Born-Haber Cycles

Last updated: 10/02/2020

Edexcel A-Level Chemistry Energetics II Born-Haber Cycles

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Question 1 of 40

1. Question
What does the Born-Haber Cycle show?
- Shows a series of intermediate steps between an ionic substance and the elements that form the ionic substance
- Shows the paths of enthalpy throughout an ionic substance
- Shows the different formations of an ionic substance
- Shows a series of intermediate steps to form a compound
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Question 2 of 40

2. Question
What is an equation that is used in the Born-Haber Cycle and Hess’ Law?
- Sum of clockwise enthalpy changes = sum of anticlockwise enthalpy changes
- Sum of clockwise enthalpy changes x sum of anticlockwise enthalpy changes
- Sum of clockwise enthalpy changes / sum of anticlockwise enthalpy changes
- Sum of anticlockwise enthalpy / sum of clockwise
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Question 3 of 40

3. Question
What is the definition of lattice enthalpy?
- The enthalpy change that accompanies the formation of one more of an ionic lattice from its gaseous ions under standard conditions
- The enthalpy change that accompanies the formation of one mole of a compound from its elements
- The enthalpy change that accompanies the removal of one mole of electrons from one mole of gaseous atoms
- The enthalpy change when one mole of gaseous atoms is formed from its elements in standard states
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Question 4 of 40

4. Question
What is the definition of standard enthalpy change of formation?
- The enthalpy change that accompanies the formation of one mole of a compound from its elements
- The enthalpy change when one mole of gaseous atoms is formed from its elements in standard states
- The enthalpy change that accompanies the removal of one mole of electrons from one mole of gaseous atoms
- The enthalpy change that accompanies the formation of one mole of an ionic lattice from its gaseous ions under standard conditions
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Question 5 of 40

5. Question
What is the definition of the standard enthalpy change of atomisation?
- The standard enthalpy change when one mole of gaseous atoms is formed from its element in standard states
- The standard enthalpy change when one mole of gaseous 2+ ions are formed from one mole of gaseous 1+ ions
- The standard enthalpy change when one mole of gaseous 1- ions is formed from gaseous atoms
- The standard enthalpy change when one mole of gaseous 2- ions is formed from gaseous 1- ions
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Question 6 of 40

6. Question
What is the definition of first ionisation energy?
- The energy change that accompanies the removal of one mole of electrons from one mole of gaseous atoms
- The enthalpy change that accompanies the formation of one mole of an ionic lattice from its gaseous ions under standard conditions
- The enthalpy change when one mole of gaseous atoms is formed from its elements in standard states
- The enthalpy change that accompanies the formation of one mole of a compound from its elements
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Question 7 of 40

7. Question
What is the definition of the second ionisation energy?
- The standard enthalpy change when one mole of gaseous 2+ ions are formed from one mole of gaseous 1+ ions
- The standard enthalpy change when one mole of gaseous 1- ions is formed from gaseous atoms
- The standard enthalpy change when one mole of gaseous 2- ions is formed from gaseous 1- ions
- The standard enthalpy change when one mole of gaseous atoms is formed from its element in standard states
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Question 8 of 40

8. Question
What is the definition of the first electron affinity?
- The standard enthalpy change when one mole of gaseous 1- ions is formed from gaseous atoms
- The standard enthalpy change when one mole of gaseous 2- ions is formed from gaseous 1- ions
- The standard enthalpy change when one mole of gaseous atoms is formed from its element in standard states
- The standard enthalpy change when one mole of gaseous 2+ ions are formed from one mole of gaseous 1+ ions
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Question 9 of 40

9. Question
What is the definition of the second electron affinity?
- The standard enthalpy change when one mole of gaseous 2- ions is formed from gaseous 1- ions
- The standard enthalpy change when one mole of gaseous 1- ions is formed from gaseous atoms
- The standard enthalpy change when one mole of gaseous 2+ ions are formed from one mole of gaseous 1+ ions
- The standard enthalpy change when one mole of gaseous atoms is formed from its element in standard states
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Question 10 of 40

10. Question
What is the definition of the standard enthalpy change of solution?
- The enthalpy change that takes place when one mole of a solute is completely dissolved in water under standard conditions
- The enthalpy change that takes place when dissolving one mole of gaseous ions in water
- The enthalpy change when one mole of gaseous atoms is formed from its element in its standard state
- The enthalpy change when one mole of gaseous 2+ ions are formed from one mole of gaseous 1+ ions
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Question 11 of 40

11. Question
What is the definition of the standard enthalpy change of hydration?
- The enthalpy change that takes place when dissolving one mole of gaseous ions in water
- The enthalpy change that takes place when one mole of a solute is completely dissolved in water under standard conditions
- The enthalpy change when one mole of gaseous 2+ ions are formed from one mole of gaseous 1+ ions
- The enthalpy change when one mole of gaseous atoms is formed from its element in its standard state
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Question 12 of 40

12. Question
What is the symbol for lattice enthalpy?
- $Δ_{LE}H^ө$
- $Δ_fH^ө$
- $Δ_aH^ө$
- $Δ_{hyd}H^ө$
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Question 13 of 40

13. Question
What is the symbol for the standard enthalpy change of formation?
- $Δ_fH^ө$
- $Δ_{LE}H^ө$
- $Δ_aH^ө$
- $Δ_{hyd}H^ө$
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Question 14 of 40

14. Question
What is the symbol for the standard enthalpy change of atomisation?
- $Δ_aH^ө$
- $Δ_{I1}H^ө$
- $Δ_{LE}H^ө$
- $Δ_fH^ө$
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Question 15 of 40

15. Question
What is the symbol for the first ionisation energy?
- $Δ_{I1}H^ө$
- $Δ_fH^ө$
- $Δ_{LE}H^ө$
- $Δ_aH^ө$
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Question 16 of 40

