for each resonance form, determine the formal charge for each atom. structure 1: :n≡n—:s: formal charge for…

for each resonance form, determine the formal charge for each atom. structure 1: :n≡n—:s: formal charge for n (left) = formal charge for n (center) = formal charge for s = structure 2: :n=n=s: formal charge for n (left) = formal charge for n (center) = formal charge for s = structure 3: :n—n≡s: formal charge for n (left) = formal charge for n (center) = formal charge for s =

for each resonance form, determine the formal charge for each atom. structure 1: :n≡n—:s: formal charge for n (left) = formal charge for n (center) = formal charge for s = structure 2: :n=n=s: formal charge for n (left) = formal charge for n (center) = formal charge for s = structure 3: :n—n≡s: formal charge for n (left) = formal charge for n (center) = formal charge for s =

Answer

Explanation:

Step1: Recall formal - charge formula

The formal - charge formula is $FC = V - N - \frac{B}{2}$, where $V$ is the number of valence electrons, $N$ is the number of non - bonding electrons, and $B$ is the number of bonding electrons.

Step2: Analyze Structure 1

  • For left N: Nitrogen has 5 valence electrons ($V = 5$). It has 2 non - bonding electrons ($N = 2$) and 6 bonding electrons ($B = 6$). So, $FC=5 - 2-\frac{6}{2}=5 - 2 - 3 = 0$.
  • For center N: Nitrogen has 5 valence electrons ($V = 5$). It has 0 non - bonding electrons ($N = 0$) and 8 bonding electrons ($B = 8$). So, $FC = 5-0-\frac{8}{2}=5 - 4=1$.
  • For S: Sulfur has 6 valence electrons ($V = 6$). It has 6 non - bonding electrons ($N = 6$) and 2 bonding electrons ($B = 2$). So, $FC=6 - 6-\frac{2}{2}=6 - 6 - 1=-1$.

Step3: Analyze Structure 2

  • For left N: Nitrogen has 5 valence electrons ($V = 5$). It has 2 non - bonding electrons ($N = 2$) and 4 bonding electrons ($B = 4$). So, $FC=5 - 2-\frac{4}{2}=5 - 2 - 2 = 1$.
  • For center N: Nitrogen has 5 valence electrons ($V = 5$). It has 0 non - bonding electrons ($N = 0$) and 8 bonding electrons ($B = 8$). So, $FC = 5-0-\frac{8}{2}=1$.
  • For S: Sulfur has 6 valence electrons ($V = 6$). It has 4 non - bonding electrons ($N = 4$) and 4 bonding electrons ($B = 4$). So, $FC=6 - 4-\frac{4}{2}=6 - 4 - 2 = 0$.

Step4: Analyze Structure 3

  • For left N: Nitrogen has 5 valence electrons ($V = 5$). It has 6 non - bonding electrons ($N = 6$) and 2 bonding electrons ($B = 2$). So, $FC=5 - 6-\frac{2}{2}=5 - 6 - 1=-2$.
  • For center N: Nitrogen has 5 valence electrons ($V = 5$). It has 0 non - bonding electrons ($N = 0$) and 8 bonding electrons ($B = 8$). So, $FC = 5-0-\frac{8}{2}=1$.
  • For S: Sulfur has 6 valence electrons ($V = 6$). It has 2 non - bonding electrons ($N = 2$) and 6 bonding electrons ($B = 6$). So, $FC=6 - 2-\frac{6}{2}=6 - 2 - 3 = 1$.

Answer:

Structure 1: Formal charge for N (left) = 0 Formal charge for N (center) = 1 Formal charge for S = - 1 Structure 2: Formal charge for N (left) = 1 Formal charge for N (center) = 1 Formal charge for S = 0 Structure 3: Formal charge for N (left) = - 2 Formal charge for N (center) = 1 Formal charge for S = 1