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Stable electronic configurations refer to fully filled electronic orbitals. The elements with stable electronic configurations are also known as noble gases. During chemical bonding (whether ionic or covalent), all the elements tend to gain or lose or share electrons to achieve stable electronic configurations.
All the three elements listed in the question: helium, xenon and neon are noble gases and have stable electronic configurations.
The atomic number of helium is 2 and its electronic configuration is `1s^2` .
The atomic number of neon is 10 and its electronic configuration is `1s^2, 2s^2, 2p^6` .
The atomic number of xenon is 54 and its electronic configuration is `1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 3d^10, 4s^2, 4p^6, 4d^10, 5s^2, 5p^6` .
In all three cases, we can see that outermost electronic orbitals are completely filled and hence the elements have stable electronic configurations.
Hope this helps.
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