Question

What is the resonance structure of co2

Answer 1

Answer:Carbon dioxide, or CO2, has three resonance structures, out of which one is a major contributor.The CO2 molecule has a total of 16 valence electrons , 4 from carbon and 6 from each oxygen atom.

Answer 2

Final answer:

The resonance structure of $CO_{2}$:

$O=C=O$ ↔ $^{+}O$ ≡ $C-O^{-}$ ↔ $^{-}O-C$ ≡ $O^{+}$

The structure $CO_{2}$ is best described as a resonance hybrid of 3 canonical forms, shown in the figure below.

Given that: We are given $CO_{2}$.

To find: We have to find the resonance structure of $CO_{2}$.

Explanation:

• If a molecule can be represented by two or more electronic structures, each of which cannot explain all the properties of the molecule, then the actual structure lies somewhere in between the possible structures.
• Each of the structures is said to contribute to the actual structure which thus has the characteristics of each of its contributors but any of they does not completely represent it. These structures will differ in the arrangement of electrons but not in the relative positions of the atomic nuclei.
• They are called resonating or resonance structures of a molecule.
• The true structure is said to be in resonance hybrid of the resonance structures.

The resonance structure of $CO_{2}$:

$O=C=O$ ↔ $^{+}O$ ≡ $C-O^{-}$ ↔ $^{-}O-C$ ≡ $O^{+}$

• In $CO_{2}$, two oxygen atoms are on either side of the carbon atom and are joined through the double bond.
• The normal $C=O$ bond length is $122$ $pm$ but in a $CO_{2}$ molecule, the bond length between carbon-oxygen atoms is $115$ $pm$.
• Also, $C$≡$O$ has a bond length of $110$ $pm$.
• This show that the bond length of the carbon-oxygen bond in a $CO_{2}$ is between $C=O$ and $C$≡$O$.

The structure $CO_{2}$ is best described as a resonance hybrid of 3 canonical forms, shown in the figure below.

To know more about the concept please go through the links

https://brainly.in/question/22881512

https://brainly.in/question/11768845

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