Topic 3 Definitions OwO Flashcards
activation energy
energy required to start/initiate a reaction by breaking the bonds
standard contitions
standard states, 298K temperature, 1 atm/ 101325 Pa pressure, 1.00 moldm-³ consentration?????
le chetalier’s principal
when a system of equilibrium is subject to change, the position of equilibrium will shift to minimise the change
exothermic reaction
reaction where the overall enthalpy? change is ΔH is negative as energy is released to the surroundings.
Bond breaking (endothermic) takes in less energy than bond forming (exothermic)
endothermic reaction
reaction where the overall enthalpy? change is ΔH is positive as energy is absorbed from the surroundings. Bond breaking (endothermic) takes in more energy than bond forming (exothermic)
1st ionisation energy
energy involved in removing 1 mol of electrons from 1 mol of gaseous atoms
metalic bonding
strong electostatic attraction between positive metal ions and sea of delocalised electrons
covalent bond
bond between 2 non-metal elements that involves sharing an electron pair
ionic bond
electrostatic attraction between differently charged ions
enthalpy
heat energy stored in a reaction
enthalpy change of formation
(ΔHf) enthalpy change when mol of a compound is formed from its elements
enthalpy change of reactions
(ΔHf) enthalpy change associated with a stated reaction equation
enthalpy change of solution
(ΔHsol) enthalpy change when 1 mol of a solute dissolves fully in a solution
enthalpy change of combustion
enthalpy change when 1 mol of a substance completely combusts (ΔHf)
enthalpy change of neutralisation
f(ΔHneut) formation of 1 mole of H20 from neutralisation enthalpy change
