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Summary lattice enthalpy and entropy, born haber cycles chemistry notes £3.06   Add to cart
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  7. A2 Unit F325 - Equilibria, Energetics and Elements

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Summary lattice enthalpy and entropy, born haber cycles chemistry notes

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summary notes on lattice enthalpy, born-haber cycles, enthalpy of solution, entropy and free energy and feasibility. including example calculations and diagrams from the textbook

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  • Chapter 22
  • June 9, 2024
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  • 2023/2024
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Lattice enthalpy
Formation of 1 mole of ionic lattice from its gaseous ions under standard conditions

Exothermic: ionic bond formation

To measure the strength of ionic bonding in a giant ionic lattice

Ionic size

Increases :

Attraction btw ions decreases

= ΔₗₑH less negative

Ionic charge

Increases:

attraction between ions increases

= ΔₗₑH more negative

Enthalpy changes of :

, 2

Atomisation: formation of 1 mole of gaseous atoms from elements in their standard
states under standard conditions

Endothermic: intermolecular forces broken to form gaseous atoms



1st ionisation energy:

Endothermic: energy is put in to overcome the attraction between the negative electron
and positive nucleus

1st electron affinity: 1 electron added to each atom in 1 mol of gaseous atoms to form 1
mol of gaseous 1- ions

Exothermic: electron being added is attracted to the positive nucleus

2nd electron affinity:

Endothermic: 2nd electron being added is repelled by the anion = energy is put in to
force the negative electron onto the negative ion (that already gained an electron)


Born-Haber cycles
● Δ𝑓H = sum of the known enthalpy changes

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