between which 2 ionization energies (1-5) would you expect to see a big jump for an element having the electron configuration 1s2 2s2 2p6 3s2 3p1?
im sorry but i don't understand this at all! thank you
im sorry but i don't understand this at all! thank you
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Between the first and the second, and then a larger one between the 3rd and 4th.
The first ionization removes 1 electron from the 3p subshell. The next ionization will have to break up a filled 3s subshell. The 4th ionization will then have to remove an electron from a completely filled shell. Each of those ionizations is much more difficult than the one before it.
The first ionization removes 1 electron from the 3p subshell. The next ionization will have to break up a filled 3s subshell. The 4th ionization will then have to remove an electron from a completely filled shell. Each of those ionizations is much more difficult than the one before it.
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Well the element is Aluminum . And I believe the biggest jump would be between 1 and 5 because it has to travel from the ground state to the 5th energy level . I could be wrong .
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I am not sure what you mean. But Al has a valence of 3+ in which it has to lose its 3s2 and 3p1 electrons, which seem more difficult than Na and Mg where only the 3s2 electrons are involved.