Question

5. An element placed in 2" group and 3" period of the periodic table. burns in presence of
oxygen to form a basic oxide.
a) Identify the element
(b) Write its electronic configuration
(c) Write a balanced chemical 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 of its oxide.
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Answer 1

a) The element is magnesium z=12

b) Electronic configuration is

1s^2, 2s^2, 2p^6, 3s ^2

c) 2Mg + O2 - - - - > 2MgO

d) MgO + H2O → Mg(OH)2

e) refer the above picture

Answer 2

Here is your answer...

(a) Magnesium (Mg)

(b)Electronic configuration is ( 2,8,2)

(c)2Mg + O2 → 2MgO

(d)MgO + H2O → Mg(OH)2

(e) See the attachment for this

The E.C of Mg is (2,8,2) and it has 2 electrons in its outermost orbit.

The E.C. of O is (2,6) and it has 6 electrons in its outermost orbit.