The intermolecular forces between $ceCO2$ molecules space dispersion forces, while the forces in between $ceCO$ molecules are mainly dipole-dipole attraction forces. So, why does $ceCO2$ have actually a greater boiling allude than the of $ceCO$?




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CO2 has more electrons 보다 CO. This way that it has a much bigger electron cloud as compared to CO, therefore its an ext easily polarised and also thus, the lull of developing instataneous dipole-induced dipole binding increases. Also though CO is a polar molecule and also it develops permanent dipole-permanent dipole bonds, in this case the id-id bonds are stronger.

P.s. Just a 17 year old A Level Chem college student here, I could be wrong


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The bigger the tiny covalent molecule, the higher the intermolecular bonds, hence higher boiling / melting point.

$ceCO2$ has actually 3 atoms connected in the molecule and is therefore larger than $ceO2$ that has actually 2 atoms. Hence, $ceCO2$ has actually a higher boiling / melting allude compared to $ceO2$. (Exception to this is water molecules.)


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