An element is placed in the 2nd group and 3rd period of the periodic table, burns in presence of oxygen to form a basic oxide. The electronic configuration of the element is ____________ .

K, M, L (2, 8, 2)

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K, L, M (2, 6, 4)

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K, M, L (4, 6, 2)

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K, L, M (2, 8, 2)

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Solution

The correct option is C K, L, M (2, 8, 2)
As it is in 3rd period, it has 3 shells and since it is in the second group, it contains 2 valence electrons. Thus, the electronic configuration will be 2,8,2.

Hence, it has 12 electrons, that is, magnesium.

$2 M g + O_{2} \to 2 M g O$ .
It satisfies given condition which is a basic oxide.

Hence the correct option is D.

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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.

(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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