CHEM 1300 Lecture Notes - Lecture 4: Uncertainty Principle, The Dilemma, Bohr Model
19 Nov 2017
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10 19 q ( electron = 1. A particle occupies a particular location, but a wave has no exact position. particular location or a variety of location. Because of their wave like properties, electrons are always spread out in space. as a result, the position of an electron cannot be precisely defined. therefore, electrons are delocalized, rather than pinpointed. The heisenberg uncertainty principle - the more accurately we know position, the more we are about motion and vice versa. So instead, we identify probable location of the electrons in an atom, not an exact one. From absorption and emission spectra of atoms, we know that electron energies are quantized when they are bound to a nucleus. Note that free electrons can take any energy. The bohr model attempts to explain this, bit it has several flaws. The bohr doesn"t take into account the wave particle duality of the electron. It only works for one electron system.
