Definitions Flashcards
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1st Ionisation Energy
energy required to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions
Successive Ionisation Energy
energy required to remove one electron from each ion in one mole of gaseous 1+ ions to form one mole of gaseous 2+ ions
Relative Atomic Mass`
the weighed mean mass of an atom of an element compared with 1/12th of the mass of an atom of carbon-12
Relative Molecular Mass
the weighed mean mass of a molecule compared with 1/12th of the mass of an atom of carbon-12
Electronegativity
the atom’s ability to attract an electron pair in a covalent bond
Standard Conditions
temperature = 298K pressure = 1 atm/100kPa concentration = 1 mol dm^-3
Enthalpy Change
the enthalpy change that occurs when equation quantities of materials react under standard conditions and with everything in it’s standard state
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
Combustion
the enthalpy change that takes place when one mole of a substance reacts completely with oxygen under standard conditions with everything in it’s standard states
Mean Bond Enthalpy
the average enthalpy change that takes place when breaking one mole of a given bond in the molecule of a gaseous species under standard conditions
Le Chatelier’s Principle
if a change is applied to a system in equilibrium, the equilibrium will shift to counteract the change
Homologous Series
a series of compounds that have similar properties and the same general formula
