Ok help me answer this question below: In describing the complex ion formed from iron(III) ion, Fe³(aq), and thiocyanate ion, SCN (aq), theformula for the complex is written as [FeNCS2+], rather than [FeSCN²+], as one might expect. Writethe Lewis structure for the SCN ion and use formal charge to show why the iron(III) ion is morelikely to link to the nitrogen end of thiocyanate.

The Lewis structure is the representation of valence electrons in a molecule. It is a representation of the arrangement of valence electrons present in an atom in a molecule. The complete Lewis structure of SCN- is given below. The formal charge can be determined using the formula Each lone pair of electrons represents two non-bonding electrons. The number of valence electrons of S is 6, there are three lone pairs (6 nonbonding electrons), and there is one bond on S. The number of valence electrons of C is 4 and there are four bonds on C. The number of valence electrons of N is 5, there is one lone pair (2 nonbonding electrons), and there are three bonds on N. In SCN-, the negative charge is present on S and C and N have no charge. The Lewis structure of NCS- is shown below. The number of valence electrons of S is 6, there are two lone pairs (4 nonbonding electrons), and there are two bonds on S. The number of valence electrons of C is 4 and there are four bonds on C. The number of valence electrons of N is 5, there are two lone pairs (4 nonbonding electrons), and there are two bonds on N. In NCS-, the negative charge is present on N and C and S have no charge. In [FeSCN]2+, the negative charge is on S, and in [FeNCS]2+, the negative charge is on N. N being more electronegative than S, thus, the negative charge on N is more stable. Hence, Fe3+ will bind to the N end of thiocyanate rather than the S end. In [FeNCS]2+, the negative charge is on N which is more stable than the negative charge on S as in the case of [FeSCN]2+. Hence, Fe3+ prefers the N-end rather than the S-end.