QQuestionAnatomy and Physiology
QuestionAnatomy and Physiology
How many of the following molecules are polar?
$\mathrm{PCl}_{5}$
CO
$\mathrm{XeO}_{3}$
$\mathrm{SeBr}_{2}$
6 months agoReport content
Answer
Full Solution Locked
Sign in to view the complete step-by-step solution and unlock all study resources.
Step 1I'll solve this problem step by step, determining the polarity of each molecule by examining their molecular geometry and bond polarities.
Step 2: Analyze $\mathrm{PCl}_{5}$ (Phosphorus Pentachloride)
- Net dipole moment: $$\vec{0}$$ (Non-polar)
- Molecular geometry: Trigonal bipyramidal - Central atom: Phosphorus (P) - Symmetrical arrangement of 5 chlorine atoms - Symmetrical distribution of electron density
Final Answer
1. CO 2. $\mathrm{XeO}_{3}$ 3. $\mathrm{SeBr}_{2}$ $\mathrm{PCl}_{5}$ is the only non-polar molecule in this set.
Need Help with Homework?
Stuck on a difficult problem? We've got you covered:
- Post your question or upload an image
- Get instant step-by-step solutions
- Learn from our AI and community of students