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57 Cards in this Set
- Front
- Back
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Equilibrium law
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states that for equilibrium aA + bB ↔ Cc + dD Kc = [C]^c [D]^d / [A]^a [B]^b
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Dynamic equilibrium
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Exists in a closed system when the rate of the forward reaction is equal to the rate of the reverse reaction
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Homogenous equlibrium
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where all species in an equilibrium are in the same physical state
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Heterogenous equilibrium
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Where species in an equilibrium are in different states
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Le chateliers principle
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when a system in dynamic equilibrium is subjected to a change, the position of equilibrium will shift to minimise the change
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Brønsted-Lowry acid
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a proton, H+, donor
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Brønsted-Lowry base
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a proton, H+, acceptor
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Alkali
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A base that dissolves in water forming OH-
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Neutralisation
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A chemical reaction in which an acid and a base react together to produce a salt and water
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Conjugate acid-base pair
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A pair of two species that transform into each other by gain or loss of a proton
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Conjugate base
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the species left after an acid has donated a proton
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Conjugate acid
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The species produced when a base has a accepted a proton
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pH
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-log[H+]
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[H+]
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10^-pH
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Strong acid
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an acid that completely dissociates in solution
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Weak acid
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an acid that partially dissociates in solution
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Acid dissociation constant, Ka
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[H+][A-] / [HA]
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pKa
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-log Ka
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Ionic product of water, Kw
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[H+][OH-] at 25degrees this is 1*10^-14
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Buffer solution
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A mixture that minimises pH changes on addition of small amounts of acid or base
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Equivalence point
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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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End point
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the point in a titration at which there are equal concentrations of the weak acid and conjugate base forms of the indicator
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Standard enthalpy change of neutralisation
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the energy change that accompanies the neutralisation of an aqueous acid by an aqueous base to form one mole of H2O under standard conditions
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Rate of reaction
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the change in concentration of a reactant or product per unit time
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Initital rate of reaction
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the change in concentration of a reactant , or product, per unit time at the start of the reaction when t=0
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The rate equation
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For reaction A + B → C is given by: rate = k [A]^x [B]^y
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The order of reaction
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the power to which the concentration of the reactant is raised in the rate equation
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The rate constant, k
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the constant that links the rate of reaction with the concentrations of the reactants raised to the powers of their orders in the rate equation
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Half-life
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the time taken for the concentration of the reactant to reduce by half
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Reaction mechanism
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a series of steps that, together, make up the overall reaction
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The rate-determining step
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the slowest step in the reaction mechanism of a multi-step reaction
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Intermediate
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a species formed in one step of a multi-step reaction that is used up in a subsequent step, and is not seen as either a reactant or a product of the overall equation
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Transition element
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a d-block elemet that forms a ion with an incomplete d sub-shell
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Complex ion
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a transition metal ion bonded to one or more ligans by coordinate bonds (Dative covalent bonds)
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Ligand
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A molecule or ion that can donate a pair of electrons with the transition metal ion to form a coordinate bond
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Coordination number
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the total number of cooridnate bonds formed between a central metal ion and its ligands
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Coordinate bond
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a bond in which one of the bonded atoms provides both electrons for the shared pair
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Stereoisomers
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species with the same structural formula but with a different arrangemet of the atoms in space
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Optical isomers
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non-superimposable mirror images
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Ligand substitution
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A reaction in which one ligand in a complex ion is replaced by another ligand
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Kstab
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The equilibrium constant for an equilibrium existing between a transition metal ion surrounded by water ligands and the complex formed when the same ion has undergone ligand substitution
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Oxidation
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loss of electrons or an increase in oxidation number
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Reduction
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gain of electrons or a decrease in oxidation number
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Standard electrode potential
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is the electromotive force of a half cell compared with a standard hydrogen half cell under standard conditions (298K, 100kPa, 1moldm^-3)
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Lattice enthalpy
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the enthalpy change accompanying the formation of one mole of an ionic compound from its gaseous ions under standard conditions
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Hess's law
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states that 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
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the enthalpy change when one mole of a compound is formed from its constituent elements in their standard states under standard conditions
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enthalpy change of atomisation
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the enthalpy change when one mole of gaseous atoms forms from the element in its standard state
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First ionisation energy
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the enthalpy change when one electron is removed from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions
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Second ionisation energy
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the enthalpy change when one electron is removed from each ion in one mole of gaseous 1+ ions to form one mole of gaseous 2+ ions
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First electron affinity
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the enthalpy change when one electron is added to each atom in mole of gaseous atoms to form one mole of gaseous 1- ions
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Second electron affinity
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the enthalpy change when one electron is added to each ion in mole of gaseous 1- ions to form one mole of gaseous 2- ions
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Standard enthalpy change of solution
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the enthalpy change when one mole of a compound is completely dissolved in water under standard conditions
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Standard enthalpy change of hydration
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the enthalpy change when one mole of isolated gaseous ions are dissolved in water forming one mole of aqueous ions under standard conditions
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Entropy, S
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the quantitative measure of the degree of disorder in a system
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Standard entropy change of reaction
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the entropy change that accompanies a reaction in the molar quantities expressed in a chemical equation under standard conditions in standard states
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Free energy change
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the balance between enthalpy, entropy and temperature for a process: ΔG = ΔH - TΔS for feasibility ΔG > 0
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