Question:

The number of unpaired electrons in a paramagnetic diatomic molecule of an element with atomic number 16 is :

Updated On: Oct 13, 2023

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The Correct Option is A

Solution and Explanation

The atomic number of the element is 16, which corresponds to sulfur (S). In a diatomic molecule of sulfur (S₂), each sulfur atom contributes six valence electrons (since sulfur is in group 16 of the periodic table). When two sulfur atoms bond together to form a diatomic molecule, they share their electrons, resulting in a total of 12 valence electrons in the molecule. To determine the number of unpaired electrons, you can use molecular orbital theory. In the case of a sulfur molecule (S₂), the molecular orbital diagram shows that there are 2 unpaired electrons.

So, the correct answer is (A): 2

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Concepts Used:

P-Block Elements

P block elements are those in which the last electron enters any of the three p-orbitals of their respective shells. Since a p-subshell has three degenerate p-orbitals each of which can accommodate two electrons, therefore in all there are six groups of p-block elements.
P block elements are shiny and usually a good conductor of electricity and heat as they have a tendency to lose an electron. You will find some amazing properties of elements in a P-block element like gallium. It’s a metal that can melt in the palm of your hand. Silicon is also one of the most important metalloids of the p-block group as it is an important component of glass.

P block elements consist of:

Group 13 Elements: Boron family
Group 14 Elements: Carbon family
Group 15 Elements: Nitrogen family
Group 16 Elements: Oxygen family
Group 17 Elements: Fluorine family
Group 18 Elements: Neon family