Respuesta :
Answer is: They orbit the central nucleus in discrete paths.
According to the Bohr model of the atom:
1. Electrons orbit the nucleus in orbits that have a set size and energy.
2. Energy levels of electrons are discrete (certain discrete values of energy).
3. Electrons can jump from one energy level to another, absorbing or emitting electromagnetic radiation with a frequency ν (energy difference of the levels).
The most appropriate statement that describes the Neils Bohr’s atomic model is
[tex]\boxed{{\text{they orbit the central nucleus in discrete paths}}}[/tex]
Further Explanation:
Postulates of Bohr’s atomic model:
1. The electrons revolve in definite orbits that are present around the nucleus. These orbits were represented either as 1, 2, 3,… or K, L, M, N,…and so on.
2. Electrons neither gain energy nor lose energy as long as it is present in a specific orbit. So these were called as stationary orbits or stationary states.
3. When an electron from its orbit jumps to any other orbit, be it higher or lower in energy then absorption or emission of energy occurs. The electron absorbs energy when it jumps from lower orbit to the higher one. It loses energy while coming to lower orbit from the higher one. This emission or absorption of energy occurs in the form of radiations.
4. The allowed orbits are those having their angular momentum quantized. Its value is an integral multiple of [tex]\frac{h}{{2\pi }}[/tex] .
Merits of Bohr’s atomic model:
1. It explained the stability of an atom. As long as the electron is present in the same orbit, it neither gains nor loses energy and therefore electron can never fall into the nucleus of an atom, resulting in its stability.
2. It explained the atomic spectra of hydrogen and hydrogen-like atoms. The experimental values of spectral lines of hydrogen atoms come out to be in close agreement with that of Bohr’s model.
Demerits of Bohr’s atomic model:
1. Bohr’s atomic model failed to explain the concept of atomic spectra of multi-electron atoms.
2. It could not explain the dual nature of electrons. Bohr’s model considers electron only as a particle, but not as a wave. So it was not in agreement with the de-Broglie hypothesis.
3. It could not explain Stark effect (effect of electric field on spectral lines) and Zeeman effect (effect of magnetic field on spectral lines).
4. It could not justify Heisenberg’s uncertainty principle.
Niels Bohr’s atomic model considers the nucleus to be similar to the sun and the electrons revolving around it to be similar to the planets. So the electrons are like the planets that revolve around the sun. Therefore, electron does not revolve in any random orbit but only in certain discrete orbits whose energies are quantized
Learn more:
1. Oxidation and reduction reaction: https://brainly.com/question/2973661
2. The main purpose of conducting experiments: https://brainly.com/question/5096428
Answer details:
Grade: High School
Subject: Chemistry
Chapter: Atomic structure
Keywords: Atomic model, Rutherford model, electromagnetic theory, nucleus, electron orbit, quantized, energy level, angular momentum, photon, principal quantum number, postulates, stationary state, Planck’s constant.
