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