born haber cycles etc

Question 1

a regular born haber cycle

Answer 1

F AT AT IE1 IE2 EA LE

Question 2

Lattice enthalpy deifntion

Answer 2

formation of 1 mole ionic compound from its gaseous ions ( not elements) UNDER STANDARD CONDITIONS

Question 3

Note: if something happens twice eg , element has “2” next to it, multply by 2

Answer 3

multiply by 2

Question 4

br- electron config

Answer 4

1s2 2s2 2p6 3s2 3p6 3d1 04s2 4p6 

Question 6

Answer 6

Question 7

note

Answer 7

agianst the arrow=opposite sign

with the arrow= same sign

Question 8

Describe and explain the factors that affect the values of lattice enthalpies. ……………………………………………………………………………………………………….

Answer 8

Decrease in (ionic) size AND more negative LE OR more exothermic OR more attraction 

Increase in (ionic) charge OR charge density AND more negative LE OR more exothermic OR more attraction 

———————————————————————————– Link between LE and attraction Lattice enthalpy correctly linked to attraction between IONS at least once  e.g. Greater attraction between ions gives more negative

Question 9

The change that produces lattice enthalpy is spontaneous but has a negative entropy change. Why is this change able to take place spontaneously? ………………………………………………………………………………………..

Answer 9

∆H < T∆S OR ∆H – T∆S < 0

ignore comments about gibbs free energy

Question 10

Explain the differences between these lattice enthalpies. In your answer, your explanation should show how different factors affect lattice enthalpy

Answer 10

Comparison of size of anions Chloride ion OR Cl– is larger (than F–) OR Cl– has smaller charge density (than F–) 

Comparison of size AND charge of cations Mg2+ is smaller (than Na+) AND Mg2+ has a greater charge (than Na+) 

Comparison of attraction between ions F– has greater attraction for Na+ / + ions AND Mg2+ has greater attraction for F– / – ions

Question 11

PAPER 1= DONE