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Here are the molecular structures of CBR4 and CH3BR. Use the images and the electronegativity chart to answer the following questions: Br Br C... Br Br H. Br Which of the following intermolecular forces does CH3BT have? Why? A. London Dispersion forces B. Dipole-Dipole forces C. Hydrogen Bonds

Here are the molecular structures of CBR4 and CH3BR. Use the images and the electronegativity chart to answer the following questions: Br Br C... Br Br H. Br Which of the following intermolecular forces does CH3BT have? Why? A. London Dispersion forces B. Dipole-Dipole forces C. Hydrogen Bonds

Chemistry
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
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--- **Title: Understanding Intermolecular Forces** Here are the molecular structures of \(CBr_4\) and \(CH_3Br\). Use the images and the electronegativity chart to answer the following questions: **Molecular Structures:** 1. Structure of \(CBr_4\): ![Molecular Structure of CBr4](image_link) - Central carbon (C) atom bonded to four bromine (Br) atoms. 2. Structure of \(CH_3Br\): ![Molecular Structure of CH3Br](image_link) - Central carbon (C) atom bonded to three hydrogen (H) atoms and one bromine (Br) atom. **Question:** Which of the following intermolecular forces does \(CH_3Br\) have? Why? A. London Dispersion forces B. Dipole-Dipole forces C. Hydrogen Bonds *Answer in the text box below (Word Limit: 10,000 words):* --- **Explanation of Graph/Diagram:** The diagrams present ball-and-stick models of the molecules \(CBr_4\) and \(CH_3Br\). In the \(CBr_4\) diagram, the carbon atom is centrally located with four bromine atoms symmetrically around it, indicating a tetrahedral shape that is non-polar. The \(CH_3Br\) diagram shows a carbon atom at the center, with three hydrogen atoms and one bromine atom arranged in a tetrahedral geometry, suggesting polarity due to the difference in electronegativity between hydrogen, carbon, and bromine. The task involves assessing which type of intermolecular force \(CH_3Br\) exhibits based on its molecular structure and the provided electronegativity chart. --- **Note:** For accurate completion, make sure to refer to the electronegativity chart and consider the differences in electronegativity between the atoms involved.
Transcribed Image Text:--- **Title: Understanding Intermolecular Forces** Here are the molecular structures of \(CBr_4\) and \(CH_3Br\). Use the images and the electronegativity chart to answer the following questions: **Molecular Structures:** 1. Structure of \(CBr_4\): ![Molecular Structure of CBr4](image_link) - Central carbon (C) atom bonded to four bromine (Br) atoms. 2. Structure of \(CH_3Br\): ![Molecular Structure of CH3Br](image_link) - Central carbon (C) atom bonded to three hydrogen (H) atoms and one bromine (Br) atom. **Question:** Which of the following intermolecular forces does \(CH_3Br\) have? Why? A. London Dispersion forces B. Dipole-Dipole forces C. Hydrogen Bonds *Answer in the text box below (Word Limit: 10,000 words):* --- **Explanation of Graph/Diagram:** The diagrams present ball-and-stick models of the molecules \(CBr_4\) and \(CH_3Br\). In the \(CBr_4\) diagram, the carbon atom is centrally located with four bromine atoms symmetrically around it, indicating a tetrahedral shape that is non-polar. The \(CH_3Br\) diagram shows a carbon atom at the center, with three hydrogen atoms and one bromine atom arranged in a tetrahedral geometry, suggesting polarity due to the difference in electronegativity between hydrogen, carbon, and bromine. The task involves assessing which type of intermolecular force \(CH_3Br\) exhibits based on its molecular structure and the provided electronegativity chart. --- **Note:** For accurate completion, make sure to refer to the electronegativity chart and consider the differences in electronegativity between the atoms involved.
