Question

determine the formal charges for the indicated atoms, as drawn.
i ii
a. 0 0
b. 0 +1
c. +1 0
d. +1 +1

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 of the neutral atom, $N$ is the number of non - bonding electrons, and $B$ is the number of bonding electrons. Oxygen has 6 valence electrons ($V = 6$).

Step2: Calculate formal charge for atom I

For atom I, the number of non - bonding electrons $N = 4$ and the number of bonding electrons $B = 2$. Using the formula $FC=V - N-\frac{B}{2}$, we have $FC = 6-4-\frac{2}{2}=6 - 4 - 1=1$.

Step3: Calculate formal charge for atom II

For atom II, the number of non - bonding electrons $N = 2$ and the number of bonding electrons $B = 4$. Using the formula $FC = V - N-\frac{B}{2}$, we have $FC=6 - 2-\frac{4}{2}=6 - 2 - 2 = 2$. But this is wrong. Let's correct it. Oxygen has 6 valence electrons. In structure II, oxygen has 2 non - bonding electrons and 4 bonding electrons. The formal charge $FC=6 - 2-\frac{4}{2}=6 - 2 - 2=0$.

Answer:

C. +1, 0