Born harber cycles and enthalpy of solution Flashcards
What is the standard molar enthalpy of formation ΔHf?
The standard molar enthalpy of formation is the enthalpy change when one mole of a compound is formed from its constituent elements under standard conditions, all reactants and products being in their standard states
What is the standard molar enthalpy of combustion ΔHc?
The standard molar enthalpy of combustion is the enthalpy change when one mole of substance is completely burned in oxygen
What is the standard enthalpy of atomisation ΔatH?
The standard enthalpy of atomisation is the enthalpy change which accompanies the formation of one mole of gaseous atoms from the element in its standard state under standard conditions.
What is the first ionisation energy ΔiH?
The first ionisation energy is the standard enthalpy change when one mole of gaseous atoms is converted into a mole of gaseous ions each with a single positive charge.
What is the second ionisation energy?
This is the standard enthalpy change when one mole of unipositive ions in the gaseous state lose one electron to form one mole of 2+ ions in the gaseous state
What is the first electron affinity ΔeaH?
The first electron affinity is the standard enthalpy change when a mole of gaseous atoms is converted into a mole of gaseous ions, each with a single negative charge
What is the second electron affinity ΔeaH?
The second electron affinity is the enthalpy change when a mole of electrons is added to a mole of gaseous ions each with a single negative charge to form ions each with two negative charges
What is the lattice enthalpy of formation ΔlH?
The lattice enthalpy of formation is the standard enthalpy change when one mole of solid ionic compound is formed from its gaseous ions.
What is the lattice enthalpy of dissociation -ΔlH?
Lattice enthalpy of dissociation is the standard enthalpy change when one mole of solid ionic compound dissociates into it gaseous ions
What is mean bond enthalpy?
Mean bond enthalpy is the enthalpy change when one mole of gaseous molecules each break a covalent bond to form two free radicals averaged over a range of compounds.
