Write reasonable Lewis structures for the following species, none of which follow the octet rule

step 1 So we're going to draw some lewish structures here. The one thing we're told is that they all vi

Write reasonable Lewis structures for the following species,...

Key Concepts

Lewis Structures

A Lewis structure is a diagram that represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist. It depicts the distribution of the total number of valence electrons among the atoms, providing a way to visualize molecular structure and predict reactivity and shape.

Octet Rule

The octet rule is the principle that atoms tend to bond in such a way that each atom has eight electrons in its valence shell, achieving a stable electronic configuration similar to that of noble gases. This rule is a useful guideline for predicting the chemical bonding and structure of many molecules.

Exceptions to the Octet Rule

Some molecules and ions do not conform to the octet rule, either having less than eight electrons (electron-deficient species) or more than eight electrons (expanded octets). Recognizing these exceptions is crucial when drawing Lewis structures for such species, as it requires adjustments to the typical bonding patterns to accurately represent the electron distribution.

Valence Electron Accounting

Counting valence electrons is a fundamental step in constructing Lewis structures. This involves adding up the valence electrons contributed by each atom, and including or excluding electrons based on the species' charge. This count is essential for correctly placing electrons into bonding and lone pair regions.

Formal Charge

Formal charge is the hypothetical charge assigned to an atom in a molecule, calculated by assuming equal sharing of bonding electrons. It is useful for determining the most stable Lewis structure among several possible arrangements by minimizing the overall charges and balancing the distribution of electrons.

Transcript

00:01 So we're going to draw some lewish structures here.

00:05 The one thing we're told is that they all violate the octet rule in some way.

00:10 Well, this one's going to be a little straightforward because we know we can only form single bonds.

00:16 Okay.

00:17 Barillium has two valence electrons, plus two more for the hydrogen is four electrons.

00:23 So that's actually our lewish structure.

00:25 Barillium always forms two bond and has no lone pairs.

00:28 So in the second one, we're going to try co with a negative charge.

00:36 So our valance electrons are 4 plus 6 plus 1 for the charge is 11.

00:41 So since we have an odd number of electrons, we're obviously going to violate our octet rule.

00:46 So let's see, let's pretend it's got single bonds, give everybody a full octet.

00:52 And we'll see that we have 14 electrons.

00:55 So is that 2 extra, or is that 4 extra? well, it's two, but not quite four, so we're going to use the rule for two extra, which means we need a double bond.

01:08 So we'll go ahead and rewrite this with a double bond here.

01:14 Again, we'll give everybody a full octet, but we still have 12 electrons now.

01:19 So i need to remove one electron, and i'm going to remove it from the element with the smaller electron negativity, which is carbon...

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