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Unformatted text preview: CH101/Ison Ch2 Worksheet Name:________, __________ last, first Orbital Energy Diagram + Energy + Energy + Energy + Energy Four quantum numbers are assigned to each electron, n, l, m l , and m s . n- the principle quantum number which corresponds to the level the electron is on. l- describes the shape of the subshell, which the electron is occupying (s = 0, p = 1, d=2, etc.) m l- describes the direction in space of the orbital (x,y,z) m s- the spin quantum number which is + or -. Rules for filling orbital energy diagrams: 1. Aufbau principle: The lowest energy levels must be filled first and in order. 2. Pauli exclusion principle: Two electrons in the same orbital have the same values of n, l, m l , so they must have opposite spins. Thus an orbital can accommodate no more than two electrons. 3. Hunds rule: Each orbital in a subshell (s, p, d, f) must be filled one electron at a time with all electrons having the same spin. Electrons may be paired only after each orbital has one electron in it. CH101/Ison...
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