Answer :
Final answer:
In diamond structure, carbon atoms form four covalent bonds that are arranged tetrahedrally. The theoretical bond angle is 109.5° but due to electron repulsion, it tends to be around 104.5° in a real-life diamond structure.
Explanation:
In the diamond structure, each carbon atom forms four covalent bonds with neighboring carbon atoms, creating a tetrahedral arrangement around each carbon atom. This arrangement results from the hybridization of the carbon atom's orbitals (sp³ hybridization) in a manner that optimizes electron pair repulsion. The integral
angle between the tetrahedral bonds of diamond is theoretically calculated to be 109.5°. However, due to molecule geometry factors, such as repulsion between electrons in the shared orbitals, in real life scenarios, the angle tends to be slightly lesser around 104.5°. This smaller bond angle is also due to the fact that the molecular structure is bent.
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