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OCR A Level Inorganic Chemistry Questions & 100% Correct AnswersLatest Test | Graded A+ | Passed
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Standard enthalpy of formation ֎ -:- The enthalpy change when one mole of a compound is formed from its elements under standard conditions, with all substances in their standard states. Standard change of atomisation ֎ -:- The enthalpy change when one mole of gaseous atoms is formed from t...

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  • 27 de agosto de 2024
  • 45
  • 2024/2025
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  • ocr a level inorganic chemistry questions 100 c

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OCR A Level Inorganic Chemistry
Questions & 100% Correct Answers-
Latest Test | Graded A+ | Passed
Standard enthalpy of formation


֎ -:- The enthalpy change when one mole of a compound is formed from its

elements under standard conditions, with all substances in their standard

states.




Standard change of atomisation


֎ -:- The enthalpy change when one mole of gaseous atoms is formed from the

element in its standard state under standard conditions.




First ionisation energy


֎ -:- The enthalpy change needed to remove one electron from each atom in

one mole of gaseous atoms to form one mole of gaseous 1+ ions.




Second ionisation energy


֎ -:- The enthalpy change required to remove one electron from each ion in one

mole of gaseous 1+ ions to form one mole of gaseous 2+ ions.




First electron affinity




26/08/2024 | © Copyright- This work may not be copied for profit.

, Excellence is key | 2024/2025 ~Page |2


֎ -:- The enthalpy change when one electron is added to each atom in one mole

of gaseous atoms to form one mole of gaseous 1- ions.




Second electron affinity


֎ -:- The enthalpy change when one electron is added to each ion in one mole of

gaseous 1- ions to form one mole of gaseous 2- ions.




Lattice enthalpy


֎ -:- The enthalpy change that accompanies the formation of one mole of a

solid compound from its gaseous ions under standard conditions.




The standard enthalpy change of solution


֎ -:- The enthalpy change when one mole of a compound is completely

dissolved in water under standard conditions.




The standard enthalpy change of hydration


֎ -:- The enthalpy change that accompanies the dissolving of gaseous ions in

water to form one mole of aqueous ions.




Entropy




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֎ -:- A measure of the dispersal of energy in a system, which is greater the more

disordered a system.




ΔS=


֎ -:- S of products - S of reactants




Effect of increasing ionic size on lattice enthalpy


֎ -:- This leads to a weaker attraction between oppositely charged ions so there

is a less exothermic lattice enthalpy.




Effect of increasing ionic charge on lattice enthalpy


֎ -:- This leads to a stronger attraction between oppositely charged ions and a

more exothermic lattice enthalpy.




Effect of increasing ionic size on hydration enthalpy


֎ -:- This leads to a weaker attraction between the ions and water molecules so

there is a less exothermic hydration enthalpy.




Effect of increasing ionic charge on hydration enthalpy




26/08/2024 | © Copyright- This work may not be copied for profit.

, Excellence is key | 2024/2025 ~Page |4


֎ -:- This leads to a stronger attraction between ions and water molecules so

there is a more exothermic hydration enthalpy.




ΔG=


֎ -:- ΔH-TΔS




A process can take place spontaneously (i.e. is feasible), when...


֎ -:- ΔG<0




Free energy change


֎ -:- The overall change in energy during a reaction.




A reaction is feasible at any temperature if...


֎ -:- The sign of its ΔH is negative and its ΔS is positive, because ΔG will always

be less than zero.




A reaction is NOT feasible at any temperature if...


֎ -:- The sign of its ΔH is positive and its ΔS is negative, because ΔG will always

be more than zero.




A reaction is only feasible at high temperatures if...


26/08/2024 | © Copyright- This work may not be copied for profit.

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