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(c) What would you predict for the lengths of the bonds in NO2- relative to N¬O single bonds and double bonds?
Ch.8 - Basic Concepts of Chemical Bonding
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 8, Problema 52a,b,c
For each of the following molecules or ions of sulfur and oxygen, write a single Lewis structure that obeys the octet rule, and calculate the oxidation numbers and formal charges on all the atoms: (a) SO2 Write a single Lewis structure that obeys the octet rule for SO2 and assign the formal charges on all the atoms. (b) SO3 Write a single Lewis structure that obeys the octet rule for SO3 and assign the formal charges on all the atoms. (c) SO32- Write a single Lewis structure that obeys the octet rule for SO32- and assign the formal charges on all the atoms.
Guida verificata passo dopo passo1
Draw the skeletal structure of the sulfite ion, SO_3^{2-}, with sulfur (S) as the central atom and three oxygen (O) atoms surrounding it.
Count the total number of valence electrons available. Sulfur has 6 valence electrons, each oxygen has 6, and there are 2 additional electrons due to the 2- charge, giving a total of 26 valence electrons.
Distribute the electrons around the atoms to satisfy the octet rule, starting by placing a single bond (2 electrons) between the sulfur and each oxygen atom.
Place the remaining electrons around the oxygen atoms to complete their octets, and then place any leftover electrons on the sulfur atom.
Calculate the formal charges for each atom using the formula: Formal Charge = (Valence electrons) - (Non-bonding electrons) - 0.5*(Bonding electrons). Assign these charges to each atom in the 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 are essential for visualizing how atoms share or transfer electrons to achieve stable electron configurations, particularly 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 chemical bonds, as atoms will gain, lose, or share electrons to fulfill this requirement.
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01:36Octet Rule
Formal Charge
Formal charge is a concept used to determine the charge of an atom in a molecule based on the number of valence electrons it possesses compared to the number of electrons it is assigned in the Lewis structure. It helps in assessing the most stable structure by minimizing the formal charges across the molecule, thus providing insight into the distribution of electrons and the overall charge of the molecule.
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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 for the following: (a) H2CO (both
H atoms are bonded to C), (b) H2O2, (c) C2F6 (contains
a C¬C bond), (d) AsO33 - , (e) H2SO3 (H is bonded to O), (f) NH2Cl.
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(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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