Thus molecular orbital theory correctly predicts that H 2 is a stable molecule. The two electrons enter an orbital whose energy is lower than that of the parent atomic orbitals, so the H 2 molecule is more stable than the two isolated hydrogen atoms. Because each H atom contributes one valence electron, the resulting two electrons are exactly enough to fill the σ 1 s bonding molecular orbital. We fill the orbitals according to the Pauli principle and Hund’s rule: each orbital can accommodate a maximum of two electrons with opposite spins, and the orbitals are filled in order of increasing energy. such as H 2, we use molecular orbitals that is, for a molecule in which two identical atoms interact, we insert the total number of valence electrons into the energy-level diagram ( Figure 6.5.2 ). To describe the bonding in a homonuclear diatomic molecule A molecule that consists of two atoms of the same element. Because the energy of the σ 1 s molecular orbital is lower than that of the two H 1 s atomic orbitals, the H 2 molecule is more stable (at a lower energy) than the two isolated H atoms. The two available electrons (one from each H atom) in this diagram fill the bonding σ 1 s molecular orbital. in Figure 6.5.2įigure 6.5.2 Molecular Orbital Energy-Level Diagram for H 2 The relative energy levels of these orbitals are shown in the energy-level diagram A schematic drawing that compares the energies of the molecular orbitals (bonding, antibonding, and nonbonding) with the energies of the parent atomic orbitals. \) (antibonding) molecular orbital is destabilized.
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