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Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory
Tro - Chemistry: A Molecular Approach 6th Edition
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Tutti i libri di testoTro 6th EditionCh.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO TheoryProblema 40c
Capitolo 11, Problema 40c

Determine the molecular geometry and sketch each molecule or ion, using the bond conventions shown in “Representing Molecular Geometries on Paper” in Section 11.4. c. ClF3

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Determine the total number of valence electrons in ClF_3. Chlorine (Cl) has 7 valence electrons, and each fluorine (F) has 7 valence electrons. Calculate the total valence electrons for ClF_3.
Identify the central atom. In ClF_3, chlorine (Cl) is the central atom because it is less electronegative than fluorine (F).
Arrange the electrons around the central atom to satisfy the octet rule for the surrounding atoms first. Place three fluorine atoms around the chlorine atom, each forming a single bond with chlorine.
Distribute the remaining valence electrons as lone pairs on the central atom (Cl) to complete its octet. Remember that Cl can have an expanded octet.
Determine the molecular geometry using VSEPR theory. ClF_3 has 3 bonded pairs and 2 lone pairs on the central atom, leading to a T-shaped molecular geometry.

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VSEPR Theory

Valence Shell Electron Pair Repulsion (VSEPR) Theory is a model used to predict the geometry of individual molecules based on the repulsion between electron pairs in the valence shell of the central atom. According to VSEPR, electron pairs will arrange themselves as far apart as possible to minimize repulsion, leading to specific molecular shapes.
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Molecular Shapes and VSEPR

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is determined by the number of bonding pairs and lone pairs of electrons around the central atom, which influences the overall shape, such as linear, trigonal planar, tetrahedral, or octahedral configurations.
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Molecular Geometry with Two Electron Groups

Bonding and Lone Pairs

In molecular structures, bonding pairs are the pairs of electrons shared between atoms, while lone pairs are the pairs of valence electrons that are not involved in bonding. The presence of lone pairs can significantly affect the molecular geometry by altering bond angles and the overall shape of the molecule, as seen in molecules like ClF3, which has both bonding and lone pairs.
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Electron Groups, Lone Pairs, and Bonding Groups Example
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