Assessment Statements4.1 Ionic bonding 4.1.1: Describe the ionic bond as the electrostatic attraction between oppositely charged ions. 4.1.2: Describe how ions can be formed as a result of ionic transfer. 4.1.3:Deduce which ions will be formed when elements in groups 1,2,3 lose electrons. 4.1.4: Deduce which ions will be formed when elements in groups 5,6, and 7 gain electrons. 4.1.5: State that transition elements can form more than one ion. 4.1.6: Predict whether a compound of two elements would be ionic from the position of the elements in the periodic table or negativity values. 4.1.7: State the formula of common polyatomic ions formed by non-metals in periods 2 and 3. 4.1.8: Describe the lattice structure of ionic compounds. 4.2 Covalent bonding 4.2.1: Describe the covalent bond as the electrostatic attraction between a pair of electrons and positively charged nuclei. 4.2.2: Describe how the covalent bond is formed as a result of electron sharing. 4.2.3: Deduce the Lewis (electron dot) structures of molecules and ions for up to four pairs of electrons on each atom. 4.2.4: State and explain the relationship between the number of bonds, bond length, and bond strength. 4.2.5: Predict whether a compound of two elements would be covalent from the position of the elements in the periodic table or from their electronegativity values. 4.2.6: Predict the relative polarity of bonds from electronegativity values. 4.2.7: Predict the shape and bond angles for species with four, three and two negative charge centres on the central atom using the valence shell pair repulsion theory (VESPR). 4.2.8: predict whether or not a molecule is polar from its molecular shape and bond polarities. 4.2.9: Describe and compare the structure and bonding in the three allotropes of carbon (diamond, graphite, fullerene). 4.2.10: Describe the structure of and bonding in silicon and silicon dioxide. 4.3 Intermolecular forces 4.3.1: Describe the types of intermolecular forces and explain how they arise from the structural features of molecules. 4.3.2: Describe and explain how intermolecular forces affect the boiling points of substances. 4.4 Metallic bonding 4.4.1: Describe the metallic bond as the electrostatic attraction between a lattice of positive ions and delocalized ions. 4.4.2: Explain the electrical conductivity and malleability of metals. 4.5 Physical properties 4.5.1: Compare and explain the properties of substances resulting from different types of bonding. |
ResourcesList of keywords for this topicIonic bondingCovalent bondingGiant Covalent MoleculesMetallic BondingPolar MoleculesIntermolecular ForcesShapes of MoleculesExtra material for HL |