Which one of the following alkaline earth metal ions has the highest ionic mobility in its aqueous solution?
- \(Be^{2+}\)
- \(Mg^{2+}\)
- \(Ca^{2+}\)
- \(Sr^{2+}\)
The Correct Option is D
Solution and Explanation
In aqueous solution, the ionic mobility is inversely proportional to the charge density on the ion. Hence \(Sr^{2+}\) has highest ionic mobility in water.
So, the correct option is (D): \(Sr^{2+}\)
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Group 2 Elements
The group two or alkaline earth metals are s-block elements with two electrons in their s-orbital. They are alkaline earth metals. They are named so because of the alkaline nature of the hydroxides and oxides.
Alkaline earth metals are characterized by two s-electrons. This group of elements includes:
- Beryllium (Be)
- Magnesium (Mg)
- Calcium (Ca)
- Strontium (Sr)
- Barium (Ba)
- Radium (Ra)
Elements whose atoms have their s-subshell filled with their two valence electrons are called alkaline earth metals. Their general electronic configuration is [Noble gas] ns2. They occupy the second column of the periodic table and so-called as group two metals also.
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