Why does phosphine have such a higher dipole moment and boiling point than CF4 despite it having non-polar bonds?
The dipole moment of $PH_3$ can be attributed to the lone pair on P, which is directed away from all three P-H bonds. You can imagine that there is a higher electron density near the lone pair, while the electron density is more or less uniform near the nonpolar P-H bonds. This does not happen for $CF_4$, so it has no dipole moment.
You are watching: Does ph3 have a dipole moment
Thanks for contributing an answer to aramuseum.org Stack Exchange!Please be sure to answer the question. Provide details and share your research!
But avoid …Asking for help, clarification, or responding to other answers.Making statements based on opinion; back them up with references or personal experience.
Use MathJax to format equations. MathJax reference.
See more: How Do You Say Nope In Spanish Translation, How Do You Say 'Nope' In Spanish
To learn more, see our tips on writing great answers.
Post Your Answer Discard
Not the answer you're looking for? Browse other questions tagged boiling-point polarity dipole vsepr-theory or ask your own question.
site design / logo © 2021 Stack Exchange Inc; user contributions licensed under cc by-sa. rev2021.9.24.40305