According to the VSEPR model, the progressive decrease in the bond angles in the series of molecules CH4, NH3, and H2O is best accounted for by the:_________

According to VSEPR theory, the presence of lone pairs caused increased repulsion of electron pairs on the valence shell of the centeral atom of the molecule. This decreases or distorts the bond angle. The decrease in bond ange depends on the number of lone pairs present on the valence shell of the central atom of the molecule. Ammonia has only one lone pair hence the bond angle is 107°, water has two lone pairs and the bond angle is 104°. Compare this this with the bond angle of 109° in methane which has only bond pairs and no lone pairs.

Martebi Martebi · Answer 2 · 2021-11-25T22:10:39+01:00

According to VSEPR model, the progressive decrease in the bond angles in the series of molecules CH4, NH3 and H2O is best accounted for by the increasing number of unshared pairs of electrons.

The VSEPR theory is centered around:

• The shape of a molecule is often dependent on the number of valence shell electron pairs around the central atom.

• The pairs of electrons in the valence shell open do not attact one another because their electron clouds are negatively charged.

• The paired electrons often occupy such positions in space that reduces repulsion and and increases the distance between them.

The presence of two or more resonance structures can stand as a molecule, the VSEPR model is used for any such structure.

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