Molecular orbital theory explains the bonding and antibonding orbitals formed when atoms combine to form molecules.
When atomic orbitals are in phase, they combine to form a bonding molecular orbital, which has a high probability of finding an electron between the nuclei.
Electrons in molecular orbitals favor the formation of molecules by occupying the region between the nuclei.
🔬 The forces between protons in a molecule favor bond formation.
🌗 Destructive interference between electron waves creates an antibonding molecular orbital.
🚫 An antibonding molecular orbital has a node where the probability of finding an electron is zero.
🔍 In the formation of an H2 molecule, the electrons are more likely to be found outside the region between the two nuclei, resulting in weak forces of attraction and a repulsive net force.
🔀 The bonding molecular orbital has a high probability of finding electrons between the nuclei, while the antibonding molecular orbital has a low probability of finding electrons between the nuclei.
🌗 Anti-bonding is associated with destructive interference, while the bonding molecular orbital is associated with constructive interference.
🔑 In molecular orbital theory, electrons are more likely to be found outside the nuclei, favoring bond formation.
🗂️ The energy diagram of a molecular orbital shows that bonding molecular orbitals have lower energy, while antibonding molecular orbitals have higher energy.
⚡ Electrons naturally fall to lower energy levels, releasing energy and promoting bond formation.
⚛️ Paramagnetic and diamagnetic substances are determined by the presence of unpaired or paired electrons, respectively.
🔢 The bond order of a molecule can be calculated by subtracting the number of antibonding electrons from the number of bonding electrons, divided by two.
🔗 Higher bond order indicates greater stability and lower energy, while shorter bonds are stronger and longer bonds are weaker.
🔗 Triple bonds are stronger and shorter than single bonds.
🧪 Bond order determines the stability and reactivity of molecules.
💥 Breaking a bond requires energy, and more energy is needed for triple bonds.
🔑 The bond order of the H2 ion is one-half, making it less stable than H2.
💻 The electron configuration of the H2- ion is sigma 1s with 2 electrons and sigma 1s* with 1 electron.
🔬 The dihelium atom does not form a stable molecule and exists as individual helium atoms.
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