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(D) The boiling points depend on intermolecular forces. $1$. $II$ ($n$-butanol) and $III$ (isobutanol) are alcohols and exhibit strong intermolecular

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$II > III > IV > I$

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(D) The boiling points depend on intermolecular forces. $1$. $II$ ($n$-butanol) and $III$ (isobutanol) are alcohols and exhibit strong intermolecular hydrogen bonding,leading to higher boiling points compared to ethers and alkanes. $2$. Between $II$ and $III$,$II$ is a straight-chain alcohol with a larger surface area,leading to stronger van der Waals forces than the branched $III$. Thus,$II > III$. $3$. $I$ (diethyl ether) is polar due to the $C-O-C$ bond,giving it a higher boiling point than the non-polar alkane $IV$ ($n$-pentane). $4$. Therefore,the order is $II > III > I > IV$.

Arrange the following in the correct order of their boiling points.
$I$. $(C_2H_5)_2O$
$II$. $CH_3(CH_2)_3OH$
$III$. $CH_3CH(CH_3)CH_2OH$
$IV$. $CH_3(CH_2)_3CH_3$

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Arrange the following in the correct order of their boiling points.$I$. $(C_2H_5)_2O$$II$. $CH_3(CH_2)_3OH$$III$. $CH_3CH(CH_3)CH_2OH$$IV$. $CH_3(CH_2)_3CH_3$