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Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory
Tro - Chemistry: A Molecular Approach 4th Edition
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Tutti i libri di testoTro 4th EditionCh.10 - Chemical Bonding II: Molecular Shapes & Valence Bond TheoryProblema 39c
Capitolo 10, Problema 39c

Determine the molecular geometry and sketch each molecule or ion using the bond conventions shown in 'Representing Molecular Geometries on Paper' in Section 10.4. c. IF2-

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Determine the total number of valence electrons for IF_2^-. Iodine (I) has 7 valence electrons, each fluorine (F) has 7 valence electrons, and the negative charge adds 1 more electron.
Calculate the total number of valence electrons: 7 (I) + 2*7 (F) + 1 (negative charge) = 22 valence electrons.
Draw the Lewis structure: Place iodine (I) in the center, and arrange the two fluorine (F) atoms around it. Distribute the electrons to satisfy the octet rule for each atom.
Determine the electron pair geometry using VSEPR theory. Count the number of bonding pairs and lone pairs around the central iodine atom.
Identify the molecular geometry based on the arrangement of bonding pairs and lone pairs around the central atom. Sketch the molecule using the bond conventions, showing the lone pairs and bond angles.

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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.
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Molecular Geometry with Two Electron Groups

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They are essential for visualizing the arrangement of electrons and help in predicting molecular geometry by showing how atoms are connected and the distribution of electron pairs.
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Lewis Dot Structures: Ions
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