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Inorganic Chemistry Summary
- Institution
- AQA
Summary of 1 pages for the course Unit 3.2.5 - Transition metals at AQA (Summary notes)
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- Lattice enthalpy of dissociation (ΔHlatt) = The energy required to break apart an ioniclattice into its constituent ions in a gaseous state under standard conditions
- Lattice enthalpy of formation (ΔHlatt) = The energy required to form an ionic lattice
from its constituent ions in a gaseous state under standard conditions
- Atomisation Enthalpy (ΔHat) = The energy required for the formation of a mole of
gaseous atoms under standard conditions
- Enthalpy of Electron Affinity (ΔHea) = The enthalpy change when one mole of electrons
is added to a mole of gaseous atoms under standard conditions
- Enthalpy of Solution (ΔHsol) = The enthalpy change when one mole of ionic solid is
dissolved in water to infinite dilutions so that the ions no longer interact under
standard conditions
- Enthalpy of Hydration (ΔHhyd) = The enthalpy change when one mole of gaseous ions
is dissolved in water to form one mole of aqueous ions under standard conditions
- Hess’s Law = The enthalpy change for a reaction is independent of the route taken
- Enthalpy of Formation = The enthalpy change when one mole of a compound is
formed from its constituent elements with all reactants and products in their standard
states and under standard conditions
- Enthalpy of Combustion = The enthalpy change when one mole of a substance is
completely burnt in oxygen with all reactants and products in their standard states and
under standard conditions
- First ionisation Energy = Enthalpy change when one mole of electrons is removed from
one mole of gaseous atoms to form one mole of gaseous 1+ ions
- Second Ionisation Energy = Enthalpy change when one mole of electrons is removed
from one mole of gaseous 1+ ions to form one mole of gaseous 2+ ions
- First electron affinity = Enthalpy change when one mole of gaseous atoms gains one
mole of electrons to form one mole of gaseous 1- ions
- Second electron affinity = Enthalpy change when one mole of gaseous 1- ions gains
one mole of electrons to from one mole of gaseous 2- ions
- Mean Bond dissociation enthalpy = Enthalpy change when one mole of covalent
bonds is broken, with all species in the gaseous state
- Equations:
Q=mcΔt
ΔH = Products – Reactants
ΔH = Bonds broken – Bonds Made
ΔG = AH - TΔS
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