Debye discusses the radiation of electrons in atoms, noting that despite high accelerations, electrons may not emit radiation. In a hydrogen molecule, two electrons orbit in a circle with a diameter of 1.05·10⁻⁸ cm, moving at a angular velocity of 4.21·10¹⁶ 1/sec. Calculations based on Maxwell-Lorentz equations suggest this motion emits enormous radiation, but the actual kinetic energy is much smaller, implying the molecule would self-destruct in 10⁻⁸ seconds. However, this contradicts the hypothesis of quantized electron motion, which must be considered radiation-free. Debye also explains how the usual dispersion can be fully explained without abandoning known principles of mechanics and electromagnetism. This implies that disturbances in the electron paths behave regularly. When measuring scattered radiation from an atomic wave, J. J. Thomson showed that the radiation follows electromagnetic laws, allowing the determination of the number of electrons per atom. Debye then calculates the scattered energy and spatial distribution for a randomly oriented collection of atoms with electron rings. The calculation shows that the total scattered radiation is proportional to the square of the number of electrons and resembles a dipole distribution. As the wavelength decreases, the radiation becomes proportional to the first power of the electron number, maintaining a dipole-like spatial distribution except near the direction of the incident radiation. Debye discusses the spatial intensity distribution of scattered radiation, linking it to the Friedrichs' interference patterns. He shows that even with random atomic orientations, regular electron arrangements within atoms can produce interference effects. For hydrogen, the scattered intensity depends on the angle between the observation and incident directions, showing asymmetry and interference patterns. These patterns are consistent with the known Friedrichs' interference observations, indicating regular electron arrangements within atoms. Debye concludes that the electron rings in atoms provide the key to understanding the Friedrichs' interference phenomenon. By observing scattered radiation, one can determine the electron arrangements within atoms, offering a method for ultramicroscopic analysis of atomic structures. The calculations show that the intensity of scattered radiation depends on the wavelength and the number of electrons, with interference patterns appearing for small wavelengths. This supports the idea that electron rings in atoms are regular and can be experimentally verified.Debye discusses the radiation of electrons in atoms, noting that despite high accelerations, electrons may not emit radiation. In a hydrogen molecule, two electrons orbit in a circle with a diameter of 1.05·10⁻⁸ cm, moving at a angular velocity of 4.21·10¹⁶ 1/sec. Calculations based on Maxwell-Lorentz equations suggest this motion emits enormous radiation, but the actual kinetic energy is much smaller, implying the molecule would self-destruct in 10⁻⁸ seconds. However, this contradicts the hypothesis of quantized electron motion, which must be considered radiation-free. Debye also explains how the usual dispersion can be fully explained without abandoning known principles of mechanics and electromagnetism. This implies that disturbances in the electron paths behave regularly. When measuring scattered radiation from an atomic wave, J. J. Thomson showed that the radiation follows electromagnetic laws, allowing the determination of the number of electrons per atom. Debye then calculates the scattered energy and spatial distribution for a randomly oriented collection of atoms with electron rings. The calculation shows that the total scattered radiation is proportional to the square of the number of electrons and resembles a dipole distribution. As the wavelength decreases, the radiation becomes proportional to the first power of the electron number, maintaining a dipole-like spatial distribution except near the direction of the incident radiation. Debye discusses the spatial intensity distribution of scattered radiation, linking it to the Friedrichs' interference patterns. He shows that even with random atomic orientations, regular electron arrangements within atoms can produce interference effects. For hydrogen, the scattered intensity depends on the angle between the observation and incident directions, showing asymmetry and interference patterns. These patterns are consistent with the known Friedrichs' interference observations, indicating regular electron arrangements within atoms. Debye concludes that the electron rings in atoms provide the key to understanding the Friedrichs' interference phenomenon. By observing scattered radiation, one can determine the electron arrangements within atoms, offering a method for ultramicroscopic analysis of atomic structures. The calculations show that the intensity of scattered radiation depends on the wavelength and the number of electrons, with interference patterns appearing for small wavelengths. This supports the idea that electron rings in atoms are regular and can be experimentally verified.