Explain Hunds rule with an example
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Hund 's rule states that: Every orbital in a sublevel is singly occupied before any orbital is doubly occupied. All of the electrons in singly occupied orbitals have the same spin (to maximize total spin).
Consider the correct electron configuration of the nitrogen (Z = 7) atom: 1s2 2s2 2p3
The p orbitals are half-filled; there are three electrons and three p orbitals. This is because the three electrons in the 2p subshell will fill all the empty orbitals first before pairing with electrons in them.
Keep in mind that elemental nitrogen is found in nature typically as dinitrogen, N2, which requires molecular orbitals instead of atomic orbitals as demonstrated above.
Consider the correct electron configuration of the nitrogen (Z = 7) atom: 1s2 2s2 2p3
The p orbitals are half-filled; there are three electrons and three p orbitals. This is because the three electrons in the 2p subshell will fill all the empty orbitals first before pairing with electrons in them.
Keep in mind that elemental nitrogen is found in nature typically as dinitrogen, N2, which requires molecular orbitals instead of atomic orbitals as demonstrated above.
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Hund's rule of maximum multiplicity is a rule based on observation of atomic spectra, which is used to predict the ground state of an atom or molecule with one or more open electronic shells.
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