Explain why the atomic emission spectrum contains certain frequencies of light

Explain why the emission spectrum Atomic emission spectrum contains certain frequencies of light is a general question in secondary chemistry and your future career is related to excellence in chemistry. These colors did not change for a single element, and this was considered the signature of the element, but the reason is unknown. Explain why the emission spectrum has the higher the energy of an electron, the farther away from the nucleus its orbit is. Each electron has a certain energy level.Explain why the atomic emission spectrum contains certain frequencies of lightExplain why the emission spectrum contains theDirect answer: Since the energies of atoms are finite, so only certain frequencies are emitted from the radiation emitted by the atom, But to fully understand the answer, you must know the following: Explain why the emission spectrum, after the heating process of a pure element, contains the excitation of its electrons, and electromagnetic waves are produced by this process, and the atomic emission is the relative intensity that characterizes the resulting waves. It contains the atomic emission spectrum . What distinguishes the atomic emission spectrum is the ability to distinguish elements from it, as no two chemical elements have the same spectrum, so by measuring the sun’s spectrometer for example, we conclude that it consists of helium and hydrogen. Therefore, the answer to a question explaining why the atomic emission spectrum contains frequencies A certain type of light according to Bohr's atomic model is: Since the energy of an atom of a particular element is known and determined, certain frequencies of radiation are emitted from it. For further clarification, follow us for the rest of the article. Bohr's atomic model. Explain why the emission spectrum is contained, for the scientist Niels Bohr, who proposed this model To represent the internal structure of the atom, his model relies on the interpretation of the spectral lines emitted by the hydrogen atom, and in the following steps we explain the most important features of Bohr’s model: Scientists noticed in the late nineteenth century that when the energy of the atoms of a particular element increases, they radiate specific bright colors and that these colors did not change for any particular element. It was considered a fingerprint of the element, but the reason why was not known. For example, if we pass an electric current through hydrogen gas (H2), the hydrogen will split into atoms (H), and we will see with the naked eye that it emits a distinctive light of one color, while if we pass the resulting The resulting light output through a glass prism, will be split into 4 colors using a wavelength finder and whenever we repeat the experiment, we get the same result. Explain why the emission spectrum contains the atomic spectrum, then, since it is the specific colors that are emitted as a result of the excitation of the pure element. Explain why Emission spectrum containment By 1913, Niels Bohr used Rutherford's atomic model, which showed that the atom consisted of negative electrons orbiting a positively charged nucleus. In explaining the frequency emitted by the hydrogen atom. Bohr's explanation was the key to understanding the movement of electrons around the hydrogen nucleus. In Bohr's model, it is shown that: Electrons revolve around the nucleus of the atom