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

I am 100% lost please help

Answer 2

The first ionisation energy is the energy required to remove the most loosely held electron from one mole of gaseous atoms to produce 1 mole of gaseous ions each with a charge of 1+. There are factors affecting the ionization energy.
1)The charge on the nucleus.
2)The distance of the electron from the nucleus.
3)The number of electrons between the outer electrons and the nucleus.
4)Whether the electron is on its own in an orbital or paired with another electron but this is not a major one when talking about a single element. this factor may be used when comparing between two elements

1)The more protons there are in the nucleus, the more positively charged the nucleus is, and the more strongly electrons are attracted to it reulting in more energy to remove.

2)An electron close to the nucleus will be much more strongly attracted than one further away.

3)Consider a Aluminium atom, with the electronic structure 2,8,3.
Between the 3rd shell and the nucleus two other shells of electrons in the first and second levels. the effect of the positive nuclear charge is less felt because of the other 10 inner electrons. As the three electrons in the n=3 are removed screening effect decreases because its more closer to the nucleus.

I hope this helps :)

Answer 3

thank you