The number of unpaired electrons in a paramagnetic diatomic molecule of an element with atomic number 16 is :
- 2
- 3
- 4
- 1
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