To determine the number of unpaired electrons in a paramagnetic diatomic molecule of an element with atomic number 16, we first need to understand the electronic configuration and related concepts:
Determine the Element: An element with atomic number 16 is sulfur (S).
Electronic Configuration of Sulfur (S): The standard electronic configuration is:
1s^2 2s^2 2p^6 3s^2 3p^4.
Valence Electrons: Sulfur has six valence electrons in the 3s and 3p orbitals.
Molecular Orbital Theory: For diatomic molecules like S2, molecular orbitals are formed. According to molecular orbital theory:
- The electronic configuration of S2 involves pairing electrons in molecular orbitals.
Determine Unpaired Electrons: In the molecular orbital configuration for S2:
- S2 molecule fills up to σ and π* orbitals.
- The π* orbitals each contain one unpaired electron because 4 electrons can only completely fill 2 of the 3 degenerate π* orbitals, leaving 2 orbitals half-filled.
Hence, the number of unpaired electrons in the S2 molecule is 2.
Conclusion: The correct answer is 2 unpaired electrons. Thus, the number of unpaired electrons in a paramagnetic diatomic molecule of sulfur is 2.
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