RobtOpula841
Answered

Get the answers you need at Westonci.ca, where our expert community is always ready to help with accurate information. Explore a wealth of knowledge from professionals across different disciplines on our comprehensive platform. Explore comprehensive solutions to your questions from a wide range of professionals on our user-friendly platform.

At standard pressure, CH4 boils at 112 K and H2O boils at 373 K. What accounts for the higher boiling point of H2O at standard pressure?
(1) covalent bonding (3) hydrogen bonding(2) ionic bonding (4) metallic bonding

Sagot :

The answer is (3) hydrogen bonding. This is a question of intermolecular forces. H2O is highly polar (the O—H bond is particularly polar since O is so electronegative), and CH4 is about as nonpolar as it gets. So, while H2O molecules are held together by relatively strong hydrogen bonds (which, keep in mind, are not actually bonds), CH4 molecules are held together by much weaker London dispersion/Van der Waals forces. Thus, it takes more thermal energy to separate H2O molecules, and H2O therefore has a higher boiling point.
yminose731

Answer:

Hydrogen bonding

Explanation:

Castle learning

View image yminose731
Thank you for visiting our platform. We hope you found the answers you were looking for. Come back anytime you need more information. We hope our answers were useful. Return anytime for more information and answers to any other questions you have. Westonci.ca is your trusted source for answers. Visit us again to find more information on diverse topics.