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Chapter 10: Problem 28

What is the angle between these two hybrid orbitals on the same atom? (a) \(s p\) and \(s p\) hybrid orbitals, (b) \(s p^{2}\) and \(s p^{2}\) hybrid orbitals, (c) \(s p^{3}\) and \(s p^{3}\) hybrid orbitals.

Short Answer

Expert verified
The bond angle between two sp hybrid orbitals is 180°, two sp2 hybrid orbitals is 120°, and two sp3 hybrid orbitals is 109.5°.

Step by step solution

01

Determine bond angles for sp orbitals

For sp hybrid orbitals, the molecule is arranged in a linear geometry. As there are only two orbitals, they are placed farthest from each other to minimize electron-electron repulsion, hence forming an angle of \(180^\circ\).
02

Determine bond angles for sp2 orbitals

For sp2 hybrid orbitals, the molecule adopts a trigonal planar geometry. The three hybrid orbitals arrange themselves as far apart as possible in a plane. Hence, the angle between any two orbitals is \(120^\circ\).
03

Determine bond angles for sp3 orbitals

For sp3 hybrid orbitals, the molecule has a tetrahedral geometry. The four hybrid orbitals are directed towards the corners of a regular tetrahedron in three-dimensional space to minimize electron-electron repulsion. Therefore, the bond angle is \(109.5^\circ\).

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