Use the data in Table 8.5 and the following data: S-S distance in S8=2.05 Å; S-O distance in SO2

step 1 Okay, in this problem, we're going to use some data in a table. And actually I wasn't sure what

Use the data in Table 8.5 and the following data: S-S...

Use the data in Table $8.5$ and the following data: $\mathrm{S}-\mathrm{S}$ distance in $\mathrm{S}_{8}=2.05 \AA ; \mathrm{S}-\mathrm{O}$ distance in $\mathrm{SO}_{2}=1.43 \AA$ to answer the following questions: (a) Predict the bond length in a S - N single bond. (b) Predict the bond length in a $\mathrm{S}-\mathrm{O}$ single bond. (c) Why is the $\mathrm{S}-\mathrm{O}$ bond length in $\mathrm{SO}_{2}$ considerably shorter than your predicted value for the $\mathrm{S}-\mathrm{O}$ single bond? (d) When elemental sulfur, $\mathrm{S}_{8}$, is carefully oxidized, a compound $\mathrm{S}_{8} \mathrm{O}$ is formed, in which one of the sulfur atoms in the $\mathrm{S}_{8}$ ring is bonded to an oxygen atom. The $\mathrm{S}-\mathrm{O}$ bond length in this compound is $1.48 \AA$. In light of this information, write Lewis structures that can account for the observed $\mathrm{S}-\mathrm{O}$ bond length. Does the sulfur bearing the oxygen in this compound obey the octet rule?

Use the data in Table $8.5$ and the following data: $\mathrm{S}-\mathrm{S}$ distance in $\mathrm{S}_{8}=2.05 \AA ; \mathrm{S}-\mathrm{O}$ distance in $\mathrm{SO}_{2}=1.43 \AA$ to answer the following questions:
(a) Predict the bond length in a S - N single bond.
(b) Predict the bond length in a $\mathrm{S}-\mathrm{O}$ single bond.
(c) Why is the $\mathrm{S}-\mathrm{O}$ bond length in $\mathrm{SO}_{2}$ considerably shorter than your predicted value for the $\mathrm{S}-\mathrm{O}$ single bond?
(d) When elemental sulfur, $\mathrm{S}_{8}$, is carefully oxidized, a compound $\mathrm{S}_{8} \mathrm{O}$ is formed, in which one of the sulfur atoms in the $\mathrm{S}_{8}$ ring is bonded to an oxygen atom. The $\mathrm{S}-\mathrm{O}$ bond length in this compound is $1.48 \AA$. In light of this information, write Lewis structures that can account for the observed $\mathrm{S}-\mathrm{O}$ bond length. Does the sulfur bearing the oxygen in this compound obey the octet rule?

Key Concepts

Octet Rule and Expanded Octet

The octet rule is a guideline suggesting that atoms tend to form bonds until they are surrounded by eight valence electrons. While this rule is strictly followed by many second-period elements, eleventh-period elements like sulfur can have an expanded octet, accommodating more than eight electrons. This capacity is important when assessing the bonding in sulfur compounds and can lead to structures where sulfur appears to exceed the sulfur octet.

Lewis Structures and Resonance

Lewis structures provide a diagrammatic way to represent the valence electrons in a molecule and to propose bonding arrangements. By drawing different resonance forms, chemists can account for delocalized electrons and fractional bond orders, which are fundamental for understanding variations in observed bond lengths beyond simple single or multiple bonding descriptions.

Covalent Bond Length

Covalent bond lengths arise from the size of the atoms involved and the nature of their bonding. They can often be estimated by adding the covalent radii of the bonded atoms, while bearing in mind that bond order and orbital overlap significantly influence the actual length. Differences in bond types (e.g., single versus double bonds) will result in differences in bond lengths.

Bond Order and Multiple Bonding

Bond order refers to the number of chemical bonds between a pair of atoms and is directly related to bond strength and bond length. Higher bond orders (as in double or triple bonds) generally result in shorter and stronger bonds than single bonds. Resonance can also lead to fractional bond orders, which helps explain intermediate bond lengths observed in some molecules.

Transcript

00:02 Okay, in this problem, we're going to use some data in a table.

00:06 And actually i wasn't sure what i did wrong here.

00:10 So i'm not exactly finding my data in the table and some other information to find a bond length.

00:20 Hang on, i've got to get down to my problem.

00:25 Okay, we're given the following information.

00:27 In s8, the s -s bond has a bond length of 2 .05 angstroms.

00:41 In s -o -2, the s -o bond is 1 .43 angstroms.

00:57 And we are asked to predict the bond length in a single s -n single bond.

01:23 And i looked, i got to get back to my page here, i'm going to just make myself a note.

01:34 So i looked at a bunch of different bond lengths on here.

01:37 Hang on.

01:38 And i found a cn bond length.

01:42 This is in your text of 1 .43, an n -o bond length.

01:51 Of 1 .36 and they didn't have any sulfur bond length on here.

02:00 So i was looking for a relationship here and if you look at a periodic table you'll see we have sulfur oxygen and nitrogen in that order.

02:11 So i knew the s -s bound length, i knew the s -o bond length and i needed to find this bond length.

02:17 So i knew this i needed to find that.

02:20 I really didn't have anything because i only had bond lengths for c's, ns, and o's on our bond length list.

02:30 So i really didn't have anything to go by on here.

02:34 So what i did, we had an ss with 2 .05 and i guess that that bond length would have to be longer than this bond length.

02:45 So i just took these two numbers and added them up and divided by two and got on 1 .74 angstroms.

02:58 Now this one was answered in the text and they had 1 .77 angstroms and i'm not sure how they got that one.

03:07 But thought i'd mention that.

03:11 Okay, let me get back to my...

03:13 I had to go to my table, which is why i needed to write that number down so i could get back to my problem.

03:23 I need six.

03:27 Okay, for b, predict the bond length of a single s -o bond...

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