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- https://chem.libretexts.org/Bookshelves/Organic_Chemistry/Organic_Chemistry_III_(Morsch_et_al.)/29%3A_Orbitals_and_Organic_Chemistry_-_Pericyclic_Reactions/29.01%3A_Molecular_Orbitals_of_Conjugated_Pi_SystemsHOMO and LUMO are often referred to as frontier orbitals and their energy difference is termed the HOMO–LUMO gap. One common way of thinking about reactions in this way is through the concept of front...HOMO and LUMO are often referred to as frontier orbitals and their energy difference is termed the HOMO–LUMO gap. One common way of thinking about reactions in this way is through the concept of frontier orbitals. This idea says that if one species is going to donate electrons to another in order to form a new bond, then the donated electrons are most likely going to come from the highest occupied energy level.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/General_Chemistry_Supplement_(Eames)/Molecular_Orbital_Theory/Frontier_MOs%3A_An_Acid-Base_TheoryIn a redox reaction, the oxidant has a low LUMO, and the reductant has a high HOMO, but this time the oxidant LUMO is lower than the reductant HOMO, so that the electrons in the reductant HOMO move co...In a redox reaction, the oxidant has a low LUMO, and the reductant has a high HOMO, but this time the oxidant LUMO is lower than the reductant HOMO, so that the electrons in the reductant HOMO move completely to the oxidant LUMO. The HOMO is high, because 3d is not so stable, and the LUMO is low, because it is also 3d and not much higher than the HOMO (there is a gap because the other atoms around the Fe(II) in hemoglobin make the d orbitals different energies).
- https://chem.libretexts.org/Courses/Oregon_Institute_of_Technology/OIT%3A_CHE_332_--_Organic_Chemistry_II_(Lund)/1%3A_Fall_term_review_sections/4%3A_Structure_Determination_I-_UV-Vis_and_Infrared_Spectroscopy_Mass_Spectrometry/4.4%3A_Ultraviolet_and_visible_spectroscopyWhile interaction with infrared light causes molecules to undergo vibrational transitions, the shorter wavelength, higher energy radiation in the UV (200-400 nm) and visible (400-700 nm) range of the ...While interaction with infrared light causes molecules to undergo vibrational transitions, the shorter wavelength, higher energy radiation in the UV (200-400 nm) and visible (400-700 nm) range of the electromagnetic spectrum causes many organic molecules to undergo electronic transitions. What this means is that when the energy from UV or visible light is absorbed by a molecule, one of its electrons jumps from a lower energy to a higher energy molecular orbital.
- https://chem.libretexts.org/Courses/can/CHEM_232_-_Organic_Chemistry_II_(Puenzo)/15%3A_Orbitals_and_Organic_Chemistry_-_Pericyclic_Reactions/15.02%3A_Molecular_Orbitals_of_Conjugated_Pi_SystemsHOMO and LUMO are often referred to as frontier orbitals and their energy difference is termed the HOMO–LUMO gap. One common way of thinking about reactions in this way is through the concept of front...HOMO and LUMO are often referred to as frontier orbitals and their energy difference is termed the HOMO–LUMO gap. One common way of thinking about reactions in this way is through the concept of frontier orbitals. This idea says that if one species is going to donate electrons to another in order to form a new bond, then the donated electrons are most likely going to come from the highest occupied energy level.
- https://chem.libretexts.org/Courses/Smith_College/Organic_Chemistry_(LibreTexts)/29%3A_Orbitals_and_Organic_Chemistry_-_Pericyclic_Reactions/29.01%3A_Molecular_Orbitals_of_Conjugated_Pi_SystemsHOMO and LUMO are often referred to as frontier orbitals and their energy difference is termed the HOMO–LUMO gap. One common way of thinking about reactions in this way is through the concept of front...HOMO and LUMO are often referred to as frontier orbitals and their energy difference is termed the HOMO–LUMO gap. One common way of thinking about reactions in this way is through the concept of frontier orbitals. This idea says that if one species is going to donate electrons to another in order to form a new bond, then the donated electrons are most likely going to come from the highest occupied energy level.