--- ### Molecular Structures and Intermolecular Forces **Here are the molecular structures of CBr<sub>4</sub> and CH<sub>3</sub>Br. Use the images and the electronegativity chart to answer the following questions:** <div> <img src="path/to/cbr4_structure.png" alt="CBr4 molecular structure"> <img src="path/to/ch3br_structure.png" alt="CH3Br molecular structure"> </div> **Molecular Structure of CBr<sub>4</sub>** The molecular structure of Carbon Tetrabromide (CBr<sub>4</sub>) displays a central carbon atom bonded to four bromine atoms arranged in a tetrahedral geometry. **Molecular Structure of CH<sub>3</sub>Br** The molecular structure of Methyl Bromide (CH<sub>3</sub>Br) shows a central carbon atom bonded to three hydrogen atoms and one bromine atom, also arranged in a tetrahedral geometry. #### Question **Which of the following intermolecular forces does CBr<sub>4</sub> have? Why?** A. London Dispersion forces B. Dipole-Dipole forces C. Hydrogen Bonds (Provide your answer below.) --- **Explanation of Graphs or Diagrams** In the diagrams above, the first figure depicts the structure of CBr<sub>4</sub>, with the carbon atom at the center and four bromine atoms symmetrically distributed around it. The second figure shows the structure of CH<sub>3</sub>Br, with a central carbon atom bonded to three hydrogen atoms and one bromine atom. **Intermolecular Forces Analysis** - **London Dispersion Forces:** These are weak intermolecular forces that arise due to the instantaneous dipoles in molecules. They are present in all molecules, even non-polar ones like CBr<sub>4</sub>. - **Dipole-Dipole Forces:** These occur between molecules with permanent dipoles. CH<sub>3</sub>Br, which has a polar bond due to the difference in electronegativity between C and Br, exhibits these forces. - **Hydrogen Bonds:** These specific intermolecular forces occur when hydrogen is bonded to highly electronegative atoms like N, O, or F. Neither CBr<sub>4</sub> nor CH<sub>3</sub
Transcribed Image Text:--- ### Molecular Structures and Intermolecular Forces **Here are the molecular structures of CBr<sub>4</sub> and CH<sub>3</sub>Br. Use the images and the electronegativity chart to answer the following questions:** <div> <img src="path/to/cbr4_structure.png" alt="CBr4 molecular structure"> <img src="path/to/ch3br_structure.png" alt="CH3Br molecular structure"> </div> **Molecular Structure of CBr<sub>4</sub>** The molecular structure of Carbon Tetrabromide (CBr<sub>4</sub>) displays a central carbon atom bonded to four bromine atoms arranged in a tetrahedral geometry. **Molecular Structure of CH<sub>3</sub>Br** The molecular structure of Methyl Bromide (CH<sub>3</sub>Br) shows a central carbon atom bonded to three hydrogen atoms and one bromine atom, also arranged in a tetrahedral geometry. #### Question **Which of the following intermolecular forces does CBr<sub>4</sub> have? Why?** A. London Dispersion forces B. Dipole-Dipole forces C. Hydrogen Bonds (Provide your answer below.) --- **Explanation of Graphs or Diagrams** In the diagrams above, the first figure depicts the structure of CBr<sub>4</sub>, with the carbon atom at the center and four bromine atoms symmetrically distributed around it. The second figure shows the structure of CH<sub>3</sub>Br, with a central carbon atom bonded to three hydrogen atoms and one bromine atom. **Intermolecular Forces Analysis** - **London Dispersion Forces:** These are weak intermolecular forces that arise due to the instantaneous dipoles in molecules. They are present in all molecules, even non-polar ones like CBr<sub>4</sub>. - **Dipole-Dipole Forces:** These occur between molecules with permanent dipoles. CH<sub>3</sub>Br, which has a polar bond due to the difference in electronegativity between C and Br, exhibits these forces. - **Hydrogen Bonds:** These specific intermolecular forces occur when hydrogen is bonded to highly electronegative atoms like N, O, or F. Neither CBr<sub>4</sub> nor CH<sub>3</sub
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