Boiling point of oxygen
According to NIST Chemistry Webbook, for oxygen: 

$$T_\mathrm{boil} = \pu{90.2\pm0.2 K}$$
$$T_\mathrm{fus} = \pu{54.8\pm0.2 K}$$
$$T_\mathrm{triple} = \pu{54.33\pm0.6 K}$$

The $T_\mathrm{boil}$ and $T_\mathrm{fus}$ are from Ref.1 while Brower and Thodos reported $T_\mathrm{triple}$ as $\pu{54.363 K}$ at pressure of $\pu{1.125 mmHg}$ (Ref.2). The uncertainties were given by Thermodynamics Research Center, NIST Boulder Laboratories, CO.

Accordingly, $T_\mathrm{boil} = \pu{-183 ^\circ C}$, $T_\mathrm{fus} = \pu{-218.4 ^\circ C}$, and $T_\mathrm{triple} = \pu{-218.8 ^\circ C}$. Therefore, as you correctly suspected, the values in the textbook is a misprint.

References:


Alex G. Streng, “Miscibility and compatibility of some liquefied and solidified gases at low temperatures,” J. Chem. Eng. Data 1971, 16(3), 357-359 (https://doi.org/10.1021/je60050a024).
Gerald T. Brower, George. Thodos, “Vapor pressures of liquid oxygen between the triple point and critical point,” J. Chem. Eng. Data 1968, 13(2), 262-264 (https://doi.org/10.1021/je60037a038).