What this topic covers
The syllabus points for Topic 2, with every question in the bank filed under exactly one of them. Each opens the bank filtered to that point.
- 2.1Elements, compounds and mixtures34 questions
- Describe the differences between elements, compounds and mixtures
- 2.2Atomic structure and the Periodic Table164 questions
- Describe the structure of the atom as a central nucleus containing neutrons and protons surrounded by electrons in shells
- State the relative charges and relative masses of a proton, a neutron and an electron
- Define proton number / atomic number as the number of protons in the nucleus of an atom
- Define mass number / nucleon number as the total number of protons and neutrons in the nucleus of an atom
- Determine the electronic configuration of elements and their ions with proton number 1 to 20, e.g. 2,8,3
- State that: (a) Group VIII noble gases have a full outer electron shell (b) the number of outer shell electrons is equal to the group number in Groups I to VII (c) the number of occupied electron shells is equal to the period number
- 2.3Isotopes93 questions
- Define isotopes as different atoms of the same element that have the same number of protons but different numbers of neutrons
- Interpret and use symbols for atoms, e.g. 6 12C, and ions, e.g. 17 35Cl –
- State that isotopes of the same element have the same chemical properties because they have the same number of electrons and therefore the same electronic configuration
- Calculate the relative atomic mass of an element from the relative masses and abundances of its isotopes
- 2.4Ions and ionic bonds100 questions
- Describe the formation of positive ions, known as cations, and negative ions, known as anions
- State that an ionic bond is a strong electrostatic attraction between oppositely charged ions
- Describe the formation of ionic bonds between elements from Group I and Group VII, including the use of dot-and-cross diagrams
- Describe the properties of ionic compounds: (a) high melting points and boiling points (b) good electrical conductivity when aqueous or molten and poor when solid
- Describe the giant lattice structure of ionic compounds as a regular arrangement of alternating positive and negative ions
- Describe the formation of ionic bonds between ions of metallic and non-metallic elements, including the use of dot-and-cross diagrams
- Explain in terms of structure and bonding the properties of ionic compounds: (a) high melting points and boiling points (b) good electrical conductivity when aqueous or molten and poor when solid
- 2.5Simple molecules and covalent bonds96 questions
- State that a covalent bond is formed when a pair of electrons is shared between two atoms leading to noble gas electronic configurations
- Describe the formation of covalent bonds in simple molecules, including H2, Cl 2, H2O, CH4, NH3 and HCl. Use dot-and-cross diagrams to show the electronic configurations in these and similar molecules
- Describe in terms of structure and bonding the properties of simple molecular compounds: (a) low melting points and boiling points (b) poor electrical conductivity
- Describe the formation of covalent bonds in simple molecules, including CH3OH, C2H4, O2, CO2 and N2. Use dot-and-cross diagrams to show the electronic configurations in these and similar molecules
- Explain in terms of structure and bonding the properties of simple molecular compounds: (a) low melting points and boiling points in terms of weak intermolecular forces (specific types of intermolecular forces are not required) (b) poor electrical conductivity
- 2.6Giant covalent structures96 questions
- Describe the giant covalent structures of graphite and diamond
- Relate the structures and bonding of graphite and diamond to their uses, limited to: (a) graphite as a lubricant and as an electrode (b) diamond in cutting tools
- Describe the giant covalent structure of silicon(IV) oxide, SiO2
- Describe the similarity in properties between diamond and silicon(IV) oxide, related to their structures
- 2.7Metallic bonding46 questions
- Describe metallic bonding as the electrostatic attraction between the positive ions in a giant metallic lattice and a ‘sea’ of delocalised electrons
- Explain in terms of structure and bonding the properties of metals: (a) good electrical conductivity (b) malleability and ductility
Learning objectives from the Cambridge 0620 syllabus 2026–28:CoreSupplement (Extended only)
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