For each of the following molecules or ions that contain...

For each of the following molecules or ions that contain sulfur, write the Lewis structure(s), predict the molecular structure (including bond angles), and give the expected hybrid orbitals for sulfur. a. $\mathrm{SO}_{2}$ b. $\mathrm{SO}_{3}$ c. $\mathrm{S}_{2} \mathrm{O}_{3}^{2-}\left[\begin{array}{c}\mathrm{Q} \\ \mathrm{S}-\mathrm{S}-\mathrm{O} \\ \mathrm{O}\end{array}\right]^{2-}$ d. $ \mathrm{S}_{2} \mathrm{O}_{8}^{2-}\left[\begin{array}{cc}\mathrm{Q} & \mathrm{Q} \\ \mathrm{O}-\mathrm{S}-\mathrm{O}-\mathrm{O}-\mathrm{S}-\mathrm{O} \\ \mathrm{O} & \mathrm{O}\end{array}\right]^{2-}$ e. $\mathrm{SO}_{3}^{2-}$ f. $\mathrm{SO}_{4}^{2-}$ g. $\mathrm{SF}_{2}$ h. $\mathrm{SF}_{4}$ i. $\mathrm{SF}_{6}$ j. $\mathbf{F}_{3} \mathbf{S}-\mathbf{S F}$ k. $\mathrm{SF}_{5}^{+}$

For each of the following molecules or ions that contain sulfur, write the Lewis structure(s), predict the molecular structure (including bond angles), and give the expected hybrid orbitals for sulfur.
a. $\mathrm{SO}_{2}$
b. $\mathrm{SO}_{3}$
c. $\mathrm{S}_{2} \mathrm{O}_{3}^{2-}\left[\begin{array}{c}\mathrm{Q} \\ \mathrm{S}-\mathrm{S}-\mathrm{O} \\ \mathrm{O}\end{array}\right]^{2-}$
d. $ \mathrm{S}_{2} \mathrm{O}_{8}^{2-}\left[\begin{array}{cc}\mathrm{Q} & \mathrm{Q} \\ \mathrm{O}-\mathrm{S}-\mathrm{O}-\mathrm{O}-\mathrm{S}-\mathrm{O} \\ \mathrm{O} & \mathrm{O}\end{array}\right]^{2-}$
e. $\mathrm{SO}_{3}^{2-}$
f. $\mathrm{SO}_{4}^{2-}$
g. $\mathrm{SF}_{2}$
h. $\mathrm{SF}_{4}$
i. $\mathrm{SF}_{6}$
j. $\mathbf{F}_{3} \mathbf{S}-\mathbf{S F}$
k. $\mathrm{SF}_{5}^{+}$

Key Concepts

Lewis Structures

Lewis structures are diagrams that show the bonding between atoms of a molecule and the lone pairs of electrons that may exist. They are constructed by counting total valence electrons, distributing them to satisfy the octet rule (or expanded octet in elements like sulfur), and assigning formal charges to achieve the most stable configuration.

VSEPR Theory

VSEPR (Valence Shell Electron Pair Repulsion) theory is used to predict the molecular geometry and bond angles of a molecule based on the repulsion between electron pairs surrounding the central atom. This theory helps in understanding the three-dimensional arrangement and deviations in bond angles due to lone pair-bonding pair interactions.

Expanded Octet

Expanded octet refers to the ability of elements in the third period and beyond, like sulfur, to hold more than eight electrons in their valence shell. This occurs as a result of available d orbitals which can participate in bonding, allowing the formation of compounds with more than four electron pairs around the central atom.

Resonance Structures

Resonance structures are multiple valid Lewis structures for a single molecule that differ only in the distribution of electrons, not in the arrangement of atoms. They are important for describing electron delocalization, which contributes to the overall stability and properties of the molecule or ion.

Hybridization

Hybridization is the concept where atomic orbitals mix to form new, equivalent hybrid orbitals that match the observed molecular geometry. Depending on the number of electron density regions, sulfur can exhibit various hybridizations (such as sp2, sp3, sp3d, sp3d2), which explain the bonding and arrangement in these compounds.

Transcript

00:01 Here we've just got a lot of structures to get through, where we will be discussing loan pairs, bond angles and structures for all of these examples.

00:10 Now, i've drawn them out already to save us time.

00:13 So let's start off with our top left here.

00:17 So we have so2, and then our bond angle here is approximately 104 .5.

00:27 Now we have a bent structure here.

00:30 Sulfa is in group 6 and so we have one loan pair.

00:34 And then moving on to our next example here, we've got s -o -3.

00:38 Now we have no charges, so we've got all of our double bonds present.

00:44 And we have bond angle of approximately 120 degrees and a trigonal planar structure.

00:51 And now moving on to this example here on the far right.

00:55 So we have four substituents and so we will have a tetrahedral confirmation and our bond angles will be approximately 109 .5 where we have two low low we have two negative charge present here two on oxygen where if we were to throw in this electron pair we would knock up this electron pair onto the oxygen and we would always have two negative charges present in the molecule now you could also do the same with the sulfur atom because we have three lone pairs there so now i'm moving on to our next example.

01:34 So in terms of structure, we have a general tetrahedral structures that will be adopted by each of the s -o -4 molecules.

01:43 However, they're joined together.

01:44 And so we will see bond angle of approximately 104 .5 in here.

01:53 And then our bond angles and our tetrahedral are approximately 109 .5.

02:01 And that's between these bonds here.

02:03 So now we've got an actual tetrahedral structure drawn out...

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