The figure that follows contains ball-and-stick drawings of three possible shapes of an AF4 molecule. (a) For each shape, give the electron-domain geometry on which the molecular geometry is based. i.

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Identify the central atom (A) and the four surrounding atoms (F) in each of the three structures.

Determine the number of electron domains around the central atom in each structure. This includes both bonding pairs and lone pairs of electrons.

For structure I, observe that there are four bonding pairs and no lone pairs around the central atom. This corresponds to a tetrahedral electron-domain geometry.

For structure II, observe that there are four bonding pairs and one lone pair around the central atom. This corresponds to a trigonal bipyramidal electron-domain geometry.

For structure III, observe that there are four bonding pairs and two lone pairs around the central atom. This corresponds to an octahedral electron-domain geometry.

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주요 개념

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Electron-Domain Geometry

Electron-domain geometry refers to the spatial arrangement of all electron domains (bonding and lone pairs) around a central atom in a molecule. It is determined by the number of electron domains, which can include single bonds, double bonds, triple bonds, and lone pairs. This geometry helps predict the overall shape of the molecule and is crucial for understanding molecular interactions.

Molecular Geometry

Molecular geometry describes the three-dimensional arrangement of atoms in a molecule, focusing only on the positions of the atoms and not the lone pairs. It is derived from the electron-domain geometry but is influenced by the repulsion between electron pairs, which can alter the shape. Common molecular geometries include linear, trigonal planar, tetrahedral, and bent, each with distinct bond angles.

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. This theory is fundamental for understanding how molecular structures are formed and how they influence chemical behavior.