Which of the following statements correctly describes the Lewis dot structure of neutral sulfur hexabromide (SBr_6)?

• A. Sulfur is surrounded by six bromine atoms, each forming a single bond, and sulfur has no lone pairs.
• B. Sulfur is surrounded by six bromine atoms, each forming a single bond, and sulfur has one lone pair.
• C. Sulfur is surrounded by six bromine atoms, each forming a double bond, and sulfur has two lone pairs.
• D. Sulfur is surrounded by four bromine atoms, each forming a single bond, and sulfur has two lone pairs.

Answer: (A)

Verified step by step guidance

1. Identify the central atom and the surrounding atoms in the molecule SBr_6. Sulfur (S) is the central atom, and it is bonded to six bromine (Br) atoms.
2. Determine the total number of valence electrons available. Sulfur has 6 valence electrons, and each bromine atom has 7 valence electrons. Calculate the total valence electrons for the molecule by adding sulfur's and all bromines' valence electrons.
3. Distribute the electrons to form bonds between sulfur and each bromine atom. Each single bond consists of 2 electrons. Since there are six bromine atoms, assign 2 electrons per bond, totaling 12 electrons used in bonding.
4. Assign the remaining electrons as lone pairs to the bromine atoms first to complete their octets. Each bromine needs 6 more electrons (3 lone pairs) after bonding to sulfur.
5. Check the sulfur atom's electron count after bonding. Since sulfur can expand its octet, it can accommodate 12 electrons (6 bonds × 2 electrons each) and does not need any lone pairs. Confirm that this matches the Lewis structure where sulfur is bonded to six bromines with single bonds and has no lone pairs.