Question

An element 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 a 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 (Mg)

b) K,L,M
2,8,2
c) $2Mg\left(s\right)+O_2\left(g\right)\to 2MgO\left(s\right)$
d) $MgO\left(s\right)+H_{2}O\left(I\right)\to Mg\left(OH{)}_2\right(aq)$