Question

If valence shell electronic configuration of an element is 3s2, 3p3


the element will belong to:

A. Group V, Period 3
B. Group II, Period 5

C. Group III, Period 3
D. Group I, Period 6
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Answer 1

Answer:

A. Group V, Period 3

Explanation:

The ground state outer electronic configuration of an element is 3s²3p³.”

Supposing that this element obeys Madelung rule, its position in the Periodic Table is easily deduced from the ground state electronic configuration. The last filled shell is 3, thus the element is located in the third period (third row from top to bottom). The p block of Periodic Table begins at the group 13 and ends at group 18. The 3p orbital is filled with three electrons, thus this element is the third of the p block, i.e. it is located at group 15.

The element is placed at group 15 of third period of Periodic Table, where phosphorus sits.

The electronic configuration of the given element is 1s²2s²2p63s²3p³

The element corresponding to above electronic configuration is Phosphorus. This element belongs to group 15 and period 3.

The element just below this is arsenic and it comes after the filling of 18 electrons due to the occurrence of transition elements (d-block).

The electronic configuration of arsenic is:

1s²2s²2p63s²3p64s²3d¹⁰4p³

This element also belongs to Group 15 but lies in 4th period.