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Y Part B Arrange the following amines in order of decreasing base strength Rank from strongest to weakest base. To rank items equivalent, overlap them. View Available Hint(s) Strongest base The correct ranking cannot be determined. | (CH2)NH | NH, | CHÍNH, | NhaB Reset Help Weakest base

Y Part B Arrange the following amines in order of decreasing base strength Rank from strongest to weakest base. To rank items equivalent, overlap them. View Available Hint(s) Strongest base The correct ranking cannot be determined. | (CH2)NH | NH, | CHÍNH, | NhaB Reset Help Weakest base

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
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Relative Amine Strength** Bases act as hydrogen ion acceptors because of the unshared electron pairs in their structure. Any group present in a base that withdraws electrons makes these electron pairs less available to accept a hydrogen ion. In contrast, any group that can act as an electron donating group, such as hydrocarbon groups (usually represented as R), can increase the base strength. Thus, the addition of electronegative atoms or groups of atoms to the structure of a base decreases the base strength, and electron donating groups increase base strength. Many common weak bases are derivatives of ammonia, in which H atom(s) of NH₃ are replaced with other groups. **Part B** Arrange the following amines in order of decreasing base strength. Rank from strongest to weakest base. To rank items as equivalent, overlap them. - \((CH_3)_2NH\) - \(NH_3\) - \(CH_3NH_2\) - \(NH_2Br\) **Diagram Explanation:** The diagram consists of four chemical groups arranged in a draggable format. There is a box divided into sections marked "Strongest base" and "Weakest base." Students are tasked with dragging each chemical group to the appropriate position according to their base strength. A checkbox is available for students to select if the correct ranking cannot be determined. Options available to the students include a "Reset" button to clear their selections and a "Help" button for additional guidance.
Transcribed Image Text:**Relative Amine Strength** Bases act as hydrogen ion acceptors because of the unshared electron pairs in their structure. Any group present in a base that withdraws electrons makes these electron pairs less available to accept a hydrogen ion. In contrast, any group that can act as an electron donating group, such as hydrocarbon groups (usually represented as R), can increase the base strength. Thus, the addition of electronegative atoms or groups of atoms to the structure of a base decreases the base strength, and electron donating groups increase base strength. Many common weak bases are derivatives of ammonia, in which H atom(s) of NH₃ are replaced with other groups. **Part B** Arrange the following amines in order of decreasing base strength. Rank from strongest to weakest base. To rank items as equivalent, overlap them. - \((CH_3)_2NH\) - \(NH_3\) - \(CH_3NH_2\) - \(NH_2Br\) **Diagram Explanation:** The diagram consists of four chemical groups arranged in a draggable format. There is a box divided into sections marked "Strongest base" and "Weakest base." Students are tasked with dragging each chemical group to the appropriate position according to their base strength. A checkbox is available for students to select if the correct ranking cannot be determined. Options available to the students include a "Reset" button to clear their selections and a "Help" button for additional guidance.
**Relative Strengths of Oxyacids and Amines** **Relative oxyacid strength** The strength of an acid is affected by the polarity of the bond connected to the acidic hydrogen. The more highly polarized this bond, the more easily the hydrogen is ionized. Electronegative atoms or groups of atoms present in the structure of an acid can act to withdraw electrons and produce additional polarization. Two common groups of acids to which this principle can be applied are oxyacids and carboxylic acids. **Part A** Arrange the following oxyacids in order of decreasing acid strength. **Rank from strongest to weakest acid. To rank items as equivalent, overlap them.** - **HClO₃** - **HClO₂** - **HBrO** - **HClO** **[Diagram Explanation]** The interface includes movable icons representing different oxyacids: HClO₃, HClO₂, HBrO, and HClO. Below these icons is a ranking chart with spaces labeled "Strongest acid" and "Weakest acid," where the icons can be placed in order. A checkbox option states, "The correct ranking cannot be determined." Additional features include buttons for "Reset" and "Help," as well as an option to "View Available Hint(s)" for assistance with the task.
Transcribed Image Text:**Relative Strengths of Oxyacids and Amines** **Relative oxyacid strength** The strength of an acid is affected by the polarity of the bond connected to the acidic hydrogen. The more highly polarized this bond, the more easily the hydrogen is ionized. Electronegative atoms or groups of atoms present in the structure of an acid can act to withdraw electrons and produce additional polarization. Two common groups of acids to which this principle can be applied are oxyacids and carboxylic acids. **Part A** Arrange the following oxyacids in order of decreasing acid strength. **Rank from strongest to weakest acid. To rank items as equivalent, overlap them.** - **HClO₃** - **HClO₂** - **HBrO** - **HClO** **[Diagram Explanation]** The interface includes movable icons representing different oxyacids: HClO₃, HClO₂, HBrO, and HClO. Below these icons is a ranking chart with spaces labeled "Strongest acid" and "Weakest acid," where the icons can be placed in order. A checkbox option states, "The correct ranking cannot be determined." Additional features include buttons for "Reset" and "Help," as well as an option to "View Available Hint(s)" for assistance with the task.
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