Order the following in terms of boiling point and explain your reasoning: Ethanol, Ethane, Propane

All three molecules have induced dipole-dipole interactions. Propane has a higher boiling point than ethane as propane has a higher molecular mass. This means there are more electrons present and the induced dipole-dipole interactions is stronger. Ethanol has the highest boiling point as it forms induced dipole-dipole interactions, permanent dipole-dipole interactions and hydrogen bonds. Hydrogen bonds are able to form due to the presence of a highly electronegative 'NOF' atom. Hydrogen bonds are the strongest intermolecular force of attraction.The stronger the bonds the more energy required to overcome the intermolecular interactions, hence the higher the boiling point. From highest to lowest the order is: ethanol, propane, ethane.

Answered by Lucy C. Chemistry tutor

10802 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

Draw the full structual diagram of ethyl-ethanoate, labeling relevent bond angles and explain why the molecule has this structure.


How is the electrophile formed for the nitration of benzene??


Define the "standard enthalpy change of atomisation".


Bethan prepared some ethoxyethane (line 6) by reacting ethanol with concentrated sulfuric acid. She used 69g of ethanol (Mr=46) and obtained a 45% yield of ethoxyethane (Mr=74). Calculate the mass of ethoxyethane obtained.


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences