🤓 Based on our data, we think this question is relevant for Professor Hoeger's class at UCSD.
We’re being asked to determine which between PF3 and PCl3 has the more polar bonds.
For this problem, we first need to do the following steps:
Step 1: Determine the central atom in this molecule.
Step 2: Calculate the total number of valence electrons present.
Step 3: Draw the Lewis structure for the molecule.
Step 4: Draw dipole arrows for each bond.
Step 5: Compare the polarity of PF3 and PCl3.
Of the molecules PF3 and PCl3, which has bonds that are more polar?
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Dipole Moment concept. You can view video lessons to learn Dipole Moment. Or if you need more Dipole Moment practice, you can also practice Dipole Moment practice problems.
What is the difficulty of this problem?
Our tutors rated the difficulty ofOf the molecules PF3 and PCl3, which has bonds that are more...as medium difficulty.
How long does this problem take to solve?
Our expert Chemistry tutor, Sabrina took 2 minutes and 58 seconds to solve this problem. You can follow their steps in the video explanation above.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Hoeger's class at UCSD.