In my search to know the bonding in structures prefer $ceSF6$ ns found plenty of sources that claimed it was since sulfur has d orbitals come accommodate an increased octet, which made sense to me. But I likewise found sources prefer the document by Reed and Weinhold (1986) the say d orbitals contribute very tiny to the bonding in $ceSF6$. An alternate explanation is the $ceSF6$ has actually three-center/two-electron bonds. What ns don"t understand is why compounds choose $ceSF6$, $ceClF5$, $cePCl5$ exist for third row aspect centers, yet not $ceOF6$ if it has actually nothing to do with d orbitals? referrals would it is in great.

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Neither oxygen nor sulfur "expands its octet". Instead, sulfur in link such together $ceSF6$ delocalizes the bonds developed with the usual octet end multiple linkages. As defined in this answer, this delocalization in a neutral molecule comes v occupying ligand-based orbitals the are about nonbonding v a large main atom, yet antibonding through a small main atom since of ligand-ligand interactions. Thus developing a compound v delocalized bonding and also increased coordination number is more favored for third duration elements 보다 for second duration elements.

We can obtain such coordination through second-period elements if the ligand-based orbitals provided above space unoccupied, because that then the net ligand-ligand overlaps through the continuing to be orbitals are bonding. This usually calls for a cationic species such together the six-coordinate carbon complex reported through Yamaguchi et al.<1>, pictured listed below from the reference.

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1.Torahiko Yamaguchi, Yohsuke Yamamoto, Daisuke Kinoshita, Kin-ya Akiba, Yun Zhang, Christopher A. Reed, Daisuke Hashizume, and Fujiko Iwasaki. "Synthesis and Structure the a Hexacoordinate Carbon Compound", J. Am. Chem. Soc. 2008, 130, 22, 6894–6895. Https://