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Draw the lewis structure of NCO⁻ (with minimized formal charges) and then choose the appropriate formal charges for each of the atoms.
Draw the lewis structure of NCO⁻ (with minimized formal charges) and then choose the appropriate formal charges for each of the atoms.A) N = 0, C = 0, 0 = -1 B) N = -1, C = +1, O = -1 C) N = 0, C = 0, 0 = 0 D) N = +1, C = -1, 0 = -1 E) N=-1, C = 0, 0 = 0
The Lewis structure of the NCO- ion with minimized formal charges results in Nitrogen and Carbon having a formal charge of 0, while Oxygen has a formal charge of -1, corresponding to option A.To draw the Lewis structure of the NCO- ion with minimized formal charges:Count the total number of valence electrons in the molecule. Nitrogen (N) has 5, carbon (C) has 4, oxygen (O) has 6, and the extra electron from the negative charge (⁻) adds one more, making a total of 16 valence electrons.Arrange the atoms with carbon in the center since it is less electronegative than nitrogen and oxygen. Connect the atoms with single bonds initially.Distribute the remaining electrons to complete the octet rule; oxygen will generally have a full octet before carbon or nitrogen.Place double bonds where needed to give all atoms full octets and to use all 16 valence electrons.Calculate formal charges for each atom to see which structure is most stable. The formula for calculating formal charge is V - (N + B/2), where V is the number of valence electrons, N is the number of non-bonding electrons, and B is the number of bonding electrons.Using the formula and knowing the electron configurations, the formal charges turn out to be:Nitrogen (N): 5 - (0 + 4/2) = 0Carbon (C): 4 - (0 + 4/2) = 0Oxygen (O): 6 - (4 + 4/2) = -1Therefore, the appropriate formal charges are N = 0, C = 0, O = -1, which corresponds to option A....