The ground state electronic configuration of Sulphur is which is quite similar to oxygen since they are both Group 16 elements. But, unlike Oxygen, Sulphur has vacant d-orbitals in its valence shell as shown here.
2. In the excited state, the vacant 3d-orbital is occupied by an electron each from 3p and 3s-orbitals as shown here.
3. Thus, in the excited state, there are six orbitals with unpaired electrons which become available for bonding. Sulphur hexafluoride () is an example of a compound where Sulphur has six bonds.
4. Sulphur can form six bonds due to the presence of vacant 3d-orbitals which get occupied on excitation and create six orbitals with unpaired electrons that become available for bonding.
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Ground State Electronic Configuration of Sulphur:
The ground state electronic configuration of Sulphur is stated as [Ne]3s²3p⁴. This configuration indicates that Sulphur has 16 electrons, with two in the 3s orbital and four in the 3p orbitals. The notation [Ne] suggests that the configuration is similar to the noble gas Neon, emphasizing the filled inner electron shells.
Comparison with Oxygen:
The article notes that Sulphur's ground state configuration is quite similar to Oxygen since they both belong to Group 16 of the periodic table. Group 16 elements, also known as the chalcogens, share similar electronic configurations.
Vacant d-Orbitals in Sulphur's Valence Shell:
Unlike Oxygen, Sulphur is mentioned to have vacant d-orbitals in its valence shell. This is a crucial distinction and becomes significant when Sulphur enters the excited state.
Excited State Configuration of Sulphur:
In the excited state, the article asserts that the vacant 3d-orbital in Sulphur's valence shell is occupied by an electron each from the 3p and 3s orbitals. This process results in six orbitals with unpaired electrons becoming available for bonding.
Availability of Orbitals for Bonding:
The article emphasizes that in the excited state, Sulphur possesses six orbitals with unpaired electrons available for bonding. This information is crucial for understanding Sulphur's ability to form multiple bonds in compounds.
Sulphur Hexafluoride (SF6):
The example of Sulphur hexafluoride (SF6) is provided to illustrate Sulphur's capacity to form six bonds. The article attributes this ability to the presence of vacant 3d-orbitals, which, upon excitation, create six orbitals with unpaired electrons available for bonding.
In summary, the article discusses the ground state electronic configuration of Sulphur, compares it with Oxygen, highlights the presence of vacant d-orbitals in Sulphur's valence shell, and explains how Sulphur can form six bonds in the excited state, using Sulphur hexafluoride (SF6) as an example. This information underscores the importance of electronic configurations and the role of excited states in chemical bonding.
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