Domanda del libro di testo
Predict the ordering, from shortest to longest, of the bond lengths in CO, CO2, and CO32- .
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Ch.8 - Basic Concepts of Chemical Bonding
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 8, Problema 54c
For each of the following ions of nitrogen and oxygen, write a single Lewis structure that obeys the octet rule, and calculate the oxidation numbers and formal charges on all the atoms: c. NO2+.
Guida verificata passo dopo passo1
Step 1: Determine the total number of valence electrons.
Step 2: Draw a skeletal structure for NO2+.
Step 3: Distribute the remaining electrons to satisfy the octet rule.
Step 4: Calculate the formal charges for each atom.
Step 5: Determine the oxidation numbers for nitrogen and oxygen.
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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 are essential for visualizing how atoms share or transfer electrons to achieve stable electron configurations, typically following the octet rule, which states that atoms tend to bond in such a way that they each have eight electrons in their valence shell.
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04:28
Lewis Dot Structures: Ions
Octet Rule
The octet rule is a chemical rule of thumb that reflects the tendency of atoms to prefer having eight electrons in their valence shell, leading to greater stability. This rule is particularly applicable to main group elements and guides the formation of covalent bonds, as atoms will share, gain, or lose electrons to achieve a full outer shell, often resulting in the formation of ions or molecules.
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01:36Octet Rule
Oxidation Numbers and Formal Charges
Oxidation numbers are assigned to atoms in a molecule to indicate the degree of oxidation or reduction, reflecting the number of electrons lost or gained. Formal charge, on the other hand, 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. Both concepts are crucial for understanding the distribution of electrons in a molecule and ensuring that the Lewis structure accurately represents the molecule's electronic structure.
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01:53Formal Charge
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Domanda del libro di testo
Which one of these statements about formal charge is true? (a) Formal charge is the same as oxidation number. (b) To draw the best Lewis structure, you should minimize formal charge. (c) Formal charge takes into account the different electronegativities of the atoms in a molecule. (d) Formal charge is most useful for ionic compounds. (e) Formal charge is used in calculating the dipole moment of a diatomic molecule.
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Domanda del libro di testo
Write Lewis structures that satisfy the octet rule for the following molecules and ions: a. NH4+, b. C2F4 (the two C atoms are bonded to one another), c. COCl2 (the Cl atoms are bonded to C), d. HSO3− (H is bonded to one of the O atoms), e. HNC (H and C are both bonded to N), f. ClO3−.
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Domanda del libro di testo
(b) With what allotrope of oxygen is it isoelectronic?
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Domanda del libro di testo
Consider the formate ion, HCO2-, which is the anion formed when formic acid loses an H+ ion. The H and the two O atoms are bonded to the central C atom. (b) Are resonance structures needed to describe the structure?
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