Orbitals and quantum numbers

Orbitals and quantum numbers - Orbitals and quantum numbers...

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Orbitals and quantum numbers Solving Schrödinger's equation for the hydrogen atom results in a series of wave functions (electron probability distributions) and associated energy levels. These wave functions are called orbitals and have a characteristic energy and shape (distribution). The lowest energy orbital of the hydrogen atom has an energy of -2.18 x 10 18 J and the shape in the above figure. Note that in the Bohr model we had the same energy for the electron in the ground state, but that it was described as being in a defined orbit . The Bohr model used a single quantum number (n) to describe an orbit , the Schrödinger model uses three quantum numbers: n, l and m l to describe an orbital . The principle quantum number 'n' Has integral values of 1, 2, 3, etc. As n increases the electron density is further away from the nucleus As n increases the electron has a higher energy and is less tightly bound to the nucleus The azimuthal (second) quantum number 'l' Has integral values from 0 to (n-1) for each value of n
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Orbitals and quantum numbers - Orbitals and quantum numbers...

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