A2 Unit 2 Chemistry Definitions

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Can you name the A2 Unit 2 Chemistry Definitions?

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The change in concentration of a reactant or product per unit time
 
The change in concentration of a reactant, or product per unit time at the start of the reaction when t=0
 
Rate = k[A]^m[B]^n
 
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
 
The time taken for the concentration of the reactant to reduce by half
 
A series of steps that together make up the overall reaction
 
The slowest step in the reaction mechanism of a multi-step reaction
 
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
 
Kc = [C]^c[D]^d/[A]^a[B]^b
 
Exists in a closed system when the rate of the forward reaction is equal to the rate of the reverse reaction
 
An equilibrium in which all the species making up the reactants and products are in the same physical state
 
An equilibrium in which all the species making up the reactants and products are in the different physical state
 
When a system in dynamic equilibrium is subjected to a change, the system readjusts itself to minimise the effect of the change and to restore equilibrium
 
A proton (H+) donor
 
A proton (H+) acceptor
 
A base that dissolves in water forming OH-(aq) ions
 
A chemical reaction in which an acid and a base react together to produce a salt and water
 
A pair of two species that transform into each other by gain or loss of a proton
 
An acid that completely dissociates in solution
 
An acid that partially dissociates in solution
 
Ka = [H+(aq)][A-(aq)] / [HA(aq)]
 
Kw = [H+(aq)][OH-
 
A mixture that minimises pH changes on addition of small amounts of acid or base
 
The point in a titration at which the volume of one solution has reacted exactly with the volume of the second solution
 
The point in a titration at which there are equal concentrations of the weak acid and conjugate base forms of the indicator
 
The energy change that accompanies the neutralisation of an aqueous base to form one mole of H2O(L) under standard conditions
 
The enthalpy change that accompanies the formation of one mole of an ionic compound from its gaseous ions under standard conditions
 
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
 
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
 
The enthalpy change that takes place when one mole of gaseous atoms forms from the element in its standard state
 
The enthalpy change accompanying the removal of one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions
 
The enthalpy 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
 
The enthalpy change accompanying the addition of one electron to each atom in one mole of gaseous atoms to form one mole of gaseous 1- ions
 
The enthalpy change accompanying the addition of one electron to each ion in one mole of gaseous 1- ions to form one mole of gaseous 2- ions
 
The enthalpy change that takes place when one mole of a compound is completely dissolved in water under standard conditions
 
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
 
The quantitative measure of the degree of disorder in a system
 
The entropy change that accompanies a reaction in the molar quantities expressed in a chemical equation under standard conditions, all reactants and products being in their standar
 
The balance between enthalpy, entropy and temperature for a process: Delta G = Delta H - T Delta S
 
The loss of electrons or an increase in oxidation number
 
The gain in electrons or a decrease in oxidation number
 
The emf of a half cell compared with a standard hydrogen half cell, measured at 298 K with solution concentrations of 1 mol dm^-3 and a gas pressure of 100kPa (1 atmosphere)
 
A d-block element that forms an ion with an incomplete d sub-shell
 
A transition metal ion bonded to one or more ligands by coordinate bonds (dative covalent bonds)
 
A molecule or ion that can donate a pair of electrons with the transition metal ion to form a coordinate bond
 
The total number of coordinate bonds formed between a central metal ion and its ligands
 
Species with the same structural formula but with a different arrangement of the atoms in space
 
A reaction in which one ligand in a complex ion is replaced by another ligand
 
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 a ligand subs
 

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Created Jan 1, 2012ReportNominate
Tags:chemistry, A Level