Why is $C O_{2}$ $CO_2$ a nonpolar molecule, whereas $C O$ $CO$ is a polar molecule?

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Why is $C O_{2}$ $CO_2$ a nonpolar molecule, whereas $C O$ $CO$ is a polar molecule?

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Answer 1 · 2017-01-23T18:05:18

Consider the vector sum of the individual bond dipoles........

Explanation:

The $C - O$ $C-O$ bond in both gases is polar to a certain, limited extent. $^{+ δ} C \equiv O^{δ -}$ $""^(+delta)C-=O^(delta-)$ has some polarity; on the other hand, for $^{δ -} O =^{δ +} C = O^{δ -}$ $""^(delta-)O=^(delta+)C=O^(delta-)$ , the vectors of the bond dipoles clearly sum to ZERO.

This polarity is not reflected in the boiling points of the 2 gases, $- {191.5}^{\circ}$ $-191.5^@$ for $C O$ $CO$ at $1 \cdot a t m$ $1*atm$ , versus a normal sublimation point of $- 78^{\circ} C$ $-78^@C$ for carbon dioxide, however, carbon dioxide is a bigger molecule, with extra dispersion forces.

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Why is $C O_{2}$ $CO_2$ a nonpolar molecule, whereas $C O$ $CO$ is a polar molecule?

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Why is $C O_{2}$ $CO_2$ a nonpolar molecule, whereas $C O$ $CO$ is a polar molecule?