(a)
Interpretation: The angles between the
Concept Introduction: VSEPR theory is used to predict the molecular shape with the help of electron pairs around the central atoms of the molecule. It is based on the assumption that the shape of the molecule is such that there is minimum electronic repulsion between the valence shell and the atom.
(a)
Explanation of Solution
According to VSEPR theory, the following table shows the relation between the total number of bonding and non-bonding pair of electrons and the geometry of a molecule.
Total number of bonding and non-bonding pairs | Hybridization | Electron pair geometry | Shape | ||||
No lone pairs | 1 | 2 | 3 | 4 | |||
6 | Octahedral | Octahedral | Square pyramidal | Square planar | T-shaped | Linear | |
5 | Trigonal pyramidal | Trigonal pyramidal | Sawhorse | T-shared | Linear | ||
4 | Tetrahedral | Tetrahedral | Trigonal planar | Bent | |||
3 | Trigonal planar | Trigonal planar | Bent | ||||
2 | Linear | Linear |
Now, the bond angle corresponding to the shape of the molecule is as follows:
Octahedral | and |
Trigonal pyramidal | and |
Tetrahedral | |
Trigonal planar | |
Linear |
Therefore, the angle between the
(b)
Interpretation: The angles between the
Concept Introduction: VSEPR theory is used to predict the molecular shape with the help of electron pairs around the central atoms of the molecule. It is based on the assumption that the shape of the molecule is such that there is minimum electronic repulsion between the valence shell and the atom.
(b)
Explanation of Solution
According to VSEPR theory, the following table shows the relation between the total number of bonding and non-bonding pair of electrons and the geometry of a molecule.
Total number of bonding and non-bonding pairs | Hybridization | Electron pair geometry | Shape | ||||
No lone pairs | 1 | 2 | 3 | 4 | |||
6 | Octahedral | Octahedral | Square pyramidal | Square planar | T-shaped | Linear | |
5 | Trigonal pyramidal | Trigonal pyramidal | Sawhorse | T-shared | Linear | ||
4 | Tetrahedral | Tetrahedral | Trigonal planar | Bent | |||
3 | Trigonal planar | Trigonal planar | Bent | ||||
2 | Linear | Linear |
Now, the bond angle corresponding to the shape of the molecule is as follows:
Octahedral | and |
Trigonal pyramidal | and |
Tetrahedral | |
Trigonal planar | |
Linear |
Therefore, the angle between the
(c)
Interpretation: The angles between the
Concept Introduction: VSEPR theory is used to predict the molecular shape with the help of electron pairs around the central atoms of the molecule. It is based on the assumption that the shape of the molecule is such that there is minimum electronic repulsion between the valence shell and the atom.
(c)
Explanation of Solution
According to VSEPR theory, the following table shows the relation between the total number of bonding and non-bonding pair of electrons and the geometry of a molecule.
Total number of bonding and non-bonding pairs | Hybridization | Electron pair geometry | Shape | ||||
No lone pairs | 1 | 2 | 3 | 4 | |||
6 | Octahedral | Octahedral | Square pyramidal | Square planar | T-shaped | Linear | |
5 | Trigonal pyramidal | Trigonal pyramidal | Sawhorse | T-shared | Linear | ||
4 | Tetrahedral | Tetrahedral | Trigonal planar | Bent | |||
3 | Trigonal planar | Trigonal planar | Bent | ||||
2 | Linear | Linear |
Now, the bond angle corresponding to the shape of the molecule is as follows:
Octahedral | and |
Trigonal pyramidal | and |
Tetrahedral | |
Trigonal planar | |
Linear |
Therefore, the angle between the
Chapter 8 Solutions
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