Domanda del libro di testo
How important is the resonance structure shown here to the overall structure of carbon dioxide? Explain.
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Ch.9 - Chemical Bonding I: The Lewis Model
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving136
- Ch.2 - Atoms & Elements112
- Ch.3 - Molecules, Compounds & Chemical Equations159
- Ch.4 - Chemical Quantities & Aqueous Reactions140
- Ch.5 - Gases118
- Ch.6 - Thermochemistry106
- Ch.7 - Quantum-Mechanical Model of the Atom62
- Ch.8 - Periodic Properties of the Elements103
- Ch.9 - Chemical Bonding I: The Lewis Model104
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory89
- Ch.11 - Liquids, Solids & Intermolecular Forces73
- Ch.12 - Solids and Modern Material59
- Ch.13 - Solutions110
- Ch.14 - Chemical Kinetics140
- Ch.15 - Chemical Equilibrium78
- Ch.16 - Acids and Bases155
- Ch.17 - Aqueous Ionic Equilibrium176
- Ch.18 - Free Energy and Thermodynamics108
- Ch.19 - Electrochemistry118
- Ch.20 - Radioactivity and Nuclear Chemistry82
- Ch.21 - Organic Chemistry150
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Capitolo 9, Problema 69
Draw the Lewis structure (including resonance structures) for the acetate ion (CH3COO-). For each resonance structure, assign formal charges to all atoms that have formal charge.
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insert step 1> Start by counting the total number of valence electrons. Carbon has 4 valence electrons, hydrogen has 1, and oxygen has 6. The acetate ion (CH3COO-) has a negative charge, which means you add one extra electron. Calculate the total number of valence electrons: 2 Carbons (2x4) + 3 Hydrogens (3x1) + 2 Oxygens (2x6) + 1 extra electron = 24 valence electrons.
insert step 2> Draw the skeletal structure of the acetate ion. Place the two carbon atoms in the center, with one carbon bonded to three hydrogen atoms (CH3) and the other carbon bonded to two oxygen atoms (COO). Connect the two carbon atoms with a single bond.
insert step 3> Distribute the remaining valence electrons to satisfy the octet rule. Start by placing lone pairs on the oxygen atoms to complete their octets. Then, place any remaining electrons on the central carbon atoms.
insert step 4> Consider resonance structures. In the acetate ion, the negative charge can be delocalized between the two oxygen atoms. Draw a double bond between one of the oxygen atoms and the central carbon, and a single bond with the other oxygen. Then, switch the positions of the double and single bonds to show the resonance structure.
insert step 5> Assign formal charges to each atom in both resonance structures. The formal charge is calculated as: Formal Charge = (Valence electrons) - (Non-bonding electrons) - 0.5*(Bonding electrons). Calculate the formal charges for each atom in both resonance structures to ensure the overall charge of the ion is -1.
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Lewis Structures
Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They use dots to represent valence electrons and lines to represent bonds. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting reactivity.
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04:28
Lewis Dot Structures: Ions
Resonance Structures
Resonance structures are different ways of drawing the same molecule that illustrate the delocalization of electrons. In molecules like the acetate ion, resonance structures help depict how electrons are shared among atoms, leading to more accurate representations of the molecule's actual electron distribution. Each resonance structure contributes to the overall hybrid structure.
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01:42Resonance Structures
Formal Charge
Formal charge is a theoretical charge assigned to an atom in a molecule, calculated based on the number of valence electrons, the number of bonds, and the number of lone electrons. It helps in determining the most stable Lewis structure by indicating how electron distribution varies among atoms. Assigning formal charges is crucial for evaluating resonance structures and ensuring charge neutrality in the overall molecule.
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01:53Formal Charge
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