Draw the Lewis resonance structures for the following molecules. SO2

Name: Problem 44, Chapter 8: Chemistry Matter and Change
Uploaded: 2019-07-24T22:33:02-08:00
Duration: 3 min 59 s
Channel: Stephanie Castillo
Description: Draw the Lewis resonance structures for the following molecules. SO2

Draw the Lewis resonance structures for the following...

Key Concepts

Octet Rule

The octet rule is a principle stating that atoms tend to form bonds in such a way that each atom (especially those in the second period) achieves eight electrons in its valence shell. This rule guides the placement of electrons in Lewis structures to ensure the molecule's stability.

Formal Charge

Formal charge is a bookkeeping method used to assign a charge to individual atoms within a molecule based on the electron distribution in a Lewis structure. By calculating formal charges, one can determine the most favorable resonance structure by selecting the one where charges are minimized or best distributed.

Resonance Structures

Resonance structures are multiple valid Lewis diagrams for a molecule that cannot be accurately represented by a single structure. They illustrate how electron density can be distributed in different ways across the molecule, which contributes to its overall stability as a resonance hybrid.

Lewis Structures

Lewis structures are diagrams that depict the arrangement of valence electrons among atoms in a molecule. They show both bonding pairs and lone pairs of electrons, allowing one to predict bond formation, molecular geometry, and reactivity.

Transcript

00:02 To draw the lewis residence structure of so2, we need to first start off with the number of valence electrons in our lewis structure.

00:12 So sulfur and oxygen are both in group six, and there's a total of three atoms.

00:17 So we're going to do six times three equaling 18 valence electrons.

00:22 However, to determine the total number of bonds needed to complete our lewis structure, it will be helpful to determine the total number of electrons.

00:32 Needed in order for each atom to satisfy its octet rule.

00:36 So we have three atoms, each needing eight electrons to satisfy its octet rules, which equals a total number of electrons of 24.

00:45 If you subtract the number of valence electrons by the total number of electrons, we are left with six shared electrons, dividing it by two to equal a pair of electrons.

00:59 We end up having three bonds in our structure.

01:05 So starting off with sulfur in the center and oxygen on the outside, as oxygen is slightly more electronegative than sulfur.

01:14 We'll go ahead and draw out the lewis, or not the lewis, we'll go ahead and draw out the electrons.

01:19 So we have one, two, three, four, five, six around oxygen, one, two, three, four, five, six around sulfur.

01:26 And then one, two, three, four, five, six around the other oxygen.

01:32 So one of these electron pairs can migrate over to form a shared covalent bond...

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