An element is placed in the 2nd group and 3rd period of the periodic table burns in presence of oxygen to form a basic oxide.

The balanced equation when this oxide is dissolved in water is :

M g O (s) + H_{2} O (l) \to 2 M g (O H)_{2} (a q)

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M g O (s) + H_{2} O (l) \to M g (O H)_{2} (a q)

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2 M g O (s) + H_{2} O (l) \to 2 M g (O H)_{2} (a q)

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M g O (s) + 2 H_{2} O (l) \to M g (O H)_{2} (a q)

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Solution

The correct option is A $M g O (s) + H_{2} O (l) \to M g (O H)_{2} (a q)$
The element is magnesium (Mg).
The balance equation when this oxide is dissolved in water is given by -
$M g O (s) + H_{2} O (l) \to M g (O H)_{2} (a q)$

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Question 42
An element is placed in 2nd Group and 3rd Period of the Periodic Table, burns in presence of oxygen to form a basic oxide.

(a) Identify the element.

(b) Write the electronic configuration.

(d) Write a balanced equation when this oxide is dissolved in water.

(e) Draw the electron dot structure for the formation of this oxide.

MgO

HCl

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