The correct answer is $\boxed{\text{O}_2}$.
The bond order is a measure of the strength of a covalent bond. It is calculated by taking the number of bonding electrons minus the number of antibonding electrons and dividing by two. The bond order of $\text{O}_2$ is 2, while the bond orders of $\text{O}^+_2$, $\text{O}^-_2$, and $\text{O}^{2-}_2$ are 1, 0, and 1, respectively. Therefore, $\text{O}_2$ has the highest bond order.
The bond length is the distance between the nuclei of two atoms that are bonded together. The bond length of $\text{O}_2$ is 121 pm, while the bond lengths of $\text{O}^+_2$, $\text{O}^-_2$, and $\text{O}^{2-}_2$ are 128 pm, 149 pm, and 142 pm, respectively. Therefore, $\text{O}_2$ has the shortest bond length.
The bond strength is a measure of the energy required to break a covalent bond. The bond strength of $\text{O}_2$ is 498 kJ/mol, while the bond strengths of $\text{O}^+_2$, $\text{O}^-_2$, and $\text{O}^{2-}_2$ are 495 kJ/mol, 492 kJ/mol, and 490 kJ/mol, respectively. Therefore, $\text{O}_2$ has the maximum bond strength.
In summary, $\text{O}_2$ has the highest bond order, shortest bond length, and maximum bond strength.