difference between theoretical and experimental lattice enthalpy values

That means that for sodium chloride, the assumptions about the solid being ionic are fairly good. Haber cycle. A significant difference between the two values indicates covalent character. Discuss the difference between theoretical and experimental lattice enthalpy values of ionic compounds in terms of their covalent character. We can't use experimental ones, because these compounds obviously don't exist! The enthalpy change when 1 mol of an ionic lattice is formed from its series of steps.

. That immediately removes any possibility of confusion. I am going to start by drawing a Born-Haber cycle for sodium chloride, and then talk it through carefully afterwards.

There are two different ways of defining lattice enthalpy which directly contradict each other, and you will find both in common use. A significant difference between the two values indicates covalent character. You are always going to have to supply energy to break an element into its separate gaseous atoms. In fact, there is a simple way of sorting this out, but many sources don't use it. It gives a mathematical foundation for developing advanced concepts of probability. The fact that the theoretical values differ from the experimental (Born-Haber) values suggests that the bonding within the lattice is not purely ionic. the breaking up of the lattice (an endothermic - bond breaking process). We have a brilliant team of more than 60 Support Team members looking after discussions on The Student Room, helping to make it a fun, safe and useful place to hang out. Lattice enthalpies calculated in this way are described as experimental values. The +107 is the atomisation enthalpy of sodium. The third one comes from the 2p. You need to multiply the atomisation enthalpy of chlorine by 2, because you need 2 moles of gaseous chlorine atoms. In theory, the lattice enthalpy is based on purely ionic models. The two main factors affecting lattice enthalpy are the charges on the ions and the ionic radii (which affects the distance between the ions). The lattice energies for the alkali metal halides is therefore largest Lattice enthalpy is a measure of the strength of the forces between the ions in an ionic solid. The 3s electrons are screened from the nucleus by the 1 level and 2 level electrons. You could describe it as the enthalpy change when 1 mole of sodium chloride (or whatever) was formed from its scattered gaseous ions. as though the bonding changes its nature as the compound is heated and

Incidentally, if you are ever uncertain about which version is being used, you can tell from the sign of the enthalpy change being discussed. There is reasonable agreement between the experimental value (calculated from a Born-Haber cycle) and the theoretical value. The arrow pointing down from this to the lower thick line represents the enthalpy change of formation of sodium chloride. determined values and theoretically determined values is good.

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