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List the following molecules in order of increasing boiling point. Explain your ranking 3) ) HF dimethyl ether CH₂O HBr CH,OH n-propanol H HI CHA diethyl ether HCI

List the following molecules in order of increasing boiling point. Explain your ranking 3) ) HF dimethyl ether CH₂O HBr CH,OH n-propanol H HI CHA diethyl ether HCI

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
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The image presents a question related to the viscosity of different molecules. The task is to rank the molecules from least to most viscous: a. CH₂O, CH₃OH, CH₄ b. CH₄, C₃H₈, C₂H₆ There are no graphs or diagrams included, only a list of chemical formulas to be ranked based on their viscosity.
Transcribed Image Text:The image presents a question related to the viscosity of different molecules. The task is to rank the molecules from least to most viscous: a. CH₂O, CH₃OH, CH₄ b. CH₄, C₃H₈, C₂H₆ There are no graphs or diagrams included, only a list of chemical formulas to be ranked based on their viscosity.
**Title: Understanding Boiling Points of Different Molecules** **Objective:** Rank the following molecules in order of increasing boiling point and explain the reasoning behind their rankings. **Molecules:** a) - **Dimethyl Ether:** Chemical structure shown with an ether group (C-O-C). - **n-Propanol:** Chemical structure with an alcohol group (-OH) attached to a propane chain. - **Diethyl Ether:** Chemical structure with an ether group between two ethyl groups (CH₃CH₂-O-CH₂CH₃). b) - **HF (Hydrogen Fluoride)** - **HBr (Hydrogen Bromide)** - **HI (Hydrogen Iodide)** - **HCl (Hydrogen Chloride)** c) - **CH₂O (Formaldehyde)** - **CH₃OH (Methanol)** - **CH₄ (Methane)** **Detailed Explanation:** - **Boiling Points:** The boiling point is determined by the strength of intermolecular forces. The stronger the intermolecular forces, the higher the boiling point. - **Hydrogen Bonding:** Molecules that can form hydrogen bonds typically have higher boiling points due to the strong attraction between molecules. - **Molecular Weight:** Generally, the greater the molecular weight, the higher the boiling point due to increased Van der Waals forces. **Guidelines for Ranking:** 1. **Identify the Type of Intermolecular Forces:** - Hydrogen bonding - Dipole-dipole interactions - London dispersion forces (Van der Waals forces) 2. **Consider Molecular Structure and Functional Groups:** - Alcohols (e.g., n-propanol) often have higher boiling points due to hydrogen bonding. - Ethers (e.g., dimethyl ether, diethyl ether) have dipole-dipole interactions but cannot hydrogen-bond to themselves. - Simple molecules like methane have only London dispersion forces. 3. **Compare Similar Molecules:** - Compare within homologous series or similar chemical families for better accuracy. **Conclusion:** - Understanding the type and strength of intermolecular forces helps in accurately ranking the boiling points. - Practical implications include predicting solubility, reactivity, and other physical properties related to boiling points.
Transcribed Image Text:**Title: Understanding Boiling Points of Different Molecules** **Objective:** Rank the following molecules in order of increasing boiling point and explain the reasoning behind their rankings. **Molecules:** a) - **Dimethyl Ether:** Chemical structure shown with an ether group (C-O-C). - **n-Propanol:** Chemical structure with an alcohol group (-OH) attached to a propane chain. - **Diethyl Ether:** Chemical structure with an ether group between two ethyl groups (CH₃CH₂-O-CH₂CH₃). b) - **HF (Hydrogen Fluoride)** - **HBr (Hydrogen Bromide)** - **HI (Hydrogen Iodide)** - **HCl (Hydrogen Chloride)** c) - **CH₂O (Formaldehyde)** - **CH₃OH (Methanol)** - **CH₄ (Methane)** **Detailed Explanation:** - **Boiling Points:** The boiling point is determined by the strength of intermolecular forces. The stronger the intermolecular forces, the higher the boiling point. - **Hydrogen Bonding:** Molecules that can form hydrogen bonds typically have higher boiling points due to the strong attraction between molecules. - **Molecular Weight:** Generally, the greater the molecular weight, the higher the boiling point due to increased Van der Waals forces. **Guidelines for Ranking:** 1. **Identify the Type of Intermolecular Forces:** - Hydrogen bonding - Dipole-dipole interactions - London dispersion forces (Van der Waals forces) 2. **Consider Molecular Structure and Functional Groups:** - Alcohols (e.g., n-propanol) often have higher boiling points due to hydrogen bonding. - Ethers (e.g., dimethyl ether, diethyl ether) have dipole-dipole interactions but cannot hydrogen-bond to themselves. - Simple molecules like methane have only London dispersion forces. 3. **Compare Similar Molecules:** - Compare within homologous series or similar chemical families for better accuracy. **Conclusion:** - Understanding the type and strength of intermolecular forces helps in accurately ranking the boiling points. - Practical implications include predicting solubility, reactivity, and other physical properties related to boiling points.
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