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A metal $M$ on heating in nitrogen gas gives $Y. Y$ on treatment with $H_2O$ gives a colourless gas which when passed through $CuSO_4$ solution gives a blue colour. $Y$ is
A metal $M$ on heating in nitrogen gas gives $Y. Y$ on treatment with $H_2O$ gives a colourless gas which when passed through $CuSO_4$ solution gives a blue colour. $Y$ is
Updated On: Jul 5, 2022
- $NH_3$
- $Mg(NO_3)_2$
- $Mg_3N_2$
- $MgO$
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The Correct Option is C
Solution and Explanation
$3\underset{\text{M}}{ {M}}$ $ {g+N2->M}$$\underset{\text{Y}}{ {g_3}}$$ {N2}$
$M\underset{\text{Y}}{ {g3}}$ $ {N2 + 6H2O ->3Mg(OH)2 + }$$\underset{\text{colourless}}{ {2NH3 ?}}$$ {}$
$M\underset{\text{}}{ {}}$ $ {CuSO4 + 4NH3 -> }$$\underset{\text{Blue complex}}{ {[Cu(NH3)4]SO4}}$$ {}$
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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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