Consider the following molecules and the description of the bonding present in each: CH3CH2CH2CH3CH3CH2CH2CH3 (C−CC−C and C−HC−H bonds only) CH3CH2CH2OH CH3CH2CH2OH (C−CC−C and C−HC−H bonds, and one C−OHC−OH bond) CH3CH2CHO CH3CH2CHO (C−CC−C and C−HC−H bonds, and one C=OC=O bond) Based on the general trends of intermolecular forces, rank these molecules in order of increasing boiling point.

Butane is a member of the CnH2n+2 homologous series is an alkane. Alkanes have C-H and C-C bonds which have Van der waals dispersion forces which are temporary dipole-dipole forces (forces caused by the electron movement in a corner of the atom). This bond is weak but increases as the carbon chain/molecule increases.

In Propan-1-ol(Primaryalcohol), there is a hydrogen bond present in the -OH group. Hydrogen bond is caused by the attraction of hydrogen to a highly electronegative element like Cl-, O- etc. This bond is stronger than dispersion forces because of the relative energy required to break the hydrogen bond. Alcohols (CnH2n+1OH) also experience van der waals dispersion forces on its C-C chain and C-H so as the Carbon chain increases the boiling point increases in the homologous series.

Propanal which is an Aldehyde (Alkanal) with the general formula CnH2n+1CHO. This molecule has a C-O, C-C and C-H bonds only. If you notice, the Oxygen is not bonded to the Hydrogen so there is no hydrogen bond but the C-O bond has a permanent dipole-dipole force caused by the electronegativity of oxygen which is bonded to carbon. It also has van der waals dispersion forces caused by the C-C and C-H as the carbon chain increases down the homologous series. The permanent dipole-dipole forces are not as easy to break as van der waals forces.

In conclusion, the hydrogen bonds present in alcohols are stronger than the permanent dipole-dipole bonds in the aldehyde and the van der waals forces in alkanes (irrespective of the carbon chain in Butane). So Butane < Propanal < Propan-1-ol

pstnonsonjoku pstnonsonjoku · Answer 2 · 2021-11-25T11:24:19+01:00

The order of intermolecular interaction is; CH3CH2CH2OH > CH3CH2CHO > CH3CH2CH2CH3CH3CH2CH2CH3

Intermolecular forces are forces of attraction that hold a molecule together in a particular state of matter. The nature of intermolecular forces in a molecule depends on the kind of bonds between the atoms in the compounds. Compounds that contain nonpolar bonds often have weaker intermolecular interaction between molecules while molecules that have polar bonds experience a greater magnitude of intermolecular forces.

The order of intermolecular interaction is; CH3CH2CH2OH > CH3CH2CHO > CH3CH2CH2CH3CH3CH2CH2CH3

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