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Step 1:: Determine the central atom and the overall charge on the molecule.
In the given compound, the central atom is Sulfur (S) and there are six Bromine (Br) atoms surrounding it. The sum of the charges on all atoms must be equal to the overall charge of the molecule, which is zero in this case.
Step 2:: Draw a rough sketch of the Lewis structure.
Place the central atom in the middle, then add the remaining atoms around it, ensuring that they are equally spaced.
Step 3:: Calculate the total number of valence electrons in the molecule.
Sulfur has 6 valence electrons, and each Bromine atom has 7 valence electrons. Since there are six Bromine atoms, the total number of valence electrons is: \text{Total valence electrons} = 6\ (\text{from Sulfur}) + 6 \times 7\ (\text{from Bromine}) = 54\ \text{valence electrons}
Step 4:: Place the valence electrons on the rough sketch.
Distribute the valence electrons as lone pairs and bonds. Remember that each Bromine atom needs one bond to complete its octet, and Sulfur needs two bonds to complete its octet.
Step 5:: Finalize the Lewis structure.
Add any remaining electrons as lone pairs on the Sulfur atom and ensure that each atom has a complete octet (except for Hydrogen, which only needs 2 electrons to complete its duet).
Step 6:: Check the formal charges of each atom.
Calculate the formal charge for each atom by subtracting the number of valence electrons from the total number of electrons around the atom. For Sulfur: \text{Formal charge} = 6\ (\text{valence electrons}) - 2\ (\text{bonds}) - 6\ (\text{lone pairs}) = 6 - 2 - 6 = - 2 For Bromine: \text{Formal charge} = 7\ (\text{valence electrons}) - 1\ (\text{bond}) - 6\ (\text{lone pairs}) = 7 - 1 - 6 = 0
Step 7:: Ensure that the overall charge is correct.
The overall charge on the molecule is zero, which is consistent with the calculated formal charges.
Step 8:: Draw the final Lewis structure for (SBr6).
Final Answer
The Lewis structure for (SBr6) is: \chemfig{S(-Br)(-Br)(-Br)(-Br)(-Br)(-Br)} The Sulfur atom has a formal charge of - 2, and each Bromine atom has a formal charge of 0.
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