QQuestionChemistry
QuestionChemistry
How many of the following molecules are polar?
$\mathrm{PCl}_{5}$
CO
$\mathrm{XeO}_{3}$
$\mathrm{SeBr}_{2}$
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Answer
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Step 1:I'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
Step 3:: Analyze CO (Carbon Monoxide)
- Linear molecule - One carbon-oxygen bond - Significant electronegativity difference between C and O - Net dipole moment: Polar - Dipole moment points from C to O
Step 4:: Analyze $\mathrm{XeO}_{3}$ (Xenon Trioxide)
- Trigonal pyramidal geometry - Central atom: Xenon (Xe) - Asymmetrical electron distribution - Significant electronegativity difference between Xe and O - Net dipole moment: Polar
Step 5:: Analyze $\mathrm{SeBr}_{2}$ (Selenium Dibromide)
- Bent molecular geometry - Central atom: Selenium (Se) - Asymmetrical electron distribution - Significant electronegativity difference between Se and Br - Net dipole moment: Polar
Final Answer
1. CO 2. $\mathrm{XeO}_{3}$ 3. $\mathrm{SeBr}_{2}$ $\mathrm{PCl}_{5}$ is the only non-polar molecule in this set.
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