The energy of an electron is determined by its position in an atom or molecule. In the H2 molecule, two hydrogen atoms come together and form a covalent bond. This bond is formed through the overlap of atomic orbitals from each hydrogen atom, resulting in the formation of two molecular orbitals - the bonding molecular orbital and the antibonding molecular orbital.
The bonding molecular orbital is formed by the constructive interference of the atomic orbitals, leading to an increase in electron density between the two hydrogen nuclei. As a result, the electron in the bonding molecular orbital experiences a more attractive force from both nuclei, and this increased attraction leads to a lower energy state for the electron.
On the other hand, the antibonding molecular orbital is formed by the destructive interference of the atomic orbitals, resulting in a decrease in electron density between the two nuclei. In this case, the electron experiences a repulsive force from both nuclei, leading to a higher energy state for the electron compared to when it was in the atomic orbital.
Therefore, the electron in the bonding molecular orbital in the H2 molecule has a lower energy than an electron in the atomic orbital.
explain why an electron in the bonding molecular orbital in the h2 molecule has a lower energy than an electron
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1 answer