For each of the following molecules or ions of sulfur and
oxygen,...

Question

For each of the following molecules or ions of sulfur and
oxygen, write a single Lewis structure that obeys the octet
rule, and calculate the oxidation numbers and formal
charges on all the atoms: (c) SO32-
Write a single Lewis structure that obeys the octet rule for SO3 2 - and assign the formal charges on all the atoms.

Accepted Answer

hey everyone. We're asked to provide a single lewis structure for our Tillery ion that obeys the octet rule and to determine the formal charges on each atom first. Let's go ahead and determine the total number of valence electrons will have for our structure. Looking at salary. Um we have one of Tillery. Um and we're going to multiply this by six since it's in our group 68. This will get us to six valence electrons. Looking at our oxygen, We have three of oxygen and we're going to multiply this by six as well since it's also in our group six a this will get us to 18 valence electrons. Now when we add these two values up we get a total of 24 valence electrons. But since we have that -2 charge, This means that we have to add two valence electrons. So in total we have 26 valence electrons in our structure. Now to draw our Lewis structure, we know that solarium is going to be our central atom since it is less electro negative than oxygen, we have three oxygen's connected to it and in order to obey the octet rule will have to add three lone pairs onto our oxygen and one lone pair onto our Tillery. Um When we count our electrons up we end up with a total of 26 valence electrons but let's go ahead and determine the formal charges of each atom. And we can do so by taking our group number and subtracting the sum of our bonds plus our non bonding electrons. Looking at our formal charge of Tillery, um we're going to take our group number of six and subtract the sum of three plus two, Which will get us to a formal charge of plus one. Next looking at the formal charge of our oxygen's, we're going to take our group number of six and subtract the sum of one plus six, which will get us to a formal charge of minus one. So each of our oxygen's will have a formal charge of -1. And this makes sense because we know that the total charge of our ion was -2 and this is going to be our final answer for this question. Now I hope that made sense. And let us know if you have any questions.

Watch next