Question

using vsper theory, what are the approximate bond angles of a compound that has the central atom with all three electron pairs shared and no lone pair electrons? the molecule will form 180° bond angles because the lack of lone pair electrons means there will be no additional repulsion forces acting upon the atoms. therefore, atoms will lie on a linear plane. the molecule will form 109.5° bond angles because the lack of lone pair electrons means there will be no additional repulsion forces acting upon the atoms. therefore, atoms will lie on a trigonal plane. the molecule will form 105° bond angles because the lack of lone pair electrons means there will be no additional repulsion forces acting upon the atoms. therefore, atoms will lie on a linear plane. the molecule will form 120° bond angles because the lack of lone pair electrons means there will be no additional repulsion forces acting upon the atoms. therefore, atoms will lie on a trigonal plane.

Explanation:

According to VSEPR theory, when a central atom has three shared electron pairs (no lone pairs), it forms a trigonal planar geometry. In a trigonal planar geometry, the bond angles are \(120^{\circ}\).

Answer:

The molecule will form \(120^{\circ}\) bond angles because the lack of lone pair electrons means there will be no additional repulsion forces acting upon the atoms. Therefore, atoms will lie on a trigonal plane.