Lattice Enthalpy
- Created by: Jennifer Chalk
- Created on: 22-02-16 18:37
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- Lattice Enthalpy
- Features
- Lattice enthalpy is an exothermic change Energy is given out when ionic bonds are being formed from gasous ions.
- Lattice enthalpy indicates the strength of an ionic lattice and is a measure of the ionic bond strength.
- Covalent structure do not have a lattice enthalpy.
- It cannot be measured directly as its impossible to form one mole of an ionic lattice from gaseous ions.
- Key defintions
- Lattice enthalpy is the enthalpy change that accompanies the formation of one mole of ionic compound form its gaseous ions under standard conditions
- Hess' law states that if a reaction can take place by more than one route and the initial and final conditions are the same, the total enthalpy change is the same for each route
- Key enthalpy changes
- The standard enthalpy of formation, one mole of a compound is formed from its constituent elements in their standard states. K(s) + 1/2Cl2(g) -> KCl(s)
- The standard enthalpy change of atomisation, one mole of gaseous atoms is formed from its element in its standard state. K(s) -> K(g)
- The first ionisation energy, one mole of gaseous 1+ ions is formed from gaseous atoms. Is an endothermic process because the electron lost has to overcome the attraction from the nucleus. K(g)-> K+(g) + e-
- The first electron affinity, one mole of gaseous 1- ions is formed from gaseous atoms. Cl(g) + e- -> Cl-(g)
- Features
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