A pair of two species that transform into each other by gain or loss of a proton
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Bronstead-Lowry acid
A species that is a proton donor
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Bronstead-Lowry base
A species that is a proton. acceptor
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Buffer solution
A system that minimises pH changes on addition of small amounts of acid or base
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Complex ion
A transition metal ion bonded to ligands by coordinate bonds
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Conjugate acid
A species that releases a proton to form a conjugate base
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Conjugate base
A species that accepts a proton to form a conjugate acid
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Coordination number
The total number of coordinate bonds formed between a central metal ion and ligands
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End point
The point in a titration where the indicator changes colour; the end point indicates when the reaction is just complete
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Entropy
Used for the dispersal of energy and disorder within the chemicals making up the chemical system
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Equivalence point
The point in a titration at which the volume of one solution has reacted exactly with the volume of the second solution
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First electron affinity
The enthalpy change that takes place when one electron is added to each atom in one mole of gaseous atoms to form one mole of gaseous 1- ions
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First ionisation energy
The energy required to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ atoms
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Free energy change
The balance between enthalpy, entropy and temperature for a process
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Half life
The time taken for the concentration of a reactant to decrease by half
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Initial rate of reaction
The change in concentration of a reactant or product per unit time at the start of the reaction
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Lattice enthalpy
The enthalpy change that accompanies the formation of one mole of an ionic compound from its gaseous ions under standard conditions
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Ligand
A molecule or ion that can donate a pair of electrons to a transition metal ion
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Ligand substitution
A reaction in which one or more ligands in a complex ion are replaced by different ligands
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Order
The power to which the concentration of a reactant is raised in the rate equation
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Overall order
The sum of all the orders of reactants in the rate equation
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Precipitation reaction
The formation of a solid from a solution during a chemical reaction
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Rate determining step
The slowest step in the reaction mechanism of a multi step reaction
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Second electron affinity
The enthalpy change that takes place when one electron is added to each ion in one mole of gaseous 1- ions to form one mole of gaseous 2- ions
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Second ionisation energy
The energy required to remove one electron from each ion in one mole of gaseous 1+ ions of an element to from one mole of gaseous 2+ ions
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Standard electrode potential
The e.m.f of a half cell compared with a standard hydrogen half cell at standard conditions
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Standard enthalpy change of atomisation
The enthalpy change that takes place when one mole of gaseous atoms forms from the element in its standard state
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Standard enthalpy change of formation
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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Standard enthalpy change of hydration
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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Standard enthalpy change of solution
The enthalpy change that takes place when one mole of a compound is completely dissolved in water under standard conditions
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Transition element
A d-block element which forms an ion with an incomplete d sub-shell
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Other cards in this set
Card 2
Front
A species that is a proton donor
Back
Bronstead-Lowry acid
Card 3
Front
A species that is a proton. acceptor
Back
Card 4
Front
A system that minimises pH changes on addition of small amounts of acid or base
Back
Card 5
Front
A transition metal ion bonded to ligands by coordinate bonds
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