Definitions Unit 5

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Enthalpy of atomisation
Enthalpy change that accompanies the formation of one mole of gaseous atoms from the element in its standard state.
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Mean Bond Enthalpy
Enthalpy needed to break one mole of gaseous covalent bonds averaged over a range of compounds.
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Bond enthalpy
Enthalpy needed to break one mole of gaseous covalent bonds to form two moles of gaseous atoms.
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Enthalpy lattice of formation
Enthalpy change when one mole of an ionic solid is formed from its constituent gaseous ions.
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Enthalpy lattice dissociation
Enthalpy change when one mole of a solid ionic lattice is separated into gaseous ions.
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Electron affinity
Enthalpy change when one mole of gaseous atoms form one mole of gaseous negative ions.
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Enthalpy of solution
Enthalpy change when 1 mole of solute dissolves in sufficient solvent that no further enthalpy change occurs on further dilution.
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Enthalpy of Hydration
Enthalpy change when 1 mole of aqueous ions is formed from gaseous ions.
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Feasible/Spontaneous
A reaction that is possible because (Gibbs free energy)
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Perfect ionic model
Ions can be regarded as perfect spheres, Only electrostatic attraction.
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Standard conditions
298K, 100kPa and all solutions at 1.00 moldm-3
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Electrochemical series
A list of reduction half-equations in order of increasing or decreasing electrode potential.
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Periodicity
A trend in properties of the elements across a period, repeated across the next period.
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Hydrolysis
Splitting up of molecules by using water.
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Complex
A central metal ion surrounded by co-ordinately bonded ligands.
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Ligand
A species that can donate one or more lone pairs of electrons.
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Co-ordination number
Number of co-ordinate bonds formed in a complex (not just the number of ligands).
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Bidentate Ligand
Has two lone pair donor atoms.
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Active site
Place where reactants are adsorbed and where reaction occurs.
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Heterogeneous catalyst
A catalyst that is in a different state to the reactants.
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Homogeneous catalyst
A catalyst that is in the same state as the reactants.
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Lewis acid
Lone pair acceptor
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Lewis base
Lone pair donor
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Other cards in this set

Card 2

Front

Enthalpy needed to break one mole of gaseous covalent bonds averaged over a range of compounds.

Back

Mean Bond Enthalpy

Card 3

Front

Enthalpy needed to break one mole of gaseous covalent bonds to form two moles of gaseous atoms.

Back

Preview of the back of card 3

Card 4

Front

Enthalpy change when one mole of an ionic solid is formed from its constituent gaseous ions.

Back

Preview of the back of card 4

Card 5

Front

Enthalpy change when one mole of a solid ionic lattice is separated into gaseous ions.

Back

Preview of the back of card 5
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