Which of the following is incorrect about intermolecular forces?[Fill in the blank]

Question

BlackTom AI · Accepted Answer

Dispersion (London) forces arise from instantaneous fluctuations in an electron cloud that create a temporary dipole, which induces a dipole in a neighbor — therefore they are present between all atoms and molecules, not only nonpolar ones.

1. Relevant knowledge points and concepts
- Types of intermolecular forces: dispersion (London) forces, dipole–dipole, ion–dipole, hydrogen bonding.  
- Dispersion forces originate from instantaneous induced dipoles and scale with polarizability and contact surface area.  
- Ion–dipole interactions involve a full charge interacting with a partial charge and are generally stronger than dipole–dipole.  
- Covalent bonds (intramolecular) are much stronger than intermolecular forces.  
- Boiling points of alkanes increase with chain length because larger molecules have greater polarizability and surface area, strengthening dispersion forces.

2. Step-by-step reasoning
- Dispersion forces mechanism: electron motion creates temporary dipoles → induces dipoles in neighbors → attractive interaction. This mechanism does not require permanent polarity.  
- Any species with electrons (noble gases, nonpolar molecules, polar molecules) can exhibit dispersion forces. For example, water (a polar molecule) also experiences London dispersion in addition to hydrogen bonding and dipole–dipole interactions.  
- Compare strengths: an ion (full charge) interacting with a dipole (partial charge) yields larger electrostatic attraction than two partial charges interacting, so ion–dipole > dipole–dipole.  
- Covalent bond energies (hundreds of kJ/mol) greatly exceed typical intermolecular energies (a few to tens of kJ/mol).  
- Increasing alkane chain length increases polarizability and contact area, enhancing dispersion forces and raising boiling points.

3. Calculations
- No numeric calculation required; reasoning is qualitative and based on relative interaction mechanisms and scaling with polarizability.

4. Why the correct answer is correct
- Option a is incorrect because dispersion forces occur between all species with electrons — not exclusively nonpolar molecules.

5. Why other options are incorrect (i.e., why they are actually correct statements)
- b: True — ion–dipole interactions are generally stronger than dipole–dipole because they involve a full charge.  
- c: True — intermolecular interactions are generally weaker than covalent bonds.  
- d: True — dispersion forces account for increasing boiling points of larger alkanes due to greater polarizability.

6. Conclusion
- The incorrect statement is option a. This matches the provided correct answer: a.

Which of the following is incorrect about intermolecular forces?[Fill in the blank]单项选择题

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Which of the following is incorrect about intermolecular forces?[Fill in the blank]单项选择题

类似问题

Which intermolecular interactions contribute most to the water solubility of organic compounds? A. ionic interactions and dispersion forces B. hydrogen bonding and ion-dipole interactions C. dispersion forces and hydrogen bonding D. dipole-dipole interactions and dispersion forces

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Question at position 3 Which of the following intermolecular forces is/are demonstrated by pure CH3F? Choose the single best answer. 1. hydrogen bonding 2. ionic forces 3. dispersion forces 4. dipole-dipole forces 3 only1 only2 and 4 only3 and 4 only4 only2 only1 and 3 only1 and 2 only

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What type of bonding interactions are possible at positions (i) O-H and (iii) N+, respectively, of the following drug?

What type of bonding interactions are possible at positions (i) O-H and (iii) N+, respectively, of the following drug?

Which intermolecular interactions contribute most to the water solubility of drugs?

更多留学生实用工具

希望你的学习变得更简单

Match the following 1: Halogen bonding is 2: Van der Waals interactions are caused by the 3: Dipolar interactions result 4: The cation-π interaction is a