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- https://chem.libretexts.org/Courses/can/CHEM_231%3A_Organic_Chemistry_I_Textbook/10%3A_Organohalides/10.05%3A_Stability_of_the_Allyl_Radical_-_Resonance_RevisitedNeither structure is correct by itself; the true structure of the allyl radical is a resonance hybrid of the two. (You might want to review Section 2.5 to Section 2.7 to brush up on resonance.) As not...Neither structure is correct by itself; the true structure of the allyl radical is a resonance hybrid of the two. (You might want to review Section 2.5 to Section 2.7 to brush up on resonance.) As noted in Section 2.6, the greater the number of resonance forms, the greater the stability of a compound, because bonding electrons are attracted to more nuclei.
- https://chem.libretexts.org/Courses/Alma_College/Organic_Chemistry_I_(Alma_College)/08%3A_Organohalides-_Radical_Halogenation_of_Alkanes_and_Alkenes/8.05%3A_Stability_of_the_Allyl_Radical_-_Resonance_RevisitedThe true structure of a species is a hybrid of the resonance contributors and is more stable (i.e., lower in energy) than any of the contributors. Experimental evidence indicates that the three bonds ...The true structure of a species is a hybrid of the resonance contributors and is more stable (i.e., lower in energy) than any of the contributors. Experimental evidence indicates that the three bonds in a carbon radical have trigonal planar geometry, and therefore the carbon is considered to be sp 2 -hybridized with the unpaired electron occupying the perpendicular, unhybridized 2p z orbital.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/25%3A_Organic_Chemistry/25.07%3A_Aromatic_HydrocarbonsThis page discusses Friedrich Kekulé, a 19th-century chemist who conceptualized benzene's cyclic structure, inspired by a dream. Benzene, an aromatic hydrocarbon with six hydrogen atoms and stabilizin...This page discusses Friedrich Kekulé, a 19th-century chemist who conceptualized benzene's cyclic structure, inspired by a dream. Benzene, an aromatic hydrocarbon with six hydrogen atoms and stabilizing delocalized pi electrons, has varied nomenclature based on its substituents. Basic naming involves alkyl groups, while arrangements with multiple substituents are identified by position numbers or ortho, meta, and para prefixes.
- https://chem.libretexts.org/Bookshelves/Organic_Chemistry/Organic_Chemistry_(Morsch_et_al.)/10%3A_Organohalides/10.04%3A_Stability_of_the_Allyl_Radical_-_Resonance_RevisitedThe true structure of a species is a hybrid of the resonance contributors and is more stable (i.e., lower in energy) than any of the contributors. Experimental evidence indicates that the three bonds ...The true structure of a species is a hybrid of the resonance contributors and is more stable (i.e., lower in energy) than any of the contributors. Experimental evidence indicates that the three bonds in a carbon radical have trigonal planar geometry, and therefore the carbon is considered to be sp 2 -hybridized with the unpaired electron occupying the perpendicular, unhybridized 2p z orbital.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/ChemPRIME_(Moore_et_al.)/21%3A_Spectra_and_Structure_of_Atoms_and_Molecules/21.08%3A_Delocalized_ElectronsFurthermore, each oxygen has a p orbital perpendicular to the plane of its sp 2 hybrids (that is, perpendicular to the plane of the three oxygen atoms), which has not yet been used for bonding. The tw...Furthermore, each oxygen has a p orbital perpendicular to the plane of its sp 2 hybrids (that is, perpendicular to the plane of the three oxygen atoms), which has not yet been used for bonding. The two electrons in the bonding MO provide a bond order of 1, but this is spread over both O—O bonds, and so it contributes a bond order of one-half between each pair of oxygens. Similarly the two electrons in the nonbonding MO correspond to a lone pair, half on the left oxygen and half on the right.
- https://chem.libretexts.org/Courses/Smith_College/Organic_Chemistry_(LibreTexts)/10%3A_Organohalides/10.05%3A_Stability_of_the_Allyl_Radical_-_Resonance_RevisitedThe true structure of a species is a hybrid of the resonance contributors and is more stable (i.e., lower in energy) than any of the contributors. Experimental evidence indicates that the three bonds ...The true structure of a species is a hybrid of the resonance contributors and is more stable (i.e., lower in energy) than any of the contributors. Experimental evidence indicates that the three bonds in a carbon radical have trigonal planar geometry, and therefore the carbon is considered to be sp 2 -hybridized with the unpaired electron occupying the perpendicular, unhybridized 2p z orbital.