16. Question
What is the symbol for the first electron affinity?
- $Δ_{EA1}H^ө$
- $Δ_{I1}H^ө$
- $Δ_fH^ө$
- $Δ_{EA2}H^ө$
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Question 17 of 40

17. Question
What is the symbol for the standard enthalpy change of solution?
- $Δ_{sol}H^ө$
- $Δ_{LE}H^ө$
- $Δ_{hyd}H^ө$
- $Δ_fH^ө$
Correct

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Question 18 of 40

18. Question
What is the symbol for the standard enthalpy change of hydration?
- $Δ_{hyd}H^ө$
- $Δ_{sol}H^ө$
- $Δ_{LE}H^ө$
- $Δ_fH^ө$
Correct

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Question 19 of 40

19. Question
Describe the trend in lattice enthalpy down the halogen group.
- Becomes less exothermic and less negative. Results in weaker attraction between ions and a higher enthalpy.
- Becomes more exothermic and more negative. Results in weaker attraction between ions and a higher enthalpy.
- Becomes less endothermic and less position. Results in weaker attraction between ions and a higher enthalpy.
- No trend in enthalpy
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Question 20 of 40

20. Question
What happens when a solid dissolves?
- Ionic lattice breaks down
- Ions become tightly bonded
- Releases free electrons
- Forms strong Van der Waals forces
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Question 21 of 40

21. Question
What standard enthalpy change takes place when a solid dissolves?
- Standard enthalpy change of solution
- Standard enthalpy change of atomisation
- Standard enthalpy change of formation
- Standard enthalpy change of hydration
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Question 22 of 40

22. Question
Which of the following are examples of an exothermic standard enthalpy change?
- Calcium chloride dissolves in water
- Ammonium nitrate dissolves in water
- Sodium chloride dissolves in water
- Potassium chloride dissolves in water
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Question 23 of 40

23. Question
Which of the following are examples of an endothermic standard enthalpy change?
- Ammonium nitrate dissolves in water
- Calcium chloride dissolves in water
- Sodium chloride dissolves in water
- Potassium chloride dissolves in water
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Question 24 of 40

24. Question
Which of the following enthalpy changes does the standard enthalpy change of solution equal to?
- -lattice enthalpy
- -first electron affinity
- -standard enthalpy change of formation
- -standard enthalpy change of atomisation
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Question 25 of 40

25. Question
Which of the following factors influence the magnitude of lattice enthalpy?
- Ionic size
- Ion density
- Volume of the solid
- Melting and boiling points of solid
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Question 26 of 40

26. Question
Which of the following factors influence the magnitude of lattice enthalpy?
- Ionic charges
- Melting and boiling points of solid
- Surface area of ions
- Number of total protons
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Question 27 of 40

27. Question
Which of the following factors influence the magnitude of lattice enthalpy?
- Ionic bond strength
- Ionic densities
- Intermolecular forces
- Ionic surface area
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Question 28 of 40

28. Question
What happens to water molecules during the standard enthalpy change of hydration?
- They surround the ions
- They dissolve the ions
- They are repelled from the ions
- They evaporate
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Question 29 of 40

29. Question
Which of the following factors influence the magnitude of the enthalpy of hydration?
- Ionic sizes
- Ionic densities
- Surface area of ions
- Ionic strength
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Question 30 of 40

30. Question
Which of the following factors influence the magnitude of the enthalpy of hydration?
- Ionic charge
- Ionic strength
- Surface area of ions
- Melting and boiling points of solid
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Question 31 of 40

31. Question
Describe the trend in enthalpy of hydration down the halogen group.
- Size increases, less exothermic. Results in a higher enthalpy.
- Size decreases, more exothermic. Results in a lower enthalpy.
- Size increases, more exothermic. Results in a higher enthalpy.
- No trend in enthalpy
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Question 32 of 40

32. Question
How can the ionic solid and gaseous ions be linked together?
- The lattice enthalpy
- The first electron affinity
- The standard enthalpy change of formation
- The standard enthalpy change of atomisation
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Question 33 of 40

33. Question
How can the ionic solid and gaseous ions be linked together?
- The standard enthalpy of solution with the standard enthalpy of hydration
- The standard enthalpy change of formation
- The standard enthalpy of solution
- The standard enthalpy change of hydration
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Question 34 of 40

34. Question
What is the relationship between how exothermic a lattice is and the strength of ionic bonds.
- The more exothermic the stronger the bonds
- It will depend on the size of the ionic charge
- There is no relationship between how exothermic an ionic lattice is and the strength of ionic bonds
- The more exothermic the weaker the ionic bonds
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Question 35 of 40

35. Question
Which type of enthalpy change is the standard enthalpy change of formation?
- Usually exothermic
- Always exothermic
- Always endothermic
- Usually endothermic
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Question 36 of 40

36. Question
Which type of enthalpy change is the standard enthalpy change of atomisation?
- Always endothermic
- Always exothermic
- Usually endothermic
- Usually exothermic
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Question 37 of 40

37. Question
Which type of enthalpy change is the first ionisation energy?
- Usually endothermic
- Always endothermic
- Always exothermic
- Usually exothermic
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Question 38 of 40

38. Question
Which type of enthalpy change is the second ionisation energy?
- Always exothermic
- Always endothermic
- Usually endothermic
- Usually exothermic
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Question 39 of 40

39. Question
Which type of enthalpy change is the first electron affinity?
- Always exothermic
- Always endothermic
- Usually endothermic
- Usually exothermic
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Question 40 of 40

40. Question
Which type of enthalpy change is the second electron affinity?
- Always endothermic
- Always exothermic
- Usually endothermic
- Usually exothermic
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