Question

A magnesium ribbon is burnt in oxygen to give a white compound X accompanied by emission of light. If the burning ribbon is now placed in an atmosphere of nitrogen, it continues to burn and forms a compound Y. Write the chemical formulae of X and Y.

(1 Point)

(a) X= MgO , Y = Mg₃N₂

(b) X= MgS , Y = MgN

(c) X=NaO , Y= MgO

(d) X= MgCl2 , Y= MgO​

Answer 1

ANSWER

Magnesium ribbon burns in oxygen(O  

2

​  

) to form magnesium oxide(MgO).  

2Mg+O  

2

​  

→2MgO

Therefore, X is MgO.

When MgO is dissolved in water following reaction takes place:

MgO+H  

2

​  

O→Mg(OH)  

2

​  

.

Answer 2

$\Large{\underline{\underline{\red{\tt{\purple{\leadsto } SolutioN:-}}}}}$

We know that when we burn magnesium ribbon it reacts with oxygen to form magnesium oxide.The reacⁿ would be :-

$\boxed{\red{\bf \blue{\bullet}\:\:\underset{\blue{Magnesium}}{2Mg}\:+\:\underset{\blue{Oxygen}}{O_2}\:\longrightarrow \underset{\blue{Magnesium\: Oxide}}{2MgO}}}$

Also we know that when magnesium burns in the presence of Nitrogen it forms magnesium nitride. Hence the reaction would be :-

$\boxed{\red{\bf \blue{\bullet}\:\:\underset{\blue{Magnesium}}{3Mg}\:+\:\underset{\blue{Nitrogen}}{N_2}\:\longrightarrow \underset{\blue{Magnesium\:Nitride}}{Mg_3N_2}}}$

Hence here we can conclude that compound X is $\green{\bf MgO}$ and compound Y is $\green{\bf Mg_3N_2}$.

$\boxed{\purple{\bf \pink{\dag}\:Hence\: correct\: option\:is\:[a].}}$

$\rule{200}2$

$\underline{\blue{\bf \leadsto Some\:related\: Information.}}$

When we burn magnesium ribbon it burns with dazzling white flame. When we try to check whether it is acid or basic we can add water to it . Then we can use litmus paper to check . It changes red litmus to blue indicating its basic behaviour.

$\boxed{\red{\bf \blue{\bullet}\:\:\underset{\blue{Magnesium\:Oxide}}{MgO}\:+\:\underset{\blue{Water}}{H_2O}\:\longrightarrow \underset{\blue{Magnesium\: hydroxide}}{Mg(OH)_2}}}$