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I don't recall seeing that structure in my notes, but assuming that carbon is the central atom, the most electronegative atom should carry the negative formal charge. In this case, N should have the negative charge since it's more electronegative than sulfur. So the most stable structure would go: S = C = N.
Yes, the example in the book also shows that the most stable structure is S = C = N. Nitrogen does have a -1 formal charge in this structure, and carbon and sulfur both have formal charges of 0. This example is on page 85 in the book. In the structure C = N = S, the formal charges are -2 for C, +1 for N, and 0 for S, and the structure C = S = N has the charges -2 for C, +2 for S, and -1 for N. In these examples, S never has a formal charge of -1.
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