- https://chem.libretexts.org/Bookshelves/Organic_Chemistry/Organic_Chemistry_I_(Morsch_et_al.)/10%3A_Organohalides/10.04%3A_Stability_of_the_Allyl_Radical_-_Resonance_RevisitedThe true structure of a species is a hybrid of the resonance contributors and is more stable (i.e., lower in energy) than any of the contributors. Experimental evidence indicates that the three bonds ...The true structure of a species is a hybrid of the resonance contributors and is more stable (i.e., lower in energy) than any of the contributors. Experimental evidence indicates that the three bonds in a carbon radical have trigonal planar geometry, and therefore the carbon is considered to be sp 2 -hybridized with the unpaired electron occupying the perpendicular, unhybridized 2p z orbital.
- https://chem.libretexts.org/Courses/Prince_Georges_Community_College/CHEM_2000%3A_Chemistry_for_Engineers_(Sinex)/Unit_2%3A__Molecular_Structure/Chapter_5%3A_Molecular_Geometry/Chapter_5.3_Delocalized_Bonding_and_Molecular_OrbitalsFigure 5.3.1 Molecular Orbitals for the H 2 Molecule (a) This diagram shows the formation of a bonding σ 1 s molecular orbital for H 2 as the sum of the wave functions (Ψ) of two H 1s atomic orbitals....Figure 5.3.1 Molecular Orbitals for the H 2 Molecule (a) This diagram shows the formation of a bonding σ 1 s molecular orbital for H 2 as the sum of the wave functions (Ψ) of two H 1s atomic orbitals. (b) This plot of the square of the wave function (Ψ 2 ) for the bonding σ 1 s molecular orbital illustrates the increased electron probability density between the two hydrogen nuclei. (Recall from Chapter 2 that the probability density is proportional to the square of the wave function.) (c) This …
- https://chem.libretexts.org/Workbench/LCDS_Organic_Chemistry_OER_Textbook_-_Todd_Trout/10%3A_Organohalides/10.05%3A_Stability_of_the_Allyl_Radical_-_Resonance_RevisitedNeither structure is correct by itself; the true structure of the allyl radical is a resonance hybrid of the two. (You might want to review Section 2.5 to Section 2.7 to brush up on resonance.) As not...Neither structure is correct by itself; the true structure of the allyl radical is a resonance hybrid of the two. (You might want to review Section 2.5 to Section 2.7 to brush up on resonance.) As noted in Section 2.6, the greater the number of resonance forms, the greater the stability of a compound, because bonding electrons are attracted to more nuclei.
- https://chem.libretexts.org/Bookshelves/Organic_Chemistry/Organic_Chemistry_(OpenStax)/10%3A_Organohalides/10.04%3A_Stability_of_the_Allyl_Radical_-_Resonance_RevisitedTo see why an allylic radical is so stable, look at the orbital picture. The radical carbon atom with an unpaired electron can adopt sp² hybridization, placing the unpaired electron in a p orbital and...To see why an allylic radical is so stable, look at the orbital picture. The radical carbon atom with an unpaired electron can adopt sp² hybridization, placing the unpaired electron in a p orbital and giving a structure that is electronically symmetrical. The p orbital on the central carbon can therefore overlap equally well with a p orbital on either of the two neighboring carbons.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/08%3A_Ionic_and_Metallic_Bonding/8.10%3A_Metallic_BondingThis page explains that metals possess unique properties due to metallic bonding, characterized by positive ions in a sea of delocalized electrons. This structure facilitates efficient electrical and ...This page explains that metals possess unique properties due to metallic bonding, characterized by positive ions in a sea of delocalized electrons. This structure facilitates efficient electrical and thermal conductivity, imparts luster through light interaction, and allows metals to be ductile and malleable, enabling shaping without breaking, in contrast to brittle ionic compounds. Overall, these properties are closely tied to the nature of metallic bonds.
