Which of the following statements correctly describes the Lewis dot structure of the ion SnF_6^{2-}?

• A. Sn is surrounded by six F atoms, each forming a double bond, and the ion carries a 2+ charge.
• B. Sn is surrounded by four F atoms, each forming a double bond, and the ion carries a 2- charge.
• C. Sn is surrounded by six F atoms, each forming a single bond, and the ion carries a 2- charge.
• D. Sn is surrounded by six F atoms, each forming a single bond, and the ion carries a 2+ charge.

Answer: (C)

Verified step by step guidance

1. Identify the central atom and the surrounding atoms in the ion SnF_6^{2-}. Here, Sn (tin) is the central atom, and it is surrounded by six fluorine (F) atoms.
2. Determine the total number of valence electrons available. Tin (Sn) is in group 14, so it has 4 valence electrons. Each fluorine atom has 7 valence electrons, and there are 6 fluorines, so total from fluorines is 6 × 7 = 42 electrons. The ion has a 2- charge, which means 2 additional electrons are added. So, total valence electrons = 4 + 42 + 2 = 48 electrons.
3. Distribute the electrons to form bonds. Since Sn is surrounded by six F atoms, and fluorine typically forms single bonds, assign one single bond (2 electrons) between Sn and each F atom. This accounts for 6 × 2 = 12 electrons used in bonding.
4. Assign the remaining electrons as lone pairs to complete the octet on each fluorine atom. Each fluorine needs 6 more electrons (3 lone pairs) to complete its octet after forming one single bond.
5. Check the overall charge and bonding. Since the ion carries a 2- charge, and all fluorines are singly bonded to Sn, the correct Lewis structure is Sn surrounded by six F atoms, each forming a single bond, and the ion carries a 2- charge.