A2 Enthalpy

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14 Terms

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Lattice enthalpy

Formation of 1 mol of ionic lattice from its gaseous ions under standard conditions

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What does lattice enthalpy show?

a measure of the strength of an ionic bond in a giant ionic lattice

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Enthalpy change of atomisation

Formation of 1 mole of gaseous atoms from the element in its standard states under standard conditions

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Enthalpy change of formation

1 mole of a compound is formed from its elements under standard conditions, with all reactants and products in their standard states

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Ionisation energy

Enthalpy change required to remove 1 electron from each atom in 1 mole of gaseous atoms to form 1 mole of gaseous 1+ ions

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Electron affinity

Enthalpy change needed when 1 electron is added to each atom in 1 mole of gaseous atoms to form 1 mole of gaseous 1- ions

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Why is the 1st electron affinity exothermic?

because the electron being added is attracted in towards the nucleus

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Why is the 2nd electron affinity endothermic?

  • Because a second electron is being gained by a negative ion, which repels the electron away

  • So energy is put in to force the electron to the anion

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Enthalpy change of solution

Enthalpy change needed when 1 mole of a solute dissolves in a solvent

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Enthalpy change of hydration

The enthalpy change that accompanies the dissolving of gaseous ions to form 1 mole of aqueous ions

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How does ionic radius affect lattice enthalpy?

  • Ionic radius increases

  • Attraction between cations and anions decreases

  • Lattice enthalpy becomes less negative

  • Melting point decreases

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How does ionic charge affect lattice enthalpy?

  • Ionic charge increases

  • Attraction between cations and anions increases

  • Lattice enthalpy becomes more negative

  • Melting point increases

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How does ionic radius affect hydration?

  • Ionic radius increases

  • Attraction between water molecule & ion decreases

  • Hydration energy becomes less negative

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How does ionic charge affect hydration?

  • Ionic charge increases

  • Attraction between water molecule & ion increases

  • Hydration energy becomes more negative