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(10.5 & 12.3) Which of the following molecules have dipole-dipole forces? More than one answer is required. OCCI4 O NH3 D CHCl3 O PC15 D CH2O

(10.5 & 12.3) Which of the following molecules have dipole-dipole forces? More than one answer is required. OCCI4 O NH3 D CHCl3 O PC15 D CH2O

Chemistry
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 Dipole-Dipole Forces **Which of the following molecules have dipole-dipole forces? More than one answer is required.** - \( \boxed{ \, } \) CCl₄ - \( \boxed{ \, } \) NH₃ - \( \boxed{ \, } \) CHCl₃ - \( \boxed{ \, } \) PCl₅ - \( \boxed{ \, } \) CH₂O ### Explanation Dipole-dipole forces occur between molecules that have permanent dipoles. This means that these molecules have regions of positive and negative charge due to the unequal sharing of electrons in their bonds. To determine which of the molecules listed above exhibit dipole-dipole forces, consider the following points: 1. **Polarity of Bonds**: Molecules with polar bonds typically exhibit dipole-dipole interactions if the overall molecule is also polar. 2. **Molecular Shape**: The molecular geometry must allow for an uneven distribution of charge. **Analysis of Each Molecule:** - **CCl₄ (Carbon Tetrachloride)**: This molecule is tetrahedral and symmetrical. Even though C-Cl bonds are polar, the symmetry causes the dipoles to cancel out, making the molecule nonpolar. **No dipole-dipole forces.** - **NH₃ (Ammonia)**: This molecule is trigonal pyramidal due to the lone pair on nitrogen, causing a net dipole. **Yes, it has dipole-dipole forces.** - **CHCl₃ (Chloroform)**: This molecule is tetrahedral with three C-Cl bonds and one C-H bond. The differing electronegativities and lack of symmetry mean the dipoles do not cancel out. **Yes, it has dipole-dipole forces.** - **PCl₅ (Phosphorus Pentachloride)**: In its solid form, it can exist in a trigonal bipyramidal structure, which is symmetrical. However, molecular PCl₅ is not typically polar because the asymmetric geometry cancels the dipoles. **No dipole-dipole forces.** - **CH₂O (Formaldehyde)**: This molecule has a trigonal planar geometry where the dipoles do not cancel out due to the different atoms attached to the carbon. **Yes, it has dipole-dip
Transcribed Image Text:### Understanding Dipole-Dipole Forces **Which of the following molecules have dipole-dipole forces? More than one answer is required.** - \( \boxed{ \, } \) CCl₄ - \( \boxed{ \, } \) NH₃ - \( \boxed{ \, } \) CHCl₃ - \( \boxed{ \, } \) PCl₅ - \( \boxed{ \, } \) CH₂O ### Explanation Dipole-dipole forces occur between molecules that have permanent dipoles. This means that these molecules have regions of positive and negative charge due to the unequal sharing of electrons in their bonds. To determine which of the molecules listed above exhibit dipole-dipole forces, consider the following points: 1. **Polarity of Bonds**: Molecules with polar bonds typically exhibit dipole-dipole interactions if the overall molecule is also polar. 2. **Molecular Shape**: The molecular geometry must allow for an uneven distribution of charge. **Analysis of Each Molecule:** - **CCl₄ (Carbon Tetrachloride)**: This molecule is tetrahedral and symmetrical. Even though C-Cl bonds are polar, the symmetry causes the dipoles to cancel out, making the molecule nonpolar. **No dipole-dipole forces.** - **NH₃ (Ammonia)**: This molecule is trigonal pyramidal due to the lone pair on nitrogen, causing a net dipole. **Yes, it has dipole-dipole forces.** - **CHCl₃ (Chloroform)**: This molecule is tetrahedral with three C-Cl bonds and one C-H bond. The differing electronegativities and lack of symmetry mean the dipoles do not cancel out. **Yes, it has dipole-dipole forces.** - **PCl₅ (Phosphorus Pentachloride)**: In its solid form, it can exist in a trigonal bipyramidal structure, which is symmetrical. However, molecular PCl₅ is not typically polar because the asymmetric geometry cancels the dipoles. **No dipole-dipole forces.** - **CH₂O (Formaldehyde)**: This molecule has a trigonal planar geometry where the dipoles do not cancel out due to the different atoms attached to the carbon. **Yes, it has dipole-dip
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