Q. Define the standard enthalpy change of atomisation.
The enthalpy change that occurs when 1 mole of gaseous atoms is formed from an element in its standard states under standard conditions.
Q. Define the standard enthalpy change of hydration.
The enthalpy change that occurs when 1 mole of gaseous ions is completely hydrated by water to form 1 mole of aqueous ions under standard conditions.
Q. Define the standard enthalpy change of solution.
The enthalpy change that occurs when 1 mole of ionic compound is completely dissolved in water to form aqueous ions, under standard conditions.
Q. Define first electron affinity.
The enthalpy change that takes place when each atom in 1 mole of gaseous atoms gains an electron to form 1 mole of gaseous ions under standard conditions.
Q. What is lattice enthalpy?
The enthalpy change that occurs when 1 mole of a solid ionic compound is formed from its gaseous ions under standard conditions.
Q. What 2 factors affect the magnitude of lattice enthalpy?
Ionic charge and ionic radius
Q. Explain how ionic radius affects lattice enthalpy?
A smaller ionic radius means the ions are closer together. As a result, the positive and negative ions are more strongly attracted together, making the lattice enthalpy more exothermic.
Q. Explain how ionic charge affects lattice enthalpy?
A greater ionic charge means greater electrostatic attraction between positive and negative ions. This makes the lattice enthalpy more exothermic.
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