In the most plausible Lewis structure for SOF4, there are

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We need to evaluate the Lewis-structure possibilities for SOF4 and decide which statement best describes the most plausible structure.

Option A: "5 single bonds and 1 double bond around S." This would imply six bonds around sulfur (five single bonds plus one double bond), which is not consistent with a typical valence-bond description for SOF4. Sulfur can expand its octet, but the common resonance form for SOF4 features five regions of electron density around S (four S–F bonds and one S=O bond as a double bond counts as one region). Having six bond interactions around S would push the structure into an unlikely hypervalent arrangement with an unusual distribution of electron density, making this option less plausible.

Option B: "4 single bonds and 1 double bond around S." This is a reasonable alternative: sulfur bonded to four fluorine atoms by single bonds and to oxygen by a double bond, giving five electron domains around S (consistent with a trigonal bipyramidal-like arrangement if we consider the lone pair considerations in related species). However, the question asks for the most plausible Lewis structure, and in many accepted representations of SOF4, the lone-pair count on S and the exact distribution can differ depending on how you count lone pairs and formal charges. This option could be plausible, but it does not uniquely capture the most widely discussed depiction for SOF4 in introductory contexts where the emphasis is on five S–X bonds rather than substituting a double bond.

Option C: "5 single bonds around S." This states that sulfur forms five single bonds (to four fluorines and to oxygen) with no lone pairs on S. This configuration uses five bonding pairs around S, which is a common way to represent certain hypervalent sulfur species where S can accommodate more than an octet. While there is debate about whether the S=O double bond is present in all resonance forms, the idea of five bonding interactions around S (five single bonds) is a simple, widely taught depiction that avoids introducing a lone pair or a formal charge on sulfur in this context. This makes Option C a strong and straightforward choice for the most plausible Lewis structure in many introductory discussions of SOF4.

Option D: "5 single bonds and 1 lone pair electrons around S." This would imply seven regions of electron density around S (five bonds plus one lone pair), which is inconsistent with the typical count for SOF4 in standard representations. Having a lone pair on S in addition to five bonds would violate the expected valence and is not supported by common Lewis structures for this molecule.

Option E: "4 single bonds, 1 double bond, and 1 lone pair electrons around S." This sums to seven regions around S (four singles = four bonds, one double = one region, plus one lone pair = another region). That exceeds the usual electron-domain count for the central sulfur in SOF4 and does not align with the standard five-domain picture used for this species. Therefore this option is unlikely.

In summary, the most consistent description among the given choices, aligning with a straightforward five-domain depiction for SOF4 and avoiding extra lone pairs or multiple counting of bonds, is Option C: five single bonds around S. The other options introduce extra bond interactions, lone pairs, or miscounted electron domains that do not match the common Lewis representations for SOF4 in this context.

In the most plausible Lewis structure for SOF4, there are

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