CIA Problem 4.2 Draw the Lewis dot structures for the molecules CO and NO. What is different about these structures compared with the general examples we have seen so far? How could these Lewis structures provide insight into the high chemical reactivity of these molecules?

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Hello. In this problem, we are asked to give the Lewis dot Structure for the molecules, carbon monoxide and phosphorus monoxide and to compare the structures and provide insight into how their structures relate to their reactivity. Let's begin with, carbon monoxide will make use of the need available share method to draw its Lewis dot Structure. Carbon and oxygen are both trying to acquire eight valence electrons. So that's a total of 16 that we need. The number available comes from their valence electrons carbons in group four A. So it has four valence electrons, oxygen's in group six A. So it has six. So we have a total of 10 electrons available. The difference between what we need and what's available tells us what we'll share, which is six. So we have carbon Sharing six electrons with oxygen. We have to count for all 10, the remaining four to go on carbon and to go on oxygen to fulfill their octet. It's this triple bond between the carbon and oxygen Contains two Pi bonds and one sigma bond pi bonds come about from the overlap of pure orbital's. This is side by side overlap. And then we have one signal bond, which results from head to hood overlap of two hybridized orbital's the side by side overlap of these bottles forming the pi bonds are easily broken. And we have a lot of electrons which means then that they are capable of forming coordinate covalin connections with substances that can accept electrons. When we form a coordinate violent bond, we have one element then providing both of the electrons that are used to form that bond. We now consider prosperous monoxide can make use of the need available. Share oxygen and phosphorus are both trying to acquire eight valence electrons. So that's a total of 16 phosphorus is in group five A. So it has five valence electrons. Oxygen is in group six A. So it has six. So this is a total of 11 electrons that available, the difference between what we need and what we have available says we're gonna share five When we form bonds, we have to have an even number of electrons. So we're gonna share four Will form a double bond between the phosphorus and oxygen. We have to account for all 11 available electrons. So the remaining 74 of those will go on the oxygen to fill its octet. And the remaining three go on phosphorus, phosphorus being less electro negative than oxygen will have that lone electron. This lone electron makes this unstable and therefore more reactive. These explanations. Then for the structure and the reactivity of carbon monoxide and phosphorus monoxide correspond to answer. C thanks for watching. Hope this helped.

CIA Problem 4.2 Draw the Lewis dot structures for the molecules CO and NO. What is different about these structures compared with the general examples we have seen so far? How could these Lewis structures provide insight into the high chemical reactivity of these molecules?

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Key Concepts

Lewis Dot Structures

Molecular Reactivity

Bond Order