### 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 ### ExplanationDipole-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

we have to select the molecules that have dipole-dipole forces

Answered: (10.5 & 12.3) Which of the following…

(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

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...

See similar textbooks

Similar questions

Identify the major intermolecular force in the following molecule: BBYJU'S the L A ö=c=ö Ô=C=Ö OByjus.com London Dispersion Dipole-Dipole O Hydrogen Bonding
For each compound in the table below, decide whether there would be any hydrogen-bonding force between molecules of the compound, or between molecules of the compound and molecules of water. hydrogen-bonding force compound Between molecules of Between formula or Lewis the compound and molecules of water? molecules of the name structure compound? Н yes yes Ci: N-chloromethylamine no no Н yes yes CH, Br bromomethane no no :0: н yes yes н —с —с—о — н | acetic acid no no н z:
Rank the forces overall of methane, methanol and water (IMF: dispersion, dipole-dipole, hydrogen-bonding)
2:35 Question 8 of 11 Submit Which one of the following would have the largest dispersion forces? A) CH;CH,SH B) CH;NH2 C) CH, D) CH;CH3 Tap here or pull up for additional resources
I need help with this question please. Also, my other question was, What intermolecular forces does Phosphorous Trifluoride (PF3) exhibit?
Determine the strongest intermolecular force for the following molecule. Both L and X are nonmetals. Electronegativity: L < X? A)Hydrogen bond B)Ionic compound C)Ion-dipole D) London E) Dipole-dipole
Which do you expect to have the greatest surface tension? ethanol CH3CH2OH, ethane CH3CH3, chloroethane CH3CHCI, bromoethane CH3CH2Br
#6
6. CH3CO2H
What is the strongest force in a sample of NaCl(aq)? Group of answer choices Ion-dipole force London force H bridge force dipole-dipole force
7The substance with the lowest known boiling point (4 K) is helium, an atomic element that has two electrons. Hydrogen is a diatomic molecule and also has two electrons, but its boiling point is significantly higher, at 20.28 K. (a) What is the dominant intermolecular force between a pair of helium atoms and a pair of H2 molecules? (b) Why do you think H2 has a higher boiling point?