determine the formal charge of each atom in this lewis structure. then, determine the overall charge of this…

Explanation:

Step1: Recall formal - charge formula

The formula for formal charge 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. Nitrogen has 5 valence electrons.

Step2: Calculate formal charge of left nitrogen

For the left nitrogen in $N = N$, it has 2 non - bonding electrons ($N = 2$) and 6 bonding electrons ($B = 6$). Using the formula $FC=V - N-\frac{B}{2}$, with $V = 5$, we get $FC = 5-2-\frac{6}{2}=5 - 2 - 3=0$.

Step3: Calculate formal charge of right nitrogen

The right nitrogen also has 2 non - bonding electrons ($N = 2$) and 6 bonding electrons ($B = 6$). Using the formula $FC = V - N-\frac{B}{2}$ with $V = 5$, we get $FC = 5-2-\frac{6}{2}=0$.

Step4: Calculate overall charge

The overall charge of a neutral molecule is the sum of the formal charges of its atoms. Since each nitrogen has a formal charge of 0, the overall charge is $0+0 = 0$.

Answer:

Left nitrogen: 0 Right nitrogen: 0 Overall charge: 0