Which ONE of the following compounds is least soluble in water? A) CH3CH2CH2NH2
B) CH3CH2CH2F
C) CH3CH(OH)CH3
D) CH3CH2COOH E) CH3CH2NHCH3

The one compound among the given options that is least soluble in water is;

Option B; CH₃CH₂CH₂F

       We know in chemistry that hydrogen bonding affects solubility in that the presence of hydrogen bonding between the molecules of a substance show us that such molecules are polar. This therefore means that the molecules will be soluble in a polar solvent such as water.

      Looking at the options, all of them form hydrogen bonds except for Option B which has Fluorine (F) alone not directly bonded to hydrogen. Instead the fluorine will be bonded to a carbon atom which means it is not going to be easily soluble in water.

     In conclusion, the one compound that would be the least soluble in water is CH3CH2CH2F.

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B) CH3CH2CH2F

Explanation:

All the other compounds listed among the options are capable of forming hydrogen bonds with water except CH3CH2CH2F.

Recall that hydrogen bonds are formed when hydrogen is directly bonded to a highly electronegative atom such as nitrogen, oxygen, fluorine, sulphur, et cetra.

Such bonds are not present in CH3CH2CH2F, rather fluorine is bonded to carbon to give a halogenoalkane. This compound will display the least solubility in water.

i just learnt this recently but i need to look through my notes again