Question

in the lewis structure of the iodate ion, io₃⁻, that satisfies the octet rule, the formal charge on the central iodine atom is
2.
1.
0.
-1
-2

question 14
1 pts
the number of resonance structures for the sulfur dioxide molecule that satisfy the octet rule is
1.
2.
3.
4.
none of these

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 of the atom in isolation, $N$ is the number of non - bonding electrons, and $B$ is the number of bonding electrons. For iodine in $IO_3^-$, iodine ($I$) has 7 valence electrons ($V = 7$). In the Lewis structure of $IO_3^-$ that satisfies the octet rule, iodine has 2 non - bonding electrons ($N = 2$) and 10 bonding electrons ($B = 10$).

Step2: Calculate formal charge

$FC=7 - 2-\frac{10}{2}=7 - 2 - 5=0$.

For the number of resonance structures of $SO_2$:
In the Lewis structure of $SO_2$, sulfur is the central atom. Sulfur has 6 valence electrons. To satisfy the octet rule, there are 2 resonance structures for $SO_2$. One has a double bond between sulfur and one oxygen and a single bond between sulfur and the other oxygen, and the other resonance structure has the double and single bonds reversed.

Answer:

Question 1: C. 0
Question 2: B. 2