62318
| Question | Answer |
| Oxidation | Loss of electrons, increase in oxidation num |
| Reduction | Gain of electrons, decrease in oxidation number |
| Standard electrode potential | e.m.f of a half cell compared with a standard hydrogen half cell, measured at 298k with solution concentration 1moldm-3 and a gas pressure of 100kpa |
| Transition metal | D-block element that forms one or more stable ions with an incomplete d-sub shell |
| Complex ion | transition metal ion bonded to one or more ligands by co-ordinate bonds (dative covalent) |
| Ligand | molecule or ion that can donate a pair of electrons to a transition metal ion to form a co-ordinate bond |
| co-ordination number | total num of co-ordinate bonds formed between central metal ion and its ligands |
| Stereoisomers | species with the same structural and molecular formula but a different arrangement in space cis/trans or optical |
| Ligand substitution | reaction in which one ligand in a complex ion is replaced by another ligand |
| Stability constant Kstab | equilibrium constant for the equilibrium existing between a transition metal ion surrounded by water ligands and the complex formed when the same ion has undergone ligand subsitution |
| Lattice enthalpy | enthalpy change that accompanies the formation of one mole of an ionic compound from its gaseous ions under standard conditions |
| Hess' law | states that if a reaction can take place by more than one rout and the initial and final conditions are the same for each, the total enthalpy change is the same for each route |
| Standard enthalpy change of formation | H change that takes place when one mole of a compound is formed from its constituent elements in their standard states under standard conditions |
| H change of atomisation | H change that takes place when one mole of gaseous atoms forms from the element in its standard state |
| first ionisation energy | h change accompanying the removal of one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions |
| 2nd ionisation energy | H change accompanying the removal of one electron from each ion in one mole of gaseous 1+ ions to form one mole of gaseous 2+ ions |
| First electron affinity | H change accompanying the addition of one electron to each atom in one mole of gaseous atoms to form one mole of gaseous 1- ions |
| 2nd electron affinity | enthalpy change accompanying the addition of one electron to one mole of gaseous 1- ions to form one mole of gaseous 2- ions |
| Standard H change of solution | H change that takes place when one mole of a compound is completely dissolved in water under standard conditions |
| Standard H change of hydration | H change that takes place when one moles of isolated gaseous ions are dissolved in water forming one mole of aqueous ions under standard conditions |
| Free energy change, Delta G | Balance between entropy, enthalpy and temperature for a process: ^G=^H-T^S Process can take place spontaneously when ^G < 0 |
| ionic product of water Kw=? | [H+(aq)][OH-(aq)] |
| Buffer solutions | mixture that minimises changes to pH upon addition of acid or base |
| equivalence point | is the point in a titration at which the volume of one solution has reacted exactly with the volume of the second solution |
| end point | point in a titration at which there are equal concentrations of the weak acid and conjugate base forms of the indicator |
| Standard enthalpy change of neutralisation | energy change that accompanies the neutralization of an aqueous acid by an aqueous base to form one mole of H2O under standard conditions |
| rate of reaction | Change in concentration of reaction or product per unit time |
| Initial rate of reaction | change in concentration of product or reactant per unit time at the start of the reaction where t=0 |
| Rate eqution for A+B=C | rate = k[A](m)[B](n) Where m is the order with respect to A and N is the order with respect to B |
| Order with respect to reactant | is the power to which the concentration of the reactant is raised in the rate equation |
| overall order | sum of individual orders |
| Rate constant, k | is the constant that links the rate of reaction with concentrations of the reactants raised to the power of there orders in the rate equation |
| Half-life | time taken for concentration of reactant to decrease by half |
| Reaction mechanism | series of steps, that together, make up the overall reaction |
| rate-determining step | slowest step in the reaction mechanism of a multi-step reaction |
| Intermediate | 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 product of the overall equation |
| Equilibrium law for aA + bB = cC + dD | [C](c)[D](d) Kc = _____________ [A](a)[B](b) |
| Dynamic equilibrium | exists in a closed system where the rate of the forward reaction = the rate of the reverse reaction and the conc of reactants stays constant |
| Homogeneous equilibrium | all species making up products and reactants are in the same physical state |
| Heterogeneous equilibrium | where all species making up reactants and products are in different physical states |
| Bronsted-Lowry acid | H+, proton donor |
| Bronsted-Lowry Base | Proton, H+, acceptor |
| Bronsted-Lowry Base | Proton, H+, acceptor |
| Alkali | base that dissolves in water giving OH- ions |
| Neutralisation | Chemical reaction in which an acid and a base react together to produce a salt and water |
| Acid-base pair | pair of two species with transform into each other by gain or loss of a proton |
| pH = ? | -log[H+] |
| [H+(aq)] =? | 10(-pH) |
| Strong acid | Completely dissociates in solution |
| Weak acid | partially dissociates in solution |
| pKa =? | -log10Ka |
| Ka = ? | 10-pKa |
| Acid dissociation constant, Ka = ? | Ka = [H+][A-] ---------- [HA(aq)] |
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