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40. Write Lewis structures for the following: (a) O2 (b) H2CO (c) ASF3

40. Write Lewis structures for the following: (a) O2 (b) H2CO (c) ASF3

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 40: Write Lewis Structures for the Following Molecules This activity requires drawing Lewis structures, which represent the valence electrons in a molecule. These structures help in understanding the bonding and the arrangement of atoms within the molecule. #### Molecules and Ions: (a) **O₂** - **Oxygen Gas:** Diatomic molecule consisting of two oxygen atoms. Determine the double bond and lone pairs present. (b) **H₂CO** - **Formaldehyde:** Consists of hydrogen, carbon, and oxygen. Recognize the carbon atom as the central atom, with hydrogen and one oxygen atom double bonded. (c) **AsF₃** - **Arsenic Trifluoride:** Contains arsenic as the central atom bonded with three fluorine atoms. (d) **ClNO** - **Chlorine Nitrosyl:** Includes chlorine, nitrogen, and oxygen. Nitrogen is typically central in this arrangement. (e) **SiCl₄** - **Silicon Tetrachloride:** A silicon atom bonded to four chlorine atoms. (f) **H₃O⁺** - **Hydronium Ion:** Comprises three hydrogen atoms and one oxygen atom, indicating a positive charge. (g) **NH₄⁺** - **Ammonium Ion:** Consists of four hydrogen atoms surrounding a nitrogen atom, with a positive charge overall. (h) **BF₄⁻** - **Tetrafluoroborate Ion:** Boron atom bonded to four fluorine atoms, and carries a negative charge. (i) **HCCH** - **Acetylene (Ethyne):** Linear structure with a triple bond between two carbon atoms, each bonded to a hydrogen atom. (j) **ClCN** - **Chlorine Cyanide:** Structures with chlorine, carbon, and nitrogen where carbon is bonded to both chlorine and nitrogen. (k) **C₂²⁺** - **Dication of Dicarbon:** Two carbon atoms with a total of two positive charges. Remember, while drawing the Lewis structures: 1. Count total valence electrons for each molecule. 2. Arrange atoms taking into account typical bonding patterns. 3. Assign remaining electrons as lone pairs to satisfy octet/duet rule. 4. Adjust for charge by adding or removing electrons where necessary.
Transcribed Image Text:### Task 40: Write Lewis Structures for the Following Molecules This activity requires drawing Lewis structures, which represent the valence electrons in a molecule. These structures help in understanding the bonding and the arrangement of atoms within the molecule. #### Molecules and Ions: (a) **O₂** - **Oxygen Gas:** Diatomic molecule consisting of two oxygen atoms. Determine the double bond and lone pairs present. (b) **H₂CO** - **Formaldehyde:** Consists of hydrogen, carbon, and oxygen. Recognize the carbon atom as the central atom, with hydrogen and one oxygen atom double bonded. (c) **AsF₃** - **Arsenic Trifluoride:** Contains arsenic as the central atom bonded with three fluorine atoms. (d) **ClNO** - **Chlorine Nitrosyl:** Includes chlorine, nitrogen, and oxygen. Nitrogen is typically central in this arrangement. (e) **SiCl₄** - **Silicon Tetrachloride:** A silicon atom bonded to four chlorine atoms. (f) **H₃O⁺** - **Hydronium Ion:** Comprises three hydrogen atoms and one oxygen atom, indicating a positive charge. (g) **NH₄⁺** - **Ammonium Ion:** Consists of four hydrogen atoms surrounding a nitrogen atom, with a positive charge overall. (h) **BF₄⁻** - **Tetrafluoroborate Ion:** Boron atom bonded to four fluorine atoms, and carries a negative charge. (i) **HCCH** - **Acetylene (Ethyne):** Linear structure with a triple bond between two carbon atoms, each bonded to a hydrogen atom. (j) **ClCN** - **Chlorine Cyanide:** Structures with chlorine, carbon, and nitrogen where carbon is bonded to both chlorine and nitrogen. (k) **C₂²⁺** - **Dication of Dicarbon:** Two carbon atoms with a total of two positive charges. Remember, while drawing the Lewis structures: 1. Count total valence electrons for each molecule. 2. Arrange atoms taking into account typical bonding patterns. 3. Assign remaining electrons as lone pairs to satisfy octet/duet rule. 4. Adjust for charge by adding or removing electrons where necessary.
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