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.10 - Chemical Bonding I: The Lewis Model
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Capitolo 10, Problema 76
Draw the Lewis structure (including resonance structures) for methyl azide (CH3N3). For each resonance structure, assign formal charges to all atoms that have formal charge.
Guida verificata passo dopo passo1
Identify the total number of valence electrons in the molecule. Carbon (C) has 4 valence electrons, each hydrogen (H) has 1, and each nitrogen (N) has 5. Since there are three hydrogens and three nitrogens, the total number of valence electrons is 4 (from C) + 3 (from H) + 15 (from N) = 22 electrons.
Draw the skeletal structure of methyl azide. Connect the carbon atom to the three hydrogen atoms forming CH3. Then, connect this CH3 group to one of the nitrogen atoms. Continue connecting the nitrogen atoms in a linear chain, N-N-N.
Distribute the remaining electrons to complete the octets of the nitrogen atoms. Start by placing lone pairs on the nitrogen atoms to fulfill the octet rule, remembering that each bond shared between atoms counts as two electrons towards each atom's octet.
Draw resonance structures by moving pi electrons between the nitrogen atoms. In azides, the negative charge can resonate between the terminal nitrogen atoms. Use arrows to show the movement of electrons and redraw the structure showing alternate double and single bonds between the nitrogen atoms.
Assign formal charges for each atom in every resonance structure. Remember, the formal charge is calculated using the formula: Formal Charge = (Valence electrons of the atom) - (Non-bonding electrons + 1/2 bonding electrons). Make sure to check each atom in every resonance structure.
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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. They are used when a single Lewis structure cannot adequately represent the electron distribution in a molecule. The actual structure is a hybrid of these resonance forms, which helps in understanding the stability and reactivity of the molecule.
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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 minimizing formal charges across the molecule. Assigning formal charges is crucial for evaluating resonance structures and understanding molecular stability.
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01:53Formal Charge
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