I guess this paragraph is trying to explain about the limitation of Lewis dot st

Question

I guess this paragraph is trying to explain about the limitation of Lewis dot structure, but I can't figure it out. Drawing the sturcture by Lewis method, the negative formal charge is located in Carbon rather than Oxygen. but for real, Oxygen is more electronegative, which makes it "delta -". .... but why does this consistent with the fact that CO structure has " small" dipole moment?? Do I have to consider the contribution as a electron density from Lewis structure? (even thogh Lewis structures not real ??) please help.... the sta The CO Molecule. The Lewis structure of carbon monoxide is Th Note that the negative formal charge is on the less electronegative carbon ator consistent with the fact that CO has a rather small dipole moment of about . his i monoxide is isoelectronic (i.e., has the same number of electrons) with N,B arbon igure 13.14 is given by shows the correlation diagram for CO. The electron configuration of CO is given b tia

Explanation / Answer

This paragraph is not trying to explain the limitations of lewis structures. This paragraph is trying to explain structural properties of carbon monoxide by discussing or explaining two basic approaches:

1. By lewis structure

2. By electronegative effects

Doubt: How the small net dipole moment of CO is consistent with the points discussed in paragraph.

Points explained in paragraph:

1. By lewis structure negative formal charge is on carbon and positive formal charge is on oxygen.

2. Oxygen is more electronegative than carbon.

Your Basic Doubt: Above two points are contradictory as ''how carbon can have negative charge considering oxygen is more electronegative''.

My explaination : Only way for carbon monoxide to exist is that oxygen have to donate its one lone pair to carbon as then only the valence electron in both atoms would be eight ( first necessity ). Now there is no way carbon monoxide molecule to exist except having negative formal charge on carbon. Hypothetically speaking that if electronegativity of carbon and oxygen would be equal , dipole moment shown by CO molecule would be high because :

Dipole Moment = charge * distance between tha charge

But in reality, oxygen atom has high electronegativity when compared with carbon. Their is no way that carbon monoxide molecule to exist without having negative charge on carbon ( octet rule ). Now CO has low dipole moment because , negative charge density on carbon in reality is shifted towards oxygen , hence decreasing the distance between the charges.

Dipole Moment = charge * distance between the opposite charges ( decreases because oxygen will attract electrons towards itself)

That's why, considering both lewis structure and electronegative effects of oxygen, CO has low dipole moment.

CO is one of that molecule where oxygen has very very very small positive charge because there is necessity for oxygen to donate its lone to carbon to form molecule with it.

Related Questions

Navigate

• Browse (All)
• Browse I
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.