Shape of ClF3 molecule is

strong{font-weight:bold !important}Explanation:Valence Electrons: Chlorine (Cl) has 7 valence electrons, and each fluorine (F) atom has 7 valence electrons. In ClF₃, chlorine forms three single bonds with fluorine atoms, using 3 of its valence electrons, leaving 4 electrons (2 lone pairs) on the chlorine atom.Electron Pair Geometry: Including the 3 bonding pairs and 2 lone pairs, there are 5 regions of electron density around the chlorine atom. According to the Valence Shell Electron Pair Repulsion (VSEPR) theory, these regions arrange themselves in a trigonal bipyramidal geometry to minimize repulsion.Molecular Shape: In this trigonal bipyramidal arrangement, the two lone pairs occupy equatorial positions due to their greater repulsive effect, while the three fluorine atoms occupy two axial positions and one equatorial position. This leads to a T-shaped molecular geometry for ClF₃.Correct option is: a) Bent T-shape

Shape of ClF3 molecule is

strong{font-weight:bold !important}Explanation:Valence Electrons: Chlorine (Cl) has 7 valence electrons, and each fluorine (F) atom has 7 valence electrons. In ClF₃, chlorine forms three single bonds with fluorine atoms, using 3 of its valence electrons, leaving 4 electrons (2 lone pairs) on the chlorine atom.Electron Pair Geometry: Including the 3 bonding pairs and 2 lone pairs, there are 5 regions of electron density around the chlorine atom. According to the Valence Shell Electron Pair Repulsion (VSEPR) theory, these regions arrange themselves in a trigonal bipyramidal geometry to minimize repulsion.Molecular Shape: In this trigonal bipyramidal arrangement, the two lone pairs occupy equatorial positions due to their greater repulsive effect, while the three fluorine atoms occupy two axial positions and one equatorial position. This leads to a T-shaped molecular geometry for ClF₃.Correct option is: a) Bent T-shape

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Shape of ClF₃ molecule is

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Trigonal bipyramidal

Bent T-shape

Pyramidal

Trigonal planar

answer is A.

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Detailed Solution

Explanation:

Valence Electrons: Chlorine (Cl) has 7 valence electrons, and each fluorine (F) atom has 7 valence electrons. In ClF₃, chlorine forms three single bonds with fluorine atoms, using 3 of its valence electrons, leaving 4 electrons (2 lone pairs) on the chlorine atom.
Electron Pair Geometry: Including the 3 bonding pairs and 2 lone pairs, there are 5 regions of electron density around the chlorine atom. According to the Valence Shell Electron Pair Repulsion (VSEPR) theory, these regions arrange themselves in a trigonal bipyramidal geometry to minimize repulsion.
Molecular Shape: In this trigonal bipyramidal arrangement, the two lone pairs occupy equatorial positions due to their greater repulsive effect, while the three fluorine atoms occupy two axial positions and one equatorial position. This leads to a T-shaped molecular geometry for ClF₃.

Correct option is: a) Bent T-shape

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