Bohr's Atomic Model: A Highlight To Knowledge Enlightenment.

Bohr's atomic model is a presentation that was proposed by a prominent scientist named Niels Bohr. His model became a significant contribution to understanding the movement and placement of atoms, how they behave in living and non-living things, and why they are constantly repeating a cycle. However, some scientists believe that Bohr's model may have limitations.

1. A HIGHLIGHT TO ENLIGHTENING OUR KNOWLEGDE ABOUT WHAT’S INSIDE EACH AND EVERYONE OF US BOHR’S ATOMIC MODEL

2. Bohr’s atomic model, proposed by niels bohr in 1913, was a groundbreaking step in our understanding of the atom’s structure. It was a significant improvement over earlier models, like Rutherford’s, and helped explain several key observations about atomic behavior.

3. Niels Henrik david bohr (1885-1962) Niels bohr was a Danish physicist who made foundational contributions to understanding the atomic structure and the quantum theory, to which he received the noble prize in physics in 1922 . he was born on October 7, 1885 and died on November 18, 1962. he was also a philosopher and a promoter of scientific research.

4. Bohr’s model of the atom Bohr developed his atomic model, in which he proposed that energy levels of electrons are discrete and that the electrons revolve in stable orbits around the atomic nucleus, but can jump from one energy level or orbit to another. His model is more often called the planetary model because of its resemblance to the solar system 1. NUCLEUS AT THE CENTER Bohr proposed that the atom’s positively charged nucleus (containing protons and neutrons) resides at the center. 2. ELECTRONS ORBITING THE NUCLEUS Electrons, negatively charged particles, orbit the nucleus in specific, circular paths called ENERGY LEVELS or ELECTRON SHELLS. These orbits are quantized, meaning electrons can only exist in specific, discrete energy levels. 3. ENERGY LEVELS Each energy level corresponds to a fixed energy value. Electrons in the innermost shell have the lowest energy, and those in outer shells have higher energy. Electrons can jump from one energy level to another by absorbing or emitting energy in the form of light (photons). 4. QUANTIZED ENERGY Bohr’s model emphasizes that electrons can only occupy specific energy levels and that the energy transitions between these levels are quantized, meaning they occur in discrete steps. This explains the emission of specific wavelengths of light when excited atoms return to their ground state.

5. 5 . GROUND STATE AND EXCITED STATE An atom is in its ground state when its electrons occupy the lowest possible energy levels. When an atom absorbs energy (for example, from heat or light), its electrons can jump to higher energy levels, putting the atom in an excited state. As the excited electrons return to their ground state, they emit photons of light at specific wavelengths, leading to the characteristic emission spectrum of each element.

6. THE Bohr model is a relatively primitive model of the hydrogen atom, compared to the valence shell model . As a theory, it can be derived as a first-order approximation of the hydrogen atom using the broader and much more accurate quantum mechanics, and thus may be considered to be an obsolete scientific theory. However, because of its simplicity, and its correct results for selected systems, the bohr model is still commonly taught to introduce students to quantum mechanics or energy level diagrams before moving on to the more accurate, but more complex, valence shell atoms.

7. RYDBERG FORMULA THE MODEL’S KEY SUCCESS LIES IN EXPLAINING THE RYDBERG FORMULA FOR HYDROGEN’S SPECTRAL EMISSION LINES. WHILE THE RYDBERG FORMULA HAD BEEN KNOWN EXPERIMENTALLY, IT DID NOT GAIN A THEORITICAL BASIS UNTIL THE BOHR MODEL WAS INTRODUCED. NOT ONLY DID THE BOHR MODEL EXPLAIN THE REASONS FOR THE STRUCTURE OF THE RYDBERG FORMULA, IT ALSO PROVIDED A JUSTIFICATION FOR THE FUNDAMENTAL PHYSICAL CONSTANTS THAT MAKE UP THE FORMULA’S EMPIRICAL RESULTS.

8. LIMITATIONS OF BOHR’S ATOMIC MODEL The bohr model is very limited in terms of size. Poor spectral predictions are obtained when larger atoms are in question. It cannot predict the relative intensities of spectral lines. It does not explain the Zeeman effect, when the spectral line is split into several components in the presence of a magnetic field. 1. it failed to give an explanation about the stability of the atom. 2. it failed to explain the arrangement of electrons around the orbit. 3. the model also couldn’t give the reason for the presence of discrete lines in the spectrum of atoms with more than 3 electrons.