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lattice enthalpy
enthalpy change that accompanies formation of one mole of an ionic compound from its gaseous ions under standard condition
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Hess's Law
If a reaction can take place by more than one route and the initial and final conditions are the same, the total enthalpy change is the same for each route.
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Standard Enthalpy change of Formation
The enthalpy change when 1 mole of a compound is formed from its constituent elements, under standard conditions.
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Enthalpy change of Atomisation.
The enthalpy change when 1 mole of gaseous atoms forms from the element in its standard state.
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First ionisation energy
The enthalpy change from the removal of 1 electron from each atom in 1 mole of gaseous atoms to form 1 mole of gaseous +1 ions.
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Second ionisation energy.
The enthalphy change accompanying the removal of 1 electron from each ion in 1 mole of gaseous 1+ ions to form 1 mole of 2+ ions.
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First electron affinity
The enthalpy change accompanying the addition of 1 electron to each atom in mole of gaseous atoms to form 1 mole of gaseous 1- ions.
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Second electron affinity
The enthalpy change accompanying the addition of 1 electron to each ion in 1 mole of gaseous 1- ions to form 1 mole of gaseous 2- ions.
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Standard enthalpy change of solution
The enthalpy change when 1 mole of a compound is completely dissolved in water.
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As ionic radius increases...
The attraction between the ions decrease and the lattice enthalpy becomes less negetive.
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Entropy
The measure of the degree of disorder in a system.
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Free energy change
The balance between enthalpy, entropy and temperature. This is equivelant to -> Delta G = Delta H - Delta S * T
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Standard electrode potential of a half cell
The emf of a half cell compared with a standard hydrogen half cell under standard conditions.
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Three main types of cells
Non rechargeable, rechargeable and fuel
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How to store hydrogen
Stored as a liqud under pressure, adsorbed onto the surface of a solid and absorbed onto the surface of a material.
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Transition element
A d-block element that can form an ion with an incomplete d sub shell.
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Physical properties of transition metals.
Shiny, High Density, High Melting Point, High Boiling Point, contains delocalised electrons so can conduct electricity.
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Reaction between Co2+ + NaOH
Blue precipitate, turns beige in air. Forms Co(OH)2
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Reaction between Fe2+ + NaOH
Green --> Green precipitate --> Rusty brown in air. Forms Fe(OH)2
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Reaction between Fe3+ + NaOH
Yellow -->Rusty Brown precipitate. Forms Fe(OH)3
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Complex ion
A transition metal ion bonded to 1 or more ligands by coordinate bonds.
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Ligands
Molecule or ion that can donate a pair of electrons with a transition metla ion toform a coordinate bond.
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Coorditation number
The number of coordinate bonds between a central metal ion and its ligands.
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Bidentate ligand
Ligand can donate 2 lone pairs to the central metal ion to form to coordinate bonds.
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Yield
Actual amount ofproduct (mol) / theoretical of moles in product *100
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Other cards in this set

Card 2

Front

Hess's Law

Back

If a reaction can take place by more than one route and the initial and final conditions are the same, the total enthalpy change is the same for each route.

Card 3

Front

Standard Enthalpy change of Formation

Back

Preview of the front of card 3

Card 4

Front

Enthalpy change of Atomisation.

Back

Preview of the front of card 4

Card 5

Front

First ionisation energy

Back

Preview of the front of card 5
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