Thomson Definitions Flashcards
Lattice Enthalpy (delta H le)
The Enthalpy change that accompanies the formation of one mile of an ionic compound from its gaseous ions under standard conditions
Give an equation for the lattice Enthalpy of KCl
K+(g) + Cl- (g) ———> KCl(s)
Give an equation for the lattice Enthalpy of KCl
K+(g) + Cl- (g) ———> KCl(s)
Standard Enthalpy of formation (delta H f)
The Enthalpy change that occurs when one mole of a compound is formed from its constituent elements under standard conditions. All reactants and products being in their standard states
Give the equation of the Enthalpy of formation for KCl (s) (delta H f)
K(s) + 1/2Cl2 ———> KCl(s)
Standard Enthalpy change of atomisation (delta H at)
The Enthalpy change that occurs when one mole of gaseous atoms form from the element on its standard state
(Making it a gas)
Give an equation for the Enthalpy change of atomisation (delta H at)
K(s) ———> K(g)
First ionisation energy (Delta H ie1)
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
Give an equation for first ionisation energy
K(g) ———> K+ + e-
Second ionisation Enthalpy (delta H ie2)
The Enthalpy change that accompanies the removal of one electron from each ion in one moles of gaseous 1+ ions to form one mole of 2+ gaseous ions
Why is the second ionisation Enthalpy higher than the first
The outer shell of electrons is pulled in as one electron is removed. The ionic radius decreases
Give an equation for the second ionisation Enthalpy
Ca+ ———> Ca2+ +e-
Why are ionisation energies endothermic
Requires energy to overcome the electrostatic attraction between the negative electrons and the positive nucleus
First electron affinity (delta H ea1)
The Enthalpy change accompanying the addition of one electron to each atom in one like of gaseous atoms to form one mole of 1- ions
Equation of first electron affinity
Cl +e- ———> Cl-