Question

How many unpaired electrons are present in the ground state of the atoms in group 6a(16)?

Answer 1

Lets take one element from Group 6A, Let it be oxygen, The electronic configuration of Oxygen is as follow,

                           O  =  8  = 1s², 2s², 2px², 2py¹, 2px¹

There are 6 electrons in the valence shell of elements present in Group 6A. The unpaired electrons in 2px and 2py are involved in forming covalent bond, while the pair of electrons in 2s and 2px are unshared and act as lone pair of electrons.

Result:
          There are TWO unpaired electrons present in the ground state of Group 6A elements.

Answer 2

There are two unpaired electrons in the ground state of atoms of elements in group 6a(16).

The periodic table is arranged in groups and periods. The atoms of elements in the same group have the same number of valence (outermost) electrons. The elements in the same period have the same number of shells.

The elements in group 6a(16) have six outermost electrons. four of them are part of two lone pairs while two are unpaired electrons that are readily available for bonding. This is why they mostly form compounds of the sort AX2 where A is the central group 6a(16) element and X are other  elements.

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