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Erwin Schrodinger formulated Quantum Mechanical Method which predicted the probability of where an electron would be in an atom S-level shell 1 plane, 2 electrons P-level shell 3 planes, 6 electrons D-level shell 5 planes, 10 electrons F-level shell 7 planes, 14 electrons atomic orbital region of space surrounding the nucleus of an atom where there is the highest probability of finding an electron of a certain energy configuration depending on the amount of electrons present in the atom Order of Atomic Energy Shells 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p Aufbau Principle states that electrons enter energy shells of the lowest energy first Pauli Exclusion Principle states that an orbital can accommodate at most 2 electrons, and those electrons must have opposite spin Hunds Rule states that electrons enter energy shells in such a way as to accommodate electrons of the same spin in an energy orbital first wavelength measurement of wave from crest to crest frequency of light symbolized by v, measure of number of waves that pass a measuring point in 1 second, measures in Hertz amplitude measurement on wave from baseline to the top of the crest of the wave wavelength x frequency= speed of light, 2.998x10^10 visible light is electromagnetic Planks Constant h= 6.626x10^-34 J.S Louis de Brogile postulated that all moving objects move in waves Werner Heisenberg stated that it was impossible to know the exact position of an electron in its orbital, called Heisenberg Uncertainty Principle