     • Alcohols and carboxylic acids
     • Cracking and addition reactions
   • Polymers
     • Addition polymerisation
     • Condensation polymers and plastics

Chemistry (0620) flashcards for Cambridge IGCSE

18 of 70 cards from the Chemistry (0620) deck — real questions with worked answers.

1. What are the three states of matter, and how do their particle arrangement and movement differ?

   Solid: particles packed in a regular fixed arrangement, vibrating about fixed positions. Liquid: particles close together but irregular, sliding past one another. Gas: particles far apart, random, fast movement. Order of energy/spacing: solid < liquid < gas.

2. Define diffusion and state how relative molecular mass affects its rate.

   Diffusion is the net movement of particles from a region of higher concentration to a region of lower concentration due to random motion. Lighter molecules (lower $M_r$) diffuse faster than heavier ones at the same temperature.

3. Name the six changes of state between solid, liquid and gas.

   Melting (solid$\to$liquid), freezing (liquid$\to$solid), boiling/evaporation (liquid$\to$gas), condensation (gas$\to$liquid), sublimation (solid$\to$gas), and deposition (gas$\to$solid).

4. What does Brownian motion provide evidence for?

   The random motion of tiny particles (e.g. smoke specks seen jiggling) provides evidence that matter is made of small particles in constant random motion, being bombarded by even smaller, invisible particles (gas molecules).

5. What are the relative charges and relative masses of a proton, neutron and electron?

   Proton: charge $+1$, mass $1$. Neutron: charge $0$, mass $1$. Electron: charge $-1$, mass $\frac{1}{1840}$ (negligible).

6. Define proton number (atomic number) and nucleon number (mass number).

   Proton number $Z$ is the number of protons in the nucleus. Nucleon number $A$ is the total number of protons plus neutrons. Number of neutrons $= A - Z$.

7. What are isotopes? Give the standard notation for an atom.

   Isotopes are atoms of the same element with the same proton number but different numbers of neutrons (different nucleon numbers). Notation: $^{A}_{Z}\text{X}$, e.g. $^{12}_{6}\text{C}$.

8. How is relative atomic mass ($A_r$) calculated from isotopic abundances?

   $A_r = \dfrac{\sum(\text{isotope mass} \times \%\text{abundance})}{100}$. It is the weighted average mass of the isotopes relative to $\frac{1}{12}$ of a carbon-12 atom.

9. State the electronic configuration of a chlorine atom (proton number 17).

   $2,8,7$ — two electrons in the first shell, eight in the second, seven in the outer (valence) shell.

10. How does the group number and period number relate to electronic structure?

    The group number equals the number of outer-shell (valence) electrons; the period number equals the number of occupied electron shells.

11. How are the elements arranged in the modern Periodic Table?

    In order of increasing proton (atomic) number, in horizontal rows called periods and vertical columns called groups, so that elements with similar properties (same number of outer electrons) fall in the same group.

12. Describe the trends in properties of Group I (alkali metals) down the group.

    Going down Group I: reactivity increases, density generally increases, and melting point decreases. They are soft metals that react with water to form alkaline hydroxides and hydrogen, e.g. $\ce{2Na + 2H2O -> 2NaOH + H2}$.

13. Describe the trends in properties of Group VII (halogens) down the group.

    Going down Group VII: colour darkens, density increases, melting/boiling point increases, and reactivity decreases. A more reactive halogen displaces a less reactive one from its salt, e.g. $\ce{Cl2 + 2KBr -> 2KCl + Br2}$.

14. What are the characteristic properties of the transition elements?

    They are hard, dense metals with high melting points; form coloured compounds; show variable oxidation states (valencies); and act as catalysts (e.g. iron in the Haber process).

15. Why are the Group VIII (Group 0) noble gases unreactive?

    They have a full (stable) outer electron shell — eight outer electrons (two for helium) — so they have little tendency to gain, lose or share electrons. They are monatomic, unreactive gases.

16. How does ionic bonding form, and in what type of elements?

    Ionic bonding is the electrostatic attraction between oppositely charged ions formed by the transfer of electrons from a metal to a non-metal. The metal loses electrons (forms cations) and the non-metal gains them (forms anions), e.g. $\ce{Na+}$ and $\ce{Cl-}$ in $\ce{NaCl}$.

17. What is a covalent bond, and between which kinds of atoms does it form?

    A covalent bond is a shared pair of electrons between two atoms, formed between non-metal atoms. Each shared pair counts toward both atoms' outer shells, allowing each to reach a noble-gas configuration.

18. Compare the properties of ionic compounds and simple molecular covalent compounds.

    Ionic: high melting/boiling points, conduct when molten or in solution, often soluble in water. Simple molecular: low melting/boiling points (weak intermolecular forces), do not conduct electricity, usually insoluble in water but soluble in organic solvents.

See more Chemistry (0620) flashcards →

Planning Chemistry (0620) for Cambridge IGCSE

Chemistry (0620) (Cambridge IGCSE) FAQ