Writing electronic configurations

Writing electronic configurations - Writing electronic...

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Writing electronic configurations The two electrons in He represent the complete filling of the first electronic shell. Thus, the electrons in He are in a very stable configuration For Boron (5 electrons) the 5 th electron must be placed in a 2 p orbital because the 2 s orbital is filled. Because the 2 p orbitals are equal energy, it doesn't matter which 2 p orbital is filled What do we do now with the next element, Carbon (6 electrons)? Do we pair it with the single 2 p electron (but with opposite spin)? Or, do we place it in another 2 p orbital? The second 2p electron in Carbon is placed in another 2p orbital, but with the same spin as the first 2p electron: Hund's rule: for degenerate orbitals, the lowest energy is attained when the number of electrons with the same spin is maximized Electrons repel each other, by occupying different orbitals the electrons remain as far as possible from one another
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A carbon atom in its lowest energy (ground state) has two unpaired electrons
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This note was uploaded on 11/22/2011 for the course CHEMISTRY CHM1025 taught by Professor Laurachoudry during the Fall '10 term at Broward College.

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Writing electronic configurations - Writing electronic...

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