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.
(c) Write the balanced equation when it burns in the presence of air.
(d) Write a balanced equation when this oxide is dissolved in water.
(e) Draw the electron dot structure for the formation of this oxide.

(a) The element is Magnesium.

(b) Its Electronic Configuration is - 2,8,2

(c) The balanced equation is shown below:
$2Mg + O_2 \rightarrow 2MgO$

(d) The balanced equation is shown below:
$MgO+ H_2O \rightarrow Mg(OH)_2$

(e) The electron dot structure is shown below:

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