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.

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Solution

(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) $2 Mg(s) + O_{2} (g) \to 2 MgO(s)$

(d) $MgO(s) + H_{2} O(l) \to {Mg(OH)}_{2} (aq)$

(e)

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

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Reaction of Metals with Oxygen (Burnt in Air)

Standard X Chemistry

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(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) 2Mg(s)+O2(g)→2MgO(s) (d) MgO(s)+H2O(l)→Mg(OH)2(aq) (e)

(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) $2 Mg(s) + O_{2} (g) \to 2 MgO(s)$

(d) $MgO(s) + H_{2} O(l) \to {Mg(OH)}_{2} (aq)$

(e)