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Mangnesium oxide soluBility...?
- Thread starter hassam
- Start date
- Messages
- 772
- Reaction score
- 149
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Remember that all compounds of 1st group are soluble in water...Mg and O are smaller ions (with greater charges) so their ionic bonds are stronger and harder to break.hassam said:
- Messages
- 677
- Reaction score
- 190
- Points
- 53
MgO has greater lattice enthalpy but a lower hydration energy.
Thereby, strong ionic bonds b/w oppositely charged Mg2+ and O2- ions can't be broken easily.
A general rule:
If lattice enthalpy = hydration energy ... compound is partially soluble
If lattice enthalpy < hydration energy ...compound is soluble .
If lattice enthalpy > hydration energy... compound is insoluble.
Thereby, strong ionic bonds b/w oppositely charged Mg2+ and O2- ions can't be broken easily.
A general rule:
If lattice enthalpy = hydration energy ... compound is partially soluble
If lattice enthalpy < hydration energy ...compound is soluble .
If lattice enthalpy > hydration energy... compound is insoluble.
- Messages
- 772
- Reaction score
- 149
- Points
- 38
But isn't lattice enthalpy included in A2 syllabus? =sbeacon_of_light said:
I don't whether Hassam's question is asked in AS question papers or Not, but IF it is asked then still we'd have to tell about lattice enthalpy?
- Messages
- 677
- Reaction score
- 190
- Points
- 53
well solubility is part of A2... most of the questions are related to solubility of sulphates down the group. Maybe such type of questions won't be asked in paper 2 ...