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- https://chem.libretexts.org/Courses/Kenyon_College/Chemistry_231_and_232_-_Kenyon_College_(Getzler_Hofferberth_and_Hunsen)/1%3A_Structure_and_Bonding_in_Organic_Molecules/1.4%3A_Electron-Dot_Model_of__Bonding_-_Lewis__StructuresOne of the situations where expanded octet structures are treated as more favorable than Lewis structures that follow the octet rule is when the formal charges in the expanded octet structure are smal...One of the situations where expanded octet structures are treated as more favorable than Lewis structures that follow the octet rule is when the formal charges in the expanded octet structure are smaller than in a structure that adheres to the octet rule, or when there are less formal charges in the expanded octet than in the structure a structure that adheres to the octet rule.
- https://chem.libretexts.org/Bookshelves/Organic_Chemistry/Map%3A_Organic_Chemistry_(Vollhardt_and_Schore)/01._Structure_and_Bonding_in_Organic_Molecules/1.4%3A_Electron-Dot_Model_of__Bonding_-_Lewis__StructuresOne of the situations where expanded octet structures are treated as more favorable than Lewis structures that follow the octet rule is when the formal charges in the expanded octet structure are smal...One of the situations where expanded octet structures are treated as more favorable than Lewis structures that follow the octet rule is when the formal charges in the expanded octet structure are smaller than in a structure that adheres to the octet rule, or when there are less formal charges in the expanded octet than in the structure a structure that adheres to the octet rule.
- https://chem.libretexts.org/Ancillary_Materials/Laboratory_Experiments/Wet_Lab_Experiments/General_Chemistry_Labs/Online_Chemistry_Lab_Manual/Chem_10_Experiments/09%3A_Lewis_Structures_and_Molecular_Shapes_(Experiment)The objectives of this laboratory are: To practice drawing Lewis Structures for various covalently bonded molecules and polyatomic ions. To use model kits to construct these molecules/ions in order t...The objectives of this laboratory are: To practice drawing Lewis Structures for various covalently bonded molecules and polyatomic ions. To use model kits to construct these molecules/ions in order to explore their structure and shapes. To practice predicting molecular shapes (using VSEPR theory) and molecular polarity
- https://chem.libretexts.org/Courses/University_of_Illinois_UrbanaChampaign/Chem_2363A_Fundamental_Organic_Chemistry_I_(Chan)/01%3A_Intro_to_Chemical_Structure_and_Resonance/1.02%3A_Electron-Dot_Model_of__Bonding_-_Lewis__StructuresA general chemistry review of how to draw good Lewis structures and calculate formal charge.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/09%3A_Covalent_Bonding/9.21%3A_Valence_Bond_TheoryThis page covers valence bond theory, detailing how covalent bonds arise from the overlap of atomic orbitals as atoms approach each other, leading to stable bonds at specific distances. It uses exampl...This page covers valence bond theory, detailing how covalent bonds arise from the overlap of atomic orbitals as atoms approach each other, leading to stable bonds at specific distances. It uses examples like H2 and F2 to illustrate key concepts. Review questions focus on electron positions in orbitals, covalent bond formation, and the necessity of overlapping orbitals being of the same type.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/General_Chemistry_Supplement_(Eames)/Valence_Bond_Theory/Formal_Charges_in_Lewis_StructuresIf you imagine a reaction between (CH 3 ) 3 N and an oxygen atom, both electrons that form the bond to O come from N (the former lone pair). (This is a rare example of a reaction that is both a Lewis ...If you imagine a reaction between (CH 3 ) 3 N and an oxygen atom, both electrons that form the bond to O come from N (the former lone pair). (This is a rare example of a reaction that is both a Lewis acid-base reaction and a redox reaction.) However, once the bond is made, these electrons are shared.
- https://chem.libretexts.org/Courses/Prince_Georges_Community_College/CHEM_2000%3A_Chemistry_for_Engineers_(Sinex)/Unit_2%3A__Molecular_Structure/Chapter_4%3A_Chemical_Bonding/Chapter_4.4%3A_Lewis_Structures_and_Covalent_BondingAdd together the valence electrons from each atom. (Recall from Chapter 2 that the number of valence electrons is indicated by the position of the element in the periodic table.) If the species is a p...Add together the valence electrons from each atom. (Recall from Chapter 2 that the number of valence electrons is indicated by the position of the element in the periodic table.) If the species is a polyatomic ion, remember to add or subtract the number of electrons necessary to give the total charge on the ion.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/09%3A_Covalent_Bonding/9.05%3A_Lewis_Electron-Dot_StructuresThis page explains cholesterol's molecular structure (C27H46O) and its detailed atomic arrangement. It describes how Lewis electron-dot structures represent valence electrons and covalent bonds throug...This page explains cholesterol's molecular structure (C27H46O) and its detailed atomic arrangement. It describes how Lewis electron-dot structures represent valence electrons and covalent bonds through shared pairs. The concept of the octet rule is introduced, emphasizing that atoms share electrons for stability, with hydrogen forming H2 to resemble helium. Other atoms also share electrons to achieve a complete set of eight valence electrons.
- https://chem.libretexts.org/Courses/Chabot_College/Chem_12A%3A_Organic_Chemistry_Fall_2022/01%3A_Introduction_to_Organic_Chemistry-_review_of_atoms_and_molecules/1.07%3A_Electron-Dot_Model_of__Bonding_-_Lewis__StructuresOne of the situations where expanded octet structures are treated as more favorable than Lewis structures that follow the octet rule is when the formal charges in the expanded octet structure are smal...One of the situations where expanded octet structures are treated as more favorable than Lewis structures that follow the octet rule is when the formal charges in the expanded octet structure are smaller than in a structure that adheres to the octet rule, or when there are less formal charges in the expanded octet than in the structure a structure that adheres to the octet rule.
- https://chem.libretexts.org/Courses/University_of_Connecticut/Organic_Chemistry_-_Textbook_for_Chem_2443/01%3A_General_Chemistry_Topics_Review/1.02%3A_Electron-Dot_Model_of__Bonding_-_Lewis__StructuresOne of the situations where expanded octet structures are treated as more favorable than Lewis structures that follow the octet rule is when the formal charges in the expanded octet structure are smal...One of the situations where expanded octet structures are treated as more favorable than Lewis structures that follow the octet rule is when the formal charges in the expanded octet structure are smaller than in a structure that adheres to the octet rule, or when there are less formal charges in the expanded octet than in the structure a structure that adheres to the octet rule.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/09%3A_Covalent_Bonding/9.07%3A_Multiple_Covalent_BondsThis page outlines the process of managing leftover electrons in Lewis structures for covalent compounds and the necessity of double and triple bonds to satisfy the octet rule. It uses ethene (\(\ce{C...This page outlines the process of managing leftover electrons in Lewis structures for covalent compounds and the necessity of double and triple bonds to satisfy the octet rule. It uses ethene (C2H4) as an example of double bonding and nitrogen (N2) for triple bonding. The text concludes with a summary of these bonding types and includes review questions for further understanding.
