e.g.īorn-Haber cycle This is an application of Hess’s Law and can be used to calculate lattice energies. The standard molar lattice enthalpy is the energy required to convert one mole of a solid ionic compound into its constituent gaseous ions under standard conditions. Lattice enthalpy indicates the strength of the ionic bonds in an ionic lattice. For ionic compounds the corresponding enthalpy is the lattice enthalpy (also called the lattice energy). The attraction acts in all directions, resulting in a giant ionic lattice containing many ions. Ionic bonding is an electrostatic attraction between oppositely charged ions. Lattice Enthalpy Bond enthalpies provide a measure of the strength of covalent bonds. Explain, in qualitative terms, the effect of ionic charge and of ionic radius on the numerical magnitude of a lattice energy.Construct Born-Haber cycles to calculate the lattice enthalpy of a simple ionic solid e.g NaCl, MgCl2, using relevant energy terms (enthalpy changes of formation, ionisation energy, enthalpy of atomisation and electron affinity.Explain and use the term ‘lattice enthalpy’ as a measure of ionic bond strength.(Lattice enthalpy will be regarded as the enthalpy of lattice breaking) When you have finished this section you should be able to: CCEA ADVANCED SUBSIDIARY CHEMISTRY Taken from a dedicated CCEA source – Author unknown, but thank you! Older Specifications, but very similar MODULE 4ĮNERGETICS Simple treatment (including calculations) of the Born-Haber cycle for the halides of Group I and II.
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