Domanda del libro di testo
Draw the Lewis structure for each organic compound from its condensed structural formula. e. CH3CHO
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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 107
Draw the Lewis structure for HCSNH2. The carbon and nitrogen atoms are bonded together, and the sulfur atom is bonded to the carbon atom. Label each bond in the molecule as polar or nonpolar.
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Identify the total number of valence electrons in the molecule. Hydrogen (H) has 1 valence electron, carbon (C) has 4, sulfur (S) has 6, and nitrogen (N) has 5. Calculate the total by adding these together.
Arrange the atoms in the specified order: H-C-S-N-H-H. Connect the atoms with single bonds initially, ensuring that C is bonded to S and N, and N is bonded to the two H atoms.
Distribute the remaining valence electrons to satisfy the octet rule for each atom, starting with the most electronegative atoms (S and N). Remember that hydrogen only needs 2 electrons.
Check the formal charges on each atom to ensure the most stable structure. Adjust the bonding if necessary to minimize formal charges, possibly by forming double bonds.
Determine the polarity of each bond by comparing the electronegativity of the bonded atoms. A bond is polar if there is a significant difference in electronegativity between the two atoms. Label each bond as polar or nonpolar based on this analysis.
Concetti chiave
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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 between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting the behavior of molecules in chemical reactions.
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04:28
Lewis Dot Structures: Ions
Polarity of Bonds
The polarity of a bond refers to the distribution of electrical charge between two atoms in a molecule. A bond is considered polar if there is a significant difference in electronegativity between the two atoms, leading to an unequal sharing of electrons. Nonpolar bonds occur when atoms share electrons equally, typically between identical atoms or those with similar electronegativities.
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02:38Molecular Polarity
Molecular Geometry
Molecular geometry describes the three-dimensional arrangement of atoms within a molecule. It is influenced by the number of bonds and lone pairs around the central atom, which can affect the molecule's polarity and reactivity. Understanding molecular geometry is crucial for predicting how molecules interact with each other and their physical properties.
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01:33Molecular Geometry with Two Electron Groups
Pratica correlata
Domanda del libro di testo
Draw the Lewis structure for urea, H2NCONH2, one of the compounds responsible for the smell of urine. (The central carbon atom is bonded to both nitrogen atoms and to the oxygen atom.) Does urea contain polar bonds? Which bond in urea is most polar?
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Domanda del libro di testo
Use Lewis structures to explain why Br3- and I3- are stable, while F3- is not.
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Domanda del libro di testo
Some theories of aging suggest that free radicals cause certain diseases and perhaps aging in general. As you know from the Lewis model, such molecules are not chemically stable and will quickly react with other molecules. According to certain theories, free radicals may attack molecules within the cell, such as DNA, changing them and causing cancer or other diseases. Free radicals may also attack molecules on the surfaces of cells, making them appear foreign to the body's immune system. The immune system then attacks the cells and destroys them, weakening the body. Draw Lewis structures for each free radical implicated in this theory of aging. c. OH
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