Apart from two electrons paired in the 1s orbit, each oxygen atom has four electrons distributed in four non-isothermal orbits, two of which are not paired. The molecular orbits are shown in Fig. . Each bond should have the same bond energy because the temperatures of orbits are equal. For N2, there are three unpaired electrons. As shown in Fig. , the bond status may be variable between three non-isothermal orbits and one isothermal orbit because all the initial temperatures of electrons are equal. The homo-pair and hetero-pair of electrons are indistinguishable. Therefore, an oscillating structure is a rational proposal. This means that the bond energy should be close to single-bond energy rather than the total energy of three single-bonds. Figure , Scheme of bonds in O2 and N2 bonds Two isothermal electrons constitute the bonds as mentioned above. For two non-isothermal electrons, using H2O as an example, the radius of an H atom is 53 pm, longer than that of oxygen, 48 pm. Meanwhile, the temperature of an H electron is T0=1.049×10 5 K, whereas, for an O atom, the temperature of surface electrons is T0=1.158×10 5 K (Tab. 2). When the O-H bond forms, the O electron transfers heat to the H electron by elongating the radius of the new orbit. Since the temperature is inversely proportional to the radius, provided the new temperature is the average of two temperatures, 𝑟 = = 50.376 pm. Meanwhile, Eq. 54 should be revised.