Bohr's Model Of An Atom

Danish physicist Niels Bohr in the early years of the twentieth century endeavour to develop the progressive atom theory that not only revolutionized the outlook on atomic form but also formed the new quantum theories of modern times. Bohr’s version succeeded in overcoming the limitation of classical physics regarding the stability of atoms and the inherent line atomic spectra. At the center of Bohr’s model are several postulates suggested, in addition to the traditional tenets of classical mechanics.

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This Story also Contains

1. Bohr's Model and its Postulates: Atomic Blueprint-
2. Solved Examples Based On (Bohr's Postulate)-
3. Conclusion

The postulates suggested by Bohr are-

Firstly, Bohr introduced that electrons in atoms are capable of being located only in certain discrete energy levels, referred to as orbits or electricity levels, each possessing a definite power value. Electrons do not have to go to intermediate stationary states to change orbital states, as they can gain or lose energy in the process of absorption or emission of power in a discrete quantum proportionate to the difference in these energy levels.

Secondly, Bohr introduced the rule that the electrons in a stable orbit cannot lose energy in the form of radiation, which was in contrast with the classical explanation of charged particles continuously emitting radiation. This brought them to the thought of ‘bound’ states, in which the electrons remain confined in their solid orbits and do not emit energy in the form of radiation.

In this article, we will cover the concept of Bohr's model and its postulates. This concept falls under the broader category of Atomic structure, which is a crucial chapter in Class 11 chemistry. It is not only essential for board exams but also for competitive exams like the Joint Entrance Examination (JEE Main), National Eligibility Entrance Test (NEET), and other entrance exams such as SRMJEE, BITSAT, WBJEE, BCECE, and more.

Bohr's Model and its Postulates: Atomic Blueprint-

Bohr’s model was proposed to be an improvement of the planetary model and was for the same reason developed; it included the electrons circling in orbits around the nucleus and in these orbits, they were only allowed to exist in certain fixed and discrete energy levels as opposed to the planetary model which predicted that electrons would move in free and smooth paths like planets around a star. These levels are quantized in the sense that they have been allocated specific values and an electron can only transfer from one level to another in quanta of energy equal to the difference between the two levels.

Bohr’s model also gave some explanation for the phenomenon that is known as stationary states, whereby the electrons in their stable orbits do not radiate as perceived by classical theories. This model was able to thoroughly account for the spectrum of hydrogen and also paved the way for something that turned out to be quantum mechanics. Even though there are significant weaknesses in Bohr’s model like the inability to explain the phenomena of multielectron atoms, this model is considered one of the important steps in the development of atomic theory as it gives a proper understanding of the electron behaviour in an atom.

1. The electron in the hydrogen atom can move around the nucleus in a circular path of fixed radius and energy. These paths are called orbits, stationary states, or allowed energy states and are arranged concentrically around the nucleus. The force of attraction between the nucleus and an electron provides the centripetal force required by the electron to carry out the circular motion.

2. The energy of an electron in the orbit does not change with time. However, the electron will move from a lower stationary state to a higher stationary state when the required amount of energy is absorbed by the electron or energy is emitted when an electron moves from a higher stationary state to a lower stationary state

3. Energy can be absorbed or emitted when an electron transitions between two different orbits, and the frequency of the photon involved can be calculated using the formula:

$\left|E_1-E_2\right|=h \nu$

4. The angular momentum of an electron is quantized. In a given stationary state, it can be expressed as

L= mvr= nh/2, n = orbit number

So only those energy states (or orbits) are allowed in which the above equation holds for the angular momentum.

Note: Bohr's model is only valid for Hydrogen species or electronic species that contain only a single electron.

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Solved Examples Based On (Bohr's Postulate)-

Example 1: Which of the following statements is incorrect for Bohr's model of an atom?

1) (correct) It is valid for a multi-electronic species

2) The angular momentum of an electron is quantized

3) The centripetal force of attraction required for circular motion is provided by the electrostatic force of attraction between the electron and the nucleus

4) Orbits have fixed energy and are referred to as stationary states

Solution:

Bohr's model is valid for only uni-electronic species.

All other given statements given in the options are correct.

Hence, the answer is the option (1).

Example 2:

Which of the following is incorrect for Bohr's model of an atom?
1) (correct) It is valid for multi-electronic species.
2) The angular momentum of an electron is quantized.
3) The centripetal force of attraction required for circular motion is provided by the electrostatic force of attraction between the electron and the nucleus.
4) Orbits have fixed energy and are referred to as stationary energy.

Solution

Bohr's model is valid for electronic species only.

Hence, the answer is the option (1).

Conclusion

The version that was presented by Bohr was able to explain the spectral traces of hydrogen. Bohr’s model of the atom can be viewed as a scientifically critical stage in the paradigm shift from the old paradigm of classical physics to the new approaches of the modern quantum mechanics paradigm. While Bohr’s model had some problems, such as its inability to deliv­er a qualitative description of multielectron atoms and the quantization of angular momentum, it was useful in develop­ing an early atomic model that helped accurately describe atomic spectra.