Why is #CO_2# a nonpolar molecule, whereas #CO# is a polar molecule?

Answer 1

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

The #C-O# bond in both gases is polar to a certain, limited extent. #""^(+delta)C-=O^(delta-)# has some polarity; on the other hand, for #""^(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^@# for #CO# at #1*atm#, versus a normal sublimation point of #-78^@C# for carbon dioxide, however, carbon dioxide is a bigger molecule, with extra dispersion forces.
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Answer 2

CO2 is nonpolar because the two oxygen atoms in CO2 are symmetrical, resulting in a linear molecular geometry with the oxygen atoms pulling equally on the carbon atom. CO, on the other hand, is polar because the oxygen atom pulls the shared electrons more strongly than the carbon atom, creating a dipole moment.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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