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HCl was passed through a solution of $CaCl_2$,$MgCl_2$ and $NaCl$. Which of the following compound(s) crystallise(s)?
HCl was passed through a solution of $CaCl_2$,$MgCl_2$ and $NaCl$. Which of the following compound(s) crystallise(s)?
Updated On: Jun 5, 2024
- Both $MgCl_2$ and $CaCl_2$
- Only $NaCl$
- Only $MgCl_2$
- $NaCl$, $MgCl_2$ and $CaCl_2$
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The Correct Option is B
Solution and Explanation
On passing $HCl$ through aqueous solution of $CaCl_2, MgCl_2$ and $NaCl$, crystals of pure $NaCl$ seperate out. Calcium and magnesium chloride being more soluble than $NaCl$, remain in solution.
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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.
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