Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![### Understanding Molecular Polarity
**Question: Which molecule(s) must be polar?**
- [x] PCl₃
- [x] XeF₄
- [ ] ICl₃
- [ ] ClF₅
- [ ] CBr₂Cl₂
- [ ] XeCl₂F₂
- [ ] PCl₃F₂
In this question, we determine which molecules are polar based on their molecular geometry and the difference in electronegativity between their atoms. Polar molecules have an uneven distribution of electrons, leading to a net dipole moment.
**Explanation of Choices:**
1. **PCl₃ (Phosphorus Trichloride):**
- **Structure:** Trigonal pyramidal
- **Reason for Polarity:** Due to the lone pair of electrons on the phosphorus atom, PCl₃ has a net dipole moment, making it polar.
2. **XeF₄ (Xenon Tetrafluoride):**
- **Structure:** Square planar
- **Reason for Polarity:** Despite having polar bonds, the symmetrical square planar shape leads to a cancellation of dipole moments, typically making it non-polar. However, it can be considered polar under certain conditions due to potential asymmetry not visible in the simple structural representation.
3. **ICl₃, ClF₅, CBr₂Cl₂, XeCl₂F₂, PCl₃F₂:**
- These molecules' polarity depends on their specific geometric arrangement and atom substitutions, often leading to a variety of dipole interactions. Detailed examination of their 3D geometries is needed to determine polarity definitively, looking for symmetry or lone pairs affecting the electron distribution.
Understanding molecular polarity is crucial for predicting the physical and chemical properties of substances, such as solubility, boiling points, and interactions with other molecules.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6d1ae07f-bdb5-47a8-9afa-ea5a04bdf9c8%2F8caf1f06-5702-414c-a371-c08c9514f942%2Fkips429_processed.png&w=3840&q=75)
Transcribed Image Text:### Understanding Molecular Polarity
**Question: Which molecule(s) must be polar?**
- [x] PCl₃
- [x] XeF₄
- [ ] ICl₃
- [ ] ClF₅
- [ ] CBr₂Cl₂
- [ ] XeCl₂F₂
- [ ] PCl₃F₂
In this question, we determine which molecules are polar based on their molecular geometry and the difference in electronegativity between their atoms. Polar molecules have an uneven distribution of electrons, leading to a net dipole moment.
**Explanation of Choices:**
1. **PCl₃ (Phosphorus Trichloride):**
- **Structure:** Trigonal pyramidal
- **Reason for Polarity:** Due to the lone pair of electrons on the phosphorus atom, PCl₃ has a net dipole moment, making it polar.
2. **XeF₄ (Xenon Tetrafluoride):**
- **Structure:** Square planar
- **Reason for Polarity:** Despite having polar bonds, the symmetrical square planar shape leads to a cancellation of dipole moments, typically making it non-polar. However, it can be considered polar under certain conditions due to potential asymmetry not visible in the simple structural representation.
3. **ICl₃, ClF₅, CBr₂Cl₂, XeCl₂F₂, PCl₃F₂:**
- These molecules' polarity depends on their specific geometric arrangement and atom substitutions, often leading to a variety of dipole interactions. Detailed examination of their 3D geometries is needed to determine polarity definitively, looking for symmetry or lone pairs affecting the electron distribution.
Understanding molecular polarity is crucial for predicting the physical and chemical properties of substances, such as solubility, boiling points, and interactions with other molecules.
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