91影视

First, we need to draw the Lewis structures for O鈧� and NO鈧傗伝 molecules. For O鈧�, the Lewis structure is: \[ \underset{ : }{ O } - \overset{ + }{ \underset{ : }{ O } } - \overset{ - }{ \underset{ : }{ O } } \] For NO鈧傗伝 ion, the Lewis structure is: \[ \underset{ : }{ N } - \overset{ + }{ \underset{ : }{ O } } - \overset{ - }{ \underset{ : }{ O } } \]

Using the Valence Shell Electron Pair Repulsion (VSEPR) theory, we can see that both molecules have one central atom with two other atoms attached and one lone pair of electrons. Therefore, both molecules have a bent VSEPR structure. The hybridization of both central atoms in O鈧� and NO鈧傗伝 is sp虏.

In the localized electron model, we consider electron pairs to be localized between the bonded atoms. In both O鈧� and NO鈧傗伝 molecules, the central atoms form two sigma (蟽) bonds using their sp虏 hybrid orbitals, and one pi (蟺) bond using their remaining p orbital. The 蟺 bond in both molecules is delocalized over the three atoms in a resonance structure, resulting in a partial double bond character between all three atoms.

In the molecular orbital model, we consider the molecular orbitals formed by the combination of atomic orbitals. In O鈧� and NO鈧傗伝, the 蟺 bonding results from the overlap of the p orbitals on the three atoms involved. This creates a delocalized 蟺 bond which extends over all three atoms, effectively lowering the energy of the molecule and stabilizing it. In summary, the localized electron model describes the bonding in O鈧� and NO鈧傗伝 using sigma bonds formed by sp虏 hybrid orbitals and a delocalized 蟺 bond using p orbitals, which are in resonance over the three atoms. The molecular orbital model describes the same 蟺 bonding as a delocalized bond that results from the overlap of the p orbitals of the involved atoms, contributing to molecular stability.