Domanda del libro di testo
Some mothballs used when storing clothes are made of naphthalene (C10H8), which has the following incomplete structure.
(a) Add double bonds where needed to draw a complete electron-dot structure.
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Ch.7 - Covalent Bonding and Electron-Dot Structures
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
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McMurry 8th EditionCh.7 - Covalent Bonding and Electron-Dot StructuresProblema 90
McMurry 8th EditionCh.7 - Covalent Bonding and Electron-Dot StructuresProblema 90Capitolo 7, Problema 90
Benzene has the following structural formula.
(b) Which statement best describes the carbon–carbon bonds in benzene?
(i) Three carbon–carbon bonds are longer and weaker than the other three carbon–carbon bonds.
(ii) All six carbon–carbon bonds are identical, and their length and strength are between a double and single bond.
(iii) The length of carbon–carbon double bond switches back and forth between the length of a double and a single bond.
Guida verificata passo dopo passo1
Step 1: Understand the structure of benzene. Benzene is a cyclic hydrocarbon with the molecular formula C6H6. It has a ring structure with alternating double and single bonds between carbon atoms.
Step 2: Recognize the concept of resonance in benzene. Benzene exhibits resonance, meaning that the electrons are delocalized over the entire ring structure, creating a hybrid of the possible resonance structures.
Step 3: Analyze the given statements. Statement (i) suggests that three carbon–carbon bonds are longer and weaker than the other three, which is not consistent with the resonance structure of benzene.
Step 4: Evaluate statement (ii). This statement suggests that all six carbon–carbon bonds are identical, with lengths and strengths between those of a single and double bond, which aligns with the concept of resonance in benzene.
Step 5: Consider statement (iii). This statement suggests that the length of the carbon–carbon double bond switches back and forth, which is not accurate for benzene as the bonds are delocalized and do not switch.
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Resonance Structures
Resonance structures are different ways of drawing the same molecule that illustrate the delocalization of electrons. In benzene, the electrons in the carbon-carbon bonds are not fixed in one position but are spread out over the entire ring, leading to equivalent structures. This concept helps explain the stability and unique properties of benzene compared to alkenes.
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01:42
Resonance Structures
Bond Length and Strength
In chemistry, bond length refers to the distance between the nuclei of two bonded atoms, while bond strength indicates the energy required to break that bond. In benzene, all carbon-carbon bonds are of equal length and strength, which is intermediate between single (longer, weaker) and double (shorter, stronger) bonds due to resonance, resulting in a stable structure.
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00:36Average Bond Order
Hybridization
Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can accommodate bonding. In benzene, the carbon atoms are sp² hybridized, which allows for the formation of three sigma bonds and one unhybridized p orbital. This p orbital participates in the delocalized pi bonding that characterizes the resonance in benzene.
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00:51Hybridization
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