- https://chem.libretexts.org/Courses/Oregon_Institute_of_Technology/OIT%3A_CHE_333_-_Organic_Chemistry_III_(Lund)/New_Page/4%3A_Structure_Determination_I-_UV-Vis_and_Infrared_Spectroscopy_Mass_Spectrometry/4.4%3A_Ultraviolet_and_visible_spectroscopyWhile interaction with infrared light causes molecules to undergo vibrational transitions, the shorter wavelength, higher energy radiation in the UV (200-400 nm) and visible (400-700 nm) range of the ...While interaction with infrared light causes molecules to undergo vibrational transitions, the shorter wavelength, higher energy radiation in the UV (200-400 nm) and visible (400-700 nm) range of the electromagnetic spectrum causes many organic molecules to undergo electronic transitions. What this means is that when the energy from UV or visible light is absorbed by a molecule, one of its electrons jumps from a lower energy to a higher energy molecular orbital.
- https://chem.libretexts.org/Bookshelves/Organic_Chemistry/Book%3A_Organic_Chemistry_with_a_Biological_Emphasis_v2.0_(Soderberg)/04%3A_Structure_Determination_I-_UV-Vis_and_Infrared_Spectroscopy_Mass_Spectrometry/4.05%3A_Ultraviolet_and_visible_spectroscopyWhile interaction with infrared light causes molecules to undergo vibrational transitions, the shorter wavelength, higher energy radiation in the UV (200-400 nm) and visible (400-700 nm) range of the ...While interaction with infrared light causes molecules to undergo vibrational transitions, the shorter wavelength, higher energy radiation in the UV (200-400 nm) and visible (400-700 nm) range of the electromagnetic spectrum causes many organic molecules to undergo electronic transitions. What this means is that when the energy from UV or visible light is absorbed by a molecule, one of its electrons jumps from a lower energy to a higher energy molecular orbital.
- https://chem.libretexts.org/Bookshelves/Organic_Chemistry/Organic_Synthesis_(Shea)/01%3A_Pericyclic_Reactions/1.04%3A_Sigmatropic_RearrangementsThis chapter highlights synthetically useful sigmatropic rearrangements including hydride shifts, the Cope rearrangement, the Claisen rearrangement, and the Wittig rearrangement.
- https://chem.libretexts.org/Courses/Brevard_College/CHE_310%3A_Inorganic_Chemistry_(Biava)/05%3A_Advanced_Theories_of_Covalent_Bonding/5.05%3A_Molecular_Orbital_Theory/5.5.04%3A_Frontier_MOs-_An_Acid-Base_TheoryIn a redox reaction, the oxidant has a low LUMO, and the reductant has a high HOMO, but this time the oxidant LUMO is lower than the reductant HOMO, so that the electrons in the reductant HOMO move co...In a redox reaction, the oxidant has a low LUMO, and the reductant has a high HOMO, but this time the oxidant LUMO is lower than the reductant HOMO, so that the electrons in the reductant HOMO move completely to the oxidant LUMO. The HOMO is high, because 3d is not so stable, and the LUMO is low, because it is also 3d and not much higher than the HOMO (there is a gap because the other atoms around the Fe(II) in hemoglobin make the d orbitals different energies).
- https://chem.libretexts.org/Courses/Providence_College/Organic_Chemistry_I/06%3A_Alkenes/6.02%3A_Bonding_Stereoisomerism_and_StabilityIn ethylene, the C=C double bond would look like this, in which there is net bonding between the carbon atoms (σC−C) AND above and below the plane of the molecule (πC−C). The atomic p or...In ethylene, the C=C double bond would look like this, in which there is net bonding between the carbon atoms (σC−C) AND above and below the plane of the molecule (πC−C). The atomic p orbital on the bridgehead is orthogonal to the atomic p orbital on the adjacent carbon, therefore there is no net bonding – the orbitals cannot mix because they are perpendicular to one another.
- https://chem.libretexts.org/Bookshelves/Inorganic_Chemistry/Inorganic_Coordination_Chemistry_(Landskron)/03%3A_Molecular_Orbitals/3.02%3A_Molecular_OrbitalsIn the point group C 2v this is the symmetry type A 1 . The symmetry type of the 2p z orbital is also A 1 . This is because the letter z is in the row for the symmetry type A 1 . Similarly, the 2p x a...In the point group C 2v this is the symmetry type A 1 . The symmetry type of the 2p z orbital is also A 1 . This is because the letter z is in the row for the symmetry type A 1 . Similarly, the 2p x and the 2p y orbitals have the symmetry type B 1 and B 2 respectively because the letters x and y are in the rows for the symmetry types B 1 and B 2 , respectively.
