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Is each molecule a Lewis acid, bronstead acid, or both?

Is each molecule a Lewis acid, bronstead acid, or both?

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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Is each molecule a Lewis acid, bronstead acid, or both?

### Molecular Structures and Their Characteristics The image above illustrates the Lewis structures of four different molecules, highlighting their atomic connectivity and electron arrangements. 1. **Boron Trifluoride (BF₃)** - Structure: The molecule is symmetrical with a boron (B) atom centrally bonded to three fluorine (F) atoms. - Bonding: Each B-F bond is a single bond. Boron in this molecule is an exception to the octet rule, having only six electrons around it. - Shape: Trigonal planar, with 120-degree bond angles. 2. **Acetic Acid (CH₃COOH)** - Structure: This molecule consists of a methyl group (CH₃-) attached to a carboxyl group (-COOH). - Bonding: The carbon in the carboxyl group is double-bonded to one oxygen (O) and single-bonded to the hydroxyl group (OH) and the methyl carbon. - Shape: The carbon with the double bond is trigonal planar, while the methyl and hydroxyl carbons are tetrahedral. 3. **Trimethyl Oxonium Ion ((CH₃)₃O⁺)** - Structure: An oxygen atom is centrally bonded to three methyl groups (CH₃-) with a positive charge on the oxygen. - Bonding: Each O-C bond is a single bond. The positive charge indicates a full octet for the oxygen atom with an additional electron deficiency. - Shape: The structure is trigonal planar around the oxygen, having bond angles slightly less than 120 degrees due to the positive charge, which reduces electron repulsion. 4. **Methylammonium Ion (CH₃NH₃⁺)** - Structure: This ion has a central nitrogen (N) atom bonded to a methyl group (CH₃-) and three hydrogen (H) atoms, with a positive charge on the nitrogen. - Bonding: The N atom forms four single bonds, achieving an octet by sharing its electrons. - Shape: The nitrogen atom is sp³ hybridized, resulting in a tetrahedral geometry; however, the presence of the positive charge might distort the bond angles slightly. These diagrams demonstrate the molecular geometry, the arrangement of atoms, and electron sharing that occurs within these compounds, significant for understanding chemical bonding and molecular behavior.
Transcribed Image Text:### Molecular Structures and Their Characteristics The image above illustrates the Lewis structures of four different molecules, highlighting their atomic connectivity and electron arrangements. 1. **Boron Trifluoride (BF₃)** - Structure: The molecule is symmetrical with a boron (B) atom centrally bonded to three fluorine (F) atoms. - Bonding: Each B-F bond is a single bond. Boron in this molecule is an exception to the octet rule, having only six electrons around it. - Shape: Trigonal planar, with 120-degree bond angles. 2. **Acetic Acid (CH₃COOH)** - Structure: This molecule consists of a methyl group (CH₃-) attached to a carboxyl group (-COOH). - Bonding: The carbon in the carboxyl group is double-bonded to one oxygen (O) and single-bonded to the hydroxyl group (OH) and the methyl carbon. - Shape: The carbon with the double bond is trigonal planar, while the methyl and hydroxyl carbons are tetrahedral. 3. **Trimethyl Oxonium Ion ((CH₃)₃O⁺)** - Structure: An oxygen atom is centrally bonded to three methyl groups (CH₃-) with a positive charge on the oxygen. - Bonding: Each O-C bond is a single bond. The positive charge indicates a full octet for the oxygen atom with an additional electron deficiency. - Shape: The structure is trigonal planar around the oxygen, having bond angles slightly less than 120 degrees due to the positive charge, which reduces electron repulsion. 4. **Methylammonium Ion (CH₃NH₃⁺)** - Structure: This ion has a central nitrogen (N) atom bonded to a methyl group (CH₃-) and three hydrogen (H) atoms, with a positive charge on the nitrogen. - Bonding: The N atom forms four single bonds, achieving an octet by sharing its electrons. - Shape: The nitrogen atom is sp³ hybridized, resulting in a tetrahedral geometry; however, the presence of the positive charge might distort the bond angles slightly. These diagrams demonstrate the molecular geometry, the arrangement of atoms, and electron sharing that occurs within these compounds, significant for understanding chemical bonding and molecular behavior.
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