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A triple bond is characterized by one sigma bond and two pi bonds. In the formation of a triple bond, the first bond that forms is a sigma bond, which is created by the head-on overlap of atomic orbitals. This bond has cylindrical symmetry around the bond axis and allows for free rotation.

The two additional bonds in a triple bond are pi bonds, which are formed by the side-by-side overlap of p orbitals. These pi bonds are located above and below the plane of the atoms involved in the bond, resulting in a strong bond due to the presence of multiple interactions between the atoms. The presence of one sigma bond and two pi bonds contributes to the overall strength and stability of the triple bond, making it one of the strongest types of covalent bonds.

In contrast, single bonds consist of one sigma bond only, and double bonds have one sigma bond and one pi bond. Network covalent bonds involve a three-dimensional structure of interconnected atoms, but do not fit the definition as provided for this question.