Question

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.

(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.

Answer 1

(a) Magnesium belongs to group 2 and period 3 and burns in presence of oxygen to form basic oxide because of its metallic nature.

(b) 2, 8, 2 in K, L and M shells respectively.

(c) $2\text{Mg(s)}+{\text{O}}_2\text{(g)}\to 2\text{MgO(s)}$

(d) $\text{MgO(s)}+{\text{H}}_2\text{O(l)}\to {\text{Mg(OH)}}_2\text{(aq)}$

(e)