Question

1st attempt
part 1 (1 point)
a negative sign (-) is required for negative numbers, but a positive sign (+) is not needed for positive numbers.
what is the formal charge on the xe atom?
fc =
part 2 (1 point)
what is the formal charge on the o atom with the double bond?
fc =
part 3 (1 point)
what is the formal charge on each of the o atoms with the single bonds?
fc =

Explanation:

Step1: Recall formal - charge formula

The formula for formal charge (FC) 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.

Step2: Determine values for Xe

For Xe, the number of valence electrons $V = 8$. Assume a typical Lewis structure of a compound with Xe. Let's assume Xe has 0 non - bonding electrons ($N = 0$) and 8 bonding electrons ($B = 8$). Then $FC=8 - 0-\frac{8}{2}=8 - 0 - 4 = + 4$.

Step3: Determine values for O with double bond

For O, the number of valence electrons $V = 6$. In an O atom with a double bond, assume 4 non - bonding electrons ($N = 4$) and 4 bonding electrons ($B = 4$). Then $FC = 6-4-\frac{4}{2}=6 - 4 - 2=0$.

Step4: Determine values for O with single bond

For O, $V = 6$. In an O atom with a single bond, assume 6 non - bonding electrons ($N = 6$) and 2 bonding electrons ($B = 2$). Then $FC=6 - 6-\frac{2}{2}=6 - 6 - 1=-1$.

Answer:

Part 1: + 4
Part 2: 0
Part 3: - 1