Home
Class 11
CHEMISTRY
A solution of sodium metal in liquid amm...

A solution of sodium metal in liquid ammonia is strongly reducing due to the presence of

A

Sodium atom

B

Sodium hydride

C

Sodium amide

D

Solvated electrons

Text Solution

AI Generated Solution

The correct Answer is:
To solve the question regarding why a solution of sodium metal in liquid ammonia is strongly reducing, we can break down the explanation into clear steps: ### Step-by-Step Solution: 1. **Understanding the Reaction**: When sodium metal (Na) is dissolved in liquid ammonia (NH₃), it reacts to form ammoniated sodium ions. The reaction can be represented as: \[ \text{Na} + \text{NH}_3 \rightarrow \text{Na}^+ + \text{e}^- + \text{NH}_3 \] 2. **Formation of Ammoniated Sodium**: The sodium ion (\( \text{Na}^+ \)) formed is surrounded by ammonia molecules, leading to the formation of ammoniated sodium. This can be represented as: \[ \text{Na}^+ \cdot \text{NH}_3 \] 3. **Presence of Free Electrons**: The reaction produces free electrons (\( \text{e}^- \)) in the solution. These electrons are not bound to any specific atom and can move freely through the liquid ammonia. 4. **Conductivity of the Solution**: The presence of these free electrons allows the solution to conduct electricity. This is why the solution is termed as "highly conducting." 5. **Reducing Nature**: The free electrons in the solution are responsible for its strong reducing nature. A reducing agent is a substance that donates electrons to another substance, thereby reducing it. Since the ammoniated electrons can easily donate electrons, the solution acts as a strong reducing agent. 6. **Color of the Solution**: The solution of sodium in liquid ammonia is blue in color due to the presence of these ammoniated electrons. This is an important characteristic that helps identify the solution. 7. **Conclusion**: Therefore, the solution of sodium metal in liquid ammonia is strongly reducing due to the presence of free electrons (also referred to as solvated or ammoniated electrons). ### Final Answer: The solution of sodium metal in liquid ammonia is strongly reducing due to the presence of **solvated electrons**. ---
To solve the question regarding why a solution of sodium metal in liquid ammonia is strongly reducing, we can break down the explanation into clear steps: ### Step-by-Step Solution: 1. **Understanding the Reaction**: When sodium metal (Na) is dissolved in liquid ammonia (NH₃), it reacts to form ammoniated sodium ions. The reaction can be represented as: \[ \text{Na} + \text{NH}_3 \rightarrow \text{Na}^+ + \text{e}^- + \text{NH}_3 \] ...
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • S-BLOCK GROUP 1 - ALKALI METALS

    CENGAGE CHEMISTRY ENGLISH|Exercise Archives Assertion Reasoning|3 Videos

  • S-BLOCK GROUP 1 - ALKALI METALS

    CENGAGE CHEMISTRY ENGLISH|Exercise Archives Fill In The Blanks|2 Videos

  • S-BLOCK GROUP 1 - ALKALI METALS

    CENGAGE CHEMISTRY ENGLISH|Exercise Archives Multiple Correct|5 Videos

  • REDOX REACTIONS

    CENGAGE CHEMISTRY ENGLISH|Exercise Archives (Integers)|1 Videos

  • S-BLOCK GROUP 2 - ALKALINE EARTH METALS

    CENGAGE CHEMISTRY ENGLISH|Exercise Ex 5.1 Objective|2 Videos

Similar Questions

Explore conceptually related problems

Alkali metals oxide are obtained by combustion of the metals.Although Na normally gives Na_2O_2 ,it will take up further oxygen at elevated pressure and temperature to form NaO_2 .The per and superoxides of the heavier alkalies can also be prepared by passing stoichiometric amounts of oxygen into their solution in liquid ammonia. The different alkali metal oxides can be distinguished by reaction with water.The superoxides reacts with CO_2 and give oxygen gas.The stability of per and superoxides is based upon that larger cation can stablise larger anion, due to larger lattice energy. Alkali metals dissolve in liquid ammonia.Dilute solutions are dark blue in colour but as the concentration increases above 3M, the colour changes to copper bronze and the solution acquires the metallic lusture due to the formation of metal ions clusters.The solutions of alkali metals in liquid ammonia are good conductors of electricity due to the presence of ammoniated cations and ammoniated electrons.However, the conductivity decreases as the concentrations increases, since ammoniated electrons and ammoniated cation associate. Solution of sodium metals in liquid ammonia is strongly reducing due to the presence of :

A solution of sodium in liquid ammonia serves as a reducing agent due to the reaction.

