Chem- AS Inorganic & Physical definitions Flashcards
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+ ions
Second ionisation energy
The energy required to remove one electron from each ion in one mole of gaseous 1+ ions to form one mole of gaseous 2+ ions
Successive ionisation energy
A measure of the energy required to remove each electron in turn
Oxidation number
A measure of the number of electrons that an atom uses to bond with atoms of a different element
Oxidation
The loss of electrons/ an increase in oxidation number (state)
Oxidising agent
A reagent which oxidises another species, it accepts electrons from the other species and is itself reduced
Reduction
The gain of electrons/ a decrease in oxidation number (state)
Reducing agent
A reagent which reduces another species, it donates electrons to the other species and is itself oxidised
Redox
A reaction where both oxidation and reduction take place
Disproportionation
A reaction in which one element is simultaneously oxidised and reduced
Displacement reaction
A redox reaction between a halogen and the halide ion of a less reactive halogen in which the halide ion is oxidised by the more reactive halogen
Exothermic
Heat is given out to the surroundings (the reactants lose energy)
Endothermic
Heat is taken in from the surroundings (the reactants gain energy)
Activation energy
The minimum energy required to start a reaction by the breaking of bonds
Standard conditions
A pressure of 100kPa (1 atmosphere), a stated temperature (usually 298K/25 C), and a concentration of 1.0 moldm^-3 (for reactions with aqueous solutions)
(Standard) enthalpy change of reaction
The enthalpy change that accompanies a reaction in the molar quantities expressed in a chemical equation (under standard conditions, all reactants and products being in their standard states)
(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)
(Standard) enthalpy change of combustion
The enthalpy change that takes place when one mole of a substance reacts completely with oxygen (in their standard states under standard conditions)
Average bond enthalpy
The average enthalpy change that takes place when breaking, by homolytic fission, 1 mole of a given type of bond in the molecules of a gaseous species
Enthalpy change of neutralisation
The energy change that accompanies the neutralisation of an aqueous acid by an aqueous base to form one mole of H2O(l) under standard conditions
Catalyst
Speeds up a reaction without being consumed by the overall reaction
Dynamic equilibrium
The equilibrium that exists in a closed system when the rate of the forward reaction is equal to the rate of the reversed reaction
Le Chatelier’s Principle
When a system in dynamic equilibrium is subjected to change, the position of equilibrium will shift to minimise the change