Enthalpy Change & Cycles Flashcards
(10 cards)
Define enthalpy change of lattice formation (∆HLF)
Heat energy change when 1 mol solid ionic compound formed from it’s (g) ions
Outline the meaning of exothermic and endothermic reactions
Exothermic = heat energy released/bonds made
Endothermic = heat energy taken in/bonds broken
Define ∆H formation (∆HF)
Heat energy change of compound formed from it’s elements
Define ∆H of atomisation (∆Hat)
Heat energy change when 1 mol (g) atoms formed from it’s elements in the standard state
Define the ∆H of 1st ionisation energy (∆HIE)
Heat energy change when 1 mol of e- lost from 1 mol of (g) atoms
Define the ∆H of 2nd ionisation energy (∆HIE2)
Heat energy change when 1 mol of e- taken from 1 mol of (g)
Define the ∆H of 1st e- affinity (∆HEA)
Heat energy change when 1 mol of e- is added to 1 mol (g) atoms
Define the ∆H of the 2nd e- affinity (∆HEA2)
Heat energy change when 1 mol of e- added to 1 mol (g) ions
Outline the standard enthalpy change of formation equation (ΔH°f)
- Write out equation at top with constituent elements below
- Input the arrows into diagram (ensure the head is the right way round)
- Input values and calculate ΔH°f
Outline the difference between the arrow directions for the equations of (ΔH°f) and (ΔH°c)
(ΔH°f) = bottom to top
(ΔH°c) = top to bottom