The enthalpy change when 1 mole of a compound is formed from its elements in their standard states under standard conditions
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Enthalpy of atomisation
The enthalpy of atomisation of an element is the enthalpy change when 1 mole of gaseous atoms is formed from the element in its standard state
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Bond dissociation enthalpy
The bond dissociation enthalpy is the standard molar enthalpy change when one mole of a covalent bond is broken into two gaseous atoms (or free radicals)
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Enthalpy of sublimation
The enthalpy change for a solid metal turning to gaseous atoms can also be called the Enthalpy of sublimation and will numerically be the same as the enthalpy of atomisation
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First Ionisation energy
The first ionisation energy is the energy required to remove 1 mole of electrons from 1 mole of gaseous atoms to form 1 mole of gaseous ions with a +1 charge (under standard conditions)
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Second Ionisation energy
The second ionisation energy is the energy required to remove 1 mole of electrons from one mole of gaseous 1+ ions to produces one mole of gaseous 2+ ions.
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First Electron affinity
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 (under standard conditions)
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Second electron affinity
The second electron affinity is the enthalpy change when one mole of gaseous 1- ions gains one electron per ion to produce gaseous 2- ions.
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Enthalpy of lattice formation
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 (under standard conditions).
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Enthalpy of lattice dissociation
The Enthalpy of lattice dissociation is the standard enthalpy change when 1 mole of an ionic crystal lattice is separated into its constituent ions in gaseous form (under standard conditions).
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How is Bond dissociation enthalpy altered for a Diatomic molecule?
The Bond dissociation enthalpy is twice the Enthalpy of atomisation of the element
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Enthalpy of Hydration
Enthalpy change when one mole of gaseous ions become hydrated (dissolved in water).
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Enthalpy of Solution
The enthalpy of solution is the standard enthalpy change when one mole of an ionic solid dissolves in an large enough amount of water to ensure that the dissolved ions are well separated and do not interact with one another
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Card 2
Front
Enthalpy of atomisation
Back
The enthalpy of atomisation of an element is the enthalpy change when 1 mole of gaseous atoms is formed from the element in its standard state
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