A solution of sodium in liquid ammonia is blue in colour due to:

Why does the solution of sodium in liquid ammonia possess strong reducing nature?

A highly pure dilute solution of sodium in liquid ammonia:

Alkali metals oxide are obtained by combustion of the metals.Although Na normally gives Na_2O_2 ,it will take up further oxygen at elevated pressure and temperature to form NaO_2 .The per and superoxides of the heavier alkalies can also be prepared by passing stoichiometric amounts of oxygen into their solution in liquid ammonia. The different alkali metal oxides can be distinguished by reaction with water.The superoxides reacts with CO_2 and give oxygen gas.The stability of per and superoxides is based upon that larger cation can stablise larger anion, due to larger lattice energy. Alkali metals dissolve in liquid ammonia.Dilute solutions are dark blue in colour but as the concentration increases above 3M, the colour changes to copper bronze and the solution acquires the metallic lusture due to the formation of metal ions clusters.The solutions of alkali metals in liquid ammonia are good conductors of electricity due to the presence of ammoniated cations and ammoniated electrons.However, the conductivity decreases as the concentrations increases, since ammoniated electrons and ammoniated cation associate. On dissolving smaller (less than 3M) amount of sodium metal in liquid ammonia at low temperature , which one of the following does not occur ?

Alkali metals oxide are obtained by combustion of the metals.Although Na normally gives Na_2O_2 ,it will take up further oxygen at elevated pressure and temperature to form NaO_2 .The per and superoxides of the heavier alkalies can also be prepared by passing stoichiometric amounts of oxygen into their solution in liquid ammonia. The different alkali metal oxides can be distinguished by reaction with water.The superoxides reacts with CO_2 and give oxygen gas.The stability of per and superoxides is based upon that larger cation can stablise larger anion, due to larger lattice energy. Alkali metals dissolve in liquid ammonia.Dilute solutions are dark blue in colour but as the concentration increases above 3M, the colour changes to copper bronze and the solution acquires the metallic lusture due to the formation of metal ions clusters.The solutions of alkali metals in liquid ammonia are good conductors of electricity due to the presence of ammoniated cations and ammoniated electrons.However, the conductivity decreases as the concentrations increases, since ammoniated electrons and ammoniated cation associate. Select the correct choice for alkali metal oxides.

Alkali metals oxide are obtained by combustion of the metals.Although Na normally gives Na_2O_2 ,it will take up further oxygen at elevated pressure and temperature to form NaO_2 .The per and superoxides of the heavier alkalies can also be prepared by passing stoichiometric amounts of oxygen into their solution in liquid ammonia. The different alkali metal oxides can be distinguished by reaction with water.The superoxides reacts with CO_2 and give oxygen gas.The stability of per and superoxides is based upon that larger cation can stablise larger anion, due to larger lattice energy. Alkali metals dissolve in liquid ammonia.Dilute solutions are dark blue in colour but as the concentration increases above 3M, the colour changes to copper bronze and the solution acquires the metallic lusture due to the formation of metal ions clusters.The solutions of alkali metals in liquid ammonia are good conductors of electricity due to the presence of ammoniated cations and ammoniated electrons.However, the conductivity decreases as the concentrations increases, since ammoniated electrons and ammoniated cation associate. KO_2 is used in oxygen cylinders in space and submarines because it :

In the following questions , a statement of assertion (A) is followed by a statement of reason (R). Br A: Dilute solutions of alkali metal in liquid ammonia are paramagnetic in nature R: Formation of ammoniated cations takes place when alkali metals dissolve in ammonia.

All alkali metals dissolve in anhydrous liquid ammonia to give blue colour solution. It is the ammoniated electron which is reponsible for the blue colour of the solution, and the electrical conductivity is due to the ammoniated cation, [M(NH_(3))_(x)]^(+) as well as the ammoniated electron, [e(NH_(3))_(y)]^(-) , value of x and y depend on the extent of solvation by NH_(3) . Dilute solutions are paramagnetic due to free ammoniated electrons. Q. Ammoniated solutions of alkali metals are reducing agents due to the presence of free ammoniated or solvated electrons that can reduce: (I) O_(2) "to" O_(2)^(2-) (II) K_(2)[Ni(CN)_(4)] " to "K_(4)[Ni(CN)_(4)] (III) Aromatic ring (IV) Non-terminal alkyne Choose the correct code:

Home
Profile