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Thermodynamics definitions
- Enthalpy change of formation: the energy
transferred when one mole of the
compound is formed from its elements
under standard conditions with all of the
reactants and products in their standard
states
- Enthalpy of atomisation: the
enthalpy change when I mole of
gaseous atoms is formed from
the element in its standard state
under standard conditions
- Mean bond enthalpy: the enthalpy
change when mole of gaseous
molecules each breaks a covalent bond
to form two free radicals averaged over
a range of compounds.
- First ionisation energy: the enthalpy change
when one mole of gaseous atoms is
converted to one mole of gaseous ions each
with a single posistive charge
- Second ionisation energy: the enthalpy change
to remove one mole of electrons from one
mole of gaseous +1 ions to produce a mole of
gaseous +2 ions.
- First electron affinity: the enthalpy change when one
mole of gaseous atoms is converted, by gaining a mole of
electrons, to a mole of gaseous ions each with a single
negative charge.
- Second electron affinity: the enthalpy change
when one mole of electrons is added to a mole of
gaseous ions each with a single negative charge to
form ions with two negative charges
- Lattic formation enthalpy: the enthalpy change
when one mole of solid ionic compound is formed
from its gaseous ions
- Enthalpy of hydration: the enthalpy change when water
molecules surround one mole of gaseous ions.
- Enthalpy of solution: the enthalpy change when one mole of
solute dissolves completely in sufficient solvent to form a
solution in which the molecules or ions are far enough apart
not to interact with each other.
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