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18 Cards in this Set
- Front
- Back
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Lattice Enthalpy
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The enthalpy change that accompanies the formation of one mole of an ionic compounds from its gaseous ions under standard conditions
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Standard enthalpy change of Formation
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The enthalpy change that takes place when one mole of a compound is formed from its constituent elements in their standard states under standard conditions
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Enthalpy change of atomisation
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The enthalpy change that takes place when one mole of gaseous atoms forms from the element in its standard state
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First ionisation energy
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The enthalpy change accompanying the removal of one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions
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Second ionisation energy
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The enthalpy change accompanying the removal of one electron from each ion in one mole of gaseous 1+ ions to form one mole of gaseous 2+ ions
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First electron affinity
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The enthalpy change accompanying the addition of one electron to each atom in one mole of gaseous atoms to form one mole of gaseous 1- ions (Exothermic, -ΔH)
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Second electron affinity
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The enthalpy change accompanying the addition of one electron to each ion in one mole of gaseous 1- ions to form one mole of gaseous 2- ions. (Endothermic, +ΔH)
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Standard enthalpy change of solution
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The enthalpy change that takes place when one mole of a compound is completely dissolved in water under standard conditions
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Standard enthalpy change of hydration
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The enthalpy change that takes place when one mole of isolated gaseous ions is dissolved in water forming one mole of aqueous ions under standard conditions
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Entropy
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The quantitative measure of the degree of disorder in a system
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Standard entropy change of reaction
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(ΔS) The entropy change that accompanies a reaction in the molar quantities expressed in a chemical equation under standard conditions, all reactants and products being in their standard states.
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Free energy change
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(ΔG) The balance between enthalpy, entropy and temperature for a process: ΔG = ΔH - TΔS
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ΔG =
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ΔH - TΔS (T is in Kelvin)
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When can a reaction take place spontaneously?
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When ΔG < 0
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Standard electrode potential
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The EMF of a half cell compared with a standard hydrogen half cell, measured at 298K with solution concentrations of 1 mol dm^-3 and a gas pressure of 100kPa
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ΔS =
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ΣS(products) - ΣS(reactants)
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When is a system more random?
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When ΔS is positive
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When is a system more ordered?
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When ΔS is negative
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