Giant structures
Covalent bonding
Ionic bonding
Know the difference between an atom and an ion, and write equations
for how ions form
Use an elements position in the Periodic Table to predict the charge of
the ion it will form
Know the formulas of the common polyatomic ions, NO3-, CO32-,
SO42-, NH4+
Know that ionic bonding typically occurs between metals and non-metals
Describe what an ionic bond is in terms of electrostatic attraction
Know what factors affect the strength of an ionic bond
Be able to represent ionic compounds using dot-cross diagrams
Be able to work out the formulae of ionic compounds
Describe and draw a giant ionic lattice
Relate ionic structure to the following properties: electrical
conductivity, melting point, solubility in water
Understand how the terms ‘molecule’ and ‘compound’ differ
Know that covalent bonds typically form between non-metals
Know what a covalent bond is in terms of shared pairs of electrons
Be able to represent covalent substances using dot-cross diagrams,
including double bonds such as in O2 and CO2 (triple bond in N2)
Know that the valency rules are broken in some examples e.g. BF3, SF6
Explain the difference between a covalent and dative covalent
(coordinate) bonds, identifying and represent these accordingly.
Relate simple covalent structures to the following properties: electrical
conductivity, melting point
Describe a giant covalent or macromolecular structure
Understand the term ‘allotrope’
Understand and use the term ‘delocalised electrons’ correctly
Describe and draw the structure of diamond
Relate the structure of diamond to its properties
Describe and draw the structure of graphite
Relate the structure of graphite to its properties
Describe and draw metallic bonding
Relate the structure of metals to their properties
Discuss limitations of bonding models
Exam ques
Revised
): S: (:
STRUCTURE, BONDING, PERIODICTY
Covered
AS Chemistry – Unit 1
Shapes
Intermolecular forces
Periodicity
Know the names and bond angles of the basic molecular shapes
Be able to interpret and apply the electron pair repulsion theory
Identify and represent delocalised pairs of electrons, and know how
these affect shapes and bond angles e.g. CH4  NH3  H2O
Be able to use the above to determine the shape of an unknown
molecule
Be able to use the above to determine the shape of an unknown
polyatomic ion
Define the term ‘electronegativity’ and the effect on a bond
Be able to identify and represent a polar bond
Be able to explain what a van der Waal force is, using the terms
‘temporary dipole’ and ‘induced dipole’
Be able to identify and explain what a permanent dipole-dipole
interaction is
Be able to identify and explain why a Hydrogen bond can form with N,
O or F, representing this bonding using fully labelled diagrams
Explain the difference in strength between the three types of
intermolecular force e.g. between HF, HCl, HBr and HI
Be able to relate melting or boiling points to molecular size and van der
Waal forces e.g. Group 7 elements
Know that Covalent bonds do not break when a simple covalent
substance melts or boils
Know that elements in the modern Periodic Table are arranged in order
of increasing Atomic number (spot problems if using Mass number)
Write electronic configurations for the first 36 elements (Cr and Cu to
be memorised)
Explain why elements appear in the s, p or d block
Explain the trend in Atomic radius across Period 2 or 3
Explain the trend in first I.E. across Period 2 or 3
Explain the trend in first I.E. down a Group
Know that across Period 2, Li and Be are metallic, B is a metalloid,
C is macromolecular, N2, O2,F2 and Ne are simple covalent
Know that across Period 3, Na, Mg and Al are metallic, Si is
macromolecular, P4, S8, Cl2 and Ar are simple covalent
Complete a graph of melting or boiling points for Period 2 and 3
Explain the trend in melting or boiling point across Period 2 and 3,
linking to elemental structure and bond strength