The incorrect order of bond angles (smallest first) in H2 S, NH3, BF3, and SiH4 is (1) H2 S<NH

step 1 The incorrect order of bond angles smallest first in H2S, NH3, BF3 and SIOH4, that is hydrogen s

The incorrect order of bond angles (smallest first) in H2...

The incorrect order of bond angles (smallest first) in $\mathrm{H}_{2} \mathrm{~S}, \mathrm{NH}_{3}, \mathrm{BF}_{3}$, and $\mathrm{SiH}_{4}$ is (1) $\mathrm{H}_{2} \mathrm{~S}<\mathrm{NH}_{3}<\mathrm{BF}_{3}<\mathrm{SiH}_{4}$ (2) $\mathrm{H}_{2} \mathrm{~S}<\mathrm{NH}_{3}<\mathrm{SiH}_{4}<\mathrm{BF}_{3}$ (3) $\mathrm{NH}_{3}<\mathrm{H}_{2} \mathrm{~S}<\mathrm{SiH}_{4}<\mathrm{BF}_{3}$ (4) $\mathrm{H}_{2} \mathrm{~S}<\mathrm{SiH}_{4}<\mathrm{NH}_{3}<\mathrm{BF}_{3}$ (a) $1,2,3$ (b) $2,3,4$ (c) $1,3,4$ (d) $1,2,4$

The incorrect order of bond angles (smallest first) in $\mathrm{H}_{2} \mathrm{~S}, \mathrm{NH}_{3}, \mathrm{BF}_{3}$, and $\mathrm{SiH}_{4}$ is
(1) $\mathrm{H}_{2} \mathrm{~S}<\mathrm{NH}_{3}<\mathrm{BF}_{3}<\mathrm{SiH}_{4}$
(2) $\mathrm{H}_{2} \mathrm{~S}<\mathrm{NH}_{3}<\mathrm{SiH}_{4}<\mathrm{BF}_{3}$
(3) $\mathrm{NH}_{3}<\mathrm{H}_{2} \mathrm{~S}<\mathrm{SiH}_{4}<\mathrm{BF}_{3}$
(4) $\mathrm{H}_{2} \mathrm{~S}<\mathrm{SiH}_{4}<\mathrm{NH}_{3}<\mathrm{BF}_{3}$
(a) $1,2,3$
(b) $2,3,4$
(c) $1,3,4$
(d) $1,2,4$

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Key Concepts

Bond Angle

Bond angles are the angles between adjacent lines representing bonds on a central atom. They are influenced by both the spatial arrangement of bonded atoms and the presence of lone pairs, with variations providing insights into the underlying electron repulsion and molecular structure.

Molecular Geometry

Molecular geometry describes the three-dimensional arrangement of atoms in a molecule. It is determined by the bonding and nonbonding electron pairs surrounding the central atom, which helps predict the relative spatial distribution of these atoms.

VSEPR Theory

The Valence Shell Electron Pair Repulsion (VSEPR) theory is a model used to predict the geometry of individual molecules from the number of electron pairs surrounding their central atoms. According to this theory, electron pairs, whether in bonds or as lone pairs, arrange themselves as far apart as possible to minimize repulsive forces.

Lone Pair Repulsion

Lone pairs of electrons occupy more space than bonding pairs, leading to greater repulsive forces. This increased repulsion can cause deviations from ideal bond angles in a molecule, as the bonding pairs are pushed closer together, altering the geometry compared to molecules without lone pairs.

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