![]() ![]() This observation is connected to the discrete nature of the allowed energies of a quantum mechanical system. In 1913, the Danish physicist Niels Bohr proposed a model of the electron cloud of an atom in which electrons orbit the nucleus and were able to produce atomic spectra. ![]() Phosphorus is neutral and its atomic number is 15, hence, the number of protons and electrons available for its Bohr diagram is also 15. It is observed that line spectra discussed in the previous sections show that hydrogen atoms absorb and emit light at only discrete wavelengths. The Bohr model of Phosphorus (P) is drawn with three electron shells, the first shell contains 2 electrons, the second shell contains 8 electrons and the third shell contains 5 electrons. Bohr's model suggests that the atomic spectra of atoms is produced by electrons gaining energy from some source, jumping up to a higher energy level, then immediately dropping. From this, it is easy to see that like charges (charges of the same sign) repel each other. Bohr's model suggests each atom has a set of unchangeable energy levels, and electrons in the electron cloud of that atom must be in one of those energy levels. If \(Q_1\) and \(Q_2\) are the same sign, then the curve which is a purely repulsive potential, i.e., the energy increases monotonically as the charges are brought together and decreases monotonically as they are separated. ![]()
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