$\underset{magnesium}{2 Mg (s)} + \underset{Oxygen}{O_{2} (g)} \to \underset{Magnesium oxide}{2 MgO (s)}$
In this reaction, explain the experiment that you conduct to decide on the product as a basic oxide.

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Solution

$\underset{magnesium}{2 Mg (s)} + \underset{Oxygen}{O_{2} (g)} \to \underset{Magnesium oxide}{2 MgO (s)}$
The experiment that is conducted to decide on the product as a basic oxide is as follows:
Take the product of the reaction [Magnesium oxide(MgO)] and dissolve it in water.
$\underset{Magnesium oxide}{MgO (s)} + \underset{Water}{H_{2} O (l)} \to \underset{Magnesium Hydroxide}{2 Mg {(OH)}_{2} (aq .)}$
3. Add red litmus paper to the aqueous solution of Magnesium oxide.
4. If a red litmus paper turns blue. This indicates that an aqueous solution of Magnesium oxide is either alkaline or basic in nature.

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2Mg(s)magnesium+O2(g)Oxygen→2MgO(s)MagnesiumoxideIn this reaction, explain the experiment that you conduct to decide on the product as a basic oxide.

$\underset{magnesium}{2 Mg (s)} + \underset{Oxygen}{O_{2} (g)} \to \underset{Magnesium oxide}{2 MgO (s)}$
In this reaction, explain the experiment that you conduct to decide on the product as a basic oxide.