Question

For each of the following pairs, pick which compound has a higher boiling point and label the intermolecular forces of each individual compound.

a) SO2 or CO2

b) SiH4 or GeH4

c) CH₃CH2-O-CH2CH₃ or (CH₃)₃COH

d) (CH₃)₃CCH₂CH₃ or CH₃(CH₂)₄CH₃

Answer 1

SO2 is molecular weight is more than CO2. Therefore boiling is more for SO2. SO2 is having dipole dipole intermolecular forces. CO2 is having London dispersion forces.

GeH4 having more molecular weight (more london dispersion forces) than SiH4. Therefore GeH4 is having more boiling point. SiH4 and GeH4 are having london dispersion forces as intermolecular forces.

2-methyl-2-propanol is having more boiling point than diethyl ether because of hydrogen bonding is present in 2-methyl-2-propanol. 2-methyl-2-propanol is having hydrogen bonding as intermolecular forces and Diethyl ether is having dipole dipole intermolecular forces and London dispersion forces.

Hexane is having more boiling point than 2,2-dimethyl butane because hexane is straight chain alkane and 2,2-dimethyl butane is branched chain alkane. Hexane and 2,2-dimethyl butane both are having london dispersion forces as intermolecular forces.