Question
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
Ask by Rogers Salinas. in the United States
Jan 22,2025
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Answer
**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.
Solution
### **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.
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Simplify this solution The Deep Dive
Chloromethane, CH₃Cl, experiences dipole-dipole interactions and London dispersion forces. First, the molecule has a polar covalent bond between carbon and chlorine, which creates a permanent dipole due to the electronegativity difference. Second, because of its molecular asymmetry, the dipoles do not cancel out, leading to overall polarity. Lastly, as a small molecule with electrons, it can also experience temporary fluctuations in electron density, allowing for London dispersion forces to occur among its molecules. Out of the listed molecules, NH₃ (ammonia) experiences hydrogen bonding. This is due to the presence of a highly electronegative element (nitrogen) bonded to hydrogen, allowing for strong interactions with other NH₃ molecules. While CH₃Cl is polar, it cannot form hydrogen bonds because the chlorine is not sufficiently small and electronegative like nitrogen or oxygen. CH₄, on the other hand, is nonpolar and lacks interactions capable of hydrogen bonding.
