Question

The geometry of the CIF₃ molecule is best described as__

A. distorted tetrahedron
B. trigonal planar
C. tetrahedral
D. T-shaped
E. trigonal pyramidal

Answer 1

The geometry of the ClF₃ molecule adopts a T-shaped molecular structure due to its three bonding pairs and two lone pairs of electrons, as predicted by the VSEPR theory.

Step-by-step explanation:

The geometry of the ClF₃ molecule is best described by examining its electron pair geometry and the VSEPR (Valence Shell Electron Pair Repulsion) theory. According to this theory, electrons pairs around a central atom will arrange themselves as far apart as possible to minimize repulsion. In the case of ClF₃, the central chlorine atom is surrounded by three bonded pairs (Cl-F bonds) and two lone pairs of electrons.

Using VSEPR theory, we can deduce that ClF₃ will adopt a geometry that minimizes the repulsions between these electron pairs. The ideal geometry for five electron pairs is a trigonal bipyramid, with three equatorial and two axial positions. However, lone pairs tend to occupy the equatorial positions because there is more space to minimize repulsion. Thus, when lone pairs occupy two of the equatorial positions, it leaves the three fluorine atoms occupying two axial positions and one equatorial position, which results in a T-shaped molecular structure.

Hence, for ClF₃ with its three bonds and two lone pairs, the most stable molecular geometry is T-shaped, aligning with option D from the question, and is not a distorted tetrahedron (A), trigonal planar (B), tetrahedral (C), or trigonal pyramidal (E).

Answer 2

The geometry of the CIF₃ molecule is best described as T-shaped, due to the presence of three bonds and two lone pairs creating a trigonal bipyramid with a T-shaped molecular structure. So, the correct option is D. T-shaped.

Step-by-step explanation:

The geometry of the CIF₃ molecule can be determined by considering its electron pair geometry and the repulsion between electron pairs according to the VSEPR theory. CIF₃ has three bonds and two lone pairs on the central chlorine atom. The VSEPR model suggests that lone pairs occupy more space than bonding pairs, hence, the most stable arrangement for CIF₃ is one where the lone pairs are placed in equatorial positions of a trigonal bipyramidal structure. This results in a T-shaped molecular structure, reflecting the uneven distribution of electrons.

Furthermore, CIF₃ exhibits sp³d hybridization on the central atom, which is consistent with the trigonal bipyramidal form assumed by molecules with such hybridization. Having two lone pairs, CIF₃ distorts into a T-shaped molecular geometry, different from other possible geometries such as tetrahedral, trigonal planar, or trigonal pyramidal. Therefore, the correct option to describe the geometry of the CIF₃ molecule is D. T-shaped.