As the lone pair repulsion is stronger than the bond pair or bond pair-lone pair repulsion, it reduces the bond angle. The Lewis structure of ammonium NH 4 + ion consists of a nitrogen (N) atom at the center.It is bonded to four atoms of hydrogen (H) at the sides. This anomaly is due to the lone pair of electrons, and the smaller size of the fluorine atom. With fewer 90° LP–BP repulsions, we can predict that the structure with the lone pair of electrons in the equatorial position is more stable than the one with the lone pair in the axial position. This angle makes the structure bent where the ideal bond angle for the bent, trigonal pyramidal structure is 109.5°. Both conditions are suitable only for a trigonal pyramidal. It says the nitrogen trichloride has a steric number of 4 and consist of one lone pair of valence electron. It can be studied in detail with the help of the Valence Shell Electron Pair Repulsion (VSEPR) Theory. If we place it in the axial position, we have two 90° LP–BP repulsions at 90°. It makes the molecular geometry of nitrogen trichloride trigonal pyramidal. However, because the axial and equatorial positions are not chemically equivalent, where do we place the lone pair? If we place the lone pair in the equatorial position, we have three LP–BP repulsions at 90°. We designate SF 4 as AX 4E it has a total of five electron pairs.
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