Energetics definitions

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  • Created by: DavidW001
  • Created on: 11-09-19 11:41
What can be deduced about the structure of a compound when experimental and theoretical lattice energies are very similar
Solid is almost totally ionic
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When experimental and theoretical lattice energies are very different
Has Covalent character
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The ability of the cation to distort the anion is known as
Polarising Power
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Cations with high charge to radius ratio have a
Higher polarising power
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Theoretical lattice energies
Underestimate lattice enthalpy
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Enthalpy change of atomisation
Enthalpy change when one mole of gaseous atoms is produced from an element in its standard state.
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Lattice energy of dissociation
Enthalpy change when one mole of an ionic compound is broken up into its constituent ions in the gas phase.
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Lattice energy
Enthalpy change when one mole of a solid ionic compound formed from its constituent ions int he gas phase.
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Measure of strength ionic bonding
Lattice energy
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Enthalpy change of solution
Enthalpy change when one mole of an ionic solid dissolves to form an infinitely dilute solution.
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Enthalpy change of hydration
enthalpy change when one mole of gaseous ion dissolves to form aqueous ions.
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Sign of enthalpy change of Hydration
Always negative due to bonds forming between water molecules and the ions.
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Sign of enthalpy change of Solution
Can be Positive or Negative
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Card 2

Front

When experimental and theoretical lattice energies are very different

Back

Has Covalent character

Card 3

Front

The ability of the cation to distort the anion is known as

Back

Preview of the front of card 3

Card 4

Front

Cations with high charge to radius ratio have a

Back

Preview of the front of card 4

Card 5

Front

Theoretical lattice energies

Back

Preview of the front of card 5
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