Domanda del libro di testo
The azide ion, N3-, is a symmetrical ion, all of whose contributing resonance structures have formal charges. Draw three important contributing structures for this ion.
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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 107c
Draw the Lewis structure for each compound. c. H3AsO4
Guida verificata passo dopo passo1
Identify the total number of valence electrons in the compound. Arsenic (As) has 5 valence electrons, each hydrogen (H) has 1, and each oxygen (O) has 6. Calculate the total valence electrons for H_3AsO_4.
Determine the central atom. Typically, the least electronegative atom that is not hydrogen is the central atom. In this case, arsenic (As) will be the central atom.
Arrange the atoms around the central atom. Place the three hydrogen atoms and four oxygen atoms around the arsenic atom.
Connect the atoms with single bonds initially. Each bond represents a pair of electrons. Connect each hydrogen to an oxygen, and then connect each oxygen to the arsenic atom.
Distribute the remaining electrons to satisfy the octet rule for each atom, starting with the outer atoms (oxygen) and then the central atom (arsenic). Adjust the bonds if necessary to ensure all atoms have a complete octet, considering the possibility of double bonds if needed.
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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
Valence Electrons
Valence electrons are the outermost electrons of an atom and are crucial in determining how an atom will bond with others. The number of valence electrons influences the atom's reactivity and the types of bonds it can form. For example, in H3AsO4, knowing the valence electrons of hydrogen, arsenic, and oxygen helps in constructing the correct Lewis structure.
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02:12Transition Metals Valence Electrons
Formal Charge
Formal charge is a concept used to determine the distribution of electrons in a molecule and to assess the stability of a Lewis structure. It is calculated by comparing the number of valence electrons in the free atom to the number of electrons assigned to it in the structure. A Lewis structure with the lowest formal charges on atoms is generally more stable, guiding the correct representation of molecules like H3AsO4.
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01:53Formal Charge
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Calculate ΔHrxn for the combustion of octane (C8H18), a component of gasoline, by using average bond energies and then calculate it using enthalpies of formation from Appendix IIB. What is the percent difference between your results? Which result would you expect to be more accurate?
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Domanda del libro di testo
The heat of atomization is the heat required to convert a molecule in the gas phase into its constituent atoms in the gas phase. The heat of atomization is used to calculate average bond energies. Without using any tabulated bond energies, calculate the average C–Cl bond energy from the following data: the heat of atomization of CH4 is 1660 kJ/mol, and the heat of atomization of CH2Cl2 is 1495 kJ/mol.
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Domanda del libro di testo
List the following gas-phase ion pairs in order of the quantity of energy released when they form from separated gas-phase ions. List the pair that releases the least energy first. Na+ F-, Mg2+F-, Na+O2-, Mg2+O2-, Al3+O2-.
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Domanda del libro di testo
Draw the Lewis structure for each compound. b. H3PO3 (two OH bonds)
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