Chemistry F235

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  • Created by: Georgina
  • Created on: 05-01-13 20:17
Enthalpy change of formation
enthalpy change when 1 mole of a substance is formed from its constituent elements in their standard states under standard conditions
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enthalpy change of atomistaion
enthalpy change when 1 mole of gaseous atoms are formed from the constituent elements in their standard states under standard conditions
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Enthalpy change of first ionisation
enthalpy change when 1 mole of gaseous 1+ ions are formed from 1 mole of gaseous atoms under standard conditions
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enthalpy change of first electron affinity
enthalpy change when 1 mole of gaseous 1- ions are formed from 1 mole of gaseous atoms under standard conditions
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standard enthalpy change of hydration
the enthalpy change when 1 mole of aqueous ions are formed from 1 mole of gaseous ions
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standard enthalpy change of neutralisation
enthalpy change when 1 mole of water is formed form a acid and base reacting under standard conditions
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standard enthalpy change of atomisation( 2nd version)
enthalpy change when 1 mole of gaseous atoms are formed from a compound in its standard state under standard conditions
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standard enthalpy change of solution
enthalpy change when 1 mole of a solute is dissolved in sufficient solvent till no further enthalpy change occurs
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Average bond enthalpy
- enthalpy change when 1 mole of covalent bonds in gaseous molecules are broken under standard conditions
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activation energy
the minimum amount of energy required for a reaction to take place
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Hess's law
the total enthalpy change of a system is independent to the route taken provided the initial and final conditions are the same
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lattice enthalpy
the enthalpy change that accompanies the formation of 1 mole of a ionic compound from its constituent gaseous ions
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rate of reaction
change in concentration of reactant and product per unit time
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rate equation
shows how the rate of reaction is affected by a change in concentration of each reactant
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rate constant
relates the rate of reaction to the concentration of each reactant
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buffer solutions
resist change in PH by maintaining a near constant PH by removing any extra added acid or alkali
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entropy
level of disorder within a system
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standard electrode potential
the potential difference between a standard hydrogen electrode and half cell under standard
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standard cell potential
the voltage formed when two half cells are connected together under standard condition
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dynamic equilibrium
rate of the forward reaction = the rate of ther reverse
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le chatliers principle
when a system at equilibrium is subject to a change the position of equilibrium shifts to minimise the effect of that change
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reversible reaction
when the reactants react t form the products and the products rereact to form the reactants
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bronsted lowry acid
proton donor
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bronsted lowry base
proton acceptor
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strong acid
fully ionises in aqueous solution
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weak acid
partially ionises in aqueous solution
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ligand
molecule or ions that donates a pair of electrons to form a co-ordinate bond with the central transition metal ion
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complex ion
central transition metal ion surrounded by ligands
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transition metal
d-block element which has at least one stable ion with a incomplete d-orbital
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electrochemical cell
two half cells connected together
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enantiomers
stereo isomers that are non-super-imposable mirror images of each other
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Other cards in this set

Card 2

Front

enthalpy change of atomistaion

Back

enthalpy change when 1 mole of gaseous atoms are formed from the constituent elements in their standard states under standard conditions

Card 3

Front

Enthalpy change of first ionisation

Back

Preview of the front of card 3

Card 4

Front

enthalpy change of first electron affinity

Back

Preview of the front of card 4

Card 5

Front

standard enthalpy change of hydration

Back

Preview of the front of card 5
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