5. What two types of intermolecular forces would chloromethane, CH 3 Cl , molecules experience? Justify your answer with at least 3 facts. 6. Which of the following molecules would experience hydrogen bonding? CH 4 CH 3 Cl NH 3

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### **Question 5: What two types of intermolecular forces would chloromethane, CH₃Cl, molecules experience? Justify your answer with at least 3 facts.**

**Answer:**
Chloromethane (CH₃Cl) molecules experience **dipole-dipole interactions** and **London dispersion forces** as their two primary types of intermolecular forces.

**Justification with Three Facts:**

1. **Polarity of the Molecule:**
   - **Dipole-Dipole Interactions:** Chloromethane is a polar molecule because of the significant electronegativity difference between carbon (C) and chlorine (Cl). This polarity results in a permanent dipole moment, allowing CH₃Cl molecules to align so that the positive end of one molecule is attracted to the negative end of another, facilitating dipole-dipole interactions.

2. **Presence of Temporary Induced Dipoles:**
   - **London Dispersion Forces:** Regardless of polarity, all molecules exhibit London dispersion forces, which arise from temporary fluctuations in the electron distribution around molecules. In CH₃Cl, these instantaneous dipoles can induce dipoles in neighboring molecules, leading to weak, transient attractions that contribute to the overall intermolecular forces.

3. **Absence of Hydrogen Bonding:**
   - **Exclusion of Hydrogen Bonding:** Unlike molecules that can engage in hydrogen bonding (which requires hydrogen atoms bonded to highly electronegative atoms like N, O, or F), CH₃Cl does not have hydrogen atoms bonded to these elements. Instead, hydrogen is bonded to carbon, which does not facilitate hydrogen bonding. This absence reinforces that only dipole-dipole interactions and London dispersion forces are present.

### **Question 6: Which of the following molecules would experience hydrogen bonding? CH₄, CH₃Cl, NH₃**

**Answer:**
Among the given molecules, only **NH₃ (ammonia)** experiences hydrogen bonding.

**Explanation:**

- **NH₃ (Ammonia):** This molecule has hydrogen atoms bonded directly to nitrogen (a highly electronegative atom). The N-H bonds are polar, and the lone pair on nitrogen allows ammonia molecules to form hydrogen bonds with each other, resulting in strong intermolecular attractions.

- **CH₄ (Methane):** In methane, hydrogen atoms are bonded to carbon, which is not sufficiently electronegative to create the polar bonds necessary for hydrogen bonding. As a result, CH₄ does not participate in hydrogen bonding.

- **CH₃Cl (Chloromethane):** While CH₃Cl is a polar molecule due to the C-Cl bond, the hydrogen atoms are still bonded to carbon rather than to highly electronegative atoms like nitrogen, oxygen, or fluorine. Therefore, CH₃Cl does not engage in hydrogen bonding.

### **Summary:**

- **Chloromethane (CH₃Cl):** Experiences **dipole-dipole interactions** and **London dispersion forces**.
- **Hydrogen Bonding:** Only **NH₃ (ammonia)** among the listed molecules experiences hydrogen bonding.
**Question 5:** Chloromethane (CH₃Cl) molecules experience **dipole-dipole interactions** and **London dispersion forces**. This is because CH₃Cl is a polar molecule with a significant electronegativity difference between carbon and chlorine, allowing for dipole-dipole attractions. Additionally, all molecules exhibit London dispersion forces due to temporary fluctuations in electron distribution, which contribute to weak, transient attractions between CH₃Cl molecules. **Question 6:** Only **NH₃ (ammonia)** among the given molecules experiences hydrogen bonding. This is because NH₃ has hydrogen atoms bonded to nitrogen, a highly electronegative atom, which allows for the formation of hydrogen bonds between ammonia molecules. Methane (CH₄) and chloromethane (CH₃Cl) do not engage in hydrogen bonding because their hydrogen atoms are bonded to carbon, not to highly electronegative elements. **Summary:** - **Chloromethane (CH₃Cl):** Dipole-dipole interactions and London dispersion forces. - **NH₃ (Ammonia):** Hydrogen bonding.

5. What two types of intermolecular forces would chloromethane, CH 3 Cl , molecules experience? Justify your answer with at least 3 facts. 6. Which of the following molecules would experience hydrogen bonding? CH 4 CH 3 Cl NH 3

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