Question:
The alkali metals dissolve in ammonia to give a deep blue solution which is conducting in nature.
$M+\left(x+y\right) NH_{3} \to\left[M\left(NH_{3}\right)_{x}\right]^{2+}+2\left[e\left(NH_{3}\right)_{y}\right]^{-}$
Which of the following is not true about the solutions of alkali metals in liquid ammonia ?
The alkali metals dissolve in ammonia to give a deep blue solution which is conducting in nature.
$M+\left(x+y\right) NH_{3} \to\left[M\left(NH_{3}\right)_{x}\right]^{2+}+2\left[e\left(NH_{3}\right)_{y}\right]^{-}$
Which of the following is not true about the solutions of alkali metals in liquid ammonia ?
Updated On: Jul 7, 2022
- The blue colour is due to ammoniated electron
- The solution is paramagnetic
- The blue colour changes to brown on standing
- In concentrated solution blue colour changes to bronze and becomes diamagnetic
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The Correct Option is C
Solution and Explanation
Answer (c) The blue colour changes to brown on standing
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Concepts Used:
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.