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20 Cards in this Set
- Front
- Back
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Enthalpy change of Formation |
The enthalpy change when 1 mole of a compound is formed from its elements in their standard states under standard conditions. |
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Bond dissociation enthalpy |
The enthalpy change when all the bonds of the same type in one mole of gaseous molecules are broken. |
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Enthalpy change of atomisation of an element |
The enthalpy change when 1 mole of gaseous atoms is formed from an element in its standard state. |
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First ionisation enthalpy |
The enthalpy change when one mole of gaseous 1+ ions is formed from one mole of gaseous atoms. |
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Second ionisation enthalpy |
The enthalpy change when one mole of gaseous 2+ ions is formed from one mole of gaseous 1+ ions. |
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First electron affinity |
The enthalpy change when one mole of gaseous 1- ions is formed from one mole of gaseous atoms. |
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Second electron affinity |
The enthalpy change when one mole of gaseous 2- ions is formed from one mole of gaseous 1- ions. |
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The enthalpy change of hydration |
The enthalpy change when one mole of aqueous ions is formed from one mole of gaseous ions. |
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The enthalpy change of solution |
The enthalpy change when one mole of solute is dissolved in sufficient solvent that no further enthalpy change occurs on further dilution. |
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Standard conditions |
100 kPa 298 K |
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Pure ionic model |
Ions are spherical and have charge evenly spread. No covalent character. |
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Partial covalent bonding |
The electrons in the negative ions are pulled towards the positive ion. |
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How to tell if purely ionic bonding or partial covalent bonding. |
If there is a large difference in the experimental and theoretical values, partial covalent bonding. If they are close, purely ionic. |
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What is the Enthalpy change of solution equal to? |
Lattice dissociation enthalpy + Enthalpy of hydration (of each ion) |
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What is entropy? |
Entropy is the measure of the number of ways that particles can be arranged. |
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How does changing state affect entropy? |
Melting or boiling increases entropy, condensing or solidifying decreases entropy. |
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How does dissolving a solid affect entropy? |
Causes an increase. |
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How does number of particles affect entropy? |
More particles lead to an increased entropy. |
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Spontaneous reaction |
A reaction that does not require any external energy to occur. |
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Free energy change |
ΔG = ΔH - T ΔS If ΔG > 0, reaction is not feasible. If ΔG < 0, reaction is feasible. (Remember to convert all units to J or kJ) |
