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6. The enthalpy change of solution is a ______ process

  • Either exothermic or endothermic
  • Endothermic values

7. The standard enthalpy change of formation is usually an ___ process

  • Exothermic
  • Endothermic

8. The second ionisation energy

  • The energy change that accompanies the neutralisation of an aqueous acid by an aqueous base to form one mole of H2O under standard conditions
  • The enthalpy change accompanying the removal of one electron from each ion in one mole of gaseous 1+ ions, to form one mole of gaseous 2+ ions
  • The enthalpy change accompanying the addition of one electron to each atom in one mole of gaseous atoms to form one mole of gaseous 1- ions

9. The standard enthalpy change of solution

  • Either exothermic or endothermic
  • The enthalpy change that takes place when one mole of a compound is completely dissolved in water under standard conditions
  • The strength of an ionic lattice and is a measure of ionic bond strength, large negative value=strong electrostatic forces

10. A covalent structure does not have lattice enthalpy because

  • There are no ions in its structure
  • The strength of an ionic lattice and is a measure of ionic bond strength, large negative value=strong electrostatic forces

11. The standard enthalpy change of formation

  • The enthalpy change accompanying the addition of one electron to each atom in one mole of gaseous atoms to form one mole of gaseous 1- ions
  • The energy change that accompanies the neutralisation of an aqueous acid by an aqueous base to form one mole of H2O under standard conditions
  • The enthalpy change that takes place when one mole of a compound is formed from its constituent elements in their standard states under standard conditions
  • The enthalpy change that accompanies the formation of one mole of an ionic compound from its gaseous ions under standard conditions

12. As ionic radius increases the attraction between ions

  • Decreases and lattice enthalpy becomes less exothermic (less negative)
  • 1 breakdown of the ionic lattice into gaseous ions 2 hydration of the ions

13. Lattice enthalpy indicates

  • The strength of an ionic lattice and is a measure of ionic bond strength, large negative value=strong electrostatic forces
  • There are no ions in its structure

14. As the charge on an ion increases, it has a greater attraction for water molecules and the hydration enthalpy is

  • More negative
  • More positive

15. The first ionisation energy

  • The enthalpy change accompanying the addition of one electron to each atom in one mole of gaseous atoms to form one mole of gaseous 1- ions
  • The enthalpy change accompanying the removal of one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions
  • The enthalpy change that accompanies the formation of one mole of an ionic compound from its gaseous ions under standard conditions

16. Lattice enthalpy is an

  • Exothermic change, with a negative sign
  • The strength of an ionic lattice and is a measure of ionic bond strength, large negative value=strong electrostatic forces

17. The breakdown of the ionic lattice into gaseous ions in (enthalpy of solution) is

  • 1 breakdown of the ionic lattice into gaseous ions 2 hydration of the ions
  • - lattice enthalpy (the energy involved has the same magnitude as lattice enthalpy but the sign is opposite)
  • Endothermic values

18. The second electron affinity is an ____ process because the electron is repelled by the 1- ion, this repulsion has to be overcome

  • Endothermic
  • Exothermic

19. Hess' Law

  • The enthalpy change accompanying the addition of one electron to each atom in one mole of gaseous atoms to form one mole of gaseous 1- ions
  • If a reaction can take place by more than one route and the initial and final conditions are the same, the total enthalpy change is the same for each route
  • The enthalpy change that accompanies the formation of one mole of an ionic compound from its gaseous ions under standard conditions

20. The standard enthalpy change of hydration

  • The enthalpy change that takes place when one mole of isolated gaseous ions is dissolved in water forming one mole of aqueous ions under standard conditions
  • 1 breakdown of the ionic lattice into gaseous ions 2 hydration of the ions