a student proposes the following lewis structure for the isocyanate (nco^-) ion.\n :c\\equiv o - \\ddot{n}…

a student proposes the following lewis structure for the isocyanate (nco^-) ion.\n :c\\equiv o - \\ddot{n}: ^-\nassign a formal charge to each atom in the students lewis structure.\n

a student proposes the following lewis structure for the isocyanate (nco^-) ion.\n :c\\equiv o - \\ddot{n}: ^-\nassign a formal charge to each atom in the students lewis structure.\n

Answer

Explanation:

Step1: Recall formal charge formula

Formal charge (=\text{Valence electrons}-\text{Non - bonding electrons}-\frac{1}{2}\text{Bonding electrons})

Step2: Calculate for (C)

Valence electrons of (C = 4). Non - bonding electrons (= 2). Bonding electrons (= 6). Formal charge (=4 - 2-\frac{1}{2}\times6=4 - 2 - 3=-1)

Step3: Calculate for (O)

Valence electrons of (O = 6). Non - bonding electrons (= 0). Bonding electrons (= 6). Formal charge (=6-0-\frac{1}{2}\times6=6 - 3=+3)

Step4: Calculate for (N)

Valence electrons of (N = 5). Non - bonding electrons (= 6). Bonding electrons (= 2). Formal charge (=5 - 6-\frac{1}{2}\times2=5 - 6 - 1=-2)

Answer:

atom formal charge
(C) (-1)
(O) (+3)
(N) (-2)