Question

As each electron is removed, one at a time, from an atom of aluminum, more ionization energy is required. Between which two successive ionization energies would you expect the greatest difference (largest change in value)? Explain your answer in terms of attraction, repulsion, and electron arrangement.

Answer 1

the electron configuration is 1s2 2s2 2p6 3s2 4s1. so i figured that the greatest difference would be between the first and second?? since the first one is in 4s and the second is in a completely different level? is that right?

Answer 2

first ionization energy is removing electron from an neutral atom hence its having low energy.
after removing one electron the charge on atom become positive and also the attraction between the nucleus and electron increases as result more energy should be put to remove the second electron.
Between the 2 electrons removed and still u want to remove another one this ionization energy is of great difference

Answer 3

so i'm right..?

Answer 4

yeah dawg

Answer 5

are you sure

Answer 6

Ionization energy is removing electrons from an neutral atom, because of this, it has low energy.
After removing one electron the charge on the atoms become positive and also the attraction between the nucleus and electron increases. This results in, more energy which removes the second electron. You still want to remove another electron after the 2 you already removed

Answer 7

what i said is right

Answer 8

there's not really an answer in what you said though

Answer 9

1st I.E. = 577 kJ mol-1
2nd I.E. = 1820 kJ mol-1
3rd I.E. = 2740 kJ mol-1
4th I.E. = 11600 kJ mol-1

Answer 10

so it's between the third and fourth??

Answer 11

between the 3rd from last and 2nd to last will likely be the largest difference