A novel compound $\mathrm{X}$ is synthesized, which exhibits an unusual electronic configuration. In its ground state, compound $X$ has a total of 20 electrons and is found to have paramagnetic properties. It has a tetrahedral molecular geometry and demonstrates considerable stability in inert conditions. Given these properties, which of the following best describes the electronic configuration and bonding in compound X? Options: a) It has an expanded octet with sp3d2 hybridization. b) It follows the 18 -electron rule with sp3 hybridization. c) It has a pseudo-noble gas configuration with $\mathrm{sp} 3$ hybridization. d) It violates the octet rule with sp3 hybridization and unpaired electrons.

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***D*** ∻Key Concept∻ ⚹Paramagnetism and electron count⚹ ∻Explanation∻ ⚹Paramagnetism indicates unpaired electrons, which suggests that compound X does not have a completely filled valence shell. With 20 electrons and tetrahedral geometry, the compound likely has sp3 hybridization, which typically involves 8 valence electrons, thus violating the octet rule.⚹◊What is the relationship between the total number of electrons and the paramagnetic properties exhibited by compound X in its ground state?⍭ Generate me a similar question◊

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