Why is the electron configuration for Ni 1s2 2s2 2p4 3s4 3p4 4s2 3d8 and not 1s2 2s2 2p4 3s4 3p4 3d10?

1 Answer
Aug 22, 2016

Neither electron configuration for Nickel is correct.

Explanation:

An s sublevel can only hold two electrons because it has only one orbital. Each orbital in any sublevel can hold only two electrons. Both of the electron configurations in your question have a 3s4 sublevel, which is impossible.

The atomic number for nickel is 28. If it is neutral, one atom of nickel has 28 protons and 28 electrons. Both of the electron configurations for nickel in your question have only 26 electrons.

In the second configuration, the 4s2 sublevel is missing.

Nickel's electron configuration is 1s22s22p63s23p64s23d8. The 4s sublevel fills before the 3d sublevel because the 4s sublevel has lower energy than the 3d sublevel.

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