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Chapter 10 Properties of Solids and Liquids
10.2 Shapes of Molecules and Ions (VSEPR Theory) Learning Goal Predict the three- dimensional structure of a molecule or a polyatomic ion and classify it as polar or nonpolar.
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VSEPR In the valence shell electron repulsion theory (VSEPR), the three-dimensional shape of a molecule is determined by drawing the electron-dot formula counting the number of electron groups (one or more electron pairs) around the central atom placing the electron groups as far apart as possible around the central atom
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VSEPR According to VSEPR theory, the shape of a molecule is determined by the number of electron groups surrounding the central atom number of atoms bonded to the central atom
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VSEPR—Two Electron Groups
Central atoms with two electron groups (two double bonds) such as CO2 have a linear electron-group geometry linear shape with a bond angle of 180° to minimize repulsion
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VSEPR—Three Electron Groups
Central atoms with three electron groups (two single bonds, one double bond) such as H2CO have a trigonal planar electron-group geometry trigonal planar shape with a bond angle of 120° to minimize repulsion
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VSEPR—Three Electron Groups
Central atoms with three electron groups (a single bond, double bond, lone pair) such as SO2 have a trigonal planar electron-group geometry bent shape with a bond angle of 120° to minimize repulsion
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VSEPR—Four Electron Groups
Central atoms with four electron groups (four single bonds) such as CH4 have a tetrahedral electron-group geometry tetrahedral shape with a bond angle of 109° to minimize repulsion The carbon-hydrogen dash indicates the bond is behind the plane of the paper, and the wedge indicates the carbon-hydrogen bond is in front of the paper plane.
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VSEPR—Four Electron Groups
Central atoms with four electron groups (three single bonds, one lone pair) such as NH3 have a tetrahedral electron-group geometry trigonal pyramidal shape with a bond angle of 109° to minimize repulsion The wedge-dash notation represents the three-dimensional shape of the molecule.
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VSEPR—Four Electron Groups
Central atoms with four electron groups (two single bonds, two lone pairs) such as H2O have a tetrahedral electron-group geometry bent shape with a bond angle of 109° to minimize repulsion The wedge-dash notation represents the three-dimensional shape of the molecule.
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Molecular Shapes
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Molecular Shapes
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Guide to Predicting Molecular Shape (VSEPR Theory)
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Learning Check Use VSEPR theory to predict the shape of N2O.
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Solution Use VSEPR theory to predict the shape of N2O. Step 1 Draw the electron-dot formula. In the electron-dot structure with 16 e−, octets are acquired using two double bonds in the central N atom.
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Solution Use VSEPR theory to predict the shape of N2O. Step 2 Arrange the electron groups around the central atom to minimize repulsion. Repulsion is minimized with two electron groups at 180°, a linear arrangement.
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Solution Use VSEPR theory to predict the shape of N2O. Step 3 Use the atoms bonded to the central atom to determine the molecular shape. The shape of a N2O molecule with two bonded atoms and no lone pairs on the central N is linear.
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Learning Check State the number of electron groups, lone pairs, and bonded atoms, and use VSEPR theory to determine the shape of the following molecules: (1) tetrahedral (2) trigonal pyramidal (3) bent PF3 B. H2S CCl4 D. PO43–
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Solution State the number of electron groups, lone pairs, and bonded atoms, and use VSEPR theory to determine the shape of the following molecules: (1) tetrahedral (2) trigonal pyramidal (3) bent A. PF3 4 electron groups, 3 bonded atoms, lone pair, trigonal pyramidal (2) H2S 4 electron groups, 2 bonded atoms, lone pairs, bent (3)
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Solution State the number of electron groups, lone pairs, and bonded atoms, and use VSEPR theory to determine the shape of the following molecules: (1) tetrahedral (2) trigonal pyramidal (3) bent C. CCl4 4 electron groups, 4 bonded atoms, lone pairs, tetrahedral (1) PO43– electron groups, 4 bonded atoms, lone pairs, tetrahedral (1)
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