1.8- Thermodynamics

The enthalpy of atomisation of an element is the enthalpy change when 1 mole of gaseeous atom is formed from the element in its standard state

The enthalpy change for a solid metal turning to gaseous atoms can also be called enthalpy of sublimation and will numerically be the same as the enthalpy of atomisation

The bond dissociation enthalpy is the standard molar enthalpy change when one mole of a covalent bond is broked into two gaseous atoms

For diatomic molecules the enthalpy of dissociation of the molecule is the same as 2x enthalpy of atomisation for an element

The first ionisation enthalpy is the enthalpy change required to remove 1 mole of electrons from 1 mole of gaseous atoms to form 1 mole of gaseous ions with a 1+ charge

The second ionisation is the enthalpy change to remove 1 mole of electrons from one mole of gaseous 1+ ions to produce one mole of gaseuous 2 + ions

The first electron affinity is the enthalpy change that occurs when 1 mole of gaseous atoms gain 1 mole of electrons to form 1 mole of gaseous ions with a -1 charge, also this is exothermic for ions that normally form negative ions

The second electron affinity is the enthalpy change when one mole of gaseous 1- ions gains one electron per ion to produce 2- ions, this is endothermic because it takes energy to overcome the repulsive force between the negative ion and the electron

The enthalpy of lattice formation is the standard enthalpy change when 1 mole of an ionic crystal lattice is formed from its constituent ions in gaseous form

The enthalpy of lattice dissociation is the standard enthalpy change when 1 mole of an ionic crystal lattice form is seperated into its constituent ions in gaseous form

Enthalpy change when one mole of gaseous ions become aqueous ions, this is always exothermic because bonds made between the ions and the water molecules

The enthalpy of solution is the standard enthalpy change when one mole of ionic solid dissolves in a large enough amount of water to ensure that the dissolved ions are well seperated and do not interact with one another

. Size of ions- The larger the ions, the less negative the enthalpies of lattice formation, as the ions become larger charges get further apart and have weaker attractive force . The charges of an ion- The bigger the charge of the ion, the greater the attraction between the ions so the stronger the lattice enthalpy values

Theoretical lattice enthalpies assumes a perfect ionic model where the ions are 100% ionic and spherical and the attraction are purely electrostatic

. When the positive ion is small . The positive ion has multiple charges . The negative ion is large . The negative ion has multiple negative charges

The charge cloud gets distorted, the theoretical and experimental born haber values are different

. The enthalpy of lattice formation for Ca+ and Cl- is not that endothermic as the charges are not that big . The enthalpy of lattice formation for Ca2+ and Cl- is more endothermic as the charge of the calcium is greater, the lattice formed is more stable . For the Ca3+ there is a very big increase in enthalpy to remove the 3rd electron from the Ca, this would not be compensated for by the stronger lattice enthalpy of formation, this would meen that the enthalpy of formation is then endothermic which is not feasible

Entropy is a description of the number of ways atoms can share energy, if there is a large number of ways for arranging the energy then the system is disorded and the entropy is high

If there is a change of state from solid or liquid to gas There is a significant increase in the number of molecules between the products and the reactants

Entropy = Entropy of products - Entropy of reactants

Gibbs = ^H - T^S Make sure you convert the J into KJ

If there is an increase in entropy then increasing temperature will make it more likely that G is negative and more likely that the reaction will occur

^H solution = ^H dissociation + ^H hydration (sum) ^H solution= -^H formation + ^H hydration (sum)

Exothermic becuase negative ions are electrostatically attracted to the + H ions on the polar water molecules, positive ions are attracted to -O also The higher the charge density the larger the hydration enthalpy, as the ions attract water molecules more strongly