Answer:



The classical electromagnetic theory, also known as classical electrodynamics, describes the behavior of electric and magnetic fields and their interactions with charged particles. This theory was developed by James Clerk Maxwell in the 19th century and forms the foundation of classical physics. When applied to the atomic model, certain statements can be made about the behavior of electrons and the radiation they emit.



According to classical electromagnetic theory, electrons orbiting the nucleus would lose energy due to electromagnetic radiation and eventually spiral inwards. This concept is known as the "classical electron radius" or the "classical electron problem." However, this statement is incorrect because it contradicts experimental observations and the principles of quantum mechanics.

In reality, electrons do not spiral into the nucleus. The behavior of electrons is governed by quantum mechanics, where electrons are described by wave-like functions called orbitals. These orbitals define the probability distribution of finding an electron in a given region around the nucleus. The concept of discrete energy levels and stable electron orbits is explained by quantum mechanics, not classical electrodynamics.



This statement is correct. According to classical electromagnetic theory, when an electron accelerates or changes its energy state within an atom, it emits electromagnetic radiation in the form of waves. However, the energy of these waves is not continuous but rather quantized. This means that the energy emitted by an electron is restricted to specific discrete values, corresponding to the energy level transitions within the atom.

This concept is the basis of the Bohr model of the atom, which combines classical electrodynamics with quantum principles. The Bohr model explains the discrete spectral lines observed in atomic emission and absorption spectra, where each line corresponds to a specific energy transition of an electron.



This statement is incorrect. According to classical electromagnetic theory, accelerating charges, such as electrons, do radiate electromagnetic waves. When an electron changes its velocity or direction, it emits radiation. This phenomenon is known as "Bremsstrahlung" or "braking radiation." However, classical electrodynamics is not sufficient to fully explain the behavior of electrons in atoms; quantum mechanics must be considered.

In the quantum mechanical description, electrons occupying stable energy levels do not radiate electromagnetic waves. They remain in their respective energy states without any energy loss. Only when an electron undergoes a transition between energy levels will it emit or absorb discrete amounts of energy in the form of electromagnetic radiation.



This statement is incorrect. According to classical electrodynamics, the positive charge of the nucleus and the negative charge of the electron do not cancel each other out entirely. The electron orbits around the nucleus due to the attractive electrostatic force between the positive and negative charges. This interaction gives rise to the stability of the atom.

Furthermore, as mentioned earlier, accelerating charges such as electrons do radiate electromagnetic waves according to classical electrodynamics. However, in the context of stable electron orbits and energy levels