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Draw the Lewis Struc these use "d" orbitals that apply. NO O 13 O BF3 O SF4

Draw the Lewis Struc these use "d" orbitals that apply. NO O 13 O BF3 O SF4

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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**Task Description: Evaluating Hybridization Using Lewis Structures** **Objective:** Draw the Lewis Structure of the following compounds: SF₄, I₃⁻, BF₃, and NO. Determine which of these compounds utilize 'd' orbitals for hybridization around the central atom. Select all that apply. **Options:** - [ ] SF₄ - [ ] BF₃ - [ ] I₃⁻ - [ ] NO **Instructions:** Analyze the given compounds through their Lewis structures to identify the use of 'd' orbitals for hybridization. Mark the appropriate options that exhibit this characteristic.
Transcribed Image Text:**Task Description: Evaluating Hybridization Using Lewis Structures** **Objective:** Draw the Lewis Structure of the following compounds: SF₄, I₃⁻, BF₃, and NO. Determine which of these compounds utilize 'd' orbitals for hybridization around the central atom. Select all that apply. **Options:** - [ ] SF₄ - [ ] BF₃ - [ ] I₃⁻ - [ ] NO **Instructions:** Analyze the given compounds through their Lewis structures to identify the use of 'd' orbitals for hybridization. Mark the appropriate options that exhibit this characteristic.
**Title: Lewis Structures and the Octet Rule** **Instructions:** Draw the Lewis Structure of SF₄, I₃⁻, BF₃, and NO to decide which of these violate the octet rule. Select all that apply. **Options:** - [ ] BF₃ - [ ] I₃⁻ - [ ] NO - [ ] SF₄ **Explanation:** - **Lewis Structures**: Diagrams that show the bonding between atoms and the lone pairs of electrons in a molecule. - **Octet Rule**: A chemical rule of thumb that reflects the tendency of main-group atoms to bond in such a way that each atom has eight electrons in its valence shell. *Considerations while answering:* 1. **SF₄ (Sulfur Tetrafluoride)**: Commonly violates the octet rule due to sulfur having more than eight electrons. 2. **I₃⁻ (Triiodide Ion)**: May involve expanded octets due to iodine. 3. **BF₃ (Boron Trifluoride)**: Often violates the octet rule because boron is stable with fewer than eight electrons. 4. **NO (Nitric Oxide)**: Known to have an odd number of electrons, often violating the octet rule. Check the appropriate boxes corresponding to the structures that do not conform to the octet rule based on your drawings and analysis.
Transcribed Image Text:**Title: Lewis Structures and the Octet Rule** **Instructions:** Draw the Lewis Structure of SF₄, I₃⁻, BF₃, and NO to decide which of these violate the octet rule. Select all that apply. **Options:** - [ ] BF₃ - [ ] I₃⁻ - [ ] NO - [ ] SF₄ **Explanation:** - **Lewis Structures**: Diagrams that show the bonding between atoms and the lone pairs of electrons in a molecule. - **Octet Rule**: A chemical rule of thumb that reflects the tendency of main-group atoms to bond in such a way that each atom has eight electrons in its valence shell. *Considerations while answering:* 1. **SF₄ (Sulfur Tetrafluoride)**: Commonly violates the octet rule due to sulfur having more than eight electrons. 2. **I₃⁻ (Triiodide Ion)**: May involve expanded octets due to iodine. 3. **BF₃ (Boron Trifluoride)**: Often violates the octet rule because boron is stable with fewer than eight electrons. 4. **NO (Nitric Oxide)**: Known to have an odd number of electrons, often violating the octet rule. Check the appropriate boxes corresponding to the structures that do not conform to the octet rule based on your drawings and analysis.
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