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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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ocr a level inorganic chemistry questions 100 c

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Excellence is key | 2024/2025 ~Page |1

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

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֎ -:- 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

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֎ -:- 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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