5.2.1-lattice enthalpy

Question 1

what is lattice enthalpy

Answer 1

enthalpy change when one mole of ionic lattice is formed from it gaseous ions

Question 2

what is enthalpy change of formation

Answer 2

enthalpy change when one mole of a compound is formed from its elements in there standard states under standard conditions

Question 3

what is first ionisation energy

Answer 3

energy required to remove one electron from each atom in one mole of gaseous atoms

Question 4

what is first electron affinity

Answer 4

making one mole (add e-) of 1- ions (g) from (g) atoms

Question 5

what is enthalpy of atomisation

Answer 5

making one mole of gaseous atoms from its elements in there standard states.

Question 6

what is enthalpy change of solution

Answer 6

when one moles of ionic lattice is dissolved in water (to form aqueous ions)

Question 7

what is enthalpy change of hydration

Answer 7

adding one moles of gaseous ions to water (to form one mole of aqueous ions)

Question 8

which lattice enthalpies are exothermic

Answer 8

-lattice enthalpy
-enthalpy of formation
-1st electron affinity

Question 9

which lattice enthalpies are endothermic

Answer 9

-enthalpy of atomisation
-ionisation energies
-2nd electron affinity

Question 10

which can be both endo and exothermic

Answer 10

-enthalpy change of solution

Question 11

how can the enthalpy change of solution be measured

Answer 11

-measure change in temperature (by measuring start and end temperature)
-measure mass of water
-measure mass of ionic compound added
you can then calculate E=mcat

Question 12

which way do endo and exothermic arrows point

Answer 12

exothermic=down
endothermic=up

Question 13

how does the enthalpy change of F- and Cl- differ

Answer 13

ΔhydH(F−) more negative/exothermic (than ΔhydH(CΓ)) AND F− has smaller size (than Cl−)

Comparison of attraction between ions and water F− OR smaller sized ion linked to greater attraction to H2O