Bohr Theory
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| Assignment 2 | | Subject: General ChemistryLecturer: Dr. Ajith H. Herath | | Name: Kavini de Silva | 4/5/’013 | |
BOHR THEORY
Introduction
Niels Bohr applies quantum theory Rutherford’s Atomic Structure by assuming that electrons travel in stationary orbits defined by their angular momentum. This led to the calculation of possible energy levels for these orbits and the postulation that the emission of light occurs when an electron moves into a lower energy orbit.
Atomic Spectrum
The Atomic Spectrum is a series of lines of color produced when light from an excited atom is passed through a prism. It is also known as a line spectrum.
Each element has its own unique atomic spectrum. Because of their unique nature, atomic spectra are also referred to as the "fingerprints of the elements." The series of lines of color that an atom will produce is related to the locations of the electrons on that atom and their relationship with the nucleus. Atomic spectra were fundamental pieces of experimental information used by chemists in the development of the electronic structures of atoms. By studying the colors emitted by the different elements, it is possible to work backwards to the sources of those colors. In this way it is possible to determine the electronic structures of the elements. Most of the basic information known today about electronic structures was derived from studying the light emitted by the atoms. |
The process of exciting an atom, involves adding energy to the atom. This can be done in a variety of ways. Simply heating a sample of an element up in an open flame will excite electrons. Passing electricity through a sample of an element will excite electrons. The colored lights observed when sky rockets explode are a result of burning gunpowder exciting electrons within atoms of elements packed with the gun powder. |
| Assignment 2 | | Subject: General ChemistryLecturer: Dr. Ajith H. Herath | | Name: Kavini de Silva | 4/5/’013 | |
BOHR THEORY
Introduction
Niels Bohr applies quantum theory Rutherford’s Atomic Structure by assuming that electrons travel in stationary orbits defined by their angular momentum. This led to the calculation of possible energy levels for these orbits and the postulation that the emission of light occurs when an electron moves into a lower energy orbit.
Atomic Spectrum
The Atomic Spectrum is a series of lines of color produced when light from an excited atom is passed through a prism. It is also known as a line spectrum.
Each element has its own unique atomic spectrum. Because of their unique nature, atomic spectra are also referred to as the "fingerprints of the elements." The series of lines of color that an atom will produce is related to the locations of the electrons on that atom and their relationship with the nucleus. Atomic spectra were fundamental pieces of experimental information used by chemists in the development of the electronic structures of atoms. By studying the colors emitted by the different elements, it is possible to work backwards to the sources of those colors. In this way it is possible to determine the electronic structures of the elements. Most of the basic information known today about electronic structures was derived from studying the light emitted by the atoms. |
The process of exciting an atom, involves adding energy to the atom. This can be done in a variety of ways. Simply heating a sample of an element up in an open flame will excite electrons. Passing electricity through a sample of an element will excite electrons. The colored lights observed when sky rockets explode are a result of burning gunpowder exciting electrons within atoms of elements packed with the gun powder. |
References: file:///C:/Users/user/Desktop/Bohr%20model%20-%20Wikipedia,%20the%20free%20encyclopedia.htm file:///C:/Users/user/Desktop/Neils%20Bohr%20-%20Atomic%20Model.htm file:///C:/Users/user/Desktop/reading-37-Bohr-Atomic-Model-Theory.html