Which one of the following alkaline earth metal sulphates has its hydration enthalpy greater than its lattice enthalpy?
- $CaSO_4$
- $BeSO_4$
- $BaSO_4$
- $SrSO_4$
The Correct Option is B
Solution and Explanation
Beryllium sulfate \((BeSO_4)\) possesses a hydration enthalpy that surpasses its lattice enthalpy. This characteristic leads to its remarkable water solubility. As you move down the group, the solubility of sulfates of alkaline earth metals diminishes. This results in barium sulfate and radium sulfate being practically insoluble.
So, the correct option is (B): \(BeSO_4\).
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Concepts Used:
Group 1 Elements
Group one of alkali metals is s-block elements with just one electron in their s-orbital. They are are alkali metals. They are named so because of the alkaline nature of the hydroxides and oxides.
Alkali metals are characterized by one s-electron in the valence shell of their atoms.
Alkali metals have a corresponding [Noble gas] ns1 electronic configuration. They occupy the first column of the periodic table. Alkali elements are:
- Lithium(Li)
- Sodium(Na)
- Potassium (K)
- Rubidium (Ru)
- Cesium (Cs)
- Francium (Fr)
They have occupied successive periods from first to seven. Francium is a radioactive element with very low half-life.
Electronic Configuration:
- Alkali metals have one electron in their valence shell.
- The electronic configuration is given by ns1. For example, the electronic configuration of lithium is given by 1ns1 2ns1.
- They tend to lose the outer shell electron to form cations with charge +1 (monovalent ions).
This makes them the most electropositive elements and due to the same reason, they are not found in the pure state.