**Understanding Intermolecular Forces** **Which intermolecular force is the weakest?** 1. ☐ Dipole-Dipole 2. ☐ Induced Dipole 3. ☐ Hydrogen Bonds 4. ☐ Dispersion Forces **Explanation of Intermolecular Forces:** Intermolecular forces are forces of attraction or repulsion between molecules. They are crucial in determining the physical properties of substances. Here's a brief explanation of each type mentioned in the question: - **Dipole-Dipole:** These occur between polar molecules where there's a separation of charges within the molecule. Positive and negative ends of different molecules attract each other. - **Induced Dipole:** These arise when a molecule with a permanent dipole induces a dipole in a neighbouring nonpolar molecule. - **Hydrogen Bonds:** A strong type of dipole-dipole interaction, hydrogen bonds occur specifically when hydrogen is bonded to a highly electronegative atom (like N, O, or F) and interacts with a similar atom on a neighbouring molecule. - **Dispersion Forces (London Forces):** These are the weakest intermolecular forces. They result from temporary shifts in electron density within molecules, causing temporary dipoles which attract each other. In this list, **Dispersion Forces** are the weakest intermolecular forces. They are universally present in all molecules, whether polar or nonpolar, but are particularly significant in nonpolar substances.

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**Understanding Intermolecular Forces**

**Which intermolecular force is the weakest?**

1. ☐ Dipole-Dipole
2. ☐ Induced Dipole
3. ☐ Hydrogen Bonds
4. ☐ Dispersion Forces

**Explanation of Intermolecular Forces:**
Intermolecular forces are forces of attraction or repulsion between molecules. They are crucial in determining the physical properties of substances. Here's a brief explanation of each type mentioned in the question:

- **Dipole-Dipole:** These occur between polar molecules where there's a separation of charges within the molecule. Positive and negative ends of different molecules attract each other.
  
- **Induced Dipole:** These arise when a molecule with a permanent dipole induces a dipole in a neighbouring nonpolar molecule.
  
- **Hydrogen Bonds:** A strong type of dipole-dipole interaction, hydrogen bonds occur specifically when hydrogen is bonded to a highly electronegative atom (like N, O, or F) and interacts with a similar atom on a neighbouring molecule.

- **Dispersion Forces (London Forces):** These are the weakest intermolecular forces. They result from temporary shifts in electron density within molecules, causing temporary dipoles which attract each other.

In this list, **Dispersion Forces** are the weakest intermolecular forces. They are universally present in all molecules, whether polar or nonpolar, but are particularly significant in nonpolar substances.
Transcribed Image Text:**Understanding Intermolecular Forces** **Which intermolecular force is the weakest?** 1. ☐ Dipole-Dipole 2. ☐ Induced Dipole 3. ☐ Hydrogen Bonds 4. ☐ Dispersion Forces **Explanation of Intermolecular Forces:** Intermolecular forces are forces of attraction or repulsion between molecules. They are crucial in determining the physical properties of substances. Here's a brief explanation of each type mentioned in the question: - **Dipole-Dipole:** These occur between polar molecules where there's a separation of charges within the molecule. Positive and negative ends of different molecules attract each other. - **Induced Dipole:** These arise when a molecule with a permanent dipole induces a dipole in a neighbouring nonpolar molecule. - **Hydrogen Bonds:** A strong type of dipole-dipole interaction, hydrogen bonds occur specifically when hydrogen is bonded to a highly electronegative atom (like N, O, or F) and interacts with a similar atom on a neighbouring molecule. - **Dispersion Forces (London Forces):** These are the weakest intermolecular forces. They result from temporary shifts in electron density within molecules, causing temporary dipoles which attract each other. In this list, **Dispersion Forces** are the weakest intermolecular forces. They are universally present in all molecules, whether polar or nonpolar, but are particularly significant in nonpolar substances.
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